Download Regular Chemistry - 1st Semester Final Practice Exam

Regular Chemistry - 1st Semester Final Practice Exam
Mr. Matthew Totaro
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1) Which statement about the scientific method is TRUE?
A) The scientific method emphasizes observation and experimentation as the way to understand the world.
B) The scientific method emphasizes observation and reason as the way to understand the world.
C) The scientific method emphasizes reason as the way to understand the world.
D) The scientific method emphasizes scientific laws as the way to understand the world.
E) All of the above statements are false.
2) You are heating a piece of glass and now want to pick it up. You should
A) use tongs.
C) pour cold waler on it.
B) pick up the end that looks cooler.
D) use a rag or paper towels.
3) Use the graph to answer the following question.
How many players on the team have a batting average between .300 - .399?
A) 7
B) 1
C) 5
4) The number 680 000 000 expressed correctly using scientific notation is __________.
A) 6.8
B) 68 × 107
C) 0.68 × 106
D) 680 × 106
1
D) 9
E) 6.8 × 108
5) The correct decimal representation of 6.453 x 103 is:
A) 6.453
B) 6.5 x 103
C) 6,453
D) 0.006453
E) none of the above
6) Which of the following numbers is the largest?
A) 4.0 × 10-8
B) 4.0 × 10-12
7)
D) 4.0 × 10-6
E) 4.0 × 10-15
Perform the following operation: (1.25 x 102 ) + (4.25 x 103 ) =
A) 5.50 x 10-1
8)
C) 4.0 × 10-2
B)
C) 5.50 x 10-1
4.375 x 103
D) 5.50 x 105
Perform the following operation: (1.02 x 105 ) x (2.00 x 102 ) =
A) 2.04 x 107
B) 2.04 x 1010
C) 2.04 x 103
9) How many inches are in 25.8 cm ( 1 inch = 2.54 cm)?
A) 28.3
B) 0.0984
C) 10.2
D) 0.10
E) none of the above
10) How many milliliters are in 17.5 L?
A) 175
B) 1.75 x 10- 2
C) 1.75 x 103
D) 1.75 x 104
E) none of the above
11) How many microliters are in 41.0 mL?
A) 0.041
B) 4.1 x 103
C) 4.10 x 104
D) 4.1 x 1010
E) none of the above
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D) 3.02 x 107
12) Given the density of Au is 19.3 g/cm3, determine the mass of gold in an ingot with the dimensions of 10.0 cm x
4.00 cm x 3.00 cm.
A) 0.161
B) 2.32 x 103
C) 3.80 x 104
D) 102
E) none of the above
13) Suppose a boat engine leaks 938 milliliters of oil into a lake. The mass of this spilled oil is 823 grams. The oil
will not mix with the lake water. Which statement is true?
A) The oil will float because its density of 0.877 g/mL is less than the density of water.
B) The oil will sink because its density of 0.877 g/mL is greater than the density of water.
C) The oil will float because its density of 1.14 g/mL is less than the density of water.
D) The oil will sink because its density of 1.14 g/mL is greater than the density of water.
E) none of the above
14) The correct prefix for the multiplier 1,000is:
A) nano.
B) kilo
C) mega.
D) micro.
E) none of the above
15) The correct multiplier for the prefix pico is:
A) 0.000000000001
B) 0.000001
C) 0.001
D) 0.000000001
E) none of the above
16) In the number 162.581, which digit is estimated?
A) 1
B) 4
C) 8
D) 9
E) None of the above, all digits are certain.
17) The correct number of significant figures in the number 865,000 is:
A) 5
B) 6
C) 4
D) 3
E) none of the above
18) The correct number of significant figures in the number 7.9 x 10-4 is:
A) 1
B) 2
C) 3
D) 4
E) none of the above
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19) The correct number of significant figures in the number 0.0012320 is:
A) 4
B) 7
C) 3
D) 5
E) none of the above
20) Determine the answer for the equation below with correct number of significant figures:
1.2 x 1.79 = ________
A) 2.15
B) 2.2
C) 2.148
D) 2.1
E) none of the above
21) Determine the answer to the following equation with correct number of significant figures:
(17.103 + 2.03) x 1.02521 = ________
A) 19.6
B) 20
C) 19.61
D) 19.6153
E) none of the above
22) How many significant digits should be reported in the answer to the following calculation?
(4.3 - 3.7) x 12.3 =
A) 3
B) 1
C) 2
D) 4
E) none of the above
23) The SI unit of temperature is __________.
A) °F
B) t
C) K
D) °C
24) Which of the following statements about matter is FALSE?
