Ch 7-10
Name______________________________________ Period____
• Chemical Equations –We use chemical equations to _________________________ –They ALWAYS have this format: • _______________________________________
–Example • _____________________________________
• Conservation of Mass –Law of Conservation of Mass • _____________________________________________________________________ _________________________________
–As you burn charcoal, the charcoal shrinks • The mass is converted in ___________________________________
• Balancing Equations –Shows that mass is _________________ during an equation –Change the coefficient so the number of elements on the __________equals the number of elements on the __________
• Counting with Moles –Use moles to ___________________________________________________ • The amount of a substance that contains approximately _____________________________________________
– Avogadro’ s number
–One mole of H has 6.02 X 10
23
particles of H
• Molar Mass –__________________________________________________ –Moles of different elements have _______________________ • Do a dozen shoes have the same mass as a dozen eggs?? • _________________________
• There are six general types of reactions: –__________________________________________________ –__________________________________________________ –__________________________________________________ –__________________________________________________ –__________________________________________________ –__________________________________________________
• Synthesis –_______________ substances react to form a ____________ substance • _______________________________
–2Na + Cl 2NaCl –2H + O 2H O 2
2
2
2
• Decomposition –A compound breaks down into ___________________ simpler substances (opposite of synthesis)
• _____________________________________ • 2H2O 2H2 + O2
–CaCO
3
CaO + CO2
• Single-Replacement –_____________ element __________________ of another element in a compound
• __________________________________
–Cu + 2AgNO 2Ag + Cu(NO ) –2K + 2H O H + 2KOH 3
2
3 2
2
• Double-Replacement –__________ different compounds exchange positive ions and form ____________________compounds
• __________________________________________
–Pb(NO ) + 2KI PbI + 2KNO –CaCO + 2HCl CaCl + H CO 3 2
3
2
3
2
2
3
• Combustion –A substance reacts rapidly with _________________, often producing ___________________________________
–FIRE –______________________________________
• Oxidation-Reduction –__________________ reaction –__________________________________________________ –LEO GER (_________________________________________) •Chemical Bonds and Energy – Chemical energy is _________________________________________________
– Chemical reactions involve the _________________________ in the reactants and the _______________________________ in the products
– Breaking bonds _______________________, and formation of bonds __________________________________
•Exothermic and Endothermic Reactions •During a chemical reaction, energy is either _________________________________________________
•Exothermic ________________________ energy •Endothermic _______________________ energy •Energy is _________________________ during a reaction
• Reaction Rate –__________________________________________________ –Tell how ______________ a reaction is going –Some are very fast (TNT), while other are very slow (leaves turning colors in the autumn)
• Factors that Affect Reaction Rate –Temperature- __________________________________ • Milk spoils __________________ if not cold
–Surface area- __________________________________ • Exposes __________ area for _________________
–Stirring- ______________________________________ • Increase ____________________ of reactants
–Concentration- _________________________________ • Concentration is the number of particles in a given volume
–Catalyst- _______________________________________ • Catalyst is a substance that affects the reaction rate without being used up
• _______________________________________
• Equilibrium is: ___________________________________________________________ ___________________________________________________________________________
– Chemical changes take place at the same rate, so no _______ change is occuring
• Physical Equilibrium – Water in a closed bottle undergoes ____________________, and then ______________________
– When the rate of evaporation _____________ the rate of condensation, __________________________ is reached
• Chemical Equilibrium – Some reactions are __________________________ – 2SO (g) + O (g) 2SO 2
2
3
• Sulfur trioxide is being made and broken down at a ___________________________
• Factors Affecting Equilibrium – Temperature- if heat is _________, the equilibrium shifts to the side that would ________________ heat from the system
– Pressure- if ______________________ pressure, the equilibrium would shift to the side that _________________ pressure
– Concentration- if you _____________________ a substance, the equilibrium would shift to the side that ____________ that substance
• A solution is ____________________________________________ _______________________________________________________
– Homogenous means that the solution appears ____________ through out. – You ______________ see _________________ substances in it.
• A solute is a ____________________________________________ _______________________________________________________
– This is the substance that is __________________________
• A solvent is the _________________________________________ _______________________________________________________
– This is the substance that ____________________________
• If I pour some sugar in a glass of water, is this a solution? – ____________
• Why?
– _________________________________________________
• What is the solute?
– _________________
• What is the solvent?
– _________________
• If I add sand to a glass of water, is this a solution? – _________________
• Why?
– _________________________________________________
• Properties of Liquid Solutions – Salt is _______________ than water, but the solution of the two is _________________ than either one.
– Three physical properties of a solution that can differ from those of its solute and solvent are:
• ______________________________ • ______________________________ • ______________________________
– Conductivity • Salt is a _______ conductor of electricity, but when it is _______________ in water it conducts electricity __________. The same with HCl.
• Freezing Point – Why do we put salt (MgCl2) on our roads in the winter?? – _____________________________________________________________ ______________________________________________________________
• Boiling Point – A coolant in most car radiators is a solution containing C2H6O2. – This _______________ the boiling point of water.
