AP Chemistry Review: Thou Shalt Not Forget

Compounds can be separated into elements by __________________

chemical changes

Mixtures can be separated by ______________

physical changes

Filtering separates particles based on differences in __________________

particle size

Distillation separates mixtures based on differences in ______________________

boiling point

Chromatography separates mixtures based on differences in _________________

polarity

In paper chromatography, the component that is most similar in polarity to the _____________________ moves up the farthest

"mobile phase"

Mass is conserved during _______________ and _________________ changes

physical, chemical

When reading the volume of a liquid, you can estimate by reading _________________

in between the graduated marks

Rank measuring devices from least to most precise

beaker, graduated cylinder, volumetric flasks, buret

The volumetric flask has ________ line on it to measure one specific volume

one

Gas densities are usually expressed in _________

g/L

Liquid/Solid densities are usually expressed in ___________ or _________

g/mL or g/cm^3

When diatomic elements are in a compound, the _________________ can vary

number of atoms

List the diatomic elements

I2, Br2, Cl2, F2, O2, N2, H2 (i brought clay for our new house)

Isotopes of an element have the same number of __________, but different numbers of ______________

protons, neutrons

__________________ allows us to measure atomic masses and abundances of isotopes

Mass spectrometry

The mol is a ____________ unit

counting

The percent composition by mass of a __________________ does not change

pure compound

___________________ in a balanced chemical equation allow us to calculate molar relationships among the reactants and products

Coefficients

__________________ gives the simplest ratio of moles of the elements in a compound

Empirical formula

The ___________________ for a compound is a whole number multiple of the empirical formula

molecular formula

(experimental/theoretical)

% yield

(experimental-theoretical)/theoretical

% error

The theoretical amount of product for a reaction is determined by the _____________________

limiting reactant

The ____________ is what dissolves into the _____________ to make a solution

solute, solvent

A solution is a _______________ mixture

homogeneous

Solutes can be classified as strong, weak or non electrolytes based on ______________

how well the solution conducts electricity

Solutes that produce ions in solution are __________________

electrolytes

A concentrated solution has a lot of ______________, whereas a dilute solution only has a small amount

solute

Concentration can be ____________

quantified

Two most common units in Chemistry are _________________

% (grams solute/grams solution) and Molarity (mols solute/L solution)

When water is added to a solution, the concentration decreases but the number of moles of solute _____________

remains the same

Dilution equation

M1V1=M2V2

A _________________ is an insoluble solid that forms when 2 solutions are mixed

precipitate

Salts containing ___________ or _______ are soluble. They are usually the spectator ions in a chemical reaction.

Group 1 cations, NH4+

The ______________ shows the ions coming together to form the precipitate

net ionic equation

_____________________ involves the precipitation of an ion to determine the concentration of that ion in the solution or to determine the percent purity of a mixture

Gravimetric Analysis

Light is emitted when an electron transitions from _____________

a higher energy state to a lower energy state

The larger the energy difference, the greater the _________________

energy of the light

___________ light has more energy, greater frequency, and smaller wavelength than _______ light

Blue, red

When an electron is in a higher energy level, it is farther away from the nucleus and therefore has less coulombic attraction to the nucleus, so is _________________

easier to remove

The farther away from the nucleus, the lower the _________________ of the electron

first ionization energy

When reading a PES, the higher the peak, the more _________ there are in that sub level, and a larger binding energy means electrons are __________ to the nucleus

electrons, closer

PES provides data that supports the ideas of __________

sublevels

________________ have a low ionization energy and generally lose electrons relatively easily

Metals

___________ are smaller than their atoms since you are removing valence electrons that are farther from the nucleus

cations (+)

____________ are larger than their atoms since adding electrons increases electron-electron repulsions

anions (-)

