PIA CHEMISTRY I

LEARNING INTEGRATIVE PRODUCT CHEMISTRY I CICLE AGO-DIC 2016

UNIVERSIDAD AUTÓNOMA DE NUEVO LEÓN Preparatoria no. 9 Group 120

Equipo: Natalia Daenna González Viera Valery Selene García Morales Luis Roberto González Guajardo Anette Montserrat Salazar Esquivel Eduardo Ortega Corpus

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INDEX INTRODUCTION

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INTEGRATIVE ACTIVITY – STAGE 1 CHEMISTRY AND ITS CONTRIBUTION TO SCIENCE AND TECHNOLOGY PROGRESS

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INFORMATION ABOUT THE ACTIVITY (MADE VIDEO): CHEMISTRY IN MEDICINE, FOODSTUFF, WAR, AND THE GLOBAL WARMING

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INTEGRATIVE ACTIVITY – STAGE 2 ELEMENTS AND COMPOUNDS AROUND US

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INFORMATION ABOUT THE ACTIVITY: MAIN ELEMENTS IN THE HUMAN BODY CONCLUSION

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INTEGRATIVE ACTIVITY – STAGE 3 THE ATOM AND THE PERIODIC TABLE

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INFORMATION ABOUT THE ACTIVITY: CHEMICAL ELEMENTS AND ITS EVERYDAY APPLICATIONS CONCLUSION

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INTEGRATIVE ACTIVITY – STAGE 4 CHEMICAL BOND

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INFORMATION ABOUT THE ACTIVITY: CHEMICAL BONDS ON INDUSTRIAL USAGE SUBSTANCES CONCLUSION

CONCLUSION

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INTRODUCTION Did you know that everything is made out of chemicals? Chemistry is the study of matter: its composition, properties, and reactivity.

Chemistry is understanding substances and atoms. Everything is made of atoms!!!

If it wasn't for chemistry, we couldn't make fire, plastic, everything we have today.

Chemistry deals with practically everything (from basic food to complex machinery). From industries to agriculture, chemistry is a foundation to be built. Although most people don't look deeper into it, Chemistry is all around us especially in this age.

Almost all what we have experienced, observer, encountered everyday can be explained by chemistry and this made me conclude that chemistry is almost everything and its very important.

We can find chemistry in all the sciences. They help each other. I refer to the Physics, Biology, Agriculture, Medicine, Petrochemistry, and many others, which helps to live better and make for the human being a better world and a daily routine easier.

Every material in existence is made up of matter — even our own bodies. Chemistry is involved in everything we do, from growing and cooking food to cleaning our homes and bodies to launching a space shuttle. Chemistry is one of the physical sciences that help us to describe and explain our world.

Many inventions such as vulcanized rubber, nylon, Kevlar, aluminum production allowed the general technology to advance leaps ahead. Heavy industry, which includes heavy chemical industries provides materials which can be processed to form products.

New materials invented and laws researched in the area of chemistry in the last 300 years allowed the great technological advance we have now. For example, the table of chemical elements allowed people to understand that there are many different metals with different properties. Today the major role of chemistry in technology advance lies also in new material research, study of electrochemical processes such as corrosion, finding cheaper processes of materials production, etc. If you look closely around you, every human made object you can see takes advantage of some prior chemical research.

The unscrambled words such as iron, copper, gold, oxygen and carbon that we come across in our daily life are said to be elements.

The molecule of an element contains two or more similar atoms.

About 99% of the mass of human body is made up of six elements (oxygen, carbon, hydrogen, nitrogen, calcium and phosphorus) and the rest 1% by other elements.

You know that a generic atom has some protons and neutrons in the nucleus and some electrons zipping around in orbitals. When those pieces start combining in specific

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numbers, you can build atoms with recognizable traits. If you have eight protons, neutrons and electrons, you will have an oxygen (O) atom. If you have seven protons, neutrons, and electrons, you will have a nitrogen (N) atom. The atoms for each element are unique, even though they are all made of similar subatomic parts.

Remember that 'atom' is the general term. Everything is made of atoms. The term 'element' is used to describe atoms with specific characteristics. There are almost 120 known elements.

The periodic table is organized like a big grid. Each element is placed in a specific location because of its atomic structure. As with any grid, the periodic table has rows (left to right) and columns (up and down). Each row and column has specific characteristics.

For example, beryllium (Be) and magnesium (Mg) are found in column two and share certain similarities while potassium (K) and calcium (Ca) from row four share different characteristics.

Even though they skip some squares in between, all of the rows read left to right. When you look at the periodic table, each row is called a period (Get it? Like Periodic table.). All of the elements in a period have the same number of atomic orbitals. For example, every element in the top row (the first period) has one orbital for its electrons. All of the elements in the second row (the second period) have two orbitals for their electrons. As you move down the table, every row adds an orbital. At this time, there is a maximum of seven electron orbitals.

Chemical compounds are formed by the joining of two or more atoms. A stable compound occurs when the total energy of the combination has lower energy than the separated atoms. The bound state implies a net attractive force between the atoms ... a chemical bond. The two extreme cases of chemical bonds are: Covalent bond: bond in which one or more pairs of electrons are shared by two atoms.

Ionic bond: bond in which one or more electrons from one atom are removed and attached to another atom, resulting in positive and negative ions which attract each other.

Other types of bonds include metallic bonds and hydrogen bonding. The attractive forces between molecules in a liquid can be characterized as van der Waals bonds.

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STAGE 1 INTEGRATIVE ACTIVITY EFFECTS OF CHEMISTRY IN THE MODERN WORLD

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This activity was a video made by our team where we use puppets to make a funny and entertaining video about Chemistry: its contributions to medicine, its applications in food, how it impacts in the war and in the global warming; we also mentioned in the video the best alternatives that we considered to the problem “The melting of polar caps threats Mexico’s climate”. To finish the video, each one of us gave an individual and team posture.

We share the video called “The Science Show” in YouTube, divided into two parts, so you can watch it with the next links: FIRST PART: https://www.youtube.com/watch?v=itv88MMR-wQ SECOND PART: https://www.youtube.com/watch?v=W2ULFxL1R94

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Chemistry: Our Life, Our Future

We hardly ever think of how much chemical inventions and innovations tend to determine our everyday life: these achievements determine the quality and quantity of the foodstuff we have and the various methods of transportation; in addition, the warmth of our home and the speed of our recovery from illnesses also depend on the achievements of chemical research and development.

Along with the above, chemistry also lays the foundations of our future life by providing us with alternative, long-term solutions for energy management, environment protection, and the protection of our globe. The great innovations introduced in a wide range of research areas have had a powerful effect on our present as well as our future.

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Contributions of Chemistry in Medicine

Medicine, is a very crucial thing that we need at all time, but, chemistry do something in medicine? The answer is yes.

Have you ever think about why does doctors know that calcium is one of the many trace elements in the human body?

Did you know why calcium is a trace element?

Did you know what is a trace element?

Trace Elements are crucial elements that are found in the human body.

So, that means that calcium is in our body, and the job that calcium has in our body is very incredible!

Calcium is set on our bones, and it job is to make stronger bones, and with strong bones the body can maintain with himself. That's why the babies should drink a lot of milk, because milk is a product that have calcium to make the babies bones stronger.

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All this knowledge won't know if chemistry doesn't exist!

Incredible, right?

And we don't finish here, this is only one example of thousands of contributions of chemistry to medicine.

Chemistry has contributed many of the life-saving breakthroughs in health and medicine in the last century that allow us to live longer, happier, and healthier.

Throughout much of human history, medicine and health care was primitive. If people became sick or injured, doctors could do little more than comfort them and keep them clean. The last 100 years have revolutionized the way that doctors heal patients by curing disease, repairing injuries, and even preventing health problems before they occur. Hard-working chemists and chemical engineers have helped to found modern medicine by developing novel pharmaceuticals, creating new medical equipment, and refining diagnostic processes. Millions of human lives have been saved and improved by the health and medical advances developed through chemistry.

Chemistry is important in medicine because most diseases, injuries, and treatments involve chemicals and chemical processes. By understanding chemistry, we are able to develop drugs that fight disease, develop better nutrition, and develop healthier environments to avoid disease.

To make antibiotics, they use chemicals and they have an specific formula to make it perfect.

They also use chemistry to make anti-cancer drugs for people with cancer.

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Applications of Chemistry in Food

Chemistry is vital for the production of food. Chemistry makes the food grow, and chemistry determines how it is preserved to get to a market or a consumer.

