REVIEW QUESTIONS

Chapter 6
  1. Binary Ionic - Type I
Assign charges for each ion below, and complete the table with formulas and names for compounds formed by the combination of each cation and anion.
Ca K 1+ Al 3+ Zn 2+
S 2- CaS ZnS
calcium sulfide potassium sulfide aluminum sulfide zinc sulfide
Cl 1- KCI
calcium chloride potassium chloride aluminum chloride zinc chloride
N 3- AIN
calcium nitride potassium nitride aluminum nitride zinc nitride
O 2- CaO ZnO
calcium oxide potassium oxide aluminum oxide zinc oxide
  1. Binary Ionic - Type II
Based on the charges given for each cation, complete the table with formulas and names (Stock and Classical) for compounds formed by the combination of each cation and anion.
Fe Cu 1+ Fe_3+ Sn_4+
I 1- CuI
iron (II) iodide copper (I) iodide iron (III) iodide tin (IV) iodide
ferrous iodide cuprous iodide ferric iodide stannic iodide
P_ 3- FeP
iron (II) phosphide copper (I) phosphide iron (III) phosphide tin (IV) phosphide
ferrous phosphide cuprous phosphide ferric phosphide stannic phosphide
O_2- FeO
iron (II) oxide copper (I) oxide iron (III) oxide tin (IV) oxide
ferrous oxide cuprous oxide ferric oxide stannic oxide
  1. Polyatomic
Assign charges for each ion below, and complete the table with formulas and names for compounds formed by the combination of each cation and anion.
Ba 2+ Al 3+ Pb 4+
_2-
barium sulfate aluminum sulfate ammonium sulfate lead (IV) sulfate
1-
barium nitrate aluminum nitrate ammonium nitrate lead (IV) nitrate
_2-
barium carbonate aluminum carbonate ammonium carbonate lead (IV) carbonate
3-
barium phosphate aluminum phosphate ammonium phosphate lead (IV) phosphate
  1. Covalent
Complete the table below with missing formulas and names.
iodine heptafluoride
bromine trifluoride
dinitrogen pentoxide
oxygen difluoride
disulfur hexachloride
sulfur tetrafluoride
  1. Complete the following table with the missing information:
Ion Number of Protons Number of Electrons Electrons Lost/Gained
19 18 1 Lost
12 10 2 lost
8 10 2 gained
Al 13 10 3 lost
  1. Classify each of the following bonds as ionic, polar covalent or non-polar covalent:
    a)
    ionic
    ( )
    b)
    ionic
    ( )
    c) ◯
  2. Arrange the following bonds in order of increasing polarity:

<
Br-Cl < < Li-F most polar
8. Draw Lewis structures and use VSEPR to predict the shape and bond angles and polarity for each of the following molecules or ions:
a)
OHSiOHOHOH
Shape: trigonal pyramidal
Bond angle:
Polarity (Y/N): Yes
b)
Shape: bent
Bond angle:
Polarity (Y/N): Yes
c)
O+HClGe
Shape: trigonal planar
Bond angle:
Polarity (Y/N): Yes
(non-symmetrical)
d)
NHN15
Shape: linear
Bond angle:
Polarity (Y/N): No
9. Write the formula for the ionic compound formed from the combination of the elements indicated by the following electron-dot symbols:
a) .
b) . XY
c)
10. Complete each of the following statements with a suitable word or phrase:
a) Polarity of a bond is caused by difference in electronegativity
b) Linear molecules with polar bonds are usually non-polar
c) Molecules with 3 bonding pairs and 1 non-bonding pair of electrons around the central atom have a pyramidal shape.
d) Bonds that have unequal sharing of electrons are classified as polar covalent
e) Molecules with 2 bonding pairs and 2 non-bonding pair of electrons around the central atom have a bent shape.