AP Chemistry chapter 1&2 worksheet-2018
Name:------------------------------------------------------------------------------Date:-----------------1) What is the volume (in cm3) of a 63.4 g piece of metal with a density of 12.86 g/cm3?
A) 4.93
B) 19.5
C) .425
D) 6.65
E) none of the above
2) The correct answer (reported to the proper number of significant figures) to the following is __________.
11.5 × 8.78 = __________
3) The correct answer (reported to the proper number of significant figures) to the following is __________.
(1815 - 1806) × (9.11 × 7.92) = __________
4) Round the following number to four significant figures and express the result in standard exponential notation:
229.613
A) 0.2296 × 103
B) 229.6
C) 2.296 × 10-2
D) 2.296 × 102
E) 22.96 × 10-1
5) Round the following number to four significant figures and express the result in standard exponential notation:
229.613
A) 0.2296 × 103
B) 229.6
C) 2.296 × 10-2
D) 2.296 × 102
E) 22.96 × 10-1
6) What decimal power does the abbreviation Milli represent?
A) 1 × 103
B) 1 × 106
C) 1 × 109
D) 1 × 10-3
E) 1 × 10-6
7) 1 milligram = __________ micrograms
8) Mass and volume are often referred to as __________ properties of substances.
9) Gases do not have a fixed __________ as they are able to be __________
10) Which of the following is the same as 0.001 cm?
A) 0.01 mm
B) 0.01 dm
C) 0.01 m
D) 100 mm
E) 1 mm
11) Round the number 0.007222 to three significant figures.
A) 0.007
B) 0.00722
C) 0.0072
D) 0.00723
E) 0.007225
12) Expressing a number in scientific notation __________.
A) changes its value
B) removes ambiguity as to the significant figures
C) removes significant zeros
D) allows to increase the number's precision
E) all of the above
13.Accuracy refers to __________.
A) how close a measured number is to zero
B) how close a measured number is to the calculated value
C) how close a measured number is to other measured numbers
D) how close a measured number is to the true value
E) how close a measured number is to infinity
14.Precision refers to __________.
A) how close a measured number is to other measured numbers
B) how close a measured number is to the true value
C) how close a measured number is to the calculated value
D) how close a measured number is to zero
E) how close a measured number is to infinity
15) Which calculation clearly shows a conversion between temperatures in degrees Celsius, t(°C), and temperature
in Kelvins, T(K)?
A) T(K) = t(°C) + 273
B) T(K) = 273 - t(°C)
C) T(K) = [t(°C) - 32] / 1.8
D) T(K) = [t(°C) + 32] × 1.8
E) T(K) = t(°C)
16) Which calculation clearly shows a conversion between temperatures in degrees Celsius, t(°C), and temperature
in Kelvins, T(K)?
A) T(K) = t(°C) + 273
B) T(K) = 273 - t(°C)
C) T(K) = [t(°C) - 32] / 1.8
D) T(K) = [t(°C) + 32] × 1.8
E) T(K) = t(°C)
17) Which of the following are chemical processes?
1. rusting of a nail
2. freezing of water
3. decomposition of water into hydrogen and oxygen gases
4. compression of oxygen gas
A) 2, 3, 4
B) 1, 3, 4
C) 1, 3
D) 1, 2
E) 1, 4
18) Of the following, only __________ is an extensive property.
A) density
B) mass
C) boiling point
D) freezing point
E) temperature
19) Which one of the following is an intensive property?
A) mass
B) temperature
C) heat content
D) volume
E) amount
20) In the following list, only __________ is not an example of a chemical reaction.
A) dissolution of a penny in nitric acid
B) the condensation of water vapor
C) a burning candle
D) the formation of polyethylene from ethylene
E) the rusting of iron
21) Gases and liquids share the property of __________.
A) compressibility
B) definite volume
C) incompressibility
D) indefinite shape
E) definite shape
22) Which of the following is an illustration of the law of constant composition?
A) Water boils at 100°C at 1 atm pressure.
B) Water is 11% hydrogen and 89% oxygen by mass.
C) Water can be separated into other substances by a chemical process.
D) Water and salt have different boiling points.
E) Water is a compound.
23) If matter is uniform throughout and cannot be separated into other substances by physical
means, it is __________.
A) a compound
B) either an element or a compound
C) a homogeneous mixture
D) a heterogeneous mixture
E) an element
24) An element cannot __________.