For processed or sugary foods, chemistry and chemical compounds form part of their makeup.

Chemistry is actually used a great deal in food production. For example, when you cook anything, a chemical reaction is taking place, so the application of chemistry is vast in cooking.

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Chemistry has had a large influence on food production, so much so that there is now an entire section of chemistry solely related to food. Food chemistry is the study of chemical processes and interactions of all the components of foods, whether natural or created. Furthermore, food chemists work on creating new types of foods by manipulating molecules to create new kinds. They also use chemistry to create new techniques for food processing and preservation.

Chemistry in The War

The Great War or the 1st World War as it is also known, was the first war to take place around the world, to result in millions of casualties and to involve many of the civilians in the warring countries. Chemists and chemistry were involved from the start.

Men responded to the call to arms and chemists were amongst them. Ernest Rutherford’s team at Manchester University which had explored the structure of the atom began to disperse. Henry Moseley joined the British Army in the Royal Engineers and died in Turkey in 1915. Hans Geiger, who had returned to Germany in 1912 served in the German artillery. Rutherford himself worked on ways of tracking submarines.

In France, Marie Curie gave up her work with radium to organize a fleet of mobile Xray units which she took to the battle lines with her daughter Irene. German radiochemist and co-discoverer of protactinium, Lise Meitner also worked as an X-ray nurse

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during the war while her long-time research partner, Otto Hahn, was conscripted into the German army to work on chemical weapons.

Gunpowder had been used in war for centuries but the Great War was the first major war in which a range of high explosives developed in the nineteenth century was used so destructively. Alfred Nobel developed dynamite (1867) and gelignite (1876) by combining highly unstable compounds such as nitro-glycerin with un-reactive materials making them safe enough to transport. Nobel intended his explosives as an aid to quarrymen and miners. He was dismayed that he became known for getting rich by finding better ways to kill people.

Nitric acid is an essential reactant in making explosives such as TNT. Until the Great War nitric acid was obtained from naturally occurring nitrates particularly found in Chile, South America. Nitrates were of course also needed as fertilizers and it was recognized that the natural resources would not last forever. By the outbreak of war, German chemists, Fritz Haber, Carl Bosch and Friedrich Ostwald, had developed methods of making first ammonia and then nitric acid using nitrogen from the air and water.

The Great War was the first in which the internal combustion engine played an important role. Cars and lorries replaced horses and carts for many uses and later in the war, tanks transformed the battlefield.

As explosives became more powerful so thicker and more effective armour was needed and in the Great War that meant steel. For the first time soldiers were given steel helmets to offer some protection from rifle and machine gun fire. The 1st World War saw the first large-scale naval battles between iron ships powered by steam.

Throughout the war the coal mines and steelworks of the industrialized countries competed to provide the fuel and materials for ships and railways and guns. Huge amounts of iron ore had to be imported from overseas.

Other metals and alloys, such as stainless steel, were also called upon and were developed during the war.

Everything is made of chemicals and chemistry is needed to make bullets and bombs but the term “chemical weapons� is reserved for substances that kill or injure not by exploding or burning but because of their toxic properties. Both sides in the Great War looked for suitable substances but it was Germany that made the first large-scale use of a poison gas. The weapon was very simple – the element chlorine. Chlorine gas irritates the eyes, nose, throat and lungs and at high concentration the damage results in death. Chlorine gas is denser than air so would sink into the trenches but it was easily dispersed by a strong wind.

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The war thanks to the chemistry relied on the mass production of machine guns, artillery weapons, rifles, and ammunition, as well as on railways and steamships to transport weaponry and supplies to the front. Death and destruction occurred on an unimaginable scale. Around ten million soldiers, sailors, airmen, medical officers, and nurses died on the battlefields, in the trenches, in tunneling operations, in the air, at sea, and in the casualty clearing stations and military hospitals. Millions of civilians also died as a result of the war. Many were caught in the cross-fire and bombing. Others were driven from their homes, villages, and towns and died from infectious diseases, malnutrition, and starvation.

The industrial-scale death and destruction during the war would not have been possible without the industrial-scale production of a vast variety of chemical substances, most importantly: • Explosives for shells, bombs, grenades, firearm ammunition, and mining operations; • Chemical warfare agents, commonly known as poison gases; • Metals and alloys for making weapons and ammunition. The care of the sick and wounded and the protection of troops and sailors also relied on chemical materials: • Chemicals for gas masks; • Metals for making armour and steel helmets; • Dyes for military uniforms; • Light-sensitive chemicals for war photography and aerial reconnaissance; • Disinfectants to stop the spread of infections in the trenches; • Antiseptics for treating the wounded; • Anesthetics for surgery; Medicines, such as painkillers. Chemists were needed to control the manufacture of “munitions, explosives, metals, leather, rubber, oil, gases, food, drugs,” noted British chemist Richard Pilcher in an article published in 1917. Pilcher was Registrar and Secretary of Britain’s Institute of Chemistry, of the forerunners of the Royal Society Chemistry. He called the war, “the chemists’ war.”

Chemical substances employed in the war not only resulted in death and destruction, but also protected and prolonged the lives of soldiers. Some chemicals were used for both purposes, for example: • Chlorine was used as a chemical weapon. The element was also a component of disinfectants such as bleaching powder and anesthetics such as chloroform.

• Picric acid was employed not only as a high explosive but also as an antiseptic to treat burns.

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• Phosphorus was used offensively as an incendiary material in shells and bombs and also defensively to generate smoke screens to conceal maneuvers from the enemy.

• Ammonium nitrate was a component of blasting explosives such as ammonal. It was also a fertilizer and used to generate the anesthetic nitrous oxide.

Only two nuclear weapons have been used in the course of warfare, both by the United States near the end of World War II. On August 6th, 1945, a uranium gun-type fission bomb code-named "Little Boy" was detonated over the Japanese city of Hiroshima. Three days later, on August 9th, a plutonium implosion-type fission bomb code-named "Fat Man" was exploded over Nagasaki, Japan. These two bombings resulted in the deaths of approximately 200,000 Japanese people—mostly civilians.

Atomic bombs are made up of a fissile element, such as uranium, that is enriched in the isotope that can sustain a fission nuclear chain reaction.

We would have also known that chemistry and chemicals were not only being employed to devastating effect in the First World War, but also that chemistry in one form or another had been applied wittingly or unwittingly to warfare since time immemorial.

Over 2,000 years ago, for example, Roman legionaries in battle wore armor made of iron, a chemical element, and helmets made of bronze, an alloy - a mixture of a metal and one or more other chemical elements.

Gunpowder provides another example of the application of chemistry to warfare. The powder consists of a mixture of charcoal, the chemical element sulfur and one chemical compound - potassium nitrate.

The application of chemistry to warfare also developed rapidly in the years between Lavoisier’s 1789 treatise and the outbreak of the First World War. The discovery of new types of powerful explosives, new medicines and drugs to treat wounded soldiers, and new types of metal alloys for weapons and military equipment during this period had a major impact on the war.

Chemical Warfare Service in the United States worked to devise new and more effective chemicals to disable and kill enemy troops, while other chemists worked on pharmaceutical and antiseptic preparations used to treat wounded and sick soldiers.

What innovation there was often focused on the development of new types of poison gas, better explosives and more efficient processes for the manufacture of the chemicals needed for the war effort. The necessity of increased production of munitions involving all types of chemical mixtures and compounds requires chemists in large numbers, not only to inspect and analyze the substances te are using, but to develop the necessary new ones.

In many people’s eyes, the use of chemicals in the First World War has become synonymous with chemical warfare and the use of poison gases against enemy troops.

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The active and creative role played by chemists in this type of warfare inevitably contributed to the subsequent widespread negative image of chemicals.

The term has a much broader context, however. The chemistry of the First World War was not just confined to poison gases and explosives, but also to the development and production of numerous other chemical products used by the military either directly or indirectly. The side that mastered the chemistry needed for warfare would be successful in the war.

Chemistry and Global Warming

Facts about Global Warming: • In the last 20 years the amount of CO2 in our atmosphere has nearly doubled.

• Average temperatures in Alaska, western Canada, and eastern Russia have risen at twice the global average.

• The last two decades were the hottest decades in 400 years.

• Arctic ice is rapidly disappearing, and it is predicted that the Arctic may have its first completely ice-free summer by 2040.

• Coral reefs, which are highly sensitive to small changes in water temperature, suffered the worst bleaching in response to stress ever recorded.

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• Things such as industrialization, deforestation, and pollution have greatly increased the concentrations of water vapor, carbon dioxide, methane, and nitrous oxide in our atmosphere.