A) Matter exists in either a solid, liquid or gas state.
B) Matter occupies space and has mass.
C) Matter is ultimately composed of atoms.
D) Matter can be divided an infinite number of times.
E) none of the above
25) Which state of matter has atomic spacing that is close together and definite shape?
A) plasma
B) solid
C) liquid
D) gas
E) none of the above
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E) T
26) Which state of matter has atomic spacing that is far apart and definite shape?
A) solid
B) plasma
C) gas
D) liquid
E) none of the above
27) Molten (liquid) iron metal has a(n) ________ volume and a(n) ________ shape.
A) indefinite; definite
B) definite; definite
C) definite; indefinite
D) indefinite; indefinite
E) insufficient information given to determine
28) A pure substance is:
A) composed of two or more different types of atoms or molecules combined in variable proportions.
B) composed of two or more different types of atoms or molecules that has constant composition.
C) composed of only one type of atom or molecule.
D) composed of two or more regions with different compositions.
E) none of the above
29) Which of the following items is a mixture?
A) helium
B) brass
C) water
D) sugar
E) none of the above
30) How would you classify salt water?
A) pure substance-element
B) pure substance-compound
C) mixture-heterogeneous
D) mixture-homogeneous
E) none of the above
31) A solution is an example of a (an)
A) heterogeneous mixture
B) compound
C) pure substance
D) element
E) homogeneous mixture
32) Physical properties are:
A) those that a substance displays only through changing its composition.
B) identical for all solid matter.
C) those that cause atoms and molecules to change.
D) those that a substance displays without changing its composition.
E) none of the above
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33) Which of the following statements about physical and chemical changes is FALSE?
A) In a physical change, matter does not change its composition.
B) Phase changes are always physical changes.
C) Chemical reactions are chemical changes.
D) In a chemical change, matter changes its composition.
E) All of the above statements are true.
34) What is the value of 335 K on the Celsius temperature scale?
A) 66.4
B) 167
C) 62
D) 608
E) none of the above
35) What is the value of 98 °F in units of °C?
A) 37
B) 22
C) 371
D) 72
E) none of the above
36) In the winter, the outdoor temperature is -12°F. What is the temperature in the Kelvin scale?
A) 249 K
B) 284 K
C) 262 K
D) 273 K
37) What is the atomic symbol for silver?
A) Ag
B) S
C) Si
D) Au
E) none of the above
38) What is the atomic symbol for tin?
A) Ti
B) Tn
C) Sn
D) Si
E) none of the above
39) What is the correct chemical symbol for mercury?
A) My
B) Hm
C) Hy
D) Me
E) none of the above
40) Which of the following is NOT a correct name, symbol combination?
A) magnesium, Mg
B) iron, I
C) beryllium, Be
D) manganese, Mn
E) silicon, Si
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E) 178 K
41) Which of the following is NOT a correct name, symbol combination?
A) silicon, Si
B) phosphorus, P
C) beryllium, Be
D) manganese, Mg
E) iron, Fe
42) Which of the following is NOT a correct name, symbol combination?
A) potassium, P
B) gold, Au
C) calcium, Ca
D) manganese, Mn
E) chromium, Cr
43) The names of the elements whose symbols are Si, P, Mn, and S are respectively,
A) silicon, phosphorus, magnesium, and sulfur.
B) silver, phosphorus, magnesium, and sulfur.
C) silicon, potassium, magnesium, and sulfur.
D) silicon, phosphorus, manganese, and sulfur.
E) silicon, potassium, magnesium, and sodium.
44) Which statement below accurately describes the contributions of Dalton?
A) discovered the existence of electrons
B) ancient Greek philosopher who proposed that matter was continuous
C) proposed the modern Atomic Theory
D) created the modern periodic table
E) none of the above
45) Which of the statements about the discovery of electrons is FALSE?
A) The negatively charged electron is located outside the nucleus.
B) Because atoms are neutral, the existence of a negatively charged particle implied there must be a
positively charged component of an atom.
C) Rutherford proved the plum-pudding model correct.
D) Thomson proposed that electrons were small particles held within a positively charged sphere.
E) All of the above statements are true.
46) The Rutherford gold foil experiment demonstrated that atoms
A) are homogeneous.
B) consist of an almost empty nucleus surrounded by a dense cloud of electrons.
C) are visible to the naked eye.
D) consist of a dense nucleus surrounded by mostly empty space.
E) consist of a single type of subatomic particle.
47) Which of the following pairs of subatomic particles have charges of equal magnitude but opposite in sign?
