Unit 1 Chemical reactions Lesson 1
Chemical combination Lesson 2
Chemical compounds Lesson 3
Chemical reactions
Unit 2 Force and Motion Lesson 1
Universal forces in nature Lesson 2
Accompanied forces with motion Lesson (3)
Wave motion
Unit 3 Earth and universe Lesson 1
Celestial bodies Lesson 2 The earth Lesson 3 Rocks and minerals Lesson 4
Earthquakes and volcanoes
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Unit 1 Chemical reactions Lesson 1
The atom and the ion
Chemical combination
Number of well known elements till now is 112. Elements can be divided into 3 types: Metals
Solids having luster (except mercury which is liquid). Good conductor of heat and electricity. Malleable and ductile. They contain from 1 3 electrons in their last energy level They tend to lose electrons. They change into positive ions. Na ) ) ) Na ) )+ 2 8 1 2 8 p= 11 p=11 e=11 e= 10 +ve ion Mg ) ) ) 2 8 2 p= 12 e= 12
Mg ) )++ 2 8 p= 12 e= 10
Non-metals
Solids or liquids with no luster (except bromine which is a liquid) Bad conductor of heat and electricity (except graphite). Not malleable or ductile. They contain from 5 7 electrons in their last energy level. They tend to gain electrons. They change into negative ions.
Cl ) ) ) 287 p= 17 e= 17
Cl ) ) )2 8 8 p= 17 e= 18 -ve ion O)) O ) )- 2 6 2 8 P=8 p=8 e=8 e = 10
Positive ion It is an atom after losing one or more electrons during a chemical reaction.
Negative ion It is an atom after gaining one or more electron during a chemical reaction. 2
Inert gases
Inactive gases They have 8 electrons in their last energy level, (completely filled) except Helium 2 electrons. They don’t need chemical combination with another atom Their molecules consist of one single atom. They are not expected to form positive or negative ions.
N.B.: Atoms of elements react together to reach the stability of the nearest inert gas.
Chemical bonds Ionic bond It is a bond resulting from the electric attraction between positive ion and negative ion. In ionic bonding, electrons are completely transferred from the atom of a metal to the atom of a non-metal.
Examples
Covalent bond It is a bond resulting from the combination of non-metallic elements by sharing electrons.
Types of covalent bonds Single: a pair of electrons between 2 atoms (one electron from each atom).
Examples
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Double: 2 pairs of electrons between 2 atoms (2 electrons from each atom).
Examples
Triple: 3 pairs of electrons between 2 atoms ( 3 electrons from each atom).
Examples
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Lesson (1)
I. Give reason for: a) When an atom loses an electron or more it became a positive ion. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… b) The bond in an oxygen molecule is double covalent. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… c) The bond in the molecule of magnesium oxide (MgO) is an ionic bond. (Mg=12, O=8) …………………………………………………………………………………………………………… ……………………………………………………………………………………………………………
II. Compare between: Metals and non-metals Metals
Non-metals
Positive ion and negative ion Positive ion
Negative ion
Ionic bond and covalent bond Ionic
Covalent
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III. Draw an illustrated diagram for: a) The bond in N2 molecule. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… b) The bond in H2O molecule. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… c) The bond in CO2 molecule. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… ……………………………………………………………………………………………………………
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Lesson 2
Chemical compounds
Valency It is the number of electrons lost , gained or shared by an atom during a chemical reaction.
Examples
Valency = 1
The element
Symbol
Valency
The element
Symbol
Valency
Lithium Potassium Sodium Calcium Magnesium Aluminum Zinc Iron Lead Copper Mercury Silver Gold
Li K Na Ca Mg Al Zn Fe Pb Cu Hg Ag Au
1 1 1 2 2 3 2 2 or 3 2 1 or 3 2 1 3
Hydrogen Oxygen Nitrogen Chlorine Fluorine Bromine Iodine Sulfur Phosphor Carbon
H O N Cl F Br I S P C
1 2 3 or 5 1 1 1 1 2, 4 or6 3 or 5 4
The atomic group (radical) It is a set of atoms joined together and act as one atom during a chemical reaction, having its own valency. Atomic group
Symbol
Valency
Atomic group
Symbol
Valency
Hydroxide Nitrate Bicarbonate Ammonium Nitrite
OHNO3HCO3NH4+ NO2-
1 1 1 1 1
Sulphate Carbonate Phosphate
SO4- CO3- PO4- - -
2 2 3
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Chemical Formula It is a formula that represents the number and type of atoms in a molecule.
