Chapter 7 review (Section 7.1-7.2)
When you are studying, make sure that you cover the following topics:
1.
Section 7.1: Nomenclature
Note: 85% of the test will be nomenclature. Spend the most time on this… a.
Cations i.
Elements which are metals, form cations ii.
The cation name is the same as the element name iii.
“1-2-3” cations: always have the same charge
1.
Group 1: 1+
2.
Group 2: 2+
3.
Group 3: 3+
4.
Ag (silver): 1+
5.
Zn (zinc) and Cd (cadmium): 2+
6.
Al (aluminum) and Ga (gallium): 3+ iv.
“Skip” cations: can have different charges
1.
All other metals b.
Anions i.
Non-metals only ii.
Anion name: suffix –ide
1.
Hydride
2.
Oxide
3.
Sulfide
4.
Selenide
5.
Nitride
6.
Phosphide
7.
Fluoride
1

2
8.
Chloride
9.
Bromide
10.
Iodide iii.
Always have the same charges
1.
Hydrogen: hydride 1-
2.
Group 15: a.
Nitride 3- b.
Phosphide 3-
3.
Group 16: a.
Oxide 2- b.
Sulfide 2- c.
Selenide 2-
4.
Group 17: a.
Fluoride 1- b.
Chloride 1- c.
Bromide 1- d.
Iodide 1- c.
Polyatomic ions i.
Memorize all polyatomic ions (formulas, names, charges) on p.
226 in book. ii.
General guidelines
1.
–ite and –ate suffixes indicate polyatomic ions, e.g. nitrite, sulfate, etc.
2.
3 exceptions a.
Cyanide CN- b.
Hydroxide OH- c.
Ammonium NH4+

3 d.
Type I compounds i.
1-2-3 cations (metal), plus anion (non-metal) ii.
Formula to name
1.
Name of cation + name of anion
2.
E.g. Na2SO4: sodium sulfate
3.
E.g. NH4Cl: ammonium chlorate
4.
E.g. MgO: magnesium oxide iii.
Name to formula
1.
Criss cross
2.
E.g. Silver oxide:
Ag+, O2-

Ag2O
3.
E.g. Magnesium Nitrate
Mg 2+ , (NO
3
) 1-
Mg(NO
3
)
2 e.
Type II compounds i.
“Skip” cations + anion ii.
Stock system: () after the cation, roman numeral in ()’s to show cation’s charge iii.
Name to formula
1.
Criss cross
2.
E.g. iron (III) sulfate Fe 3+ , SO
4
2-
Fe
2
(SO
4
)
3
3.
E.g. chromium (I) oxide
Cr1+, O2-
Cr
2
O iv.
Formula to name
1.
Reverse criss cross (charges must match!)

4
2.
E.g. Pb
2
(SO
4
)
3
Pb3+, SO
4
2-
Lead (III) sulfate f.
Type III compounds i.
Covalent compounds (nonmetals only), ex CO2 ii.
Prefix system iii.
Prefixes to remember
1.
mono
2.
di
3.
tri
4.
tetra
5.
penta
6.
hexa
7.
hepta
8.
octo
9.
nona
10.
deca iv.
Prefixes used for subscript numbers v.
First element has normal name (prefix only if has subscript); second element always has a prefix, “mono” if no subscript vi.
E.x. CO
2
= carbon dioxide vii.
E.g. N
2
F
4
= dinitrogen tetrafluoride
2.
Section 7.1: oxidation numbers a.
Three steps i.
Make algebraic statement: sum of oxidation numbers = charge of the compound (0, if it’s a compound, the ionic charge if it’s a polyatomic ion)

5 ii.
Assign known oxidation numbers iii.
Solve for the unknown iv.
Known oxidation numbers
1.
Senior class: group 1 (+1), group 2 (+2), fluorine (-1)
2.
Junior class: H (+1), O (-2)
3.
Sophomore class: the element with the higher electronegativity (closer on periodic table to fluorine)
4.
The other elements