Chemistry Unit 7 & 8

Oxidation

LEO - lose electrons

Reduction

GER- Gain electrons

molarity (M or m/L)

= moles/Liters

percent yield

(exp. yield / theoretical yield) \* 100

synthesis

2+ reactants make 1 product

decomp

one product breaks down to 2 or more products

single replacement

anion replaces anion, cation replaces cation

double replacement

anions switch

neutralization

acid + base → H2O & Cl

combustion

organic combustion: O2 reactant → CO2 + H2O

metallic combustion: O2 reactant

For products to form, reactants have to:

collide

specific orientation

enough eA

endothermic- starts w/

low energy

exothermic-starts w/

high energy

Change in enthalpy

energy of products- energy of reactants

What speeds up chemical reactions

Increased molarity, temperature, surface area, catalyst

All reactions are redox except

double replacement

oxidation rule for single elements/diatomic

0

oxidation rule for ions

assume charge

oxidation rule for hydrogen

\+1, -1 when w metal

oxidation rule for oxygen

\-2, -1 in H2O2

Diatomic elements

BrINClHOF

Decomp of carbonates (CO3) produces

CO2 gas and metal oxide

Decomp of chlorates (ClO3) produces

O gas and metal chloride

Self ionization of water equation

H2O + H2O

Arrhenius Acid

Produce H+ ions when broken in water

Arrhenius Base

Produce OH+ ions when broken in water

Bronsted-Lowry acids are proton

donors

Bronsted-Lowry bases are proton

acceptors

Bronsted-Lowry theory: Water can be acid or base, so it is:

amphoteric

pH stands for

power of hydrogen

Acid base reactions are ______ reactions

neutralization

Acid base reactions produce

Salt & Water

Nature of soluts

even, can’t be filtered, can be separated by evaporation, not visible

Suspension

appears uniform but separates when agitation stops

Colloid

Mixture’s particles larger than size of molecule

Tyndall effect

Light beams scatter in colloids

Solution examples

Air, carbonated water, vinegar, steel, ocean

Factors that effect solubility

polarity/IMFs, temperature, pressure

Substances must have _______ IMFs for solutions

similar

Solids: higher temp= ________ solubility

greater

Gases: higher temp= ________ solubility

lower

Gases: higher pressure= ________ solubility

greater

Four factors affecting rate of solvation

Particle size, stirring, temperature, amount of solute already dissolved (increases, rate decreases)

Supersaturated solution

dissolved at high temperature, cooled after

Strong electrolytes- electric current

dissociate in water, + & - ions

Weak electrolytes- electric current

Dissociates slightly, few ions and undissociated molecules

Nonelectrolytes

dissolve as molecules, no ions, no electric current

Liquid boils when

vapor pressure = atm pressure

diff IMF=

diff vapor pressure

Stronger the IMF, _______ the vapor pressure

lower

Colligative properties (depend on # of solute particles)

vapor-pressure lowering, boiling point elevation, freezing point depression

Chromatography separates chemical species by taking advantage of the different ________ between components of the solution (mobile phase) w surface components of stationary phase.

Strength of IMFs

Cellulose paper is

polar, stationary phase

Cellulose will attract to solvent molecules to the exposed

Hydroxyl (OH) groups

retention factor =

distance traveled by component/distance traveled by solvent

Dilution formula

M1V1=M2V2