How to write the chemical formula of a compound? Write the symbol of element or atomic group forming the compound. Write the valency of each element or atomic group. Cross-multiplication for numbers written. Complete the following table: Compound
chemical formula
Sodium carbonate
Na2CO3
Copper carbonate
CuCO3
Sodium hydroxide
NaOH
Magnesium hydroxide
Mg(OH)2
Aluminium sulphate
Al2(SO4)3
Calcium carbonate
CaSO4
Sodium oxide
Na2O
No. of atoms
No. of elements
Types of compounds In nature there is a countless number of existing compounds. There are acids, bases, salts and oxides. Type of compounds Acids
Bases
Name
Chemical formula
Hydrochloric Acid
HCl
Sulphuric Acid
H2S04
Nitric Acid
HNO3
Sodium Hydroxide
NaOH
Potassium Hydroxide
KOH
Calcium Hydroxide
Ca(OH)2
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Acids They are materials that dissolve in water producing positive ions of hydrogen (H+). Properties of acids 1. Sour taste 2. Changing the colour of litmus into red due to the presence of the hydrogen ion (H+). Acids can be either : a. Mineral acids called oxygenated acids such as H2SO4 (sulphuric acid) or HNO3 (nitric acid). b. Non-oxygenated acid like HCl ( hydrochloric acid).
Bases They are compounds that dissolve in water producing negative hydroxide ion ( OH )Properties of bases a. Aqueous solutions of bases taste bitter and feel slipper. b. Changing the color of litmus paper to blue due to the presence of OH-
Oxides a. An element combined with oxygen. b. Metal oxide such as sodium oxide Na2O or aluminum oxide Al2O3. c. Non-metal oxide such as carbon dioxide CO2 or sulfur dioxide SO2.
Salts They are produced as a result of the combination of a positive metal ion (or positive atomic group) with a negative ion or a negative atomic group (except oxygen). Properties of salts a. They exist in earth’s crust or dissolved in water. b. They are different in some of their properties such as taste, color, smell, solubility in water and others. Salts that dissolve in water
Salts that don’t dissolve in water
Sodium chloride NaCl Potassium sulphate K2SO4 Calcium nitrate Ca(NO3)2 Magnesium carbonate MgCO3 Sodium sulphide Na2S
Silver chloride AgCl Lead bromide PbBr2 Lead sulphate PbSO4
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Lesson (2)
I.
Write the chemical formula for each of the following:
a. Sodium nitrate …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… b. Calcium carbonate …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… c. Nitric acid …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… d. Aluminum hydroxide …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… e. Ferric chloride …………………………………………………………………………………………………………… ……………………………………………………………………………………………………………
II.
Define each of the following:
a. Valency …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… b. The atomic group …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… c. The acid …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… d. The base …………………………………………………………………………………………………………… ……………………………………………………………………………………………………………
III.
Compare between Acids and Alkalis : Acids
Alkalis
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Lesson 3
Chemical reactions Chemical reaction It is breaking of bonds in reactants molecules and formation new bonds in the products.
Chemical equation It is a set of symbols and chemical formulae representing the reactants, the products and the condition if existed. A chemical equation should be balanced : Number of reactant atoms of an element = number of its atoms produced. The total amount of reactants masses = the total amount of products masses.
N.B. : A chemical reaction is always accompanied with a thermal change. Exothermic reactions They are reactions accompanied by evolution (releasing) of heat.
+ heat Endothermic reactions They are reactions that need heat energy absorption to be occurred.