For almost all of 4.5 billion years, natural forces have shaped Earth’s environment. But, during the past century, as a result of the Industrial Revolution, which has had enormous benefits for humans, the effects of human activities have become the main driver for climate change. The increase of atmospheric carbon dioxide caused by burning fossil fuels for energy to power the revolution causes an energy imbalance between incoming solar radiation and outgoing planetary emission. The imbalance is warming the planet and causing the atmosphere and oceans to warm, ice to melt, sea level to rise, and weather extremes to increase. In addition, dissolution of part of the carbon dioxide in the oceans is causing them to acidify, with possible negative effects on marine biota. As citizens of an interconnected global society and scientists who have the background to understand climate change, we have a responsibility first to understand the science.

To fully appreciate the urgency of climate change, it's important to understand the ways it affects society and the natural environment. Sea levels are rising and glaciers are shrinking; record high temperatures and severe rainstorms and droughts are becoming increasingly common. Changes in temperatures and rainfall patterns alter plant and animal behavior and have significant implications for humans.

The term "global warming" refers to an increase in Earth's mean global temperature because a part of Earth's outgoing infrared radiation is retained by several trace gases in the atmosphere whose concentrations have been increasing because of human industrial, commercial, and agricultural activities. These gases have the ability to absorb radiation, leading to the tendency of the atmosphere to create warmer climates than would otherwise be the case.

The atmosphere that surrounds the earth is like a greenhouse. These gases help to trap the earth’s heat keeping it warm. However think about this. If the earth’s greenhouse gases became too hot, then how can we cool the earth? There is no way we can open a window or door to let the heat out. This is why the release or emission of greenhouse gases is an important topic for global warming.

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As greenhouse gases increase in the atmosphere, the earth starts to become warmer.

This is called global warming. If we continue to produce many greenhouse gases, the earth will become a much warmer place to live in. This means, the weather patterns of the earth will change - summers will be hotter and winters will be shorter. The polar ice caps will start melting and the water in the sea will increase.

Global warming is, in the end, not about the noisy political battles here on the planet’s surface. It actually happens in constant, silent interactions in the atmosphere, where the molecular structure of certain gases traps heat that would otherwise radiate back out to space. If you get the chemistry wrong, it doesn’t matter how many landmark climate agreements you sign or how many speeches you give.

Yes. Most scientists now conclude that observed increases in Earth’s average temperature are evidence that enhanced greenhouse effect, or global warming, is taking place.

We are all scientists. As scientists, our responsibilities are not only to understand the natural and human-influenced processes, but to help others understand them, and work with them to adapt to and reduce any negative consequences.

It is a responsibility of prepared scientists who have knowledge of something that can affect the environment to shed enough light on it, so that action actually takes place.

If not us, who? If not now, when? Please take action now.

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Best alternatives of Solution for the problem “The Melting of the Polar Caps�

Even if the ice caps are melting slower than usual, this is not a sigh of relief in saying that all is well, and that humans should ignore the melting polar ice caps along with all the many other effects of climate change.

It is important to remember that ice sheets absorb a great deal of the sun's heat.

Ice caps also to do their part in reflecting the sun’s rays which keep the Earth cooler (see albedo).

Without a decent reflective shield and solid heat absorption mechanism, the troposphere will further rise in temperature.

In essence, the melting of the polar ice caps will accelerate global warming which will in turn cause more rapid melting.

We need to be concerned about melting polar ice caps because of the rising sea levels which will ensue.

It is simple science and logic; with excess water comes rising sea levels which have the potential of swallowing islands and nations whole.

There is the wildlife factor as well.

Polar bears are losing their habitats across the glacier regions, and many are drowning as a result of the excessive floodwaters.

This has severe implications for marine life that dwell in the Arctic and Antarctic along with other animals such as walrus, penguins and seals.

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Ultimately, the melting ice caps could render many marine and land mammal species extinct.

At a time when so many other animal species on Earth are already facing extinction, it is important to preserve any animal’s habitat wherever possible.

Clearly, we have to do our part each and every day to make sure we are reducing our impact on global warming by decreasing our greenhouse gas emissions.

We must get to the root of the problem by trying to find new solutions to help stop climate change.

Nowadays, factors such as pollution and the increasing carbon dioxide levels must always be considered if we are to solve the climate crisis.

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It is crucial that we do not underestimate the gravity of the situation and that we do not give heed to disinformation regarding this predicament bestowed upon us that will in one way or another, affect all life on Earth.

What we have to do?

The one solution that really makes sense, is nuclear power, which creates no CO2, is cleaner and less costly than any other form of energy, with the possible exception of wind power. Problem with wind power being all of the dead birds.

Stop using Chlorofluorocarbons from like bug sprays etc., VOC's from paint, leaded gases. Instead we can use alternative cleaner fuels like ethanol in vehicles produced from sugar cane or corn. Control the methane gas production by cows as this actually helps to make the ozone layer thinner causing an increase in atmospheric temperatures. We can have laws to prevent deforestation as trees help to take in CO2 from the air. CO2 had more heat than atmospheric air like inhaled air for example. we can have more energy efficient homes that can save energy and prevent pollution. We can have better disposal of gases from factory outlets.

If we reduce black carbon emissions worldwide by 50% by fully deploying all available emissions-control technologies, we could delay the warming effects of CO2 by one to two decades and at the same time greatly improve the health of those living in heavily polluted regions. the answer is for every person to take personal responsibility for their actions. Hence, changes to our lifestyle are significant. That means taking public transport more and walking or using a bicycle, using bio-fuels instead of fossil fuels, using energy-efficient

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appliances and unplugging when not in use and buying only what we really need.

These are all small steps that every individual can take to save this beautiful planet.

The most important change, is to stop eating meat.

So to be part of the solution, encourage everyone to adopt the compassionate and distinctly more “eco-friendly” vegetarian or vegan diet!

What I think about Chemistry

What I love about chemistry is the constant sense of discovery: looking at the simplest reactions on a molecular level is like glimpsing a whole new world. I am keen to learn at the cutting edge of current knowledge and to contribute to new discoveries…

The most fascinating aspect of chemistry is the knowledge that everything around us, the whole universe in fact, comprises a grand total of some 92 natural elements, to some degree or another. I have always been fascinated by the elements, and the relation each element has to all the others in what is known as the Periodic Table…

From the smallest molecule to the most important issues of the modern world, chemistry is fundamental. The burgeoning world energy crisis, for example, will only be solved with the help of Chemistry, and the possibility to be involved in this is an ambition of mine…

Nowadays, science and technology play a vital role in people's lives. They have become a dominant factor in the development of society. Therefore, many countries are striving to diversify their economies through the development and application of new and advanced technologies like the ones that operate on nanoscale…

Chemistry is all around us. From the very clothes on our back to the products we use every day, chemistry has been involved in their development. As it is a multi-faceted and ever-evolving subject, providing endless fascination, there are constantly new challenges and questions which must be answered...

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STAGE 2 INTEGRATIVE ACTIVITY

ELEMENTS AND DAILY CHEMICAL COMPOUNDS

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Introduction There are a lot of elements in our human body that we don’t know that are there but they have a lot of important functions and we don’t really know about them. There are a lot of elements that make our body function in the right way, if one of them isn’t in our body or its very Little the amount of that element, our body will destabilize and we will feel sick or tired or maybe we will have other complications depending on the element that isn’t in the body.

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Development of the topic

Carbon (C) The element carbon is not found in a pure form in the human body, but rather in compounds within the body. Carbon constitutes roughly 18 percent of body mass, and millions of carbon atoms form the thousands of molecules in virtually every cell. Carbon is the basic building block required to form proteins, carbohydrates and fats, and it plays a crucial role in regulating the physiology of the body.

Gaseous and liquid compounds that contain carbon also can affect the body. It is used in: -

Cellular respiration

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The respiratory system

Carbon monoxide can kill. The gas forms when there is not enough oxygen to produce carbon dioxide, essentially when the carbon in fuel is not burned completely. Carbon monoxide prevents oxygen in the blood from being carried throughout the body, causing asphyxiation. Exposure to carbon monoxide can severely affect the elderly and people with cardiovascular or lung disease. Low concentrations can cause headache, loss of alertness, nausea, fatigue, hyperventilation, confusion and disorientation. High concentrations can result in a coma or death.