A) be part of a heterogeneous mixture
B) be part of a homogeneous mixture
C) be separated into other substances by chemical means
D) interact with other elements to form compounds
E) be a pure substance
25) Homogeneous mixtures are also known as __________.
A) solids
B) compounds
C) elements
D) substances
E) solutions
26) Which one of the following is often easily separated into its components by simple techniques such as filtering
or decanting?
A) heterogeneous mixture
B) compounds
C) homogeneous mixture
D) elements
E) solutions
27) A combination of sand, salt, and water is an example of a __________.
A) homogeneous mixture
B) heterogeneous mixture
C) compound
D) pure substance
E) solid
28) The law of constant composition applies to __________.
A) solutions
B) heterogeneous mixtures
C) compounds
D) homogeneous mixtures
E) solids
29) In the following list, only __________ is not an example of matter.
A) planets
B) light
C) dust
D) elemental phosphorus
E) table salt
30) There are __________ ng in a pg.
A) 0.001
B) 1000
C) 0.01
D) 100
E) 10
31) The quantity __________ m is the same as 3 km.
A) 3000
B) 300
C) 0.003
D) 0.03
E) 30
32) The length of the side of a cube (in cm) having a volume of 44.4 L is __________.
A) 875
B) 35.4
C) 6.66
D) 66.6
E) 0.354
33) "Absolute zero" refers to __________.
A) 0 Kelvin
B) 0° Fahrenheit
C) 0° Celsius
D) °C + 9/5(°F - 32)
E) 273.15°C
34) A temperature of 400 K is the same as __________°F.
A) 261
B) 286
C) 88
D) 103
E) 127
35) The freezing point of water at 1 atm pressure is __________.
A) 0°F
B) 0 K
C) 0°C
D) -273°C
E) -32°F
36) A separation process that depends on differing abilities of substances to form gases is called __________.
A) filtration
B) solvation
C) distillation
D) chromatography
E) all of the above are correct
37) The SI unit for mass is __________.
A) kilogram
B) gram
C) pound
D) troy ounce
E) none of the above
38) A concise verbal statement or mathematical equation that summarizes a broad variety of observations and
experiences is called a(n) __________.
A) law
B) theory
C) hypothesis
D) experiment
E) test
39) The initial or tentative explanation of an observation is called a(n) __________.
A) law
B) theory
C) hypothesis
D) experiment
E) test
40) If matter is uniform throughout, cannot be separated into other substances by physical processes, but can be
decomposed into other substances by chemical processes, it is called a (an) __________.
A) heterogeneous mixture
B) element
C) homogeneous mixture
D) compound
E) mixture of elements
41) A certain mass of carbon reacts with 13.6 g of oxygen to form carbon monoxide. __________ grams of oxygen
would react with that same mass of carbon to form carbon dioxide, according to the law of multiple proportions?
A) 25.6
B) 6.8
C) 13.6
D) 136
E) 27.2
42) Methane and ethane are both made up of carbon and hydrogen. In methane, there are 12.0 g of carbon for every
4.00 g of hydrogen, a ratio of 3:1 by mass. In ethane, there are 24.0 g of carbon for every 6.00 g of hydrogen, a ratio
of 4:1 by mass. This is a statement of the law of __________.
A) constant composition
B) multiple proportions
C) conservation of matter
D) conservation of mass
E) octaves
43) Which statement below correctly describes the responses of alpha, beta, and gamma radiation to an electric
field?
A) Both beta and gamma are deflected in the same direction, while alpha shows no response.
B) Both alpha and gamma are deflected in the same direction, while beta shows no response.
C) Both alpha and beta are deflected in the same direction, while gamma shows no response.
D) Alpha and beta are deflected in opposite directions, while gamma shows no response.
E) Only alpha is deflected, while beta and gamma show no response
44) The atomic number indicates __________.
A) the number of neutrons in a nucleus
B) the total number of neutrons and protons in a nucleus
C) the number of protons or electrons in a neutral atom
D) the number of atoms in 1 g of an element
E) the number of different isotopes of an element
45) Which group in the periodic table contains only nonmetals?
A) 1A
B) 6A
C) 2B
D) 2A
E) 8A
46) Elements in Group 2A are known as the __________.
A) alkaline earth metals
B) alkali metals
C) chalcogens
D) halogens
E) noble gases
47) Elements in Group 6A are known as the __________.
