Binary Molecular Compounds Binary Ionic Compounds Ternary Ionic Compounds Acids

To Write Name: To Write Name: To Write Name: To Write Name:

Does it contain oxygen?

______ide ______( ) ______ide ______( ) ______If NO:

prefix name of 1st prefix root of 2nd name of charge of name of name of charge of name of hydro______ic acid

(but never element (always) element metal ion metal ion nonmetal positive ion metal ion negative ion root of

mono-) Cu, Sn, ion (usually Cu, Sn, (usually a nonmetal ion

Pb, Fe a metal) Pb, Fe polyatomic ion)


Example: C3H8 Example: MgBr2 Example: Mg(ClO3)2 ______acid

root of ate to ic

tricarbon octahydride magnesium bromide magnesium chlorate polyatomic ion ite to ous

Example: SO4 Example: Sn3N2 Example: Cu3PO3 Example: HF

sulfur tetraoxide Look to negative ion to Look to negative ion to hydrofluoric acid

determine charge of metal ion! determine charge of metal ion!

Example: HClO3

Sn3? N2-3 Cu3? (PO3)1-3

ClO3 is chlorate so HClO3 is:

tin (II) nitride copper (I) phosphite chloric acid

To Write Formula: To Write Formula: To Write Formula: To Write Formula:

Prefix indicates the # of atoms present. Determine charge of positive Same rules as BIC. Same rules as BIC and TIC.

ion and charge of negative ion. H+1 will always be the positive ion.

Example: The correct formula has a

carbon tetrahydride charge = 0. “crossing over”

Example: Example:

CH4 Example: sodium oxalate hydrobromic acid

potassium nitride Na+1 (C2O4)-2 so +1+1-2=0 H+1 Br-1 so +1-1=0

K+1 N-3 so +1+1+1-3=0

Example: Na2C2O4 HBr

Carbon monoxide K3N

Example: Example:

CO Example: iron (III) phosphide lead (II) carbonate carbonic acid (change ic to ate)

Fe+3P-3 so +3-3=0 Pb+2 (CO3)-2 so +2-2=0 H+1 (CO3)-2 so +1+1-2=0


% = Part X 100


% composition = Elements Mass X 100

Compounds Mass

Ex: What is the % O in H2O?

% O = 16.00 g X 100 = 88.79%

18.02 g

Empirical Formula (EF):

smallest ratio/reduced form

Ex: CrCl3, FeSO3, CH2, CH3

How to calculate EF:

% to mass,

mass to mole,

divide by small,

multiply till whole,

Ex: 45.77% S and 54.23% F

% to mass: 45.77g and 54.23g

mass to mole:

S: 45.77g/32.07g/mol=1.427mol

F: 54.23g/19.00g/mol=2.854mol

divide by small:

S: 1.427mol/1.427mol=1

F: 2.854mol/1.427mol=2

multiply till whole:

not needed for this example

Answer: SF2

Molecular Formula (MF):

actual ratio/not reduced form

Ex: C6H12O6, C2H4, C6H12, C3H6

How to calculate MF:


n=MF molar mass (given in problem)

EF molar mass

MF=C6H12O6 EF=CH2O n=6

n=180.18g/mol = 6