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 1023 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 + Cl2 2NaCl

–2H2 + O

2 2H

2O

•Decomposition

–A compound breaks down into ___________________ simpler

substances (opposite of synthesis)

•_____________________________________

•2H2O 2H

2 + O

2

–CaCO3 CaO + CO

2

•Single-Replacement

–_____________ element __________________ of another element in a

compound

•__________________________________

–Cu + 2AgNO3 2Ag + Cu(NO

3)

2

–2K + 2H2O H

2 + 2KOH

•Double-Replacement

–__________ different compounds exchange positive ions and form

____________________compounds

•__________________________________________

–Pb(NO3)

2 + 2KI PbI

2 + 2KNO

3

–CaCO3 + 2HCl CaCl

2 + H

2CO

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 __________________________

–2SO2(g) + O

2(g) 2SO

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 ChemistryTHE 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 ___________________________________