Chapter 6 Practice Test
1) When does the “cross your charges” technique NOT work?
2) Write the names and formulae of sufficient ionic and molecular compounds to give examples of all the rules and exceptions discussed in class. Don’t forget acids!
3) Name this one: NaBH2. What’s different about this chemical?
4) Name the following: HCN, KCN, C3N4
5) Write out the formulas for the following acids: sulfuric acid, sulfurous acid, hydrosulfuric acid.
6) List all the diatomic elements. Write down the names for at least three of them.
7) Calculate the molar mass of the following compounds: (Hint: get their formulas right FIRST!)
barium hydrogen carbonate aluminum dihydrogen phosphate chloric acid
8) What’s the difference between sulfur trioxide and the sulfite ion?
9) What’s the difference between carbon monoxide and cobalt?
10) What’s the difference between hafnium metal and hydrofluoric acid?
11) Write out the names and formulas for the oxides of each of the manganese ions. (check the back of your periodic table)
12) Write out the formulas for three binary ionic compounds here. Name them. Do not use any transition metals. Make sure the subscripts are different for each compound.
13) Write out the formulas for the two sulfates of mercury. Name them.
14) Combine the two hexacyanoferrate ions with the three chromium ions. (Six compounds, total). Write out their names and formulas.
15) Go back and make sure you do #86 in your textbook.
16) Be prepared to compare and contrast molecular and ionic compounds.
17) What’s the charge of the sulfur in a sulfate ion? in a sulfite ion?
18) What’s the charge of the nitrogen in a nitrite ion? in an ammonium ion?
19) Name this compound: CaOs(O2)2
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