_______________ bonds are formed between 2 nonmetals sharing electrons

Covalent

_____________ bonds are formed when a metal transfers electrons to a nonmetal and the opposite charges attract

Ionic

The greater the electronegativity difference between two bonded atoms, the more _____________ the bond becomes

polar

Asymmetric molecules are _____________

polar

Symmetrical molecules are ___________

nonpolar

There is rotation around single bonds, but there can't be rotation around double or triple bonds due to ____________________

pi bonding

IMF's generally form from ___________ to ____________

weakest, strongest

List the IMF's from weakest to strongest

London Dispersion, dipole-dipole, hydrogen bonding, ion-ion

All molecules contain LDF, and this force gets _________ as the molecule gets larger

stronger

Larger electron cloud means more __________________

polarizable

All polar molecules contain ______________ forces, and this force gets stronger as the molecule gets more polar

dipole-dipole

H-bonds are between _______________

F/O/N

Boiling point and melting point ______________ as IMF's increase

increase

Vapor pressure and volatility __________________ as IMF's increase

decrease

When a molecular solid melts or boils, the _____________ between the molecules break, not the covalent bonds

IMF's

The stronger the IMF, the more energy it takes to _________ or ________ the substance

melt, boil

-ΔH, feels hot, heat is a product, temperature goes up

exothermic reaction

ΔHrxn= ____________ - ______________

bonds broken - bonds formed

Breaking bonds is ______________

endothermic

Forming bonds is ________________

exothermic

If a reaction is exothermic, the bonds formed in the products are ____________ than the reactant bonds

stronger/more stable

_________________ is constant during a phase change

Temperature

____________________ is the measure of how much energy it takes to raise the temperature of a substance

Specific heat capacity

Metals have a _________ heat capacity and their temperature changes quickly

low

Water has a _________ heat capacity meaning a lot of energy is involved in temperature changes

high

________________ allows us to calculate energy changes involved in a process

Calorimetry

When two objects of different temperatures are brought into contact, heat flows from the warmer object to the cooler object until _____________ is reached

thermal equilibrium

Thermodynamically favorable (spontaneous) reactions have a ____________

- ΔG

Entropy refers to ____________

disorder

Reactions with _________ and ________ are always thermodynamically favorable (spontaneous)

- ΔH and +ΔS (lower energy and greater entropy)

Reactions that increase the number of moles of gas have a ____________

+ΔS

Gibbs Free Energy equation that allows us to determine spontaneity is ________________

ΔG= ΔH-TΔS

If a process is spontaneous, the reverse is ________________

not spontaneous

ΔG=0 at ________ and ___________

equilibrium and phase changes

Spontaneity may be ____________ dependent (ex: melting)

temperature

In order for a reaction to occur, particles must collide at the correct orientation and with a minimum energy to break bonds. This minimum energy is called the _______________________

activation energy

The rate law shows how rate depends on concentration of the reactants and must be determined experimentally. It has the form: rate= k[A]^m[B]^n where m and n are the ___________________

orders of the reactants

In a _________________, when the concentration is doubled, the rate doesn't change

zero order reaction

In a _____________________, when the concentration is doubled, the rate is also doubled

first order reaction

In a __________________, when the concentration is doubles, the rate is quadrupled

second order reaction

The rate constant (k) _____________ with increasing temperature

increases

The rate usually ____________ over time because the reactant concentrations decrease

decreases

The ___________________ shows how the rate changes over time

integrated rate law

The ________________ gives information about the relationship between the variables

equation of the line

______________ is the time it takes for half of your sample to react or decay

Half-life

A 1st order reaction has a __________ half-life regardless of the initial concentration

constant

______________ decay is 1st order

nuclear

The taller the hill (or activation energy), the ____________________ the reaction

slower

The _____________ will dictate the speed of the reaction and this step will determine the rate law

slow step (rate determining step)

________________ are produced in one step and used up in a later step

Intermediates

___________________ are used up in one step and produced in a later step. They are NOT used up during the reaction.

Catalysts

Gas mixtures are ______________ because of the constant random motion of the particles

homogeneous

Gases are ______________ because of large spaces between the particles

compressible