1. Unit 4 Chemical Formulas Ionic Molecular Cation (+) Anion (-) No ions
All nonmetals
metals
nonmetals
Ammonium compounds are ionic even though they contain only nonmetals
NH4+1
Acids are molecular compounds that begin with the element H.
This means they produce hydrogen ions in solution. H+
Bases are ionic compounds that end with hydroxide ions
OH-1
Salts are ionic compounds that don’t have hydroxide

2. Location of metals and nonmetals
Note: Hydrogen is a nonmetal
Metals
Nonmetals
Metalloids

3. HCl NaNO3 CaCO3 CO2 FeCl3 O2 H3PO4 Mg(OH)2 molecular (Acid) ionic
Hydrogen is a nonmetal
Acids start with “H”
Ionic compounds start with metals or ammonium, NH4+ .
Bases have OH- anions
molecular
(Acid)
HCl
NaNO3
ionic
(salt)
ionic
CaCO3
CO2
(salt)
molecular
ionic
(salt)
FeCl3
molecular O2
H3PO4
Mg(OH)2
molecular
(Acid)
ionic
(base)

4. NH4Cl SO2 HNO3 NaCl KOH NO2 ionic (salt) molecular molecular (acid)
Hydrogen is a nonmetal
Acids start with “H”
Ionic compounds start with metals or ammonium, NH4+ .
Bases have OH- anions
ionic
(salt)
NH4Cl
SO2
molecular
HNO3
NaCl
molecular
(acid)
ionic
(salt)
KOH
NO2
ionic
(base)
molecular

5. NAMING Chemical Formulas Ionic Molecular Cation (+) Anion (-)
Monatomic anion
ends in “ide”
Transition metals with multiple charge use Roman numerals.
(Reference sheet)
CaCl2
calcium
chloride
CuCl2
copper (II)
chloride
Polyatomic ions (Use Reference sheet)
KMnO4
potassium
permanganate

6. Polyatomic ions Reference:
ammonium, NH4+1
hydroxide, OH-
nitrate, NO3-1
carbonate, CO32- -2
lithium
chloride
LiCl
KNO3
potassium
nitrate
MgCO3
Na2O
magnesium
carbonate
sodium
oxide +6 -6
Fe3+
-2(3)
Iron (III)
oxide
Fe2O3
Iron (II)
oxide
FeO
NH4NO3
Mg(OH)2
ammonium
nitrate
magnesium
hydroxide

7. Polyatomic ions Reference:
ammonium, NH4+1
hydrogen carbonate, HCO31-
(bicarbonate)
dichromate, Cr2O72-
sulfite, SO32-
sulfate, SO42-
phosphate, PO43-
ammonium
chloride
NH4Cl
CaCr2O7
calcium
dichromate
sodium
hydrogen carbonate
sodium
bicarbonate
NaHCO3
Ca3(PO4)2
calcium
phosphate
sodium
sulfate
Na2SO4
calcium
sulfite
CaSO3

8. NAMING Chemical Formulas Ionic Molecular Cation (+) Anion (-)
mono 1 di 2
tri 3
tetra 4
penta 5
hexa 6
hepta 7
octa 8
nona 9
deca 10
Cation
(+)
Anion
(-)
All nonmetals
Use prefixes
Use periodic table
and
(Reference sheet)
carbon
monoxide CO
carbon
dioxide
CO2
carbon
tetrachloride
CCl4
dinitrogen
monoxide
N2O

9. Naming Binary Molecular Compounds
- Compounds between two nonmetals
- First element in the formula is named first.
- Second element is named as if it were an anion.
- Use prefixes
- Only use mono on second element -
CO =
carbon monoxide
CO2 =
carbon dioxide
CCl4 =
carbon tetrachloride
N2O =
dinitrogen monoxide

10. SO2 N2O4 NO2 P2O5 PCl3 PCl5 SF8 XeF4 NO OF2 AsCl3 NI3 sulfur dioxide
mono 1 di 2
tri 3
tetra 4
penta 5
hexa 6
hepta 7
octa 8
nona 9
deca 10
dinitrogen
tetraoxide
N2O4
nitrogen
dioxide
NO2
P2O5
diphosphorus
pentaoxide
phosphorus
trichloride
PCl3
phosphorus
pentachloride
PCl5
sulfur
octafluoride
SF8
xenon
tetrafluoride
XeF4
nitrogen
monoxide NO
oxygen
difluoride
OF2
arsenic
trichloride
AsCl3
nitrogen
triiodide
NI3

11. Molecular Formulas (Acid Naming)
Acids without oxygen: General formula HA where A = “anion”
Hydro_______ic acid
HF =
Hydrofluoric acid
HCl =
Hydrochloric acid
HBr =
Hydrobromic acid
HI =
Hydroiodic acid
HCN =
Hydrocyanic acid
CN- = cyanide anion

12. Naming Acids H+ + (anions with oxygen)
Acids with oxygen: “ate-ic ite-ous”
Anion name Acid name
____ate ____ic acid
___ite ___ous acid
HNO3 =
Nitr__?__ acid
Anion NO3-1 = nitrate
Nitric acid
HNO2 = Nitr__?__ acid
Anion NO2-1 = nitrite
Nitrous acid

13. Naming Acids H+ + (anions with oxygen)
Formula H+ with Anion Acid name
H2SO4
2H+ + SO42- = sulfate
Sulfuric acid
H2SO3
2H+ + SO32- = sulfite
Sulfurous acid
HC2H3O2
H+ + C2H3O2-1 = Acetate
Acetic acid
H3PO4
3H+ + PO43- = Phosphate
Phosphoric acid
HClO4
H+ + ClO41- = Perchlorate
Perchloric acid
H2CO3
2H+ + CO32- = Carbonate
Carbonic acid