Chem 11 Review – Chapters 1, 2, 3, 4
Name: _______________________________________
1. The branch of chemistry that studies chemicals containing carbon is _____________ chemistry.
a) Physical
b) inorganic
c) analytical
d) organic
2. An analytical chemist is most likely to
a) Explain why paint is stirred before it is used
b) Explain what keeps paint attached to the steel frame of an automobile
c) Identify the type of paint chips found at the scene of a hit and run accident
d) Investigate the effect of leaded paint on the development of a young child
3. Chemists who work in the biotechnology field are most likely to work with :
a) X-ray technicians
b) geologists
c) physicians
d) physicists
4. Describe the difference between an extensive property and an intensive property and give an example of each.
5. Classify each of the following as homogeneous or heterogeneous mixtures.
a) Chocolate chip ice cream
b) green ink
c) cake batter
d) cooking oil
6. Fingernail polish remover (mostly acetone) is a liquid at room temperature. Would you describe acetone in the gaseous
state as a vapor or a gas? Explain your answer.
7. What is the goal of a distillation? Describe briefly how this goal is accomplished.
8. How could you distinguish an element from a compound?
9. Classify each of the following as a physical or chemical change. For any chemical change, list at least one clue to
support your answer.
a) A copper wire is bent
b) charcoal burns in a grill
c) Bread dough rises when yeast is added d) sugar dissolves in water
10.) Use the arrangement of particles in solids and gases to explain why solids are not as easy to compress as gases.
11.) Identify each of the following items as a mixture or compound. Classify the mixtures as homogeneous or heterogeneous
a) raw egg
b) ice
c) gasoline
d) blood
12.) Classify the following properties of the element silicon as chemical or physical properties.
a) blue-gray colour
b) brittle c) doesn’t dissolve in water
d) melts at 14100C e) reacts vigorously with fluorine
13.) The wax appears to disappear as a candle burns. How can the law of conservation of mass apply to this reaction?
14.) Which of the following is not a chemical change?
a) paper being shredded b) steel rusting
c) charcoal
d) a newspaper yellowing in the sun
15.) Which phrase best describes an apple?
a) heterogeneous
b) homogeneous compound
c) heterogeneous substance
d) homogeneous mixture
16.) The state of matter characterized by a definite volume and an indefinite shape is a:
a) solid
b) liquid
c) mixture
d) gas
17.) Which list contains elements that fall within the same group on the periodic table?
a) He, Ar, Xe
b) O, F, Ne
c) K, Rb, Ba
d) H, He, Li
18.) Which answer represents the measurement 0.00428 g rounded to two significant figures?
a) 4.28 x 103 g
b) 4.3 x 10-3 g
c) 4.3 x 103 g
d) 4.0 x 10-3 g
19.) An over the counter medicine has 325 mg of its active ingredient per tablet. How many grams does this mass represent?
a) 325 000 g
b) 32.5 g
c) 3.25 g
d) 0.325 g
20.) An atom composed of 16 protons, 16 electrons, and 16 neutrons is:
21.) Which of these descriptions is incorrect?
a) proton; positive charge, in nucleus, mass of 1 amu
b) electron; negative charge, mass of 0 amu, in nucleus
c) neutron; mass of 1 amu, no charge
22.) Thallium has two isotopes, thallium-203 and thallium-205. Thallium’s atomic number is 81 and its atomic mass is 204.38
amu. Which statement about the thallium isotopes is true?
a) There is more thallium-203 in nature.
b) Atoms of both isotopes have 81 protons.
c) Thallium-205 atoms have fewer neutrons.
d) The most common atom of thallium has a mass of 204.38 amu.
23.) The four isotopes of lead are shown below, each with its percent by mass abundance and the composition of its nucleus.
Using these data, calculate the approximate atomic mass of lead.
24.) Review each of the scientists associated with the “atomic theory” . . . who are they and, what did each accomplish?