A) alkali metals
B) chalcogens
C) alkaline earth metals
D) halogens
E) noble gases
48) Potassium is a __________ and chlorine is a __________.
A) metal, nonmetal
B) metal, metal
C) metal, metalloid
D) metalloid, nonmetal
E) nonmetal, metal
49) Oxygen is a __________ and nitrogen is a __________.
A) metal, metalloid
B) nonmetal, metal
C) metalloid, metalloid
D) nonmetal, nonmetal
E) nonmetal, metalloid
50) __________ are found uncombined, as monatomic species in nature.
A) Noble gases
B) Chalcogens
C) Alkali metals
D) Alkaline earth metals
E) Halogens
51) __________ typically form ions with a 2+ charge.
A) Alkaline earth metals
B) Halogens
C) Chalcogens
D) Alkali metals
E
52) __________ typically form ions with a 2+ charge.
A) Alkaline earth metals
B) Halogens
C) Chalcogens
D) Alkali metals
E) Transition metals
) Transition metals
53) Aluminum reacts with a certain nonmetallic element to form a compound with the general formula AlX.
Element X is a diatomic gas at room temperature. Element X must be __________.
A) oxygen
B) fluorine
C) chlorine
D) nitrogen
E) sulfur
54) Potassium forms an ion with a charge of __________.
A) +2
B) -1
C) +1
D) -2
E) 0
55) Calcium forms an ion with a charge of __________.
A) -1
B) -2
C) +1
D) +2
E) 0
7
56) Barium forms an ion with a charge of __________.
A) +1
B) -2
C) +3
D) -3
E) +2
57) Aluminum forms an ion with a charge of __________.
A) +2
B) -3
C) +1
D) +3
E) -1
58) Fluorine forms an ion with a charge of __________.
A) -1
B) +1
C) +2
D) +3
E) -3
59) Iodine forms an ion with a charge of __________.
A) -7
B) +1
C) -2
D) +2
E) -1
60) Oxygen forms an ion with a charge of __________.
A) -2
B) +2
C) -3
D) +3
E) +6
61) Sulfur forms an ion with a charge of __________.
A) +2
B) -2
C) +3
D) -6
E) +6
62) The correct name for SrO is __________.
A) strontium oxide
B) strontium hydroxide
C) strontium peroxide
D) strontium monoxide
E) strontium dioxide
63) The correct name for SO is __________.
A) sulfur oxide
B) sulfur monoxide
C) sulfoxide
D) sulfate
E) sulfite
64) The correct name for SO is __________.
A) sulfur oxide
B) sulfur monoxide
C) sulfoxide
D) sulfate
E) sulfite
65) A molecule of water contains hydrogen and oxygen in a 1:8 ratio by mass. This is a statement of __________.
A) the law of multiple proportions
B) the law of constant composition
C) the law of conservation of mass
D) the law of conservation of energy
E) none of the above
66) Which one of the following is not one of the postulates of Dalton's atomic theory?
A) Atoms are composed of protons, neutrons, and electrons.
B) All atoms of a given element are identical; the atoms of different elements are different and have different
properties.
C) Atoms of an element are not changed into different types of atoms by chemical reactions: atoms are neither
created nor destroyed in chemical reactions.
D) Compounds are formed when atoms of more than one element combine; a given compound always has the same
relative number and kind of atoms.
E) Each element is composed of extremely small particles called atoms.
67) Consider the following selected postulates of Dalton's atomic theory:
(i) Each element is composed of extremely small particles called atoms.
(ii) Atoms are indivisible.
(iii) Atoms of a given element are identical.
(iv) Atoms of different elements are different and have different properties.
Which of the postulates is(are) no longer valid?
A) (i) and (ii)
B) (ii) only
C) (ii) and (iii)
D) (iii) only
E) (iii) and (iv)
68) Which one of the following is not true concerning cathode rays?
A) They originate from the negative electrode.
B) They travel in straight lines in the absence of electric or magnetic fields.
C) They impart a negative charge to metals exposed to them.
D) They are made up of electrons.
E) The characteristics of cathode rays depend on the material from which they are emitted.
69) The charge on an electron was determined in the __________.
A) cathode ray tube, by J. J. Thompson
B) Rutherford gold foil experiment
C) Millikan oil drop experiment
D) Dalton atomic theory
E) atomic theory of matter
70) __________-rays consist of fast-moving electrons.
A) alpha
B) beta
C) gamma
D) X
E) none of the above
71) The gold foil experiment performed in Rutherford's lab __________.