Hydrogen (H) One of the major ways that hydrogen is used in the body is in water. Water is made up of two-thirds hydrogen atoms. According to the Mayo Clinic, water is so important that it makes up over 60 percent of your body. Because of hydrogen, the cells are able to remain hydrated, toxins and waste are able to be eliminated from the body, nutrients are able to be transported to the cells that need them, your joints are lubricated, and your body's immune system is able to send defensive cells to fight of infectioncausing fungus, bacterias and viruses. Hydrogen also plays a crucial role in energy production in the body. For our bodies to function, they must have energy in the form of adenosine triphosphate (ATP).

Your body gains energy through consuming foods rich in substances such as carbohydrates. Once ingested, the body uses enzymes to break down your food into more basic substances such as glucose.

These basic parts are then further broken down through glycolysis and beta oxidation, leaving your body with acetyl CoA. Acetyl CoA is then broken down into hydrogen, oxygen and carbon. The hydrogen ions are transported to the mitochondria of the cells, which then uses the hydrogen to create ATP.

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Having too much Hydrogen ions dissolved in the blood without a buffering source, compensation mechanism, or an elimination mechanism could cause your blood pH to to become acidic to a point that is not conducive to life. Bicarbonate (HCO3-) in the blood is the buffer. When combined with Hydrogen it creates CO2 and H2O. The CO2 is then breathed out through alveolar exchange with oxygen and the water is eliminated through the body's filtering processes.

When an abundance of CO2 is present in the blood the body will produce higher rates of HCO3- in order to bring the pH to homeostasis. This is only a compensatory means of control and the cause of the increased acidity in the blood should be corrected in order to avoid permanent damage.

Nitrogen (N) Nitrogen molecules naturally found in the atmosphere are stable and generally nonreactive, but the same cannot be said of the forms of nitrogen found in fertilizer. Microbes transform these nitrates and nitrites so they can then easily pass through dirt, water and air. Unfortunately, the increased use of fertilizers has drastically multiplied the level of reactive nitrates and nitrites found in food and water supplies.

Drinking water contaminated by nitrates can cause methemoglobinemia, also known as “blue-baby syndrome.� It can also lead to a vitamin A deficiency, as well as a crippling of the thyroid gland. Nitrites can react with hemoglobin found in red blood cells and limit the amount of oxygen they transport.

Furthermore, both nitrates and nitrites are known to create nitro amines, a leading cause of cancer.

Respiratory systems can also be affected by nitrogen in nitrous oxide form, which can lead to a worsening of illnesses like asthma.

Calcium (Ca) Calcium is a mineral that is an essential part of bones and teeth. The heart, nerves, and blood-clotting systems also need calcium to work.

Calcium is used for treatment and prevention of low calcium levels and resulting bone conditions including osteoporosis (weak bones due to low bone density), rickets (a condition in children involving softening of the bones), and osteomalacia (a softening of bones involving pain). Calcium is also used for premenstrual syndrome (PMS), leg cramps in pregnancy, high blood pressure in pregnancy (preeclampsia), and reducing the risk of colon and rectal cancers.

Some people use calcium for complications after intestinal bypass surgery, high blood pressure, high cholesterol, Lyme disease, to reduce high fluoride levels in children, and to reduce high lead levels.

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Calcium carbonate is used as an antacid for “heartburn.� Calcium carbonate and calcium acetate are also used for reducing phosphate levels in people with kidney disease. Calcium-rich foods include milk and dairy products, kale and broccoli, as well as the calcium-enriched citrus juices, mineral water, canned fish with bones, and soy products processed with calcium.

Calcium can interact with many prescription medications, but sometimes the effects can be minimized by taking calcium at a different time.

Potassium (K) Potassium is a mineral that plays many critical roles in the body. Food sources of potassium include fruits (especially dried fruits), cereals, beans, milk, and vegetables.

Potassium is used for treating and preventing low potassium levels. It is also used to treat high blood pressure and prevent stroke.

Some people use it to treat high levels of calcium, a type of dizziness called Menière's disease, thallium poisoning, insulin resistance, symptoms of menopause, and infantcolic. It is also used for allergies, headaches, acne, alcoholism, Alzheimer's disease, confusion, arthritis, blurred vision, cancer, chronic fatigue syndrome, an intestinal disorder called colitis, constipation, dermatitis, bloating, fever, gout, insomnia, irritability, mononucleosis, muscle weakness, muscular dystrophy, stress, and with medications as treatment for myasthenia gravis.

Healthcare providers give potassium intravenously for treating and preventing low potassium levels, irregular heartbeats, and heart attack. Potassium plays a role in many body functions including transmission of nerve signals, muscle contractions, fluid balance, and various chemical reactions.

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Graphical representation

Elements 20 18 16 14 12 10 8 6 4 2 0 Elements in human body Carbon

Hydrogen

Calcium

Nitrogen

Potassium

Conclusion In the human body we can found a lot of elements that are important for its processes, but, as all the things, these elements in excess can be a danger to our health. The human body has a balance between all the parts of it. It is very important that this balance isn’t altered because there will be a lot of complications that affect our development in the daily life.

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STAGE 3 INTEGRATIVE ACTIVITY

CHEMICAL ELEMENTS AND ITS APPLICATIONS IN EVERYDAY MATERIALS

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INTEGRATIVE ACTIVITY

Chemical elements and its applications in everyday materials

EQUIPO: NATALIA DAENNA GONZÁLEZ VIERA VALERY SELENE GARCÍA MORALES ANETTE MONSERRAT SALAZAR ESQUIVEL EDUARDO ORTEGA CORPUS LUIS ROBERTO GONZÁLEZ GUAJARDO

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Universidad Autónoma de Nuevo León Preparatoria No. 9 - Group 120 Stage 3 - Integrative Activity Date: 21/10/16

INTRODUCTION Living organisms are made of chemical elements, and so are the things they consume in order to remain alive. So I would say they are very important.

Probably everything you’re living with is built by elements. Without elements there will be no you, us, and the entire beings. The most basic example, 99.95% of your total body weight contains of elements.

Studies by chemical experts have shown that the human body is composed of a combination of elements; 11 elements including carbon, hydrogen, oxygen, nitrogen, potassium, sodium, calcium, magnesium, sulfur, phosphorus and chlorine are called the macro (constant) elements, and they represent 99.95% of total body weight. The other 0.05% Is composed of elements called trace elements. The abundance of various elements in the human body is close to that of the earth’s crust.

Our oxygen (which help us breathe), radon (which helps with cancer and predicts earthquakes), hydrogen (without it there would not be water), aluminum (used basically in everything: cars, buses, planes, etc.). There are a lot of important stuff to basically all the elements. They usually make up just about everything in the world.

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DEVELOPMENT

A chemical element, or an element, is a material which cannot be broken down or changed into another substance using chemical means. Elements may be thought of as the basic chemical building blocks of matter.

Depending on how much evidence you require to prove a new element has been created, there are 117 or 118 known elements.

A chemical element is the simplest form of matter that cannot be broken down using any chemical means. Any substance made up of one type of atom is an example of that element. All atoms of an element contain the same number of protons. For example, helium is an element -- all helium atoms have 2 protons. Other examples of elements include hydrogen, oxygen, iron, and uranium. • While every atom of an element has the same number of protons, the number of electrons and neutrons can vary. Changing the number of electrons forms ions, while changing the number of neutrons forms isotopes of an element. • The same elements occur everywhere in the universe. Matter on Mars or in the Andromeda Galaxy consists of the same elements found on Earth. • The elements were formed by nuclear reactions inside stars.

Initially, scientists thought only 92 elements occurred in nature, but now we know many of the short-lived radioactive elements are also made in stars.

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Chemical elements constitute all of the ordinary matter of the universe.

However astronomical observations suggest that ordinary observable matter is only approximately 15% of the matter in the universe: the remainder is dark matter, the composition of which is unknown, but it is not composed of chemical elements. The two lightest elements, hydrogen and helium were mostly formed in the Big Bang and are the most common elements in the universe. The next three elements (lithium, beryllium and boron) were formed mostly by cosmic ray spallation, and are thus more rare than those that follow. Formation of elements with from six to twenty six protons occurred and continues to occur in main sequence stars via stellar nucleosynthesis. The high abundance of oxygen, silicon, and iron on Earth reflects their common production in such stars. Elements with greater than twenty-six protons are formed by supernova nucleosynthesis in supernovae, which, when they explode, blast these elements far into space as supernova remnants, where they may become incorporated into planets when they are formed.