25.) Do all questions at the end of Sections 4.1, 4.2 and 4.3.
Practice Worksheet for Significant Figures
1. State the number of significant digits in each measurement.
1)
5)
2804 m
4.6 x 105 m
10)
75.00 m
2)
2.84 km
6)
3)
4.06 x 10-5 m
7)
5.029 m
750 m
11) 75,000.0 m
4)
0.003068 m
8) 75 m
9)
75,000 m
12) 10 cm
2. Round the following numbers as indicated:
To four figures:
3.682417
21.860051
To one decimal place:
1.3511
2.473
375.6523
112.511
45.4673
5.687524
7.555
8.235
0.03062
3.4125
41.86632
To two decimal places:
22.494
79.2588
3. Solve the following problems and report answers with appropriate number of significant digits.
1) 6.201 cm + 7.4 cm + 0.68 cm +12.0 cm =
2) 1.6 km + 1.62 m +1200 cm =
3) 8.264 g - 7.8 g =
4) 10.4168 m - 6.0 m =
5) 12.00 m+15.001 kg=
6) 1.31 cm x 2.3 cm =
7) 5.7621 m x 6.201 m =
8) 20.2 cm / 7.41 s =
9) 40.002 g / 13.000005 g =
4. Express the following numbers in their equivalent standard notational form:
1)
123,876.3 2) 1,236,840 3) 422000
4) 0.000000000000211
5) 0.000238
6) 0.0000205
5. Identify the sums or differences of the following:
1)
(8.41 X 104) + (9.71 X 104) = 2)
(5.11 X 102) - (4.2 X 102) =
3)
(8.2 X 103) + (4.0 X 103) = 4)
(6.3 X 10-2) - (2.1 X 10-2) =
6. Express the product and the quotients of the following:
1)
(3.56 X 105) (4.21 X 106) = 2)
(2 X 107) (8 X 10-9) =
4)
8.45 X 107 / 6.74 X 103 = 5)
9.7 X 108 / 8.6 X 10-2 =
3) (4.11 X 10-6) (7.51 X 10-4) =
6) 4.7 X 10-2 / 5.7 X 10-6 =
Answers
1. The branch of chemistry that studies chemicals containing carbon is _____________ chemistry.
b) Physical
b) inorganic
c) analytical
d) organic
2. An analytical chemist is most likely to
a) Explain why paint is stirred before it is used
b) Explain what keeps paint attached to the steel frame of an automobile
c) Identify the type of paint chips found at the scene of a hit and run accident
d) Investigate the effect of leaded paint on the development of a young child
3. Chemists who work in the biotechnology field are most likely to work with :
b) X-ray technicians
b) geologists
c) physicians
d) physicists
4. Describe the difference between an extensive property and an intensive property and give an example of each.
An extensive property depends on the amount of matter; an intensive property depends on the type of matter. Mass and
volume are extensive and color and hardness are intensive.
5. Classify each of the following as homogeneous or heterogeneous mixtures.
b) Chocolate chip ice cream
b) green ink
c) cake batter
d) cooking oil
a) heterogeneous
b) homogeneous
c) depends on how well the cake batter is mixed, I would
say heterogeneous because you can usually see air bubbles
d) homogeneous
6.
7.
8.
Fingernail polish remover (mostly acetone) is a liquid at room temperature. Would you describe acetone in the gaseous
state as a vapor or a gas? Explain your answer.
A vapor, the term vapor is used to refer to the gaseous state of a substance which is normally a liquid or a solid at room
temperature.
What is the goal of a distillation? Describe briefly how this goal is accomplished.
The goal is to separate the components of a solution. The solution is boiled to produce a vapor, which is condensed to a
liquid. Dissolved solids are left behind.
How could you distinguish an element from a compound?
Compounds can be separated by chemical means into simpler substances, elements cannot.
9.
