S332 Chemistry
09-10 First Semester Review
Name: _________________________
This packet is optional, however, it will really help you review the concepts that
will be on the final exam.
12 inches = 1 foot
3 feet = 1 yard
16.5 feet = 1 rod
5280 feet = 1 mile
40 rods = 1 furlong
6 feet = 1 fathom
1 gallon = 231 inch3 ö
16 ounces = 1 pint
2 pints = 1 quart
4 quarts = 1 gallon
English to metric conversion:
1 kilometer = 1000 meters
1 hectometer = 100 meters
1 decameter = 10 meters
10 decimeters = 1 meter
100 centimeters = 1 meter
1000 millimeters = 1 meter
1 milliliter = 1 centimeter3
1000 milliliters = 1 liter
2.54 centimeters = 1 inch ö
*For the most part, the equivalencies in this table are exact and therefore will not affect the number of significant figures in the answer to the
problems in this chapter. The exceptions are marked with an ö.
1.
Convert each of the following quantities into the required unit.
a. 12.75 mm to ? kilometers
b. 277 cm to ? meters
c. 81.9 cm2 to ? square meters
d. 10.74 cm3 to ? liters
e. 7.48 m2 to ? square inches
f. 3.72 L/hour to ? cubic centimeters per minute
g. 6.12 km/day to ? meter per second
2.
A textbook measures 250. mm long, 224 mm wide, and 50.0 mm thick. It has a mass of 2.94 kg.
a. What is the volume of the book?
b. What is the density of the book in grams per cubic centimeter?
3.
A gas has a density of 5.56 g/L.
a. What is the volume in milliliters if you have 4.17 grams of the gas in a container?
b. What would be the mass in kilograms if you have 1.00 m3 of the gas in a container?
4.
How many significant figures are represented in each of the following numbers?
a. 640 cm2
f. 20.900 cm
b. 200.0 mL
g. 0.04002 kg/m2
c. 0.5200 g
h. 665 ft
d. 10.005 kg
i. 12.5 in
e. 10,000 L
5.
Calculate the following problems and give the answers rounded to the correct number of significant
figures.
a. 47.0 m ÷ 2.2 s
b. 140 cm × 35 cm
c. 5.88 kg ÷ 200 m3
d. 0.0050 m2 × 0.042 m
6.
Calculate the following problems and give the answers rounded to the correct number of significant
figures.
a. 22.0 m + 5.28 m + 15.5 m
b. 0.042 kg + 1.229 kg + 0.502 kg
c. 170 cm2 + 3.5 cm2 – 28 cm2
d. 3200 mg +325 mg -688 mg
7.
Carry out the following calculations and give the answer in scientific notation, while also using proper
significant figures.
a. 7.20 × 103 cm × 8.080 × 103 cm
b. 3.7 × 104 mm × 6.60 × 104 mm × 9.890 × 103 mm
c. 2.290 × 107 cm ÷ 4.33 × 103 cm
d. 4.73 × 10-4 g ÷ (2.08 × 10-3 km × 5.60 × 10-4 km)
8.
Express the following numbers in scientific notation.
a. 11,200,000 km
b. 3,578.020 hours
9.
Convert the following numbers into standard notation.
a. 8.50 × 105 days
b. 9.640 × 10-8 miles
10. Calculate the percent of the requested element in each given compound.
a. aluminum in Al2O3
b. silver in AgCN
c. selenium in Na2SeO3
11. When a piece of potassium metal is placed in water, a violent reaction occurs. When a piece of copper is
placed in water, however, nothing happens. Is this a physical or chemical property of the metals?
12. Give five examples of evidence that a chemical change occurred.
13. Identify each of the following as an element, compound, or mixture. If it is a mixture, classify it as
homogeneous or heterogeneous.
a. CH4
b. S8
c. coffee (with sugar and cream)
d. bottled water
e. salt water
f. CH2O
14. What are the five principles of Dalton’s atomic theory?
15. What type of electrical charge does an electron carry?
16. How did the results of the gold foil experiment lead Rutherford to recognize the existence of atomic
nuclei?
17. The fact that the large majority of alpha particles passed undeflected through the gold foil indicates what
about atoms?
18. What does the atomic number represent?
19. What three subatomic particles are important in chemistry? What is the electric charge of each?
20. One particular atom of calcium can be represented as
does this atom have?
44
20
Ca . How many of each type of subatomic particle
21. Describe the major differences between electrons, protons, and neutrons in terms of size, charge and
location.
22. How does Bohr’s model of the atom differ from Rutherford’s?
23. How does an electron go from ground state to excited state? What happens when the electron returns to
ground state from excited state?
24. Explain why the following electron configurations or orbital diagrams are incorrect.
1s22s32p63s1
Explain the error in each and draw a correct diagram.
a.