A) confirmed the plum-pudding model of the atom
B) led to the discovery of the atomic nucleus
C) was the basis for Thompson's model of the atom
D) utilized the deflection of beta particles by gold foil
E) proved the law of multiple proportions
72) In the Rutherford nuclear-atom model, __________.
A) the heavy subatomic particles, protons and neutrons, reside in the nucleus
B) the three principal subatomic particles (protons, neutrons, and electrons) all have essentially the same mass
C) the light subatomic particles, protons and neutrons, reside in the nucleus
D) mass is spread essentially uniformly throughout the atom
E) the three principal subatomic particles (protons, neutrons, and electrons) all have essentially the same mass and
mass is spread essentially uniformly throughout the atom
73) Cathode rays are deflected away from a negatively charged plate because __________.
A) they are not particles
B) they are positively charged particles
C) they are neutral particles
D) they are negatively charged particles
E) they are emitted by all matter
74) In the absence of magnetic or electric fields, cathode rays __________.
A) do not exist
B) travel in straight lines
C) cannot be detected
D) become positively charged
E) bend toward a light source
75) Of the three types of radioactivity characterized by Rutherford, which is/are electrically charged?
A) β-rays
B) α-rays and β-rays
C) α-rays, β-rays, and γ-rays
D) α-rays
E) α-rays and γ-rays
76) Of the three types of radioactivity characterized by Rutherford, which is/are not electrically charged?
A) α-rays
B) α-rays, β-rays, and γ-rays
C) γ-rays
D) α-rays and β-rays
E) α-rays and γ-rays
77) Of the three types of radioactivity characterized by Rutherford, which are particles?
A) β-rays
B) α-rays, β-rays, and γ-rays
C) γ-rays
D) α-rays and γ-rays
E) α-rays and β-rays
78) Of the three types of radioactivity characterized by Rutherford, which is/are not particles?
A) β-rays
B) α-rays and β-rays
C) α-rays
D) γ-rays
E) α-rays, β-rays, and γ-rays
79) Which atom has the smallest number of neutrons?
A) carbon-14
B) nitrogen-14
C) oxygen-16
D) fluorine-19
E) neon-20
80) Which atom has the largest number of neutrons?
A) phosphorous-30
B) chlorine-37
C) potassium-39
D) argon-40
E) calcium-40
81) Isotopes are atoms that have the same number of __________ but differing number of __________.
A) protons, electrons
B) neutrons, protons
C) protons, neutrons
D) electrons, protons
E) neutrons, electrons
82) The nucleus of an atom does not contain __________.
A) protons
B) protons or neutrons
C) neutrons
D) subatomic particles
E) electrons
83) Different isotopes of a particular element contain the same number of __________.
A) protons
B) neutrons
C) protons and neutrons
D) protons, neutrons, and electrons
E) subatomic particles
84) Different isotopes of a particular element contain different numbers of __________.
A) protons
B) neutrons
C) protons and neutrons
D) protons, neutrons, and electrons
E) None of the above is correct
85) Gravitational forces act between objects in proportion to their
A) volumes
B) masses
C) charges
D) polarizability
E) densities
86) Gravitational forces act between objects in proportion to their
A) volumes
B) masses
C) charges
D) polarizability
E) densities
87) The average atomic weight of copper, which has two naturally occurring isotopes, is 63.5. One of the isotopes
has an atomic weight of 62.9 amu and constitutes 69.1% of the copper isotopes. The other isotope has an abundance
of 30.9%. The atomic weight (amu) of the second isotope is __________ amu.
A) 63.2
B) 63.8
C) 64.1
D) 64.8
E) 28.1
88) The average atomic weight of copper, which has two naturally occurring isotopes, is 63.5. One of the isotopes
has an atomic weight of 62.9 amu and constitutes 69.1% of the copper isotopes. The other isotope has an abundance
of 30.9%. The atomic weight (amu) of the second isotope is __________ amu.
A) 63.2
B) 63.8
C) 64.1
D) 64.8
E) 28.1
89) An unknown element is found to have three naturally occurring isotopes with atomic masses of 35.9675
(0.337%), 37.9627 (0.063%), and 39.9624 (99.600%). Which of the following is the unknown element?
A) Ar
B) K
C) Cl
D) Ca
E) None of the above could be the unknown element.
90) Elements __________ exhibit similar physical and chemical properties.