Classify each of the following as a physical or chemical change. For any chemical change, list at least one clue to
support your answer.
b) A copper wire is bent
b) charcoal burns in a grill
c) Bread dough rises when yeast is added d) sugar dissolves in water
a) physical
b) chemical (color)
c)chemical (gas produced)
d) physical
10.) Use the arrangement of particles in solids and gases to explain why solids are not as easy to compress as gases.
The particles in s solid are packed tightly together. The particles in a gas are spaced relatively far apart.
11.) Identify each of the following items as a mixture or compound. Classify the mixtures as homogeneous or heterogeneous. a)
raw egg
b) ice
c) gasoline
d) blood
heterogeneous
compound
homogeneous
heterogeneous
12.) Classify the following properties of the element silicon as chemical or physical properties.
a) blue-gray colour
b) brittle c) doesn’t dissolve in water
d) melts at 14100C e) reacts vigorously with fluorine
physical
physical
physical
physical
chemical
13.) The wax appears to disappear as a candle burns. How can the law of conservation of mass apply to this reaction?
The wax appears to disappear because the products of the reaction – carbon dioxide and water vapour – are colourless gases.
14.) Which of the following is not a chemical change?
a) paper being shredded b) steel rusting
c) charcoal
15.) Which phrase best describes an apple?
a) heterogeneous b) homogeneous compound
d) a newspaper yellowing in the sun
c) heterogeneous substance
d) homogeneous mixture
16.) The state of matter characterized by a definite volume and an indefinite shape is a:
a) solid
b) liquid
c) mixture
d) gas
17.) Which list contains elements that fall within the same group on the periodic table?
a) He, Ar, Xe
b) O, F, Ne
c) K, Rb, Ba
d) H, He, Li
18.) Which answer represents the measurement 0.00428 g rounded to two significant figures?
a) 4.28 x 103 g
b) 4.3 x 10-3 g
c) 4.3 x 103 g
d) 4.0 x 10-3 g
19.) An over the counter medicine has 325 mg of its active ingredient per tablet. How many grams does this mass represent?
a) 325 000 g
b) 32.5 g
c) 3.25 g
d) 0.325 g
20.) An atom composed of 16 protons, 16 electrons, and 16 neutrons is: “c”
21.) Which of these descriptions is incorrect?
a) proton; positive charge, in nucleus, mass of 1 amu
b) electron; negative charge, mass of 0 amu, in nucleus
c) neutron; mass of 1 amu, no charge
22.) Thallium has two isotopes, thallium-203 and thallium-205. Thallium’s atomic number is 81 and its atomic mass is 204.38
amu. Which statement about the thallium isotopes is true?
a) There is more thallium-203 in nature.
b) Atoms of both isotopes have 81 protons.
c) Thallium-205 atoms have fewer neutrons.
d) The most common atom of thallium has a mass of 204.38 amu.
23.) The four isotopes of lead are shown below, each with its percent by mass abundance and the composition of its nucleus.
Using these data, calculate the approximate atomic mass of lead.
(82 + 122) x 0.014 = 2.9
(82 + 124) x 0.241 = 49.6
(82 + 125) x 0.221 = 45.7
(82 + 126) x .524 = 108
206 amu
24.)








Democritus all matter made up of tiny particles but not believed as Socrates didn’t believe and
therefore 4 element theory “stuck”
Millikan - charge and mass of electron
John Dalton (1808) proposed the Atomic Theory. According to Dalton, matter is made up of tiny particles
called atoms. The atom is the smallest particle of matter that takes part in a chemical reaction.
Atoms are indivisible and cannot be created or destroyed. Further, atoms of the same element are
identical in every respect.
J. J. Thomson (1897) discovered electrons in Cathode Ray experiments. According to Thomson, atoms
are divisible. Atoms contain very tiny negatively charged particles called electrons.
E. Goldstein (1900) discovered protons in Anode Ray experiments. According to Goldstein, atoms
contain positively charged particles called protons. Since atoms contain negatively charged
particles, they must contain positively charged particles for them to be electrically neutral.