The modern periodic table is similar to the periodic table developed by Mendeleev, but his table ordered elements by increasing atomic weight. The modern table lists the elements in order by increasing atomic number (not Mendeleev's fault, since he did not know about protons back then). Like Mendeleev's table, the modern table groups elements according to common properties. Element groups are the columns in the periodic table. They include alkali metals, alkaline earths, transition metals, basic metals, metalloids, halogens, and noble gases. The two rows of elements located below the main body of the periodic table are a special group of transition metals called the rare earth elements. The lanthanides are the elements in the top row of the rare earths. The actinides are elements in the bottom row.

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Symbol: Li Atomic Number: 3 Atomic Weight: 6.939 Lithium is a member of the alkali group of metals. It is soft, silvery-white in color with the symbol Li, located under number 3 in the table. The other alkali metals are sodium, cesium, rubidium, potassium, and francium.

Alkali metals are similar in that as you go down the table, their electro-negativity is reduced while their reactivity increases. Their boiling and melting points also decrease when moving in this direction.

Source: Lithium does not occur as a free element in nature. It is found in small amounts in ores from igneous rocks and in salts from mineral springs. Pure lithium metal is produced by electrolysis from a mixture of fused (molten) lithium chloride and potassium chloride.

Isotopes: Lithium has 7 isotopes whose half-lives are known, with mass numbers 5 to 11. Naturally occurring lithium is a mixture of its two stable isotopes 6Li and 7Li with natural abundances of 7.6% and 92.4% respectively.

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A soft, silvery metal. It has the lowest density of all metals. It reacts vigorously with water.

Lithium is soft and silvery white and it is the least dense of the metals. It is highly reactive and does not occur freely in nature.

Freshly cut surfaces oxidize rapidly in air to form a black oxide coating. It is the only common metal (but see radium) that reacts with nitrogen at room temperature, forming lithium nitride.

Lithium burns with a crimson flame, but when the metal burns sufficiently well, the flame becomes a brilliant white.

Lithium has a high specific heat capacity and it exists as a liquid over a wide temperature range.

The most important use of lithium is in rechargeable batteries for mobile phones, laptops, digital cameras and electric vehicles. Lithium is also used in some non-rechargeable batteries for things like heart pacemakers, toys and clocks.

Lithium metal is made into alloys with aluminium and magnesium, improving their strength and making them lighter. A magnesium-lithium alloy is used for armour plating. Aluminium-lithium alloys are used in aircraft, bicycle frames and high-speed trains.

Lithium oxide is used in special glasses and glass ceramics. Lithium chloride is one of the most hygroscopic materials known, and is used in air conditioning and industrial drying systems (as is lithium bromide). Lithium stearate is used as an all-purpose and high-temperature lubricant. Lithium carbonate is used in drugs to treat manic depression, although its action on the brain is still not fully understood. Lithium hydride is used as a means of storing hydrogen for use as a fuel.

Lithium is corrosive, causing skin burns as a result of the caustic hydroxide produced in contact with moisture. Women taking lithium carbonate for bi-polar disorder may be advised to vary their treatment during pregnancy as lithium may cause birth defects.

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Symbol: C Atomic Number: 6 Atomic Weight: 12.01115 Carbon (atomic number 6, symbol C) is a chemical element, which is tetravalent and nonmetallic. It is among the few elements that have been known to people since antiquity. Carbon has several allotropes, among which are amorphous carbon, diamond, and graphite. Depending on the allotropic form, carbon's physical properties can vary widely. Graphite, for instance, is black and opaque, while diamond is very transparent. Graphite is so soft that it can produce a streak on paper while diamond is one of the hardest materials. Graphite has good conductor properties, and diamond has poor electrical conductivity.

Source: Carbon can be obtained by burning organic compounds with insufficient oxygen. The four main allotropes of carbon are graphite, diamond, amorphous carbon and fullerenes.

Natural diamonds are found in kimberlite from ancient volcanoes.

Graphite can also be found in natural deposits.

Fullerenes were discovered as byproducts of molecular beam experiments in the 1980s.

Amorphous carbon is the main constituent of charcoal, soot (carbon black), and activated carbon.

Isotopes: 13 whose half-lives are known, with mass numbers 8 to 20. Naturally occurring carbon is a mixture of two isotopes and they are found in the percentages shown: 12C (99%) and 13C (1%).

Isotope 14C, with a half-life of 5730 years, is widely used to date carbonaceous materials such as wood, archeological specimens, etc. for ages up to about 40 000 years.

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There are a number of pure forms of this element including graphite, diamond, fullerenes and graphene.

Diamond is a colourless, transparent, crystalline solid and the hardest known material. Graphite is black and shiny but soft. The nano-forms, fullerenes and graphene, appear as black or dark brown, soot-like powders.

Carbon can exist with several different 3 dimensional structures in which its atoms are arranged differently (allotropes).

Three common crystalline allotropes are graphite, diamond, and (usually) fullerenes. Graphene has a 2D crystal structure.(Fullerenes can sometimes exist in amorphous form.)

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Carbon is unique among the elements in its ability to form strongly bonded chains, sealed off by hydrogen atoms. These hydrocarbons, extracted naturally as fossil fuels (coal, oil and natural gas), are mostly used as fuels. A small but important fraction is used as a feedstock for the petrochemical industries producing polymers, fibres, paints, solvents and plastics etc.

Impure carbon in the form of charcoal (from wood) and coke (from coal) is used in metal smelting. It is particularly important in the iron and steel industries.

Graphite is used in pencils, to make brushes in electric motors and in furnace linings. Activated charcoal is used for purification and filtration. It is found in respirators and kitchen extractor hoods.

Carbon fibre is finding many uses as a very strong, yet lightweight, material. It is currently used in tennis rackets, skis, fishing rods, rockets and aeroplanes.

Industrial diamonds are used for cutting rocks and drilling. Diamond films are used to protect surfaces such as razor blades.

The more recent discovery of carbon nanotubes, other fullerenes and atom-thin sheets of graphene has revolutionised hardware developments in the electronics industry and in nanotechnology generally.

150 years ago the natural concentration of carbon dioxide in the Earth’s atmosphere was 280 ppm. In 2013, as a result of combusting fossil fuels with oxygen, there was 390 ppm. Atmospheric carbon dioxide allows visible light in but prevents some infrared escaping (the natural greenhouse effect).

This keeps the Earth warm enough to sustain life. However, an enhanced greenhouse effect is underway, due to a human-induced rise in atmospheric carbon dioxide. This is affecting living things as our climate changes.

Pure carbon has very low toxicity. Inhalation of large quantities of carbon black dust (soot/coal dust) can cause irritation and damage to the lungs.

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Symbol: Si Atomic Number: 14 Atomic Weight: 28.086 Silicon (atomic number 14, symbol Si) is a metalloid and a chemical element which is solid at room temperature. It was isolated in 1824 by the Swedish chemist Jons Berzelius who also identified elements such as cerium, thorium, and selenium. Silicon is one of the most abundant elements in the universe, together with helium, hydrogen, carbon, nitrogen, neon, and oxygen. It is one of the most abundant elements in the earth's crust as well, along with calcium, iron, aluminum, and oxygen.

Source: Silicon is the second most abundant element in Earth’s crust, after oxygen and the eighth most abundant in the Universe. It is most commonly found as silicon dioxide (silica). Two elements, silicon and oxygen, make up almost three-quarters of our planet’s crust.

Commercial quantities of silicon are obtained by the reaction of silicon dioxide and carbon in an electric furnace using carbon electrodes. The carbon reduces the silicon dioxide to silicon. Silicon produced in this way is about 98% pure.

Isotopes: Silicon has 14 isotopes whose half-lives are known, with mass numbers 22 to 36.

Naturally occurring silicon is a mixture of its three stable isotopes and they are found in the percentages shown: 28Si (92.2%), 29Si (4.7%) and 30Si (3.1%).

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The element, when ultrapure, is a solid with a blue-grey metallic sheen.

Silicon is a hard, relatively inert metalloid and in crystalline form is very brittle with a marked metallic luster.

Silicon occurs mainly in nature as the oxide and as silicates.

The solid form of silicon does not react with oxygen, water and most acids.

Silicon reacts with halogens or dilute alkalis.

Silicon also has the unusual property that (like water) it expands as it freezes.

Four other elements expand when they freeze; gallium, bismuth, antimony and germanium.

Silicon is one of the most useful elements to mankind. Most is used to make alloys including aluminium-silicon and ferro-silicon (iron-silicon). These are used to make dynamo and transformer plates, engine blocks, cylinder heads and machine tools and to deoxidise steel.

