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)
ONLY ONLY If YES:
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
FeP PbCO3 H2CO3
% = Part X 100
Whole
% 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:
MF=(EF)n
n=MF molar mass (given in problem)
EF molar mass
MF=C6H12O6 EF=CH2O n=6
n=180.18g/mol = 6
30.03g/mol