A) proton and positron
B) gamma ray and neutron
C) proton and electron
D) neutron and proton
E) electron and neutron
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48) In an atom, the nucleus contains __________.
A) all the protons and electrons
B) only protons
C) only neutrons
D) all the protons and neutrons
E) an equal number of protons and electrons
49) The atomic number of an atom is equal to the number of __________.
A) electrons plus protons
B) protons
C) neutrons
D) nuclei
E) neutrons plus protons
50) The number of neutrons in an atom is equal to the __________.
A) atomic number
B) mass number - the atomic number
C) mass number
D) mass number + the atomic number
E) number of protons
51) The mass number of an atom can be calculated from the __________.
A) number of electrons
B) number of protons
C) number of protons plus neutrons
D) number of electrons plus protons
E) number of neutrons
52) The atomic number of fluorine is __________.
A) 19
B) 28
C) 29
D) 10
E) 9
53) The atomic mass of lithium is __________.
A) 6.94
B) 3.00
C) 7.41
D) 7.00
E) 4.00
54) The correct symbol for the isotope of potassium with 22 neutrons is __________.
41
15
22
37
K
P
K
P
A)
B)
C)
D)
19
37
19
15
55) The correct symbol for a uranium atom with a mass number of 235 is __________.
327
235
143
235
U
U
U
U
A)
B)
C)
D)
92
92
92
91
56) Which of the following is NOT true for the atoms 13N, 14N, and 15N?
A) They all have 7 protons.
B) They are isotopes.
C) They all have the same atomic number.
D) They all have the same mass number.
E) They all have 7 electrons.
8
E)
19
K
41
E)
235
Ur
92
57) How many electrons are in Br- ?
A) 7
B) 4
C) 36
D) 34
E) none of the above
58) What happens to an atom when it absorbs energy?
A) The atom re-emits the energy as heat.
B) The atom re-emits the energy as light.
C) The atom stores the energy for later use.
D) The extra energy increases the speed of the electrons in their orbitals.
E) none of the above
59) The atomic orbital depicted below would be found in a ________ sublevel.
A) 6p
B) 4f
C) 2s
D) 3p
60) What is the maximum number of electrons that the “f” subshell can hold?
A) 14
B) 10
C) 5
E) 5d
D) 6
61) The electron configuration of Ga is __________.
A) 1s2 2s2 2p6 3s2 3p6 4s2 4d104p1
B) 1s2 2s2 2p6 3s2 3p6 3d104s2 4p1
C) 1s2 2s2 3s2 3p6 3d104s2 4p1
D) [Ar]4s2 3d11
E) 1s2 2s2 2p6 3s2 3p6 3d104s2 4d1
62) What is the electron configuration for potassium (atomic number 19)?
A) 1s2 2s2 2p 6 3s2 3p 5 3d 2
B) 1s2 2s2 2p 6 3s2 3p 7
C) 1s2 2s2 2p 6 3s2 3p 5 4s1
D) 1s2 2s2 2p 8 3s2 3p 5
E) 1s2 2s2 2p 6 3s2 3p 6 4s1
63) What element has the electron configuration 1s2 2s2 2p6 3s2 ?
A) Be
B) Mg
C) Ca
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D) Na
E) Si
64) Which of the following electron configurations is incorrect as written?
2 2 6 2 6
A) 1s 2s 2p 3s 3p
2 2
B) 1s 2s 2p 6
2 2 6 2 6 2 10 4
C) 1s 2s 2p 3s 3p 4s 3d 4p
2 2 6 2
D) 1s 2s 2p 3s
2 2 6 2 6 10
E) 1s 2s 2p 3s 3p 3d
65) Which electron configuration represents a violation of the Pauli exclusion principle?
A)
B)
C)
D)
E)
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66) Which of the following denotes an orbital diagram for a boron atom?
A)
B)
C)
D)
E)
67) Which one of the following elements occupies position period 5 and group IIA in the periodic table?
A) Y
B) Kr
C) Ga
D) B
E) Sr
68) Which of the following element-classification pairings is incorrect?
A) Po - halogen
B) Th - inner transition metal
C) Ar - noble gas
D) K - representative element
E) Mo - transition element
69) Which of the following pairs is incorrectly matched?
Element
Type of Element
A) antimony
metal
B) nitrogen
nonmetal
C) arsenic
metalloid
D) silicon
metalloid
E) gold
metal
70) Which element would be expected to have chemical and physical properties closest to those of fluorine?