Silicon is also used to make silicones. These are silicon-oxygen polymers with methyl groups attached. Silicone oil is a lubricant and is added to some cosmetics and hair conditioners. Silicone rubber is used as a waterproof sealant in bathrooms and around windows, pipes and roofs.

The element silicon is used extensively as a semiconductor in solid-state devices in the computer and microelectronics industries. For this, hyperpure silicon is needed. The silicon is selectively doped with tiny amounts of boron, gallium, phosphorus or arsenic to control its electrical properties.

Granite and most other rocks are complex silicates, and these are used for civil engineering projects.

Sand (silicon dioxide or silica) and clay (aluminium silicate) are used to make concrete and cement.

Sand is also the principal ingredient of glass, which has thousands of uses. Silicon, as silicate, is present in pottery, enamels and high-temperature ceramics.

Silicon carbides are important abrasives and are also used in lasers.

Silicon is not known to be toxic, but if breathed in as a fine silica/silicate dust it may cause chronic respiratory problems. Silicates such as asbestos are carcinogenic.

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Symbol: Ca Atomic Number: 20 Atomic Weight: 40.08 Calcium (atomic number 20, symbol Ca) is an alkaline earth metal and one of the most abundant elements found in the Earth's crust in terms of mass. This soft gray element is rather hard, and it is important for life on earth, especially for cell physiology whereby the calcium ion Ca2+ moves out and into the cytoplasm, signaling different cellular processes. It is the main component in the mineralization of shells and bones, and the most abundant element of all by mass in many living organisms. Calcium is an important constituent of teeth, leaves, and bones.

Source: Calcium occurs in nature in various minerals including limestone (calcium carbonate), gypsum (calcium sulfate) and fluorite (calcium fluoride). Commercially it can be made by the electrolysis of molten calcium chloride, CaCl2. The pure metal can also be produced by replacing the calcium in lime (CaCO3) with aluminum in hot, low pressure retorts.

Isotopes: Calcium has 19 Isotopes whose half-lives are known, with mass numbers 35 to 53.

Naturally occurring calcium is a mixture of six isotopes and they are found in the percentages shown: 40 Ca (97%), 42Ca (0.6%), 43Ca (0.1%), 44Ca (2%), 46Ca (0.004%) and 48Ca (0.2%).

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Calcium is a silvery-white, soft metal that tarnishes rapidly in air and reacts with water.

Calcium is reactive and, for a metal, soft. With a bit of effort, it can be cut with a sharp knife.

In contact with air, calcium develops a mixed oxide and nitride coating, which protects it from further corrosion.

Calcium reacts easily with water and acids and the metal burns brightly in air, forming mainly the nitride.

Calcium metal is used as a reducing agent in preparing other metals such as thorium and uranium. It is also used as an alloying agent for aluminium, beryllium, copper, lead and magnesium alloys.

Calcium compounds are widely used. There are vast deposits of limestone (calcium carbonate) used directly as a building stone and indirectly for cement. When limestone is heated in kilns it gives off carbon dioxide gas leaving behind quicklime (calcium oxide). This reacts vigorously with water to give slaked lime (calcium hydroxide). Slaked lime is used to make cement, as a soil conditioner and in water treatment to reduce acidity, and in the chemicals industry. It is also used in steel making to remove impurities from the molten iron ore. When mixed with sand, slaked lime takes up carbon dioxide from the air and hardens as lime plaster.

Non-toxic and an essential metal for living organisms.

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Symbol: Br Atomic Number: 35 Atomic Weight: 79.909 Bromine (atomic number 35, symbol Br) is a chemical element belonging to the halogen group. It is the only nonmetallic, liquid element and a reddish brown, mobile, volatile, and heavy liquid. The vapor irritates the throat and eyes and has an unpleasant, strong odor. Elemental bromine exists in a liquid form at room temperature and is toxic and corrosive. Its properties are similar to those of iodine and chlorine.

Free bromine is not found it nature, and occurs in the form of soluble, colorless, crystalline halide salts.

Source: Bromine is obtained from natural brine deposits. Some bromine is still extracted today from seawater, which contains only about 70 ppm.

Isotopes: Bromine has 26 isotopes whose half-lives are known, with mass numbers 68 to 94.

Naturally occurring bromine is a mixture of its two stable isotopes and they are found in the percentages shown: 79Br (50.7%) and 81Br (49.3%).

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Bromine is a deep-red, oily liquid with a sharp smell. It is toxic.

Pure bromine is diatomic, Br2.

Bromine is the only nonmetallic element that is liquid at ordinary temperatures.

It is a dense, reddish-brown liquid which evaporates easily at room temperature to a red vapor with a strong, chlorine-like odor.

Bromine is less reactive than chlorine or fluorine but more reactive than iodine. It forms compounds with many elements and, like chlorine, acts as a bleaching agent.

Bromine is used in many areas such as agricultural chemicals, dyestuffs, insecticides, pharmaceuticals and chemical intermediates. Some uses are being phased out for environmental reasons, but new uses continue to be found.

Bromine compounds can be used as flame retardants. They are added to furniture foam, plastic casings for electronics and textiles to make them less flammable. However, the use of bromine as a flame retardant has been phased out in the USA because of toxicity concerns.

Organobromides are used in halon fire extinguishers that are used to fight fires in places like museums, aeroplanes and tanks. Silver bromide is a chemical used in film photography.

Before leaded fuels were phased out, bromine was used to prepare 1,2-di-bromoethane, which was an anti-knock agent.

Bromine is poisonous and causes skin burns.

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Symbol: Co Atomic Number: 27 Atomic Weight: 58.993 Cobalt (symbol Co, number 27) is a chemical element occurring naturally only in a combined compound form. When isolated, it is a silvergray, lustrous, hard metal. It is used quite effectively as a blue pigment and has been used this way since antiquity for jewelry and other decorative items, to give glass a blue tinge, and more. Eventually, it emerged that the metal bismuth had this function. This metal is also known as goblin ore (German) because of the blue color it produced and because it gives off poisonous fumes upon smelting.

Source: Cobalt is not found as a free element in nature. It is found in mineral ores. The main ores of cobalt are cobaltite (CoAsS), erythrite (hydrated arsenate of cobalt), glaucodot (Co,Fe)AsS, and skutterudite (Co,Ni)As3. Cobalt is generally produced as a by-product of nickel and copper mining.

Isotopes: Cobalt has 22 isotopes whose half-lives are known, with mass numbers 50 to 72.

Naturally occurring cobalt consists of its one stable isotope, 59Co.

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A lustrous, silvery-blue metal. It is magnetic.

Cobalt is a bluish-white, lustrous, hard, brittle metal. It is ferromagnetic.

The metal is active chemically, forming many compounds. Cobalt stays magnetic to the highest temperature of all the magnetic elements (it has a Curie point of 1121oC).

Cobalt, like iron, can be magnetised and so is used to make magnets. It is alloyed with aluminium and nickel to make particularly powerful magnets.

Other alloys of cobalt are used in jet turbines and gas turbine generators, where high-temperature strength is important.

Cobalt metal is sometimes used in electroplating because of its attractive appearance, hardness and resistance to corrosion.

Cobalt salts have been used for centuries to produce brilliant blue colours in paint, porcelain, glass, pottery and enamels.

Radioactive cobalt-60 is used to treat cancer and, in some countries, to irradiate food to preserve it.

Cobalt and its compounds are considered to be slightly toxic by skin contact and moderately toxic by ingestion.

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Symbol: I Atomic Number: 53 Atomic Weight: 126.904 Iodine (atomic number 53, symbol I) is a chemical element with low toxicity, which dissolves easily in chloroform, hexane, and other organic solvents due to its lack of polarity. The color of iodine solutions depends on the solvent and its polarity. Solutions are violet in color in hexane and other non-polar solvents and dark crimson in moderately polar ones. Solutions are brown or orange in strongly polar solvents, for example, ethanol and acetone. When iodine is dissolved in carbon disulphide, carbon tetrachloride, or chloroform, it yields purple-colored solutions. Iodine is slightly soluble in water and gives a yellow solution.

Source: In nature, iodine occurs in the form of iodide ions, mainly in seawater. It is introduced into the food chain via seaweed and other sea-plants. Iodine is found in some minerals and soils.

Commercially, iodine is obtained in several ways, such as taking iodine vapor from processed brine, by ion exchange of brine or by releasing iodine from iodate taken from nitrate ores.

Isotopes: 34 whose half-lives are known, with mass numbers 108 to 141. Naturally occurring iodine consists of the one stable isotope: 127I

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A black, shiny, crystalline solid. When heated, iodine sublimes to form a purple vapour.

