AP Chemistry Exam Review

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Boyle’s Law

Pressure is inversely proportional to Volume

P1V1=P2V2

Charle’s Law

Volume is proportional to temperature

V1/T1=V2/T2

Gay-Lussac’s Law

Pressure is proportional to temperature

P1/T1=P2/T2

Avogadro’s Law

mole is proportional to volume

N1/V1=N2/V2

ideal gas law

PV=nRt

molar mass

mass of sample/moles of sample

density of ga gas

(p*m)/(R*temperature at K)

kinetic molecular theory

gases are in constantly random motion, elastic, volumes are small, attractive forces are negligible, kinetic energy is proportional to temperature

as volume decreases what hawppens to collisions

collisions increase, inversely proportional

as pressure decreases what happens to the collisions

collisions decrease, proportional

graham’s law of effusion

kinetic energy formula

KE=1/2mv²

effusion

movement of gas molecules into a tiny hole

diffusion

gas move into another container filled with gas

dalton’s law of partial pressure

Pi=Xi*Pt

Xi

Xi/Xt

element/total moles

dipole-dipole

think of like a magnet

polar molecules

coulomb’s law

K(+)(-)/r²

as attractive forces increase in coulomb’s law

the distance decreases

as pressure increases in coulomb’s law

kinetic energy decreases

london dispersion forces

present in all molecules, nonpolar and then becomes polar for an instant

how to tell what compound has a higher boiling point

if they have the same intermolecular forces, check on moles

hydrogen bonds

H with NOF, strongest intermolecular forces

surface tension

increased attractive forces at surface of a liquid compared to center of liquid

evaporation

liquid to gas

vaporization

liquid to vapor

condensation

gas to liquid

visosity

liquid’s resistance to flow

ex. ionic compounds are viscous because of their structure and can’t move freely

vapor pressure

pressure of gas above a liquid → evaporation does happen but can’t escape a container

dynamic equilibrium based on vapor pressure

liquid molecules and gas molecules are start colliding with each other until the rates are equal to each other

metallic crystals

rigid structure and are alloys

substitutional alloy

replace ions

interstitial alloy

go in between ions because so small

ionic crystals

positive and negative ion structure

based on coulomb’s law

molecular crystals

covalent and nonmetals

held by any intermolecular force

<ionic, softer and low melting point

comparing compounds based on certain thing

whichever has the greater attractive force will have the higher boiling point and vaporization and a lower evaporation and vapor pressure

network crystal

structure filled with covalent bonds in empirical formulas

amorphous

soft and cannot form crystals

heating curve order

solid heating solid melting liquid heating liquid boiling (this is where superheating can happen) and then gas heating

cooling curve order

gas cooling, gas condense, liquid cooling, liquid crystallize, solid cooling

saturated solutions

maximum amount of solute dissolved in the solvent

unsaturated solution

some of solute dissolved in solvent

supersaturated solution

more than maximum amount of solute dissovled in the solvent

how to tell if two compounds are soluble with each other

similar interactive forces interact and can be soluble with each other

dissasociate

molecules break apart after dissolving with water

ionization

molecules break apart into ions after dissolving with water

strong electrolyte

conduct electricity, ionizable and dissociate

ionic compounds mainly but HI, HBR, HCL

weak electrolyte

slightly ionizable and dissociate

weak acids and bases

molarity

moles of solute/liters of solution

as temperature increases what happens to gases in liquid

decrease

which state of matter is easiest to compress

gas

henry’s law

solubility of gas = k * pressure of gas

intermediate

cannot be present in rate law

present in first and second steps

what is the criteria for a reaction to happen

1. colliding

2. proper orientation

3. sufficient energy

what step do you use to determine the rate law

slow

how many steps will the addition of a catalyst be

>=2

how to tell if activation energy diagram will be endothermic or exothermic

reactant>product exothermic

reactant<product endothermic

single elementary step

molecules collide at the same time

first order units

1/s

zero order units

m/s

second order units

1/ms

as temperature increases what happens to the reaction rate

increases

as concentration increases what happens to the reaction rate

increases

as a catalyst is added what happens to the reaction rate

increases

as volume increases what happens to the reaction rate

decreases

as surface area increases

reaction rate increases and particle size decreases

beer’s law

absorbance is proportional to concentration

base

loses a proton (H+)

acid

gains a proton (H+)

stoichiometry steps

balance equation

convert to moles

mole ratio

convert back to grams of question element

how to convert to another element if needed and have the right information

use mole ratios

titration problems on finding moarlity

to find moles of solute → convert to liters the moles then mole ratio

then divide that answer by solution (probably given(

precipitation reaction

synthesis

redox reaction

includes OH- and H2O

acid-base reaction

can clearly tell the acid and bases

beer lambert law formula

absorbance = molar absorptivity * path length * concentration

if the rate of forward > rate of reverse

favors reactants

products increase and reactants decrease to make equal

if the rate of reverse > rate of forward

favors products

products decrease and reactants increase to make equal

reaction quotient

products/reactants

when to use q

determine direction of reactant

when to use k

determine if there are more reactants or products at equilibrium

k>1

prod>react num>den

k<1

react>prod den>num

k=0

prod=react num=den

le chatelier’s principle

adding stress can knock out of equilibrium

if reactant increases

consumes reactants and creates more products

reactant decreases

consumes product and create more reactants

when evaporating or adding

whatever side added will consume and other side will create more

goes onto the lowest side

pressure increases and volume decreases

goes onto the highest moles

pressure decreases and volume increases

solvent increases what happens to molarity

decreases, inversely proportional

addition of catalysts equilibrium

increases both sides

what side does heat favor

endothermic side → reactants

what happens to temperature surroundings in endothermic forces

temperature decreases

what happens to temperature surroundings in exothermic forces

temperature increases

enthalpy

delta H

exothermic or endothermic

endothermic

break forces

unfavorable

exothermic

form forces

favorable

specific/molar heat