Chapter 4
Binary
compounds-contain 2 elements
1) metal w/ charge and non-metal (Type I)
2) Transition metal and non-metal (Type II)
3) two non-metals (Type III)
(Type I)
 Cation- 1st – same name as element
 Anion- 2nd- root + ide
Examples
 NaI
 CaO
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1) write element symbol and charge
2) net charges must equal zero
3) add subscripts if charges don’t add up to
zero
Barium sulfide
Magnesium phosphide
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How to write formula from name
1) write element symbol and charge
2) net charges must equal zero
3) add subscripts if charges don’t add up to
zero
Lead (II) oxide
Iron (III) sulfide
Roman numeral= charge of transition metal
Write name from formula
• Need to figure out the charge
• Include roman numeral in name
 FeCl2
(__x 1) + (-1 x 2)= 0
Fe+2
Iron (II) chloride
 ic- higher charge Fe+3 Ferric
 ous- lower charge Fe+2 Ferrous
 Example 4.2, 4.3
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1) name the first element by its element name
2) second element is named as though it were
an anion (ide ending)
3) prefixes are used to denote the number of
atoms (Table 4.3 pg 95)
4) mono is never used for the first element
Example 4.4, 4.5
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Example 4.6
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Polyatomic ion- charged entities composed
of several atoms bound together
Oxyanions- SO3 and SO4
ite
ate
hypo-less than
per- more than
ClO- hypochlorite
ClO2 – chlorite
ClO3 – chlorate
ClO4 - perchlorate
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Must know
- name of polyatomic ion
- charge of polyatomic ion
- recognize polyatomic ion
NH4C2H3O2
FeSO4
Example 4.7
more than one polyatomic ion or
polyatomic ions with a subscript require
parentheses
(NH4)2SO4
Fe3(PO4)2
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Polyatomic ions names do not change
Ammonium nitrate
Calcium hydroxide
Lead (II) sulfate
Acids- when dissolved in H2O, they produce
H+ ions
 Sour taste
Naming
 1) if the anion does not contain O2 then use
hydro prefix, element root + ic (ex: HCl)
 2) if O2 is in the anion, then look at the
ending of the polyatomic ion (HNO3 and
HNO2)
ite- ous  acid ending
ate- ic

Calcium hydroxide
Ca(OH)2
 Iron (II) oxide
FeO
Example 4.9

1.
2.
3.
4.
5.
6.
7.
HF
HBr
H3PO4
HNO2
Nitric acid
H2SO3
H2SO4
9. Chlorous Acid
10. HClO3
11. HClO4
12. carbonic acid
13. HC2H3O2
14. HClO
15. HI
1.
2.
3.
4.
5.
6.
7.
8.
Hydrofluoric Acid
HCl
Hydrobromic Acid
Phosphoric Acid
Nitrous Acid
HNO3
Acid
Sulfurous Acid
Sulfuric Acid
9. HClO2
10. Chloric Acid
11. Perchloric Acid
12. H2CO3
13. Acetic Acid
14. Hypochlorous
15. Hydroiodic Acid