+ heat
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Types of chemical reactions Direct combination reactions a. An element combines with another element : Carbon + oxygen C
carbon dioxide.
+ O2
CO2
Magnesium + oxygen
+
heat
magnesium oxide . heat
2Mg +
O2
2MgO
b. A compound combines with another compound : Reaction of ammonia with hydrochloric acid forming a white cloud of ammonium chloride. NH3
+
HCl
NH4Cl
Thermal decomposition reactions Copper carbonate CuCO3 (green)
copper oxide + carbon dioxide. heat
CuO (black)
+
CO2
Sodium nitrate decomposes partially producing sodium nitrite and oxygen. heat NaNO3 NaNO2 + O2 (white) (yellowish white)
Double replacement reactions In such reactions, the two reacting ions are exchanging mutually, forming new compounds.
Neutralization It is the reaction of an acid with an alkali forming salt and water. Acid + alkali salt + H+Cl- + Na+OHNa+Cl+
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water H2O
: Double replacement among salt solution NaCl
+
AgNO3
NaNO3
+ AgCl (white ppt)
The precipitate means that salt is not dissolved in water.
Advantage of chemical reaction in our life It is produced a thousands of compounds are commonly used in many industries such as medicines, fertilizers, fuel, plastics and others.
Disadvantage of chemical reaction in our life Fuel burning is an example for environmental pollution such as: 1. Carbon dioxide: It increases the atmospheric temperature where it acts as a green house. 2. Carbon monoxide: It has a dangerous impact on the human beings, that it causes headache, fainting in addition to serve stomach aches and may lead to death. 3. Sulphur dioxide and sulphur trioxide: They are acidic gases causing malfunctions in respiratory system of livings and corrosion of buildings. 4. Nitrogen oxides: They are resulted at the time of lightning. They are poisonous, and they are acidic gases that affect the nervous system and the eye. 5. Burning of coal and cellulose fibers such as paper and cigarettes causing air pollution and lung cancer.
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Lesson (3)
I.
Write the chemical equation representing the following reactions, and then indicate the type of each reaction:
a. Heating copper carbonate. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… b. Hydrochloric acid reacts with ammonia gas. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… c. Carbon burning in the presence of oxygen. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… d. Hydrochloric acid reacts with sodium hydroxide. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… ……………………………………………………………………………………………………………
II.
Define each of the following:
a. Neutralization reaction. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… b. Endothermic reaction. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… c. Exothermic reaction. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… d. Chemical reaction. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… e. Chemical equation. …………………………………………………………………………………………………………… ……………………………………………………………………………………………………………
III.
From the following equation 2Mg
+
O2
Δ
2MgO
If the mass of Mg = 24 and O =16, calculate the mass of reactants and products. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… 14
IV.
Compare between each pair of the following :
a. Exothermic and endothermic reactions Exothermic reactions
Endothermic reactions
b. Direct combination and double substitution reactions Direct combination
V.
Double substitution
Give reasons for:
a. Chemical equation should be balanced. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… b. A white precipitate is formed when NaCl solution reacts with AgNO3 solution. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… c. The reaction of hydrogen with oxygen to form water is considered as an exothermic reaction. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… d. The reaction of nitrogen with oxygen to form nitrogen dioxide is considered as an endothermic reaction. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… ……………………………………………………………………………………………………………
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Unit 2 Force and Motion Lesson 1
Universal forces in nature Lesson 2
Accompanied forces with motion Lesson (3)
Wave motion
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Unit 2 Force and Motion Lesson 1
Universal forces in nature
Force It is an effect attempts to change the object phase from being static to motion or vice versa, or attempts to change the motion direction. (Kicking a ball –Pushing objects)
Examples Types of Forces 1- Attraction forces.
