I.
Bonding, Chemical Names & Formulas
1. Define the following types of bonding:
a. Ionic bond ____________________________________________________________________
b. Covalent bond ____________________________________________________________________
c. Polar covalent ____________________________________________________________________
d. Nonpolar covalent ____________________________________________________________________
e. Metallic bond - _____________________________________________________________
2. Write the chemical formulas for the following compounds and circle if they are ionic (I), covalent
(C), acid (A) or base (B):
a. Phosphorous tetroxide
I, C, A, B
__________________________
b. magnesium fluoride
I, C, A, B
__________________________
c. ammonium sulfide
I, C, A, B
__________________________
d. nitrous acid
I, C, A, B
__________________________
e. carbon monochloride
I, C, A, B
__________________________
f. hydrocyanic acid
I, C, A, B
__________________________
g. beryllium chlorite
I, C, A, B
__________________________
h. calcium sulfate
I, C, A, B
__________________________
i. phosphoric acid
I, C, A, B
__________________________
j. aluminum carbonate
I, C, A, B
__________________________
k. potassium hydroxide
I, C, A, B
__________________________
3. Write the names for the following compounds and circle if they are ionic (I), covalent (C), acid (A)
or base (B):
a. Na3P
I, C, A, B
___________________________________________
b. HIO3
I, C, A, B
__________________________________________________________________
c. NaOH
I, C, A, B
____________________________________________
d. SiF2
I, C, A, B
____________________________________________
e. MnOH
I, C, A, B
____________________________________________________________________
f. MgO
I, C, A, B
____________________________________________
g. (NH4)2SO3
I, C, A, B
____________________________________________
h. TiS2
I, C, A, B
_________________________________________________________________
i. N2O7
I, C, A, B
____________________________________________
j. HC2H3O2
I, C, A, B
____________________________________________
4. What is the percent composition of oxygen in Cr2(C2O3)3 ?
5. What is the percent of water in Ba(OH)2 * 8 H2O (barium hydroxide octahydrate)
6. What is the empirical formula for a compound that is 52% carbon, 13% oxygen, and 35%
hydrogen?
Use this Electronegativity table for the following problems:
H
2.1
Li
1.0
Na
0.9
K
0.8
Be
B
1.5
2.0
Mg
Al
1.2
1.5
Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga
1.0 1.3 1.5 1.6 1.6 1.5 1.8 1.9 1.9 1.9 1.6 1.6
C
2.5
Si
1.8
Ge
1.8
N
3.0
P
2.1
As
2.0
O
3.5
S
2.5
Se
2.4
F
4.0
Cl
3.0
Br
2.8
7. Classify the following bonds as nonpolar covalent, polar covalent, or ionic based on the EN
difference.
a) Mg-F ____________________________
b) C-N _____________________________
c) Si-S _____________________________
Overall, nonpolar covalent bonds have a
very ______________ difference in EN,
polar covalent bonds have a
___________________________
difference in EN, and ionic bonds have a
very ______________ difference in EN.
d) N-N _____________________________
8. For the following [4 pts each]:
a) draw Lewis structures
b) predict the VSEPR geometry
c) classify molecule as nonpolar or polar
Lewis Structure
ammonia,
NH3
Methane, CH4
VSEPR Geometry
Polar Covalent or
Nonpolar Covalent
PCl3
oxygen, O2
Water
CO2
SF4
9. How does the strength of IMFs between molecules affect properties like boiling and melting
points?
10. List the fours IMFs in order of increasing strength: dipole-dipole, hydrogen bonding, London
dispersion, and ion-dipole.
11. Why does water have such a high boiling point and specific heat capacity when compared to other
polar molecules like H2S or C4H10O?
II.
Reactions
12. For the following reactions:
Write balanced chemical formulas (including states of matter!) for reactions below. Classify each
reactions as either: Redox, synthesis, decomposition, combustion, single replacement, double
replacement, or acid/base.
a) Magnesium metal combines with chlorine. _____________________________________
b) Lithium metal is submerged in a solution of chromium (II) nitrate. ________________________
d) Sulfuric acid is added to potassium hydroxide. ______________________________________
e) Iron (II) carbonate decomposes into a solid metal oxide and carbon dioxide gas. ____________
e) Solutions of ammonium iodide and lead (II) acetate combine. __________________________
III.
Stoichiometry
13. How many atoms of iron are there in 3.59 moles of Fe3(PO4)2 ?
14. How many moles of nitrate ions would be present in an aqueous solution made from 17.44 g of
Be(NO3)2?
15. Consider the combustion of 33.5 g of ethane with 128 g oxygen.
a) Write the balanced chemical reaction.
b) What is the maximum mass of carbon dioxide that could be produced?
c) State the limiting and excess reactants in the reaction.
d) How much excess reactant would be left over after the reaction is complete?
e) If only 91.7 grams of carbon dioxide were collected in the laboratory, what is the % yield of this
reaction?
16. Circle which of the following would be considered strong electrolytes. If it is a strong electrolyte,
state the how many of each type of ion that would be present.
LiCl (aq)
LiCl (s)
Ca(OH)2 (aq)
Al2(SO4)3 (aq)
(NH4)2S (aq)
PbI2 (s)
Ba(OH)2 (s)
HC2H3O2 (aq)
HCl (aq)
12. Write the balanced molecular and net ionic equations for the following reactions:
a)
Solutions of magnesium chloride and lead (II) acetate are mixed.
b)
Potassium metal is submerged in phosphoric acid.
c)
Solutions of silver nitrate and sodium carbonate are mixed.