• Heat of Solution – During the formation of a solution, energy is either __________________________________________________
• If released, it is called __________________________
• If absorbed, it is called _________________________
– When NaOH dissolves in water, the solution becomes warmer. • Is this endothermic or exothermic?? • ____________________________
• Factors Affecting Rates of Dissolving – The rate of dissolving depends on the _____________________________ of collisions that occur between the particles of the ___________________________.
– Three factors affecting it are: • __________________________________ • __________________________________ • __________________________________
• Surface Area – The ______________ the surface area of a solid _________, the _____________ frequent the collisions are between solute and solvent particles.
– To ___________________ surface area, you can _________ the solid (______________________).
• Stirring – Moves the ____________________ particles away from the ________________ of the solid, and allows for more _______________.
• Temperature – ______________________ temp also increases __________ thus causing the particles to move ____________ and have ____________ collisions
• Solubility
–_____________________________________________________________ ______________________________________
• Expressed as g (solute) per 100g (solvent)
–They are described as _________________, _______________________, and ______________________.
• Saturated –_____________________________________________________________ ______________________________________.
–Table sugar _____________________ very easily in water. • At 20°C, 203.9g of sugar can dissolve in water. If more is added, it does ______________________________.
• The solution is __________________________.
• Unsaturated –_____________________________________________________________ ______________________________________
–Most drinks are unsaturated solutions of water and sugar. • If you add more sugar to your lemonade, it __________.
• Supersaturated –_____________________________________________________________ ______________________________________
–These solutions are very ____________________ –You can accomplish this by ________________ the solution.
• Three factors that affect the solubility of a solution are: –_________________________________________ –_________________________________________ –_________________________________________
• Polar and Nonpolar Solvents
–Oil does not ___________________ in water b/c oil is nonpolar and water is polar
–“ __________”dissolves “ ___________” –A solution is more likely to occur if both the solute and solvent are either polar or nonpolar.
• Temperature –The solubility of solids _________________ as the solvent temperature _____________________.
–When a glass of cold water warms up to room temp, bubbles form on the inside of the glass.
• These bubbles are ____________ that were dissolved in the water.
• Pressure –______________________ the pressure on a gas __________________ its solubility in a liquid.
• Manufacturers use this to make carbonated __________. • Use pressure to force CO2 to dissolve in a liquid.
• Acid –A compound that produces ___________________________ when dissolved in water
• HCl + H2O H3O+ + Cl-
–Properties of acids: • ______________________________________ • ______________________________________ • ______________________________________
• Sour taste –______________________________________________
• Reactivity with metals
–Single-replacement reaction –__________________ over spaghetti sauce
• Color change in indicator –Indicator- any substance that ________________________ in the presence of an acid or base
–Acids turn ________________________
• Base –A compound that produces ___________________________ when dissolved in water
• NaOH Na+ + OH-
–Properties of bases: • ___________________________________ • ___________________________________ • ___________________________________
• Bitter Taste –________________________________________________
• Slippery Feel –_______________________________________________
• Color change in Indicator –Bases turn _______________________
• Neutralization and Salts –Reaction between an _____________________ that forms a __________
–(H3O+ + Cl-) + (Na+ + OH-) 2H2O + (Na+ + Cl-)
• The pH scale – Number scale from ______________ to describe the concentration of hydronium ions in a solution
– 0 to 7 are ___________ – 7 to 14 are _________ – 7 is ___________ FOR YOUR INFORMATION: Hydronium ions= H3O+ Hydroxide ions= OH-
• Strong Acids and Bases – Strong acids almost completely ionize into mostly H3O+ ions, weak acids do not
• HCl is strong, acetic acid is weak –
Strong bases almost completely dissociated into OH- ions, weak bases do not
• NaOH is strong, ammonia is weak
• Buffers – A solution that is resistant to large changes in pH – Made of weak acids and bases
Ch.10 Nuclear Chemistry THE POWER OF THE ATOM Atom Review
An atom is the _________________________________ that can be part of a _________________________________
Cannot be _________________________________________________ by non-nuclear means.
Atoms are made up of __________________________________________ __________________________________________________________________
–Protons and Neutrons in the _____________________________ –Electrons in the __________________________________________ Nuclear Energy
Energy found ________________________________________________ In nuclear _____________________, nuclei of light elements combine to form the bigger nucleus of a heavier element
Example: Hydrogen combines to form helium Fusion
When hydrogen nuclei ______________________________, a type of nuclear reaction called ________________ occurs
Fusion requires __________________________________________ (millions of degrees Celsius)
Example of Fusion The energy coming from the ___________.
The sun is composed of mostly
_____________________
The heat produced from the ______________________________ warms the Earth Fission
A nuclear process in which _____________________________________ __________________________________________________________________
It produces energy for _______________________________ but it is also used peacefully every day to produce energy in ______________________________________ Fission and Fusion
In both, some mass is _________________________.
This is replaced by a
tremendous amount of ______________________.
Several different energy transfers are involved when nuclear power is applied to meet our energy needs Nuclear Power Plants
Nuclear power plants use ________________________ to heat water The water turns to ________________ and powers a turbine engine This in turn runs a generator that produces _____________________ Problems with Nuclear Energy
Environmentally, nuclear energy is ___________________. Disposing of radioactive wastes is _______________________ and extremely _______________________
When uranium can no longer be used to produce nuclear energy, its wastes are still ___________________________________