2- Electromagnetic forces. 3- Strong nuclear forces. 4- Weak nuclear forces
First: Attraction forces 1- Earth's gravity force to objects: Earth attracts object to its center by a force known as the object weight, this force increases when the object's mass becomes larger. Object weight: It is the product of an
object mass X Earth's gravity acceleration
N.B. An object weight changes from one place to another on earth's surface. 2- Newton's general attraction law. Every two objects attract to each other by a force which is directly proportional to the product of the two object masses (M1 × M2) and inversely proportional to the square distance between the objects centers (d2). Newton's general attraction law =
M1 × M2 d2
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Second: Electromagnetic forces 1- Electric force: Brush your hair fast for 10 seconds by a comb then approach it to small paper pieces. The comb attracts paper pieces, but they fall down after a while. WHY? When you rub the comb with your hair, a weak electric charge is generated making the comb able to attract small paper pieces which were not charged at the beginning. Some charges have been passed from comb to the paper pieces which are similar to those of the comb so the repulsion occurred and paper pieces fall down after a while. Objects with like charges repel whereas objects with unlike charges attract to each other Coulomb's law The attraction or repulsion forces between two charges are directly proportional to the product of the 2 charges (q1 Ă— q2) and inversely proportional to the square distance (d2). 2- Electromagnetic forces: The electric current has magnetic effect (ability to attract iron objects). Electromagnet: It is made up of an isolated copper wire coiling around a bar of soft iron. When electric current passes through it, it works as a magnet. The uses of electromagnet: 1- Electric winches.
2- Electric bell.
Electric generators: They are devices that convert the mechanical energy into electric energy (Dynamo). Electric motors: They are devices that convert the electric energy into mechanical energy.
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Third: Nuclear forces The atom stores a massive amount of energy inside the nucleus. This massive energy is accompanied with forces known as nuclear forces which can be divided into:
1- Weak nuclear forces: It is used to get radioactive elements and radiation used in medicine, in scientific researches and in industry.
2-Strong nuclear forces: It is used in producing electric energy and in military purposes (Atomic bomb).
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Lesson (1)
I.
Define each of the following:
1- Force. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… 2- Weight. …………………………………………………………………………………………………………… ……………………………………………………………………………………………………………
II.
Mention each of the following:
1- Newton's general attraction law. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… 2- Coulomb's law . …………………………………………………………………………………………………………… ……………………………………………………………………………………………………………
III.
Give reasons for:
1- Gravity acceleration varies on earth's surface from place to another. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… 2- An object weight is not the same from place to another. …………………………………………………………………………………………………………… ……………………………………………………………………………………………………………
IV.
Compare between each pairs of the following:
1- Weak nuclear forces and strong nuclear forces. Weak nuclear forces
Strong nuclear forces
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Lesson 2
Accompanied forces with motion
Inertia It is the property of an object to resist the change of its phase from rest to motion in regular speed and in straight line unless an external force acted upon it.
Examples 1- Passengers rushed forward when the bus stops suddenly . 2- Football player rushed forward and falls down if tripped during running . 3-Throwing solid objects from a moving car, object falls down and continues running . Safety belts and inertia forces: The safety belts work on stopping the forces of inertia, to protect passengers in cars or planes, when a sudden change in motion occurs.
Centrifugal force It is generated when objects move in circular paths.
Examples I. Cars moving in circles in the park . II. Motorcycle rotating in a cage.
N.B. 1-The centrifugal force which affects an object increases when the object speed increases. 2-Centrifugal force is directly proportional to the square of the speed .
Friction Friction generates a force against the motion to resist it.
Examples Brakes decrease the speed of cars, bikes etc‌..
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Benefits of friction: 1- It prevents feet from slipping on road during walking. 2- It helps to slow, to stop and start car's motion. Harms of friction: I. It causes a great loss of mechanical energy because this energy is changed into heat energy. II. Generated heat due to friction causes some parts of machines to get hot; in addition this heat causes expansion of these parts so it affects their performance. III. It causes the errosion of machines parts.
Forces inside living systems There are forces inside living systems which enable living organisms to do their different biological operations such as: I. Heart muscle contraction and relaxation. II. Pulse inside blood vessels. III. Liquids transport through pores and the walls of cells from the lower concentration to higher one. IV. The contraction and relaxation of muscles to move the body organs.
