Chemistry Manual 2012-2013 - Edison State College
Chemistry Manual 2012-2013 - Edison State College
Chemistry Manual 2012-2013 - Edison State College
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Blake Schmidt - Unit 6 Page 33<br />
1.<br />
U6 EP2<br />
Unit 6: Example Problems 2<br />
Ionic Compounds<br />
Name and/or write the formula for the following ionic compounds. Be prepared to draw each<br />
as both an electrically neutral empirical compound and dissociated ions.<br />
a. Na2O<br />
5.<br />
a. lithium bromide<br />
9.<br />
a. sodium nitrate<br />
b. K2S<br />
b. sodium iodide<br />
b. aluminum phosphate<br />
c. MgCl2<br />
c. silver sulfide<br />
c. calcium carbonate<br />
d. CaBr2<br />
d. cesium oxide<br />
d. sodium carbonate<br />
e. BaI2<br />
e. beryllium iodide<br />
e. calcium nitrate<br />
f. Al2S3<br />
f. barium hydride<br />
f. aluminum carbonate<br />
2.<br />
a. CsBr<br />
6.<br />
a. silver oxide<br />
10.<br />
a. K2SO4<br />
b. AgF<br />
b. aluminum sulfide<br />
b. Mg(NO2)2<br />
c. Na3N<br />
c. sodium nitride<br />
c. AgNO3<br />
d. K2O<br />
d. barium chloride<br />
d. Cu3PO4<br />
e. AgBr<br />
e. strontium hydride<br />
e. Be(OH)2<br />
f. MgI2<br />
f. aluminum fluoride<br />
f. Al3HCO3<br />
3.<br />
a. SnBr2<br />
7.<br />
a. chromium(III) chloride<br />
11.<br />
a. potassium hydroxide<br />
b. SnBr4<br />
b. tin(IV) oxide<br />
b. ammonium hydroxide<br />
c. CrO<br />
c. lead(II) oxide<br />
c. potassium bicarbonate<br />
d. Cr2O3<br />
d. copper(II) iodide<br />
d. zinc carbonate<br />
e. Hg2I2<br />
e. cobalt(II) oxide<br />
e. cobalt(II) hydroxide<br />
4.<br />
f. HgI2<br />
a. PbCl2<br />
8.<br />
f. cobalt(III) oxide<br />
a. chromium(III) sulfide<br />
12.<br />
f. iron(III) phosphate<br />
+<br />
a.<br />
Na<br />
b. Fe2O3<br />
b. manganese(IV) oxide<br />
c. SnI2<br />
c. gold(III) chloride<br />
b. K Cl<br />
d. Hg2O<br />
d. titanium(IV) chloride<br />
e. HgS<br />
f. CuI<br />
e. iron(II) bromide<br />
f. iron(II) oxide<br />
c.<br />
+<br />
Na<br />
O<br />
O<br />
S<br />
O<br />
2-<br />
O
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