A) S
B) Fe
C) O
D) Ne
E) Cl
71) The abbreviated electron configuration for a boron atom (Atomic number = 5) is __________.
A) 1s2 2s2 2p 1
B) 1s2 2s2 2p 6
C) [H]2s2 2p 1
D) [He]2s2 2p 1
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E) [Ne]2s2 2p 1
72) Group IA elements are called:
A) halogens
B) alkaline earth metals
C) noble gases
D) alkali metals
73) The elements in groups IA, VIIA and VIIIA are called, respectively:
A) alkali metals, halogens, noble gases
B) alkaline earth metals, transition metals, halogens
C) alkali metals, chalcogens, halogens
D) alkaline earth metals, halogens, chalcogens
74) The number of known nonmetals is ________ the number of known metals.
A) about 1/4 that of
B) about double
C) about four times greater than
D) very small compared to
75) Which of the following element-classification pairings is incorrect?
A) Mo - transition element
B) K - representative element
C) Ar - noble gas
D) Po - halogen
76) Calcium is a __________ block element.
A) d
B) s
C) f
D) g
E) p
77) Sulfur is a __________ block element.
A) g
B) f
C) d
D) s
E) p
78) One element that has 5 valence electrons is __________.
A) carbon
B) lithium
C) neon
D) nitrogen
E) sulfur
79) One element that has 7 valence electrons is __________.
A) sodium
B) bromine
C) nitrogen
D) oxygen
E) phosphorus
80) How many core electrons are in a chlorine atom?
A) 17
B) 1
C) 7
D) 10
E) none of the above
81) The elements in group IIA of the periodic table all have electron configurations ending in ________.
A) p4
B) d4
C) f4
D) p2
E) s2
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82) Chlorine and bromine have very similar chemical properties. This is best explained by the fact that both
elements
A) have the same number of valence electrons.
B) are in period 3 of the Periodic Table.
C) are gases.
D) have equal number of protons and electrons.
E) none of the above
83) What is the element in which at least one electron is in the d-orbital?
A) K
B) Sc
C) Ca
D) Ar
E) none of the above
84) The Group 8A(18) elements
A) are liquids at room temperature.
B) are good conductors of electricity.
C) melt at high temperatures.
D) are unreactive.
E) react vigorously with water.
85) What is the symbol of the element in Period 4 and Group 2?
A) Be
B) C
C) Ca
D) Si
E) Mg
86) Which of the following atoms is the largest?
A) Na
B) Li
D) K
E) Cs
87) Which of the following elements has the highest ionization energy?
A) Ca
B) Ne
C) Cl
D) Ba
E) Al
88) Which of the following atoms has the least metallic character?
A) Na
B) Li
C) Cs
D) Rb
E) K
89) Of the atoms below, __________ is the most electronegative.
A) Cl
B) S
C) Rb
D) Ca
E) Si
90) What is the missing particle?
231
Th
90
____ +
C) Rb
231
Ac
89
A) beta particle
B) alpha particle
C) positron
D) gamma particle
E) none of the above
91) The isotope
A)
1
n
0
126
126
Sn decays to
Sb. What type of radiation does it emit in this process?
50
51
B)
4
He
2
C)
-1
e
0
13
D)
0
e
-1
E)
92) Which of the following nuclides will undergo beta decay to produce
A)
247
Cm
96
B)
243
Np
93
C)
244
Bk
97
D)
243
Pu
94
243
Am?
95
E) none of the above
93) The half-life of bromine-74 is 25 min. How much of a 4.0 mg sample is still active after 75 min?
A) 4.0 mg
B) 1.0 mg
C) 2.0 mg
D) 0.25 mg
E) 0.50 mg
94) When an atom of uranium-235 is bombarded with neutrons, it splits into smaller nuclei and produces a great
amount of energy. This nuclear process is called __________.
A) fission
B) fusion
C) chain reaction
D) ionization
E) decomposition
TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false.
95) The element manganese (symbol = Mn) has five valence electrons.
96) Bromine has 17 valence electrons.
97) Bromine has 28 core electrons.
98) The ionization energy of lithium is higher than that of fluorine.
99) Based on relative location on the periodic table, a carbon atom is larger in atomic size than a phosphorous atom.
100) Based on relative location on the periodic table, vanadium (symbol = V) is expected to have more metallic
character than selenium (symbol = Se).
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Answer Key
Testname: REGULAR CHEMISTRY - 1ST SEMESTER FINAL EXAM PRACTICE TEST
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Answer Key
Testname: REGULAR CHEMISTRY - 1ST SEMESTER FINAL EXAM PRACTICE TEST
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