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Lesson 2
I. Define each of the following: 1- Inertia. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… 2- Centrifugal force. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… 3- Friction force. …………………………………………………………………………………………………………… ……………………………………………………………………………………………………………
II. Give reason for each of the following: 1- The car passengers are pushed forward when the car stops suddenly. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… 2- Lubricating and oiling mechanical machines. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… 3- Traffic signs are placed where roads are curved referring to reduce speed. …………………………………………………………………………………………………………… ……………………………………………………………………………………………………………
III. Mention two benefits and three harms of friction forces : …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… ……………………………………………………………………………………………………………
IV. Mention the forces inside living organisms : …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… ……………………………………………………………………………………………………………
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Lesson (3)
Wave motion
Relative motion Change an object position or its direction with time passes in proportion to another object and in proportion to a fixed point known as a frame of reference.
Examples When you drive a car in the street then you stop, watching other moving cars give you a feeling that your car is moving although it is in rest.
Types of motion A- Periodic motion: It is a motion which is regularly repeated in equal periods of time .
Examples 1- Vibrating motion: such as the pendulum. 2- Circular motion: such as fan arm. 3- Wave motion: such as water waves. B- Transitional motion: It is the motion in which the object position is changed in proportion to a fixed frame of reference from time to time from an initial position to final one.
Examples The train and bike motion.
Applications on wave motion Lightning and thunder: We see lightning before hearing the thunder because thunder sound transfers in a form of mechanical waves but lightning flash transfers in another type of waves known as electromagnetic waves. 24
Types of waves Mechanical waves
Vibration of medium particles. They need a medium to transfer through. Their speed is relatively low.
Examples: Sound waves. Water waves.
Electromagnetic waves
They are accompanied with electromagnetic forces. They spread out in all media and space. Their speed are extremely great and can be accounted as: 300 million m/s
Examples: Light waves – radio and TV waves – ultra violet – infrared rays
Some technological applications for mechanical waves 1- Examining and curing sets for human body using sound waves. 2- Stringed musical instruments such as violin, lute and guitar. 3- Pneumatic musical instrument such as flute and the reed pipe. 4- Amplifiers and sets of distributing and controlling sound used in broadcasting studios. Some technological applications for electromagnetic waves 1- Applications for infra red rays: Night vision – remote sensing – cooking food – making remote sets. 2- Applications for ultraviolet rays: Sterilizing the sets of surgical operations rooms. 3- Applications for X-rays: Photographing bones – examining mineral raw in industry. 4- Application for gamma rays: It is used in medical purposes such as treatment and discovering some swellings. 5- Visible light: It is used in photographic cameras, Television cameras and data show.
Graphing motion When an object moves in straight line, the displacement occurred to the object changes with the time passes from the object original position.
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1- If the displacements occurring every second are equal, it is called uniform velocity, and it is represented as follow:
Regular speed motion
Displacement
Time
2- If the displacements occurring every second are not equal, it is called non- uniform velocity.
Irregular speed motion
Displacement
Time
3- If the displacement value is fixed (it doesn't change with time passing), it is said that the object is in static state.
Displacement
Time
Displacement: It is the distance at which an object moves away from its original position at any moment. 26
Lesson (3)
A. Define each of the following: 1- Relative motion. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… 2- Transitional motion. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… 3- Periodic motion. …………………………………………………………………………………………………………… ……………………………………………………………………………………………………………
B. Compare between each pair of the following: 1- Periodic motion and transitional motion. Periodic motion
Transitional motion
2- Mechanical waves and electromagnetic waves. Mechanical waves
Electromagnetic waves
C. Complete the following table: Technological applications
Rays used
Night vision Cooking food Sterilizing the sets of surgical rooms Photographing bones Medical purposes
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Unit 3 Earth and universe Lesson 1
Celestial bodies Lesson 2 The earth Lesson 3 Rocks and minerals Lesson 4
Earthquakes and volcanoes
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Unit 3 Earth and universe Lesson 1
Celestial bodies Stars, planets, moons, and rocky or gaseous bodies which rotate in the space.
