Chemistry: Thou Shalt Not Forget

Everything up to unit 6 excluding unit 5 is in here.

When an electron is in a higher energy level, it is farther away from the nucleus, and therefore has ______ Coulombic attraction to the nucleus and is therefore ________ to remove

Less…easier

moving across a row on the periodic table, the Zeff _______, therefore the valence electrons are ______ attracted to the nucleus, therefore the atomic radius __________ and the ionization energy _______

increases…more…decreases…increases

When reading a PES graph, the higher the peak, the _______ electrons there are in that sublevel, and a larger binding energy means that the electrons are _______ to the nucleus

more…closer

when writing electron configuration for a cation, remove the ______ electrons first…the ones in the p-orbital and s-orbital… then you can remove d-orbital electrons if necessary

valence 

isotopes for an element have the same number of _______, but different numbers of ________

protons…neutrons

Mass spectroscopy graphs measure ____________ of isotopes

atomic masses

elements in the ________ groups have similar chemical and physical properties

same

metals are on the ______ side of the zig-zag line and nonmetals are on the _______ side of the zig-zag line. metalloids _______ the zig-zag line

left…right…touch

cations are ________ than their neutral atom since you are removing the valence electron that are _______ from the nucleus. Cations also have a _______ Zeff, so a _________ positive force is pulling on the electrons

smaller…farthest…higher…greater

Anions are _____ than their neutral atoms since ______ extra electrons increases ________-_________ repulsions

larger…adding…electron-electron

IMF’s from weakest to strongest:

London dispersion forces, dipole-dipole, hydrogen bonding, ion-dipole

all molecules contain_______ forces, and this force gets stronger as the molecule is _____… _____ electron cloud = more _____ = more polarizable

London dispersion…larger…larger…London dispersion

All ______ molecules contain dipole-dipole forces, and this force gets _______ as the molecule is more _______

polar…stronger…polar

__-______ are between a NOF in one compound to a hydrogen that’s already bonded to a NOF in another compound

H-bonds

Boiling point and melting point ________ as IMF’s increase

increase

Vapor pressure and volatility ________ as IMF’s increase

decrease

Molecular solids have _____ melting/boiling points, and they ______ conduct electricity.

Low… don’t

Ionic solids have ________ melting/boiling points, and _____ conduct electricity as a solid,but ____ conduct as a liquid or (aq)

high…don’t…do

SiO 2 (quartz) and diamonds are _________________ , and they have very ______ boiling/melting points

covalent network solids….high

When a molecular solid melts or boils, it is _________ between the molecules that break, not the covalent bonds

IMF’s

Gas mixtures are ____________ b/c of the constant random motion of the particles

homogeneous

Gases are ____________ b/c of the large spaces between the particles.

compressible 

Gas pressure is caused by _________ of particles with the walls of the container. More ________ = more pressure 

collisions… collisions 

P and V are ________ related...doubling the volume of a container will cut the pressure of the gas in ________

inversely…half

T and V are ________ related...If you heat a balloon, it will expand.

directly

T and P are _______ related… if you heat a rigid container, the pressure of the gas will ________

directly… increase 

___________ which gas law uses these units: Temperature = Kelvin; Volume = Liters; Pressure = atm Use this gas constant: R=0.08206

PV=nRT

One mole of an ideal gas = 22.4 Liters ONLY at _______

STP

Gas pressure and # of moles are _________ related… if you double the mole of gas in a container, the pressure will ______

directly…double

what is the gas law that solves for molar mass and uses density?

Molar Mass = dRT/P

The more molar mass a gas has, the ________ it moves at a given temperature

slower

When collecting a gas by water displacement what is the equation?

P total= P dry gas + P water vapor

________ separates mixtures based on differences in particle size

filtering

__________ separates mixtures based on differences in boiling point

distillation

When reading a volume of a liquid in a container, read the _______ of the meniscus

bottom

Rank measuring devices from lest precise to most precise

beaker, graduated cylinder, volumetric flasks, burette

What are the diatomic elements?

H, O, N, Cl, Br, I, F

Empirical formula steps?

% to mass, mass to mole, divided by smallest mole, multiply till whole

The _______________________ for a compound is a whole # multiple of the empirical formula ratio

molecular formula 

percent yield equation?

% yield = (experimental/ theoretical) x 100%

the amount of product for a reaction is determined by the __________

limiting reactant

________ is conserved in both chemical and physical changes

mass

___________ reactions: (−) ΔH; feels hot; heat is a product; temperature goes _____

exothermic…up

___________ reactions: (+) ΔH; feels cold; heat is absorbed; temperature goes _____

endothermic…down

ΔH=∑(ΔH products)−∑(ΔH reactants ) (multiply by coefficients)

this isn’t a question you should just know that equation

bond energy: ΔH= (bonds broken)−(bonds formed)

this isn’t a question you should just know that equation

breaking bonds is _________

endothermic

forming bonds is ________

exothermic

when doubling a reaction ΔH ___________

doubles 

when reversing a reaction sign ___________

changes/ flips

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

stronger/ more stable

Chromatography separates mixtures based on differences in ________

polarity

In paper chromatography, the component that is most ______ in polarity to the “________ phase” moves up the farthest.

similar… polarity

_________ bonds are formed between two nonmetals _________ electrons

Covalent…sharing

______ bonds are formed when a metal ________ electrons to a nonmental and the opposite charges ________

Ionic…transfers…attract

The ________ the electronegativity difference between 2 atoms, the _____ polar the bond becomes

greater…more

_______ reactions make CO2 and H2O

Combustion

Carbon makes a total of ______ bonds in a compound

4

study bond angles

not a question just something you should do

study hybrid orbitals

not a question just something you should do

single bonds are also called _______ bonds

sigma

double bonds are also called ____ bonds

pi

a triple bond consists of 1 _____ bond and 2 _____ bonds

sigma…pi

_________ energy is the energy to break and ionic bond in a compound

Lattice

Lattice Energy _______ as the ion’s charge increases (and vise versa)

increases

Formal charge involves comparing the number of _______ ________ an atom has to the number of ___________ _________ __ in the Lewis structure (bonded electrons get evenly split between the atoms)

valence electrons…electrons around it

Formal charge = Valence electrons - lone pair electrons - ½ bonding electrons

not a question just an equation you should know

Obey the __________ rule first when drawing the Lewis structure, then use __________ charge if necessary.

octet…formal

Extra electrons can go on the ______ central atom, and if you have too few electrons, start making some ________ __ ________ bonds

larger…double or triple

_______ bonds are between metals, and they ___________ conduct electricity and their hardness _______.

metallic…always…varies

Interstitial alloys are made when ______ atoms fit into the gaps between larger atoms of a metallic crystal.

smaller

Substitutional alloys are made when the radii of the metals are ________ in size and are substituted into the crystal lattice.

similar

gases at the same temperature have the _____ average kinetic energy

same

Real gases behave most like an ideal gas at _____ temperatures and at _____ pressure.

high…low

The _____ polar a gas is and the ______ a gas is, the more it will deviate from the ideal behavior (_____,_____ gases are the most ideal)

more…larger…small, nonpolar

Compounds can be separated into elements by _______ changes, and mixtures can be separated by ________ changes.

Chemical…physical

the percent composition by mass for a pure compound ____ ___ change

does not

M1V1=M2V2

not a question just something you should know

percent error= (experimental-theoretical)/theoretical x100

not a question just something you should know