Oxygen
b. Calcium
2p
2p
3d
2p
3p
2s
3s
1s
2p
2s
1s
2p
2p
3p
3p
3d
3d
3d
3d
25. Give the long form AND short form electron configuration for Ni.
26. Write the electron configuration and draw the orbital diagram for Al.
27. The element chlorine has an electron configuration of 1s22s22p63s23p5.
a. What does the superscript 5 refer to?
b. What does the letter s refer to?
c. What does the number 3 refer to?
28. Identify the following elements.
a. 1s22s22p2
b. 1s22s22p63s23p1
c. 1s22s22p63s23p64s23d104p65s24d9
d. [Xe]6s25d14f13
29. Define the Aufbau principle, Hund’s Rule and the Pauli exclusion principle.
30. In the fifth period, which elements are metals, metalloids, and nonmetals?
31. Who arranged the first periodic table? How did he arrange it?
32. Where are the alkali metals? alkaline earth metals? Halogens? Noble gases?
33. What led Mendeleev to predict that some elements had not yet been discovered?
34. Often, gold is described in jewelry as being 14 Karat or 24 K gold. This is an alloy of gold. What is an
alloy?
35. What is ionization energy?
36. What periodic trends exist for ionization energy?
37. What trends are evident in atomic size (radius) as you proceed down a group of elements? How does the
trend progress as you move from left to right on the periodic table, within a period of elements?
38. Going from left to right, across a period of elements, what effect does electron shielding have on atomic
size? on ionization energy?
39. When an atom loses an electron, what happens to its charge?
40. When an atom gains two electrons, what happens to its charge?
41. What property do the noble gases share? How does this property relate to the electron configurations of
the noble gases?
42. What families make up the Main Group elements?
43. Why would you never expect Ca+1 or Na+2 ions to exist?
44. Define cation. Define anion.
Use the following diagrams to answer the next five questions.
A
B
C
D
45. Please choose the container that could represent the oxygen we breathe, O2.
46. Which container could represent our exhaled carbon dioxide, CO2?
47. Helium, now used in balloons, is an atomic substance, while H2 (Hydrogen) was used previously to fill
balloons. Which container could have both of these substances?
48. Which container(s) represent pure substances? (There may be more than one answer.)
49. Which container(s) has a mixture of elements? (There may be more than one answer.)
50. How would each of the following atoms react to achieve the octet rule?
a. iodine
b. sulfur
c. barium
d. krypton
51. Write formulas for the following binary ionic compounds.
a. calcium chloride
g. copper (I) bromide
b. magnesium oxide
h. aluminum selenide
c. sodium iodide
i. iron (II) oxide
d. magnesium fluoride
j. iron (III) oxide
e. calcium sulfide
k. niobium (V) chloride
f. potassium nitride
52. Name the following binary ionic compounds. If the metal can form more than one cation, be sure to
identify the charge.
a. Rb2O
b. BaCl2
c. FeF3
d. CrCl3
e. Na2O
f. Mg3P2
53. In terms of electron configurations and Bohr diagrams, explain why potassium bromide has the formula
KBr instead of K2Br or KBr2.
54. Name the following compounds.
a. NaClO3
b. K2SO3
c. (NH4)2CrO4
d. Al2(SO4)3
55. Write formulas for the following compounds.
a. mercury (II) sulfate
b. calcium cyanide
c. potassium chromate
d. lithium thiosulfate
56. Name the following covalent compounds.
a. CO
b. NO2
c. SO3
d. P2O5
57. Write the formulas for the following covalent compounds.
a. dinitrogen tetroxide
b. sulfur dioxide
c. phosphorous pentachloride
58. Complete the following chart:
Element / Ion
4
2
7
3
He
Li
12
6
+1
C
80
35
Br
-1
35
17
Cl
-1
40
20
24
12
Ca
Mg
31
15
P
197
79
197
79
32
16
+2
-3
Au
Au
S
+1
-2
Atomic
Number
Atomic Mass
Mass Number
# of Protons
# of Neutrons
# of Electrons
59. Define…
a. Independent Variable
b. Pie Graph
c. Units
d. Title
e. Ordered Pair
f. Dependent Variable
g. Indirect relationship
h. Extrapolation
i. Direct relationship
j. Bar Graph
k. Interpolation
l. EXPLAIN the difference between a scatter plot graph and a line graph.
A.
___________ Increment of Accuracy
B.
A.
___________ Increment of Precision
___________ Measurement
________ Number of Sig. Figs. in measurement
B.
___________ Increment of Accuracy
___________ Increment of Precision
___________ Measurement
________ Number of Sig. Figs. in measurement
60. What types of elements combine to make ionic compounds?
61. What types of elements combine to make covalent compounds?
1
20
10