Basic Chemistry

Hydronium

H3O+

Ammonium

NH4+

Acetate

CH3CO2- or CH3COO-

Cyanide

CN-

Hypochlorite

ClO-

Chlorite

ClO2-

Chlorate

ClO3-

Perchlorate

ClO4-

Hypobromite

BrO-

Bromite

BrO2-

Bromate

BrO3-

Perbromate

BrO4-

Hypoiodite

IO-

Iodite

IO2-

Iodate

IO3-

Periodate

IO4-

Dihydrogen Phosphate

H2PO4-

Hydrogen Carbonate or Bicarbonate

HCO3-

Hydrogen Sulfate or Bisulfate

HSO4-

Hydroxide

OH-

Permanganate

MnO4-

Nitrate

NO3-

Nitrite

NO2-

Carbonate

CO3^2-

Chromate

CrO4^2-

Dichromate

Cr2O7^2-

Peroxide

O2^2-

Hydrogen Phosphate

HPO4^2-

Sulfate

SO4^2-

Sulfite

SO3^2-

Thiosulfate

S2O3^2-

Phosphate

PO4^3-

Phosphite

PO3^3-

Anion ends with -ate

Acid ends with -ic

Anion ends with -ite

Acid ends with -ous

Water-Soluble Compounds rule 1 (alkali)

Compounds containing alkali metal cation (Li, Na, K, Rb, Cs) or the ammonium ion (NH4+); no exceptions

Water-Soluble Compounds rule 2

Compounds containing the nitrate ion (NO3-) acetate ion (C2H3O2-) or chlorate ion (ClO3-); no exceptions

Water-Soluble Compounds rule 3

Compounds containing the chloride ion (Cl-) bromide ion (Br-) or iodide ion (I-); except Compounds containing Ag+, Hg2^2+, or Pb^2+

Water-Soluble Compounds rule 4

Compounds containing the sulfate ion (SO4^2-); except Compounds containing Ag+, Hg2^2+, Pb^2+, Ca^2+, Sa^2+, Ba^2+

Water-insoluble Compounds rule 1

Compounds containing the carbonate ion (CO3^2-) phosphate ion (PO4^3-) chromate ion (CrO4^2-) or sulfide ion (S^2-); except Compounds containing alkali metal cation (Li, Na, K, Rb, Cs) or the ammonium ion (NH4+)

Water-insoluble Compounds rule 2

Compounds containing the hydroxide ion (OH-); except Compounds containing alkali metal cation (Li, Na, K, Rb, Cs), the ammonium ion (NH4+), and Ba^2+

Strong Acids (7)

Hydrochloric (HCI)

Hydrobromic (HBr)

Hydroiodic (HI)

Nitric (HNO3)

Chloric (HCIO)

Perchloric (HCIO)

Sulfuric (H2SO4)

Strong Bases (8)

Lithium hydroxide (LiOH)

Sodium hydroxide (NaOH)

Potassium hydroxide (KOH)

Rubidium hydroxide (RoOH)

Cesium hydroxide (CsOH)

Calcium hydroxide (Ca(OH)2)

Strontium hydroxide (Sr(OH)2)

Barium hydroxide (Bа(ОН)2)

Molarity (M)

dividing the number of moles solute by the liters solution (mol/L)

Percent by mass

Mass of solute divided by mass of solution (solute+solvent) * 100%

Avogadro's number, 1 mole

6.022x10^23

Moles of element

Mass of element g / molar mass of element g/mol

Formula mass

Sum of atomic masses of a formula unit (ionic compounds)

Molar mass

Mass in g of 1 mole of substance (# g/mol)

Mass percentage composition

Of each element in a compound; % = n*molar mass of element/molar mass compound x 100%

Calculate Celsius

Fahrenheit - 32/ 1.8 or K - 273

Calculate kelvin

Celsius + 273

Calculate Fahrenheit

1.8(celcius) + 32

Density

Mass/volume

Accuracy

How close to actual value

Precision

How close measurements are to each other

To find highest electrical conductivity

Molarity * # of ions = M elec conductivity

Molarity

n/V

number of moles (n)

n = mass (m)/molar mass (M)

Dilution

M1 V1 = M2 V2

Oxidation Numbers Rule 1

The oxidation number of any element, in its elemental form, is zero.

Oxidation Numbers Rule 2

oxidation numbers must sum to zero for any molecule, and must sum to the charge on any polyatomic ion.

Oxidation Numbers Rule 3

Fluorine is -1

Oxidation Numbers Rule 4

Group 1A or 2A metal

+1 or +2, respectively

Oxidation Numbers Rule 5

Hydrogen

+1

EXCEPT Any combination with a Group 1A or 2A metal to form a metal hydride.

Oxidation Numbers Rule 6

Oxygen

-2

EXCEPT Any combination with something higher on the list that necessitates its having a different oxidation number

Oxidation Numbers Rule 7

Group 7A (other than Fluorine)

-1

EXCEPT Any combination with something higher on the list that necessitates its having a different oxidation number