The light year The distance covered by the light in a year = 0.467Ă—1012 Km.
Galaxies They are the biggest units that compose the universe. The galaxy that our solar system belongs to is known as (The way of chopped hay) or (The Milky Way).
Solar system
The sun
Planets
Moons
Asteroids
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Comets
Meteors
Meteorites
Planets Eight spherical bodies revolving around the sun (anti clockwise) in elliptical path.
Moons Small planets rotating around the large ones due to gravity. Planet
No. of moons rotating around it
Mercury
None
Venus
None
Earth
1
Mars
2
Jupiter
62
Saturn
60
Uranus
27
Neptune
12
Asteroids They are thousands of different sized rocky masses. Most of them rotate between the two orbits of Mars and Jupiter in a certain region known as the wondered asteroids belt which separates the outer from the inner planets.
Comets It consists of head and tail. A- Head which contains : 1- Ice spheres contain (CO2 – N2 – methane). 2- Rocky parts (dust – water molecules). B- Tail which consists of gaseous clouds. The most famous comet is Halley.
Meteors Small rocky masses that fall within the atmosphere and burn due to the heat of friction, they appear as luminous arrows that can be seen with the naked eye. 30
Meteorites Huge solid rocky masses that fall and didn’t burn completely as they penetrate the atmosphere. The biggest meteorite till now has a mass of 80 tons and exists at the southern west of Africa. Arrangement of planet according to the distance away from the sun : Mercury – Venus – Earth – Mars – Jupiter – Saturn – Uranus – Neptune
Classification of planets Points of comparison
Inner planets
Outer planets
Size Density Surface Atmosphere
Small High (3.3 to 5.5 gm/cm3) Solid They have atmosphere except Mercury They have few numbers Mercury – Venus – Earth Mars
Big Low (0.7 to 1.3 gm/cm3) Gaseous They haven’t atmosphere
No of moons Names
They have large numbers Jupiter – Saturn – Uranus – Neptune
Isaac Newton proved that there is a force of gravity between any two objects in the space. This force of gravity depends on the mass of the two objects and the distance between them. Planet
Force of gravity on the surface (m/s)
Mercury
3.78
Venus
8.60
Earth
9.78
Mars
3.72
Jupiter
22.88
Saturn
9.05
Uranus
7.77
Neptune
11.00
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Telescope It is an instrument used to identifying the celestial bodies. Types of telescope: 1- Reflecting
2- Refracting
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Lesson 1
I.
Define each of the following:
1-Asteroids: ………………………………………………………………………………………..…………………… …………………………………………………………………………………………………………….. 2-Meteors: ………………………………………………………………………………………..…………………… ………………………………………………………………………………………..…………………… 3-Meteorites: ………………………………………………………………………………………..…………………… ………………………………………………………………………………………..…………………… 4-Comets: ………………………………………………………………………………………..…………………… ………………………………………………………………………………………..……………………
II.
Complete the following table
Points of comparison
Inner planets
Outer planets
1-Planets names
2-Distance from the sun
3-Composition
4-Density
III.
Give reasons for:
a-The density of outer planets is low. ………………………………………………………………………………………..…………………… ………………………………………………………………………………………..…………………… b-The gravity on earth’s surface is larger than that on Mars surface. ………………………………………………………………………………………..…………………… ………………………………………………………………………………………..…………………… C-Astronomers do not measure the distance between the planets by kilometers. ………………………………………………………………………………………..…………………… ………………………………………………………………………………………..…………………… 33
Lesson 2
The earth Earth location within the solar system The earth occupies the third location among the planets, it lies between Mercury and Venus. The distance between the earth and sun is about 150 million kilo meters.
Earth shape I. It is a spherical object flattening at the two poles and indented at the equator. II. The tropical radius increases 22 km than the polar radius. III. Earth occupies the fourth order regarding to the volume, its average radius is about 6368 km.
Earth mass Earth is considered as having the biggest mass in the inner planets; its mass is 5.9 X 1024 Kg.
Reasons causing life to continue on earth 1 - Atmosphere Group of gases surrounding the earth causing living to breath, protecting them from harmful radiations.
