Chemistry H Final Review

Boyle's Law

P1V1 = P2V2

Charles' Law

V1/T1 = V2/T2

Avogadro's Law

V1/n1 = V2/n2

ideal gas law

PV = nRT

frequency

number of wavelengths in one second, directly proportional to energy

wavelength

distance between peaks of a wave, inversely proportional to energy

double slit experiment

wave-particle duality of light

EMS (low -> high wavelength)

gamma, x-ray, UV, visible, infrared, microwave, radio

colors (light) (low -> high wavelength)

violet, indigo, blue, green, yellow, orange, red

Bohr model

nucleus surrounded by rings that electrons jump to and from

atomic line spectra

each ring corresponds to a different color released

s orbital

sphere

p orbital

hourglass

d orbital

clover

f orbital

balloon animal

hund's rule

electrons prefer their own space and will only share if they have to

pauli exclusion principle

an orbital can hold up to 2 electrons (opposite spin)

aufbau principle

electrons go to lowest-energy subshell available

aufbau exceptions

groups 6, 11

valence configuration

s, p subshells (highest PQN), outer shell

shorthand configuration

noble gas + electrons

full configuration

lists every electron

orbital diagram

arrows, subshells

s-block

groups 1 and 2 and He

p-block

groups 13-18

d-block

groups 3-12

f-block

inner transition metals

atomic radius

largest on the bottom left (low Zeff, high PQN)

ionic radius (cations)

dramatically smaller (lost valence shell + high Zeff)

ionic radius (anions)

moderately larger (same PQN, lower Zeff)

Zeff

atomic number - inner electrons

ionization energy

amount of energy needed to remove highest-energy electron (creates a cation)

Ei trends

greatest at top right (low PQN, high Zeff)

subsequent ionizations

harder to do because Zeff keeps increasing, very hard after valence shell removed

octet rule

representative elements tend to undergo reactions leaving them with a noble gas configuration (8ve)

ionic bonding

ions stick together in salts

lattice energy

amount of energy needed to split an ionic compound

lattice energy factors

greater charges and smaller ions = stronger bonds

formation of covalent bonds

atoms don't collide due to repulsion but stay near each other due to attraction, share electrons to fill valence shell

length/strength of bonds

the more bonds you have, the shorter and stronger they are (triple vs single)

electronegativity

the ability of an atom to attract shared electrons in a covalent bond

electronegativity trends

highest in top right (ignore noble gases)

en trend explanation

small radius (can get close to other element), high Zeff (pulls electrons closer)

nonpolar covalent bond

equal sharing (same element or similar en values)

polar covalent bonds

unequal sharing skews electron density to one side of the bond (moderately different en values)

ionic bonds

occur when en values are too different to allow sharing

electron dot symbols

represent an element and its valence electrons (paired = unavailable)

Lewis dot structure

represents a molecule using the dot symbols of the atoms

radicals

molecules with an unpaired electron (least en atom has unfilled octet)

octet violators

H (2), Be (4), B (6), P (8, 10), S (8, 10, 12)

resonance structures

when a structure can be drawn by moving electrons but no atoms

if not enough electrons

more bonds

if too many electrons

more lone pairs

formal charges

a way to track the charges on an atom, should add up to the total charge

polar molecules

asymmetrical molecule

polar bond, nonpolar molecule

symmetrical

london dispersion force

temporary dipole forms, more common in larger molecules

dipole-dipole force

attraction between partial positive and partial negative in a polar molecule

hydrogen bonding

when hydrogen is bonded to F, N, or O

ion-dipole force

attraction between cation and partial negative and anion and partial positive

network covalent solids

all atoms joined by covalent bonds, hard with high melting point

potential energy

stored energy from the position of an object

kinetic energy

energy of motion

state function

same result regardless of the pathway

temperature

average energy of motion of the particles of a substance

heat

transfer of thermal energy

calorimeter equation

q = smAt

specific heat of water

4.18 J, 1 cal

hess's law

enthalpy = state function

pressure

force/area

standard atmospheric pressure

760mmHg, 1 atm

Boyle definition

pressure is inversely proportional to volume

Charles definition

temperature is directly proportional to volume

Avogadro definition

volume is directly proportional to moles

temperature (gas)

average speed of the particles, arrows in diagram

volume (gas)

amount of space between particles, container size in diagram

pressure (gas)

force of particles colliding with the container, impact lines in diagram

moles

amount of particles, increase or decrease in diagram

molar volume of ideal gas

22.4 L/mol

assumptions of ideal gas

no attraction or repulsion, particles very far apart and small

Arrhenius acid

produces H+ in water

Arrhenius base

produces OH- in water

HClO4

perchloric acid, strong

H2SO4

sulfuric acid, strong

HBr

hydrobromic acid, strong

HCl

hydrochloric acid, strong

HNO3

nitric acid, strong

H3PO4

phosphoric acid, weak

HF

hydrofluoric acid, weak

HNO2

nitrous acid, weak

CH3CO2H

acetic acid, weak

KOH

potassium hydroxide, strong base

NaOH

sodium hydroxide, strong base

Ba(OH)2

barium hydroxide, strong base

Ca(OH)2

calcium hydroxide, strong base

NH3

ammonia, weak base

neutralization reaction

acid + base -> salt + water

strong vs weak acid/base

strong acid/base = strong eelctrolyte, weak acid/base = weak electrolyte

pH or pOH (given concentration)

-log(concentration)

pH + pOH

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