Download Final Exam Review – Free Response Section Name: 1. A sample of

Final Exam Review – Free Response Section
Name: __________________________________
1. A sample of chalk (Calcium carbonate) weighs 1.75 g. Calculate the mass of calcium in the sample of chalk in both grams and ounces (there are 28.35 g in 1 ounce). Calculate how many oxygen
atoms are in the sample of chalk.
2. A sample of saline solution has a concentration of 0.107 ng/µL. What is the concentration in
mg/mL?
3. Draw the Lewis structure for H2O. Indicate its shape, whether it is polar or nonpolar, the type of
intermolecular force that it would exhibit, if that intermolecular force is weak, strong, or very
strong, whether the boiling point would be relatively high or low, and predict if it would tend to be
a liquid or a gas at room temperature.
a. Lewis Structure
b. Shape
c. Polar or Nonpolar __________________
d. Intermolecular force _____________________
e. Weak, strong, very strong intermolecular force _______________________
f. High Boiling Point or Low Boiling Point ________________________
g. Liquid or Gas ______________________
4. a. Indicate the shapes for the following molecules:
NH3 ____________________
SF6 ____________________
PCl5
____________________
CCl3F ____________________
SiS2
____________________
AB3 E ____________________
b. Put NBr3, SiS2, and CCl3F in order by increasing boiling point ____________________
5. Lysine is an essential amino acid with a molecular mass of 146.19 g/mol. Lysine is experimentally
determined to be 19.2% nitrogen, 9.64% hydrogen, 49.3% C, and 21.9% oxygen. Determine the
molecular formula for lysine.
6. 5.00 g of nickelic chlorate is mixed with 5.00 g of sodium phosphate in water.
a. Write the formula equation,
b. the total ionic equation
c.
the net ionic equation.
d.
Identify the product that is a precipitate
e. Identify the limiting reagent
f. Identify the excess reagent
g. calculate how much precipitate can be formed from this reaction.
7. 2.00 L of a gas at 25 oC and 1.05 atm is heated to 30 oC and the pressure is reduced to 0.550 atm.
Calculate the new volume.
8. Write and balance the following equations. Indicate if the reaction does not occur.
a. Magnesium and nitrous acid
_______________________________________________________________
b. C8H18 + O2
_______________________________________________________________
c. Stannic chloride and ammonium hydroxide
_______________________________________________________________
d. MgCO3
_______________________________________________________________
e.
H2O + SO3
_______________________________________________________________
f. sulfurous acid and potassium hydroxide
_______________________________________________________________
g. Silver and lithium chloride
_______________________________________________________________
h. Calcium and cobalt (II) chlorate
_______________________________________________________________
i. Cupric fluoride and sodium carbonate
_______________________________________________________________
Activity Series of the Elements
Activity of Metals
Li
Rb
Can react with
K
cold water and
Ba
acids, replacing
Sr
hydrogen
Ca
Na
Mg
Al
Can react with
Mn
acids or steam,
Zn
but not usually
liquid water, to
Cr
replace hydrogen
Fe
Cd
Co
Can react with
Ni
acids but not
water, to replace
Sn
hydrogen
Pb
H2
React with
Sb
oxygen, forming
Bi
oxides
Cu
Hg
Fairly unreactive.
Ag
Form oxides only
Pt
indirectly
Au
Activity of Halogen Nonmetals
F2
Cl2
Br2
I2
Name: _______________________________________________
Write and balance the equations provided.
If it is a single displacement reaction, use the activity series to
determine if it will occur. If it will not occur, write “no reaction.”
If it is a double displacement, use the solubility rules to determine
if it will occur. If it will not occur, write “no reaction.” If it will
occur, write the balanced chemical equation, the total ionic
equation, and the net ionic equation.
Solubility rules:
1. All common compounds of Group I and ammonium ions are
soluble.
2. All nitrates, acetates, and chlorates are soluble.
3. All binary compounds of the halogens (other than F) with
metals are soluble, except those of Ag, Hg(I), and Pb. Pb halides
are soluble in hot water.)
4. All sulfates are soluble, except those of barium, strontium,
calcium, lead, silver, and mercury (I). The latter three are slightly
soluble.
5. Except for rule 1, carbonates, hydroxides, oxides, silicates,
and phosphates are insoluble.
6. Sulfides are insoluble except for calcium, barium, strontium,
magnesium, sodium, potassium, and ammonium.