REVIEW QUESTIONS

Chapter 3
  1. Using only a periodic table, assign charges for each ion below, then complete the table with formulas and names for compounds formed by the combination of each cation and anion.
Ca K 1+ Al 3+ _1+
S_2- CaS
Calcium sulfide Potassium sulfide Aluminum sulfide Ammonium sulfide
Cl_1- KCI
Calcium chloride Potassium chloride Aluminum chloride Ammonium chloride
N_3- AlN
Calcium nitride Potassium nitride Aluminum nitride Ammonium nitride
1-
Calcium nitrite Potassium nitrite Aluminum nitrite Ammonium nitrite
_2-
Calcium sulfate Potassium sulfate Aluminum sulfate Ammonium sulfate
1-
Calcium nitrate Potassium nitrate Aluminum nitrate Ammonium nitrate
_2-
Calcium carbonate Potassium carbonate Aluminum carbonate Ammonium carbonate
_1-
Calcium chlorate Potassium chlorate Aluminum chlorate Ammonium chlorate
OH 1- KOH
Calcium hydroxide Potassium hydroxide Aluminum hydroxide Ammonium hydroxide
_3-
Calcium phosphate Potassium phosphate Aluminum phosphate Ammonium phosphate
  1. Fill in the missing name or formula for each compound listed below. Fill in column 1 without using any notes, and then fill in column 2 with the use of notes.
1 2
Barium nitrate
Ferrous chloride
Silver hydroxide AgOH
Strontium phosphate
Copper(II) acetate
Zinc nitrite
Potassium sulfite
Ammonium carbonate
Iodine heptafluoride
Bromine trifluoride
copper(I) perchlorate
silver sulfate
dinitrogen pentoxide
mercury(I) iodide
lead (IV) oxide
oxygen difluoride
  1. For each compound shown below, determine if the name or formula is incorrect, and write the correct form in the space provided:
    a)
    c)
    d)
    e) PbS
    f)
    g)
    h)
    i)
    j)
    b) MgOH Magnesium hydroxide
Disilver sulfide
Magnesium hydroxide
Galcium (II) nitrate
Tin (II) oxide
Lead sulfide
Zine dichloride
Sodium dioxide
Galcium sulfide
Barium oxide
Copper (II) oxide
Silver sulfide

Calcium nitrate
Tin (IV) oxide
Lead (II) sulfide
Zinc chloride
Sulfur dioxide
Calcium sulfate
BaO
Copper (I) oxide
4. Balance the following equations by providing the missing coefficients:
a)
b)
c)
d)
e)
f)
5. Write a balanced equation for each reaction described below. Include state designations:
a) When an aqueous solution of potassium dichromate is added to and aqueous solution of lead(II) nitrate, solid lead(II) dichromate and aqueous potassium nitrate are formed.
b) When chlorine gas is bubbled though an aqueous solution of potassium bromide, bromine gas and aqueous potassium chloride are formed.
c) When zinc metal is reaction with aqueous nitric acid, the reaction produces nitrogen gas, water and aqueous zinc nitrate.
  1. What mass of chlorine is present in 12.2 g of ?
  1. How many atoms of oxygen are present in 2.15 g of ?
  1. What is the percent composition of caffeine ( ?
  1. Determine the empirical formula for a compound with the following composition:
    62.1% C
    5.21% H
    12.1% N
    20.7% O
(6) (12)
  1. Combustion analysis of a 12.01-g sample of an unknown acid-which contains only carbon, hydrogen and oxygen-produced 14.08 g and . Determine the empirical formula for this acid.
  1. A phosphorous compound that contains phosphorus by mass has the formula . Identify the element X .
Assuming of sample,
  1. A 3.41 -g sample of a hydrate of copper(II) chloride was heated to drive off the water of hydration. The anhydrous salt was found to have a mass of 2.69 g . Determine the formula for this hydrate.
  1. Classify each hydrocarbon below as alkane, alkene or alkyne, and write a molecular formula for each:
a)
c)
alkene ( )
b)
d)
Alkyne ( )
alkene ( )