Importance of atmosphere 1 – It consists of several gases mixed together in definite ratio. Gas
Ratio
Importance
nitrogen
Oxygen
21 %
Respiration of livings Burning process
oxygen
Nitrogen
78 %
Decreases the effect of oxygen Formation of proteins
Carbon dioxide
0.03 %
Photosynthesis process
Water vapour
Variable %
-
Other gases
Very little %
-
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carbon dioxide
water vapour and other gases
Other importance for earth’s atmosphere 1 – Burning of meteors before reaching earth’s surface. 2 – Decreasing the speed of meteorites. 3 – Climate phenomena. 4 – Keep suitable temperature on earth. 5 – It contains the ozone layer’s protecting livings from U.V. dangerous radiation.
2 – Earth’s hydrosphere Water represents 71 % of the earth’s surface.
Water
Salty water 97 %
Fresh water 3 %
Underground water which exists in the pores of rocks
Importance of water for living organisms 1 – Photosynthesis process. 2 – Completion of food digestion and absorption. 3 – Blood formation and keeping the body temperature constant. 4 – Keeping temperature on land during day and night within proper limits. 5 – Suitable environment for aquatic living organisms.
land water
salty water fresh water
3 – Suitable temperature The presence of earth in the third order far from the sun makes the temperature suitable for the continuity of living organisms.
4 – The gravity 1 - Helps in fixing objects and living organisms on its surface. 2 – Fixing the hydrosphere on its surface. 3 – Keeping the earth surrounded with the atmosphere. 5– The suitable atmospheric pressure. Atmospheric pressure equal 76 cm ∕ Hg. 35
The inner structure of earth
The crust 5 – 40 km
The mantle 2885 km
The core
Inner core 1216 km
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Outer core 2270 km
Lesson 2 I.
Mention the importance of water for living organisms
a-…………………………………………………………………………..……………………………… b-…………………………………………………………………………………………………..……… c-………………………………………………………………………………………………………….. d-…………………………………………………………………………………………………………..
II.
Compare between the inner and outer core Points of comparison
Inner core
Outer core
Thickness State
III.
Give reasons for:
a - Temperature on earth’s surface suits the life of living organisms. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… b - Earth’s inner core is solid. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… c - Steadfastness of the hydrosphere on earth’s surface. ………………………………………………………………………………………..…………………… ……………………..………………………………………………………………………………………
IV.
Explain briefly the importance of:
a-Oxygen gas. 1-…………………………………………………………...……………………………………………... 2-………………………………………………………………………………………...………………... 3-………………………………………………………………………………………………………….. b-Carbon dioxide gas. 1-……………………………………………………………………………...…………………………... 2-………………………………………………………………………………...………………………...
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Lesson 3
Rocks and minerals
Classification of rocks
( Igneous rocks )
(Sedimentary rocks)
(Metamorphic rocks)
Formed from the molten material which exist underneath earth’s crust
Form a thin cover that wrap about 75 % of the earth’s solid surface, it represents 5 % only of earth’s crust rocks
Originated as a result of exposing the old rocks to high pressure and temperature
(Plutonic igneous rocks)
(Volcanic igneous rocks)
Formed inside earth’s crust at great depths
Formed when the magma reaches earth’s surface
Ex: granite
Ex: basalt
Ex:
(Sand stone )
(Lime stone)
Yellow color Coarse textured Thin layers
White color Smooth touch
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marble
Granite I. Its color is pink or grey, it exists in the eastern desert and Sinai Peninsula. II. It is heavy rough, solid cohesive and hard breakable. III. It consists of three main minerals which are quartz, feldspar and mica.
Basalt I. It exists in abu-zaabal and close to abu-rawash and faiyoum. II. It is a dark colored rock. III. It consists of olivine and pyroxene. Granite
Quartz
Feldspar
Mica
Basalt
Pyroxene
Olivine
Sandstone
Limestone
Marble
Basalt
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Lesson 3 I.
