Chemistry
Semester Review
Name:
Use dimensional analysis (the factor-label method) to solve the following problem:
1. If you drove a distance of 34.9 miles, how many kilometers would that be? 1 ft = 30.48 cm
Use the formula for density to solve the following problems:
2. If a substance has a mass of 55.78 grams and a volume of 7.9 mL, what is the density of this
substance?
3. If you had a 32 gram sample of gold, (Density = 19.3 g/mL) how much space would it
occupy?
Complete the following calculations using correct sig fig rules:
4. 40.7 ml + 3.09 ml + 23.57 ml
5. 0.048 g + 7.08 g + 0.395 g
___________________
___________________
State the number of significant figures in each of the following measurements.
6. 28009 m ________________
7. 0.00450 kg ______________
8. 2.0570 s ________________
9. 850 g __________________
Perform the following multiplication and division and express your answer to the correct number
of significant figures. Include units.
10. 235 cm x 2.3 cm
______________________
11. 2.587 g x 1.90 g
______________________
12. Complete the following table:
Element
Symbol
Atomic
number
Mass
number
Atomic
Mass
p+
n
e-
Antimony
Sn
88
13. Element X has two isotopes. The first isotope has a mass of 63.001 amu and has a percent
abundance of 69.1 %. The second isotope has a mass of 65.000 amu and has a percent
abundance of 30.9 %. Calculate the average atomic mass of this element and determine the
identity of the element.
14. Write the symbols for alpha, beta, and gamma particles. Be sure to include numbers.
15. Complete the following nuclear equations:
Uranium-238 undergoes alpha decay
Silicon 27 undergoes beta decay
16. What is the maximum number of electrons that could be placed in each of the following?
An s subshell: ____________________
A p subshell: ___________________
A d orbital: ___________________
The second energy level: __________________
17. Complete the orbital notation, full electron configuration, and noble gas configuration for the
element Barium:
18. Explain why a neon lamp emits light.
19. How many moles are there in 6.35 x 1024 particles of CH4?
20. How many particles are there in 17 moles of Sulfur?
21. Find the mass (in grams) of 3.71 moles of Al2O3.
22. How many liters are there in 3.9 moles of CO2 at STP?
23. An 8.20 gram piece of Magnesium combines with 5.40 grams of oxygen to form a
compound. What is the percent composition of this compound?
24. What is the percent of each element in the compound Ca(NO3)2?
25. A.) Calculate the empirical formula of each compound with the following percent
composition:
79.8 % C
20.2 % H
B.) If the molar mass of this compound is 45.104 g/mol, what is the molecular formula?
26. What is the molecular formula of the molecule that has an empirical formula of CH2O and a
molar mass of 120.12 grams/mol?
27. Using the activity series, predict whether each of the possible reactions listed below will
occur. For the reactions that will occur, write the products. Then balance. If no reaction occurs,
write NR.
a.
b.
Ag (s)
Li (s)
+
FeCl2 (aq) ---------->
+
Cu(NO3)2 (aq) --------->
28. List 4 signs that a reaction has occurred:
29. Sodium solid and chlorine gas combine in an irreversible reaction to form solid sodium
chloride.
a.) Write a balanced chemical equation for this reaction. (include all proper symbols)
b.) What type of reaction is this?
30. Classify the following reactions by type: (they may not be balanced, that's ok)
CH4 (g) +
O2 (g) ------> CO2 (g) + H2O (l)
NaCl (aq)
+ AgNO3 (aq) -----> AgCl
(s) + NaNO3 (aq)
H2O (l) ------> H2 (g) + O2 (g)
31. Consider the following reaction:
2 C2H6
+
7 O2

4 CO2
+
6 H2O
a. How many grams of oxygen are needed to react with 47.8 grams of ethane (C2H6)?
b. How many Liters of carbon dioxide will be produced when 45.0 grams of ethane are burned?
c. How many particles of oxygen are needed in order to produce 50.6 grams of water?
d. If this reaction produces 75.0 grams of carbon dioxide, how many grams of water will be
produced?
32. You mix 6.88 grams sodium fluoride with 13.2 grams sulfuric acid.
a. Find the LR and the theoretical yield of HF.
2
NaF
+
H2SO4
--------->
2 HF
+ Na2SO4
b. If 2.87 grams of HF is actually produced, what is the percent yield for this reaction?
33. Complete the following:
Name
Formula
Type of compound
(ionic, molecular or acid)
Barium Bromide
__________________
_____________________
____________________
NH4NO2
_____________________
Oxalic Acid
__________________
_____________________
____________________
P2O5
_____________________
Carbon Tetrafluoride
__________________
_____________________
____________________
H3PO4
_____________________
Sodium Nitride
__________________
_____________________
____________________
F2
_____________________
Aluminum Borate
__________________
_____________________
___________________
H2Cr2O7
_____________________
Nitrogen
__________________
_____________________
___________________
P4O7
_____________________
Sulfurous Acid
__________________
_____________________
Aluminum Acetate
__________________
_____________________
___________________
HBr
_____________________
Ammonium Phosphide
__________________
_____________________
34. Decide whether the following compounds would be more likely to contain ionic or covalent
bonds:
KBr
CCl4
H2O
PbI2
SO3
35. Draw the Lewis Dot Structure and Structural formulas for the following compounds:
H2O
NH3
N2
SiI4
36. What is the shape of each compound above?
37. What is the trend for atomic size across a period and down a group?
38. Which element is the most electronegative? The least?
39. A standardized solution of 0.075 M HCl is titrated with a saturated solution of calcium hydroxide to
determine its molarity. It takes 35.0 mL of base to neutralize 10.0 mL of the acid.
a. Write the balanced equation for this neutralization reaction.
b. What is the molarity of the base?
40. What is the molarity of a solution prepared from 0.583 moles of LiCl to make a solution of
650 mL?
41. What is the molarity of a solution that is prepared from 50.0 g of KCl and has a solution
volume of 450 mL?
42. If a sample of nitrogen gas occupies a volume of 1.7 L at a temperature of 30C and a
pressure of 740 mm Hg, how many grams of nitrogen are present?
43. How many calories would be required to change 35.0 grams of ice at -45C to liquid water
at 57C?
Smile! You’re finally done! 