Iodine is a bluish-black, lustrous solid. Although it is less reactive than the elements above it in group 17 (fluorine, chlorine and bromine) it still forms compounds with many other elements.

Although iodine is a non-metal, it displays some metallic properties.

When dissolved in chloroform, carbon tetrachloride or carbon disulfide, iodine yields purple colored solutions. It is barely soluble in water, giving a yellow solution.

Iodine is important in medicine, in both radioactive and non-radioactive forms. Iodide and thyroxin, which contains iodine, are used inside the body.

A solution containing potassium iodide (KI) and iodine in alcohol is used to disinfect external wounds.

Elemental iodine is also used as a disinfectant.

Silver iodide is used in photography.

Iodine is sometimes added to table salt to prevent thyroid disease.

Iodine’s other uses include catalysts, animal feeds and printing inks and dyes.

In small doses, iodine is slightly toxic and it is highly poisonous in large amounts. Elemental iodine is an irritant which can cause sores on the skin. Iodine vapor causes extreme eye irritation.

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Symbol: Pb Atomic Number: 82 Atomic Weight: 207.2 Lead is a chemical element in the carbon group under number 82. Its symbol is Pb, after the Latin plumbum. As we know, in the past, all the plumbing was made of lead, which results in poisoning and death.

Thankfully, it no longer is.

Lead is soft and considered a poor metal, which means that it is a metallic element in the p-block. It is not clear why these elements are considered poor metals. What sets them apart from the others is that their electro-negativity is higher while their melting and boiling points are lower than that of transition metals.

Source: Lead rarely occurs naturally in nature and is can be found in ores, mainly with copper, zinc and silver. The principal lead mineral is lead sulfide (galena, PbS). Other common minerals are cerussite (lead carbonate, PbCO3) and anglesite (lead sulfate, PbSO4). Lead is refined from galena (PbS) by heating. A large amount of lead is also recovered from recycling.

Isotopes: Lead has 35 isotopes whose half-lives are known, mass numbers 181 to 215. Naturally occurring lead is a mixture of four isotopes and they are found in the percentages shown: 204Pb (1.4%), 206Pb (24.1%), 207Pb (22.1%) and 208Pb (52.3%).

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A dull, silvery-grey metal. It is soft and easily worked into sheets.

Lead is a bluish-gray, soft, dense metal that has a bright luster when freshly cut.

It tarnishes slowly in moist air to form a dull gray coating.

The metal is highly ductile and malleable.

Lead is extremely resistant to corrosion and is a poor conductor of electricity.

This easily worked and corrosion-resistant metal has been used for pipes, pewter and paint since Roman times. It has also been used in lead glazes for pottery and, in this century, insecticides, hair dyes and as an anti-knocking additive for petrol. All these uses have now been banned, replaced or discouraged as lead is known to be detrimental to health, particularly that of children.

Lead is still widely used for car batteries, pigments, ammunition, cable sheathing, weights for lifting, weight belts for diving, lead crystal glass, radiation protection and in some solders.

It is often used to store corrosive liquids. It is also sometimes used in architecture, for roofing and in stained glass windows.

Lead and its compounds are poisonous.

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Symbol: Ti Atomic Number: 22 Atomic Weight: 47.90 Titanium (atomic number 22, symbol Ti) is a transition metal and element from the Periodic Table that was discovered in 1791 by the British mineralogist and clergyman William Gregor who studied Cornish minerals.

Titanium has a silvery-white metallic color, very high strength-to-density ratio, and good corrosion resistance. It is alloyed with different elements, including molybdenum, vanadium, aluminum, iron, and others. At high temperatures, the element reacts with sulfur, silicon, boron, carbon, nitrogen, and other nonmetals. Compounds such as borides, carbide, and nitride have good refractory properties and are hard and stable.

Source: Titanium is the ninth most abundant metal in the Earth’s crust. Titanium is not found freely in nature but is found in minerals such as rutile (titanium oxide), ilmenite (iron titanium oxide) and sphene (titanite or calcium titanium silicate).

Isotopes: Titanium has 18 isotopes whose half-lives are known, with mass numbers 39 to 57.

Naturally occurring titanium is a mixture of its five stable isotopes and they are found in the percentages shown: 46Ti (8.2%), 47Ti (7.4%), 48Ti (73.7%), 49Ti (5.4%) and 50Ti (5.2%). The most naturally abundant of these isotopes is 48Ti at 73.7%.

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Pure titanium is a light, silvery-white, hard, lustrous metal. It has excellent strength and corrosion resistance and also has a high strength to weight ratio.

Titanium’s corrosion rate is so low that after 4000 years in seawater, corrosion would only have penetrated the metal to the thickness of a thin sheet of paper. (3) At high temperatures the metal burns in air and, unusually, titanium also burns in pure nitrogen.

Titanium is ductile and is malleable when heated.

It is insoluble in water, but soluble in concentrated acids.

Titanium is as strong as steel but much less dense. It is therefore important as an alloying agent with many metals including aluminium, molybdenum and iron. These alloys are mainly used in aircraft, spacecraft and missiles because of their low density and ability to withstand extremes of temperature.

They are also used in golf clubs, laptops, bicycles and crutches.

Power plant condensers use titanium pipes because of their resistance to corrosion. Because titanium has excellent resistance to corrosion in seawater, it is used in desalination plants and to protect the hulls of ships, submarines and other structures exposed to seawater.

Titanium metal connects well with bone, so it has found surgical applications such as in joint replacements (especially hip joints) and tooth implants.

The largest use of titanium is in the form of titanium(IV) oxide. It is extensively used as a pigment in house paint, artists’ paint, plastics, enamels and paper. It is a bright white pigment with excellent covering power. It is also a good reflector of infrared radiation and so is used in solar observatories where heat causes poor visibility.

Titanium(IV) oxide is used in sunscreens because it prevents UV light from reaching the skin.

Nanoparticles of titanium(IV) oxide appear invisible when applied to the skin.

Titanium metal is considered to be non-toxic. As metal shavings, or powder, it is a considerable fire hazard. Titanium chlorides are corrosive.

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Symbol: U Atomic Number: 92 Atomic Weight: 238.03 Uranium (atomic number 92, symbol U) is a metal and chemical element which occurs in nature as three isotopes - U-234, U-235, and U-238. The metal was discovered in 1789 by Martin Klaproth, a German scientist who also isolated cerium and zirconium.

Uranium forms different compounds such as carbonates and oxides, including triuranium octoxide, uranium trioxide and dioxide, and others. Some of the carbonates are water soluble. It reacts with different metals and forms intermetallic compounds, solids, and solutions.

Source: Uranium occurs naturally in several minerals such as uraninite (uranium oxide), carnotite and autunite. Canada is the world’s largest supplier of uranium, producing 20 to 30 percent of supplies. Commercially, uranium is produced through the reduction of uranium halides with alkali earth metals. Although most people think uranium is extraordinarily rare, it is in fact more abundant than familiar elements such as mercury and silver.

Isotopes: Uranium has 21 isotopes whose half-lives are known, with mass numbers 218 to 242.

Natural uranium consists of three major isotopes: 234U, 235U, and 238U. All are radioactive. 238U is the most stable isotope, with a half-life of 4.51 x 109 years (almost the age of the Earth).

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Uranium is a dense, silvery-white, slightly paramagnetic, radioactive metal. It is also ductile and malleable. The metal tarnishes in air acquiring a dark layer of oxide. When finely powdered, uranium ignites spontaneously in air.

Uranium is a highly reactive metal and reacts with almost of all the nonmetallic elements and many of their compounds. It dissolves in acids, but it is insoluble in alkalis.

When present in compounds, uranium exists mostly in oxidation state IV and oxidation state VI. All isotopes of uranium are radioactive, some more so than others. Its radioactivity – in particular its capacity to undergo thermonuclear chain reactions – has led to uranium’s use in energy generation, both for civilian and military purposes.

Uranium is a very important element because it provides us with nuclear fuel used to generate electricity in nuclear power stations. It is also the major material from which other synthetic transuranium elements are made.

Naturally occurring uranium consists of 99% uranium-238 and 1% uranium-235. Uranium-235 is the only naturally occurring fissionable fuel (a fuel that can sustain a chain reaction). Uranium fuel used in nuclear reactors is enriched with uranium-235. The chain reaction is carefully controlled using neutron-absorbing materials. The heat generated by the fuel is used to create steam to turn turbines and generate electrical power.

