Category 3 - Ionic Compounds April 5
Metals and non-metal form ions when they get near each other.
Remember an ion is an atom that has lost or gained electrons.
Review Sheet. A
Ions show the combining capacity/valence as determined by the outer electron orbitals.
Their charges can be determined by their
- group in the P.T.
- by looking at the Table found on the back of your P.T.
“Names, formulae, and Charges of Some Common Ions”
Anions (-) Cations (+)
WRITING PROPER FORMULA
- balancing + and – integer method
- criss cross method
NOMENCLATURE
- write the full name of the metal first,
space,
write the non-metal second changing the ending to “ide”
· Do not use prefixes!
Category 4 - Ionic Compounds with multiple Ion charges (valences)
Some elements can form several ions depending on the conditions when the compound forms. These ions are mainly found in the transitions metal section of the P.T.
Why?...
their valence electrons can be removed from the s or d configurations.
Examples:
Fe
Fe2+ Iron (II) or ferrous
Fe3+
Iron (III) or ferric
To make ionic compounds use the same criss cross rules as in regular ionic compounds.
* But in naming these compounds,
ALWAYS show the Roman Numeral to indicate which ion was used!
Practice Sheet 3
Text p. 55 Q.4,5
Quiz out of 10 tomorrow.
#3
a. KBr
b. MgCl2
c. CaO
d. AlI3
e. BaF2
f. NaI
g. CaBr2
h. K2O
i. BeCl2
j. Al2O3
#4
a. 2+ Tin(II) oxide
b. 4+ Tin (IV) bromide
c. 2+ Iron (II) sulfide
d. 3+ Iron (III) chloride
e. 3+ Chromium (III) oxide
f. 2+ nickel (II) chloride
#5
a. SnCl4
b. FeF2
c. SnO2
d. Fe2S3
e. FeF2
f. HgO
g. Co2O3
#6
a. Ca(C2H3O3)2
b. Na3PO4
c. CuSO4
d. Fe3(PO4)2
e. Al(OH)3
f. Ca((HCO3)2
g. (NH4)3PO4
h. Li2Cr2O7