What are the main factors that lead to the formation of the metamorphic rocks?
…………………………………………………………………………………………………………… ……………………………………………………………………………………………………………
II.
What is meant by?
a-Igneous rocks: …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… b-Sedimentary rocks: …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… c-Metamorphic rocks: …………………………………………………………………………………………………………… ……………………………………………………………………………………………………………
III.
Give an example for each of the following:
a-Plutonic igneous rock (……………………….………) b-Volcanic igneous rock (………………………….……) c-Sedimentary rock (………………………….…….) d-Metamorphic rock (……………………………….)
IV.
Mention the main minerals that share in the structure of the following rocks:
a-Granite …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… b-Basalt …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… c-Limestone …………………………………………………………………………………………………………… ……………………………………………………………………………………………………………
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Lesson 4
Earthquakes and volcanoes
Earthquakes Rapid and successive shaking of the ground, takes place one after the other.
Causes of earthquakes 1-The breaking of rocks suddenly due to the fractures in rocks of earth’s crust called fault. 2-Volcanoes.
The fault It is a fracture in earth’s crust which causes the sliding of rocks
Fault with horizontal displacement
Fault with vertical displacement
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Earthquakes intensity Varies from unfelt smooth shakes to extremely violent ones. Seismograph structure: as shown in the figure
Idea of operating When an earthquake occurs, the waves shake the ground, so the cylinder is also shaked, where is the metallic weight remains steady therefore, the pencil draw a zigzag line, called the seismic record on the paper.
The unit of measuring the intensity of earthquake Richter.
Harms of earthquakes 1-Losses in spirits and buildings. 2-Roads blocking, dams destroying and occurrence of fires. 3-Extremely high waves (Tsunami) which destroy and submerge coastal cities.
Benefits of earthquake Studying of the internal structure of the earth.
The volcano It is an opening in the earth’s crust which allows the passage of molten materials (lava) and gases outside it to the earth’s surface.
Parts of volcano 1-volcanic vent: An opening at the top of volcano. 2-The pipe or neck: It is a cylindrical cavity which reaches the earth’s surface. 3-The cone: It is the body of volcano.
The materials ejected during the volcanic eruptions materials: A-Fragmented The materials that the volcano emanates them. B-Lava and lava flow: Molten materials that spread out of the volcano. C-Volcanic gases: Water vapour, oxides of carbon, nitrogen and sulfur. 42
Harms of volcanoes 1- Lava and lava flows cover whole towns and villages. 2- Emission of harmful gases and dust. 3- Fire catches the cultivated lands and neighboring places.
Benefits of volcanoes 1-Production of electricity. 2-Increase the fertility of the soil. 3-Formation of new islands in the sea. 4-Formation of volcanic rocks with great economic values.
Safety precautions at natural catastrophes A-At the time of earthquake: 1-Take a position under a hard table. 2-If you were outdoor, go away from the building. 3-If you were in the car, remain inside it. B-Directly after the earthquake: 1-Before you’re going out from home, cut out the electricity, gas and water. 2-Don’t enter buildings harmed by earthquake. 3-Listen to the radio to follow the instructions.
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Lesson 4 I.
Define each of the following:
A-Earthquake: …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… B-Volcano: …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… C-Vent: …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… d-The cone: …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… e-The pipe: …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… F-Seismograph: …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… G-Richter: …………………………………………………………………………………………………………… ……………………………………………………………………………………………………………
II.
Mention the benefits of each of the following:
A-Earthquakes: …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… B-Volcanoes: …………………………………………………………………………………………………………… ……………………………………………………………………………………………………………
III.
Give reasons for:
1-Volcanic ash covers areas far away from the volcano. …………………………………………………………………………………………………………… …………………………………………………………………………………………………………… 2-Earth shaking takes place at the occurrence of earthquakes. …………………………………………………………………………………………………………… ……………………………………………………………………………………………………………
IV.
What are the most important volcanic gases?
a-……………………………………………………..………………………………………………….. b-………………………………………………………………………..……………………………….. c-…………………………………………………………………………………………..……………..
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