BENCHMARK REVIEW
1. Molarity problems. M = mol/L
a. How many liters are in a solution that has a molarity of 0.50 M
and contains 68 g of HCl?
b. How many grams are needed to make a 750 mL solution of
5.6 M H2SO4?
2. Write the general formulas for the following reaction types:
a. Synthesis
b. Decomposition
c. Single replacement
d. Double replacement
e. Combustion
f. Neutralization
3. Write box diagrams (hint: electron configuration) for the
following elements:
a. Si
b. P
c. S
d. Cl
4. Discuss how you applied Hund’s rule and the Pauli Exclusion
Principle in #3.
5. Be able to read a graph!
6. Be able to balance equations! (Several questions)
7. Using the following equation (NaCl + H2O  NaOH + HCl),
if you begin with 10 g of NaCl and 10 g of water and you produce
7 g of HCl…how many grams of NaOH should you produce?
8. Identify element X in the Lewis dot structure.
9. Compare and contrast precision and accuracy.
10.
Name the following molecules:
a. SiCl4
b. MgCl2
11.
1 mole of gas = 22.4 L
a. How many liters (or what is the volume) of 23.0 g of helium at
STP?
12.
What happened when an atom takes a positive or negative
charge?
13.
Define heat of fusion and heat of vaporization.
14.
What is the formula for:
a. Phosphorus pentabromide
b. Zinc fluoride
15.
Define chromatography.
16.
A sample of gas occupies 5 L at 30oC and 101.3 kPa. What
would be the volume at 10oC and 202.6 kPa?
17.
What is the Lewis dot structure for silicon?
18.
If the empirical formulas for a substance is CH and the
molecular mass is 78 g/mol…what is the molecular formula?
19.
Define equilibrium.
20.
How many grams of chlorine are present in 3 moles of
hydrochloric acid?
21.
Explain the relationship between gas temperature and
volume…Charles’ law.
22.
Moles to atoms conversions
a. Convert 2 moles of carbon atoms to moles.
b. Convert 3.6 x 1024 atoms of magnesium to moles.
23.
What are the diatomic elements?
24.
What is the molar mass of
a. MgCl2
b. (NH4)2SO4
25.
What is the shape of CO, CO2, BCl3, CH4, NH3?
26.
Specific heat calculations (q = cmT)…look in you notes for
last unit!
27.
Subatomic particles for different elements (protons,
neutrons and electrons).
28.
Difference between natural and synthetic polymers.
29.
pH + pOH = 14
a. If a substance has a pH of 6…what is its pOH?
30.
Be able to read a solubility curve (from your solutions notes
– before Spring Break)
31.
Discuss the differences between Thompson, Rutherford,
Bohr and Quantum atomic theory.
32.
Know the families on the periodic table.
33.
Know the following trends
a. Atomic radius (size)
b. Electronegativity
c. Ionization energy
34.
MV = MV
a. If you have 30 mL a 2.0 M H2SO4 solution…how many
milliliters of 0.5 M H2SO4 can you make?
35.
Convert the following gases at STP to liters (volume)
a. 6 g Ne
b. 4 moles He
c. 1.2 x 1023 molecules of CO
36.
Discuss the difference between ionic and covalent bonding.