In a breeder reactor uranium-238 captures neutrons and undergoes negative beta decay to become plutonium-239. This synthetic, fissionable element can also sustain a chain reaction.

Uranium is also used by the military to power nuclear submarines and in nuclear weapons.

Depleted uranium is uranium that has much less uranium-235 than natural uranium. It is considerably less radioactive than natural uranium. It is a dense metal that can be used as ballast for ships and counterweights for aircraft. It is also used in ammunition and armour.

Uranium is harmful both through its chemical toxicity and its radioactivity. Exposure to uranium increases your risk of getting a variety of cancers due to its radioactivity.

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CONCLUSION What we can conclude about this activity is that all the elements independent of the corresponding group, the period, atomic number, or age, all of them helps us pretty much, although many of them are toxic. But most of them help us and contribute by an extremely and incredible way.

If the elements exist in the world is because a determined cause, a purpose: benefit the world, benefit the people and make the complex world an easier world.

In this activity we show you some chosen elements: Li, C, Si, Ca, Br, Co, I, Pb, Ti and U; all of those symbols show mainly their atomic number, their name (of the element); each element shows his general description, their isotopes, etc. Then shows by a periodic table’s image his location. His chemical and physical properties, applications and uses, and if the element perjuries the people or not by some natural effect.

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RESOURCES:

http://www.chemicool.com/elements/uranium.html http://www.chemicool.com/elements/titanium.html http://www.rsc.org/periodic-table/element/22/titanium http://www.chemicool.com/elements/lead.html http://www.chemicool.com/elements/iodine.html http://www.elementsdatabase.com/Lithium-Li-3-element/ http://chemistry.about.com/od/chemistryfaqs/f/element.htm http://chemistry.about.com/od/chemicalcomposition/f/What-IsThe-Moon-Made-Of.htm https://www.quora.com/What-are-importance-of-elements http://www.answers.com/Q/What_is_the_importance_of_elements_in _life?#slide=2 http://www.ptable.com/?lang=es http://pmm.umicore.com/en/prices/palladium/ http://elements.wlonk.com/ElementUses.htm http://www.elementalmatter.info/periodic-table-chart.htm

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STAGE 4 INTEGRATIVE ACTIVITY

CHEMICAL BONDS ON INDUSTRIAL USAGE SUBSTANCES

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Introduction This activity is about the chemical bond on industrial usage substances, for this we searched on web pages about some substances like the glass, paper, beverage, paint, cement and steel. About these we searched the substances that compose them, the kind of bond, among other things. Each one of the substances has a specific use in the industry for the elaboration of common objects.

Glass: The first one is the glass is a non-crystalline amorphous solid that is often transparent and has widespread practical, technological, and decorative usage in, for example, window panes, tableware, and optoelectronics. Scientifically, the term "glass" is often defined in a broader sense, encompassing every solid that possesses a non-crystalline structure at the atomic scale and that exhibits a glass transition when heated towards the liquid state. The glass is in solid state at temperature room. It is not a good electricity conductor. Some glasses are soluble in water producing an alkaline solution.

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Paper: The elements that make up paper are cellulose from tree wood and various chemicals that give different types of paper their special properties. Hemp, bamboo, flax and cotton are also used, but 95 percent of the raw elements come from trees. Properties of paper include the thickness, weight, texture, folding endurance, strength and size of the paper. Some grades of paper tear easily, while others resist tearing. The moisture retention capacity is another important property of paper. Some grades of paper dry very quickly and do not absorb moisture. The paper is in solid state at temperature room. It is not a good conductor and is soluble in water

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Beverage: Beverages fortified with calcium account for a significant part of the growing functional beverage market, as consumers become increasingly aware that calcium is a necessary ingredient for good nutrition and bone health.

The beverages are in liquid state at temperature room, some are good conductors of electricity and are soluble in water.

Paint and coating: Paint is used to decorate, protect and prolong the life of natural and synthetic materials, and acts as a barrier against environmental conditions. Paints may be broadly classified into Decorative paints, applied on site to decorate and protect buildings and other objects, and Industrial coatings which are applied in factories to finish manufactured goods such as cars.

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Paints contain: - pigment(s) - prime pigments to impart colour and opacity - binder (resin) - a polymer, often referred to as resin, forming a matrix to hold the pigment in place - extender - larger pigment particles added to improve adhesion, strengthen the film and save binder - solvent (sometimes called a thinner) - either an organic solvent or water is used to reduce the viscosity of the paint for better application. Water-borne paints are replacing some paints that use volatile organic compounds such as the hydrocarbons which are harmful to the atmosphere.

- additives - used to modify the properties of the liquid paint or dry film - The binder (resin) and solvent together are sometimes known as the vehicle. The binder may be dissolved as a solution or carried as a dispersion of microscopically small particles in a liquid.

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Depending on the type of paint and intended use, additives may include: - dispersants - to separate and stabilize pigment particles - silicones - to improve weather resistance - thixotropic agents - to give paints a jelly-like consistency that breaks down to a liquid when stirred or when a brush is dipped into it - driers - to accelerate drying time - anti-settling agents - to prevent pigment settling - bactericides - to preserve water based paints in the can - fungicides and algaecides - to protect exterior paint films against disfigurement from molds, algae and lichen Paints are formulated according to their proposed use - primer, undercoat, special finishes (matt, gloss, heat resistance, anti-corrosion, abrasion resistance). The pigment powder is broken down into individual particles which are coated by and dispersed in the binder (resin) - known as 'wetting out'. Solvent is then added to give the required consistency.

Each batch of ingredients is thoroughly mixed in large, stirred containers with the required additives.

Amounts ranging up to 40 000 dm3 of paint may be made in a single batch.

Cement: Portland cement gets its strength from chemical reactions between the cement and water.

The process is known as hydration. This is a complex process that is best understood by first understanding the chemical composition of cement.

Portland cement is manufactured by crushing, milling and proportioning the following materials: - Lime or calcium oxide, CaO: from limestone, chalk, shells, shale or calcareous rock - Silica, SiO2: from sand, old bottles, clay or argillaceous rock - Alumina, Al2O3: from bauxite, recycled aluminum, clay - Iron, Fe2O3: from clay, iron ore, scrap iron and fly ash - Gypsum, CaSO4.2H20: found together with limestone

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The materials, without the gypsum, are proportioned to produce a mixture with the desired chemical composition and then ground and blended by one of two processes - dry process or wet process. The materials are then fed through a kiln at 2,600ยบ F to produce grayishblack pellets known as clinker. The alumina and iron act as fluxing agents which lower the melting point of silica from 3,000 to 2600ยบ F. After this stage, the clinker is cooled, pulverized and gypsum added to regulate setting time. It is then ground extremely fine to produce cement.

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Steel: The primary types of structural steel are usually classified according to the following chemical composition categories: - Carbon-manganese steels - High-strength, low-alloy (HSLA) steels - High-strength quenched and tempered alloy steels The carbon-manganese steels, whose primary chemical components are carbon and manganese in addition to iron, are referred to as carbon steels or mild structural steels.

The materials of this type are generally least expensive; they have quite adequate strength and ductility characteristics, and are therefore by far the most widely used grades.

The high-strength low-alloy steels represent a relatively recent development in steelmaking.

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Conclusion: In this activity we learned that all the materials in our daily life have chemical characteristics that identify them in chemistry.

The have some chemicals that make a chemical bond between them and in that way the material is created. The bonds can be covalent or ionic depending on the group in which the chemicals are and the way they are going to connect. The material as the chemicals can change its state depending on the temperature around it.

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INTEGRATING LEARNING PRODUCT (ILP)

CONCLUSION

What we can conclude about this final product of Chemistry I in the first semester is that first of all we taught about the main benefits and contributions of the chemistry in our daily life, what we think about it if it’s dangerous or not: explaining its contribution in The War and in the making of powerful weapons; which is the contribution of the Chemistry in the fields of the Medicine and the Foodstuff, and how the elements interact and exist in our body. In the second stage, with its selected Integrative Activity we conclude that there are a lot of elements in our body as the carbon, also compounds like the water which is the mainly and most abundant. In the third integrative activity we conclude that each one of the elements showed in the periodic table has a giant amount of properties, characteristics, reactions, localizations, etc. so it’s almost impossible for us to memorize all of them but what we are able to do is to know as well the periodic table for obtain its characteristics or properties by ourselves. In the forth and the last integrative activity joined in this document we can conclude that again all the elements has a lot of benefits and thanks to them we have a lot of things that make our life easier than could be without the chemistry.

THANKS YOU!

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