CHM 2045 Midterm Williams

Density formula

Density = mass/volume

SI Base Units: Mass

kilogram (kg)

SI Base Units: Time

seconds (s)

SI Base Units: Length

meter (m)

SI Base Units: Temperature

Kelvin (K)

SI Base Units: Amount of substance

mole (mol)

SI base units - electric current

ampere, A

SI Base Units: Luminous intensity

candela (cd)

Metric System - Giga

G 10^9

metric system - mega

M 10^6

metric system- kilo

k 10^3

Metric System Base Units

1

metric system deci

d 10^-1

metric system centi

c 10^-2

metric system milli

m 10^-3

metric system micro

M 10^-6

metric system nano

n 10^-9

Temperature (Kelvin and Celsius)

add 273 for C to K and subtract for K to C

symbolic representation of elements

atomic and mass # switched for periodic table

n=

neutrons

Z=

protons

Percent abundance formula

# of atoms of an isotope/ total # of atoms all isotopes of that element*100%

atomic weight formula

% abundance of isotope 1/100 x mass of isotope 1 + % abundance of isotope 2/100 x mass of isotope 2

Binary molecular prefix 1

mono

Binary molecular prefix 2

di

Binary molecular prefix 3

tri

Binary molecular prefix 4

tetra

Binary molecular prefix 5

penta

Binary molecular prefix 6

hexa

Binary molecular prefix 7

hepta

Binary molecular prefix 8

octa

Binary molecular prefix 9

nona

Binary molecular prefix 10

deca

Hydronium

H3O+

Ammonium

NH4+

Cyanide

CN-

Acetate

C2H3O2-

Carbonate

CO3 2-

Hydrogen Carbonate

HCO3-

Oxalate

C2O4 2-

Hypochlorite

ClO-

Chlorite

ClO2-

Chlorate

ClO3-

Perchlorate

ClO4-

Nitrite

NO2-

Nitrate

NO3-

Phosphate

PO4 3-

hydrogen phosphate

HPO4 2-

Dihydrogen Phosphate

H2PO4-

Chromate

CrO4 2-

Dichromate

Cr2O7 2-

permanganate

MnO4-

hydroxide

OH-

Sulfite

SO3 2-

Sulfate

SO4 2-

Hydrogen Sulfate

HSO4-

Polyatomic cations end in

ium

monoatomic anions end in

-ide

(cations/anions) go before (cations/anions) when forming equations

cations then anions

Ionic compouds are?

metals or NH4

Molecular compounds are?

nonmetals (2 or more)

moles equals

6.02 X 10^23 molecules/atoms

Mol to mass conversion

moles times grams/1 mol

mass to mol conversion

grams times mol/1 gram

percent composition formula

mass of element/mass of compound x 100

empirical formula

percent g times mol. molar mass in grams equals _____ mol, once all formulas composition is used then divide all by smallest amount of mols. These will be the lower subscript for the formula.

Molecular formula

molar mass g/mol divided by emperical formula mass=n. n is then multiplied by the original coefficents from the empirical formula

Solubility

if a substance is not soluble on the solubility chart, the product will form a solid)

Complete Ionic Equation (CIE)

every element written out besides the solids

net ionic equation (NIE)

formula left after spectator ions are removed from complete ionic equation

strong acids and bases __________ dissolve

completely

1 multiple choice option

weak acids and bases________ dissolve

do not completely

1 multiple choice option

Strong acids: Hydrochloric acid

HCl

strong acids- hydrobromic acid

HBr

strong acids- Hydroiodic Acid

HI

Strong acids: Nitric acid

HNO3

Strong Acids chloric acid

HClO3

Strong acids: Perchloric acid

HClO4

Strong acids: Sulfuric acid

H2SO4

Weak Acid- Hydrofluoric

HF

Weak Acid: Phosphoric Acid

H3PO4

Weak Acid: Carbonic Acid

H2CO3

strong base lithium hydroxide

LiOH

Strong Base: Sodium Hydroxide

NaOH

Strong Base: Potassium Hydroxide

KOH

strong base barium hydroxide

Ba(OH)2

strong base strontium hydroxide

Sr(OH)2

Weak Base: Ammonia

NH3

A acid_____ h+ ions

donates

a base ____ H+ ions

accepts

1 multiple choice option

a strong base/acid

dissociate completely

a weak base/acid

partial dissociates

OIL RIG stands for

Oxidation is loss of electrons

Reduction is gain of electrons

oxidizing agent

gains electrons (reduction)

reduction agent

loses electrons (oxidization)

Oxidation rules: Each atom in a pure substance has a ON of

0

Oxidation rules: monoatomic ions have a ON of

their individual charge

Oxidation rules: F is always

-1 except when other elements are involved

Oxidation rules: oxygen is often

-2

Oxidation rules: halogens have a ON of

-1 unless paired with F or O