CHEM 1001 - FINAL STUDY GUIDE

OH^-

hydroxide

NO₃^-

nitrate

NO₂^-

nitrite

SO₃^-2

sulfite

SO₄^-2

sulfate

HSO₄^-

hydrogen sulfate

CO₃^-2

carbonate

PO₄^-3

phosphate

HCO₃^-

hydrogen carbonate

ClO^-

hypochlorite

ClO₂^-

chlorite

ClO₃^-

chlorate

ClO₄^-

perchlorate

CN^-

cyanide

NH₄⁺

ammonium

p_iV_i = p_fV_f

Boyle’s Law

V_i / T_i = V_f / T_f

Charles Law

p_iV_i / T_i = p_fV_f / T_f

Combined Gas Law

pV = nRT

Ideal Gas Law

Celsius to Kelvin

K = C + 273.15

Strong Acids

HCl

HBr

HI

HClO₃

HClO₄

HNO₃

H₂SO₄

Weak Acids

HF

HCHO₂

HC₇H₅O₂

Strong Bases

LiOH

NaOH

KOH

RbOH

CsOH

Ca(OH)₂

Sr(OH)₂

Weak Bases

NH₃

As volume decreases,

pressure increases

As temperature increases,

pressure increases

As n (# of gas molecules) increases

pressure increases

Electron domain geometry

# of electron domains

Molecular Geometry

Determined by central atom

Nonpolar

Net dipoles cancel out/go in opposite directions, electronegativity difference less or equal to 0.4, one or more domains is different than others

Polar

Electronegativity difference more than 0.4, same domains, pulling in same general direction

Formal Charge Equation

Formal Charge = valence electrons - bonding - nonbonding

linear bond angle

180

trigonal planar bond angle

120

bent bond angle when 1 lone pair

120

bent bond angle when 2 lone pairs

109.5

trigonal pyramidal bond angle

109.5

tetrahedral bond angle

109.5

hydrogen bonds can only occur with

H atoms attached to N, O, or F atoms

list the forces/bonds from weakest to strongest

London —> Dipole-Dipole —> Hydrogen Bonding —> Ion-Dipole

n quantum number

n = 1, 2, 3…

orbital size, energy, shell #

l quantum number

l = 0, 1, …n-1

orbital shape, angular momentum

m_l quantum number

m_l = -l —> +l

orientation of orbital in space

m_s quantum number

m_s = ± 1/2

electron spin

l = 0

s-orbital (sphere)

l = 1

p-orbital (dumbell)

l = 2

d-orbital

l = 3

f-orbital

best lewis structure

lowest possible formal charge on most electronegative atom

Density Equation

d = mass (grams) / volume (liters)

2 domains, 0 lone pairs

linear

3 domains, 0 lone pairs

trigonal planar

3 domains, 1 lone pair

bent

4 domains, 0 lone pairs

tetrahedral

4 domains, 1 lone pair

trigonal pyramidal

4 domains, 2 lone pairs

bent

5 domains, 0 lone pairs

trigonal bipyramidal

5 domains, 1 lone pair

seesaw

5 domains, 2 lone pairs

t-shaped

5 domains, 3 lone pairs

linear

6 domains, 0 lone pairs

octahedral

6 domains, 1 lone pair

square pyramidal

6 domains, 2 lone pairs

square planar

Dilution Equation

M₁V₁ = M₂V₂

Molarity

M = mol / L

Average Atomic Mass Equation

AAM = (abundance_A x mass_A) + (abundance_B x mass_B) …

Combustion

C_xH_y + O₂ —> CO₂ + H₂O

VSEPR MODEL

The Valence Shell Electron Pair Repulsion (VSEPR) model predicts that the optimum geometry of a molecule is established by minimizing the repulsions of the electron domains on the central atom.

non-Electrolytes

The compound dissolves in water but does not create ions necessary to carry the charge.

Strong Electrolyte

Ionic compounds that fully dissolve and completely ionize are strong electrolytes because they produce ions that carry charge.

Weak Electrolytes

Ionic materials that are highly soluble but only partially ionize are weak electrolytes.

Color and Temperature relationship

Red light = lower energy

Blue light = higher energy

Infrared —> Red —> Yellow —> White —> Blue-white

Melting Point

The molecules with the strongest forces will require more energy to melt and will have the highest melting point.

London

All molecules have London forces.

Larger molecules —> larger London forces

Dipole-Dipole

Polar molecule

Hydrogen bond

H-F, H-N, or O-H bonds

Ion-Dipole

1. Ion (Na⁺, NH₄⁺, NO₃^-)

2. Polar molecule usually the solvent

Kinetic-Molecular Theory of Gases

1. Gases contain a large number of molecules in continuous random motion.

2. Most of the volume is empty space.

a. As a result, gases are very compressible.

3. The pressure of the gas comes from the force exerted by the particle when it hit the container wall.

a. The force arises from the change in momentum (mv) that occurs when the particle hits the wall and changes direction.

Less Electrons than an Octet

The atoms H, He, Li, Be, B will have less than an octet of electrons.

Odd Number of Total Valence Electrons

When the total valence electrons is an odd number there is no way to satisfy each atom with an octet of electrons. These molecules are called radicals.

n-type semiconductors

P, As, Sb

p-type semiconductors (holes)

B, Ga

A large gap between the conduction band and valence band.

Insulators

The conduction band and valence band overlap.

Metals

A little gap between the conduction band and valence band.

semi-conductors

Al

+3

Ag

+

Ni

+2

Zn

+2

Atomic Radius

Increasing (down)

Increasing (left)

Ionization Energy

Increasing (up)

Increasing (right)

Greenhouse Effect

H₂O

CO₂

CH₄

N₂O