E. Rutherford (1911) discovered the nucleus and provided the basis for the modern atomic structure
through his alpha particle scattering experiment. According to Rutherford, the atoms is made of two
parts: the nucleus and the extra-nuclear part. His experiments proved that the atom is largely empty
and has a heavy positively-charged body at the center called the nucleus. The central nucleus is
positively-charged and the negatively-charged electrons revolve around the nucleus.
James Chadwick (1932) disovered neutrons. According to Chadwick, atoms contain neutral particles
called neutrons in their nucleus along with the subatomic particles (i.e., electrons and protons).
N. Bohr (1940) provided the modern concept of the atomic model. According to Bohr, the atom
is made of a central nucleus containing protons (positively-charged) and neutrons (with no charge).
The electrons (negatively-charged) revolve around the nucleus in different imaginary paths called
orbits or shells.
Classify the following properties as extensive (depend on amount of matter present) or intensive.
a) color
intensive
b) volume extensive
c) mass extensive
d) boiling point intensive
25.)
Practice Worksheet for Significant Figures
1. State the number of significant digits in each measurement.
1)
2804 m 4
4)
0.003068 m
7)
750 m
10)
4
2 or 3
75.00 m
4
2)
2.84 km 3
5)
4.6 x 105 m
8) 75 m
2
2
11) 75,000.0 m 6
3)
5.029 m 4
6)
4.06 x 10-5 m
9) 75,000 m
2, 3, 4, or 5
12) 10 cm 1 or 2
2. Round the following numbers as indicated:
To four figures:
3.682417
3.682
21.860051
21.86
375.6523
375.7
112.511
112.5
45.4673
45.47
5.687524
7.555
8.235
To one decimal place:
1.3511
2.473
3
1.4
2.5
5.7
7.6
8.2
To two decimal places:
22.494
79.2588
0.03062
22.50
79.26
0.03
3.4125
41.86632
3.41
41.87
3. Solve the following problems and report answers with appropriate number of significant digits.
1)
6.201 cm + 7.4 cm + 0.68 cm +12.0 cm = 26.3 cm
2)
1.6 km + 1.62 m +1200 cm =
1.2 x 103 or 1.20 x 103 or 1203 m
3)
8.264 g - 7.8 g =
4)
10.4168 m - 6.0 m = 4.4 m
5)
12.00 m+15.001 kg=
6)
1.31 cm x 2.3 cm =
7)
5.7621 m x 6.201 m = 35.73 m2
0.5 g
can’t add m and kg
3.0 cm2
8)
20.2 cm : 7.41 s =
2.73 cm/s
9)
40.002 g : 13.000005 g = 3.0771
4. Express the following numbers in their equivalent standard notational form:
1)
123,876.3 1.238763 x 105
2)
1,236,840 1.23684 x 106
3)
422000 4.22000 x 105
4) 0.000000000000211 2.11 x 10-13
5)
0.000238 2.38 x 10-4
6) 0.0000205 2.05 x 10-5
5. Identify the sums or differences of the following:
1)
(8.41 X 104) + (9.71 X 104) = 1.81 x 105
2)
(5.11 X 102) - (4.2 X 102) = 91
3)
(8.2 X 103) + (4.0 X 103) = 1.22 x 10 4
4)
(6.3 X 10-2) - (2.1 X 10-2) =
4.2 x 10-2
6. Express the product and the quotients of the following:
1)
(3.56 X 105) (4.21 X 106) = 1.50 x 1012
2)
(2 X 107) (8 X 10-9) =
3)
(4.11 X 10-6) (7.51 X 10-4) = 3.09 x 10-9
4)
8.45 X 107 / 6.74 X 103 = 1.25 x 104
5)
9.7 X 108 / 8.6 X 10-2 =
1.1 x 1010
6)
4.7 X 10-2 / 5.7 X 10-6 =
8.2 x 103
0.2