A) with similar chemical symbols
B) with similar atomic masses
C) in the same period of the periodic table
D) on opposite sides of the periodic table
E) in the same group of the periodic table
91) Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical
properties?
A) H, Li
B) Cs, Ba
C) Ca, Sr
D) Ga, Ge
E) C, O
92) Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical
properties?
A) O, S
B) C, N
C) K, Ca
D) H, He
E) Si, P
93) Which one of the following is a nonmetal?
A) W
B) Sr
C) Os
D) Ir
E) Br
94) Of the following, only __________ is not a metalloid.
A) B
B) Al
C) Si
D) Ge
E) As
95) The elements in groups 1A, 6A, and 7A are called, __________, respectively.
A) alkaline earth metals, halogens, and chalcogens
B) alkali metals, chalcogens, and halogens
C) alkali metals, halogens, and noble gases
D) alkaline earth metals, transition metals, and halogens
E) halogens, transition metals, and alkali metals
96) An element in the upper right corner of the periodic table __________.
A) is either a metal or metalloid
B) is definitely a metal
C) is either a metalloid or a non-metal
D) is definitely a non-metal
E
97) An element that appears in the lower left corner of the periodic table is __________.
A) either a metal or metalloid
B) definitely a metal
C) either a metalloid or a non-metal
D) definitely a non-metal
E) definitely a metalloid
98) Which one of the following does not occur as diatomic molecules in elemental form?
A) oxygen
B) nitrogen
C) sulfur
D) hydrogen
E) bromine
99) Which type of formula provides the most information about a compound?
A) empirical
B) molecular
C) simplest
D) structural
E) chemical
100) A molecular formula always indicates __________.
A) how many of each atom are in a molecule
B) the simplest whole-number ratio of different atoms in a compound
C) which atoms are attached to which in a molecule
D) the isotope of each element in a compound
E) the geometry of a molecule
101) An empirical formula always indicates __________.
A) which atoms are attached to which in a molecule
B) how many of each atom are in a molecule
C) the simplest whole-number ratio of different atoms in a compound
D) the isotope of each element in a compound
E) the geometry of a molecule
102) The molecular formula of a compound is always __________ the empirical formula.
A) more complex than
B) different from
C) an integral multiple of
D) the same as
E) simpler than
103) Which one of the following is most likely to lose electrons when forming an ion?
A) F
B) P
C) Rh
D) S
E) N
104) Which one of the following is most likely to lose electrons when forming an ion?
A) F
B) P
C) Rh
D) S
E) N
105) Which pair of elements is most apt to form an ionic compound with each other?
A) barium, bromine
B) calcium, sodium
C) oxygen, fluorine
D) sulfur, fluorine
E) nitrogen, hydrogen
106) Which pair of elements is most apt to form a molecular compound with each other?
A) aluminum, oxygen
B) magnesium, iodine
C) sulfur, fluorine
D) potassium, lithium
E) barium, bromine
107) Which pair of elements is most apt to form a molecular compound with each other?
A) aluminum, oxygen
B) magnesium, iodine
C) sulfur, fluorine
D) potassium, lithium
D) barium, bromine
108) The suffix -ide is used __________.
A) for monatomic anion names
B) for polyatomic cation names
C) for the name of the first element in a molecular compound
D) to indicate binary acids
E) for monoatomic cations
109) The charge on the __________ ion is -3.
A) sulfate
B) acetate
C) permanganate
D) oxide
E) nitride
110) Which one of the following polyatomic ions has the same charge as the hydroxide ion?
A) ammonium
B) carbonate
C) nitrate
D) sulfate
E) phosphate
111) Which element forms an ion with the same charge as the ammonium ion?
A) potassium
B) chlorine
C) calcium
D) oxygen
E) nitrogen
112) When a fluorine atom forms the fluoride ion, it has the same charge as the __________ ion.
A) sulfide
B) ammonium
C) nitrate
D) phosphate
E) sulfite
113) Which metal does not form cations of differing charges?
A) Na
B) Cu
C) Co
D) Fe
E) Sn
114) Which metal forms cations of differing charges?
A) K
B) Cs
C) Ba
D) Al
E) Sn
115) Carbon can exist in different forms called __________.
116) Which element in Group IA is the most metallic?
117) Which element in the halogen family would require the greatest ionization energy?
118) The formula for potassium sulfide is __________.
119) An ion has 8 protons, 9 neutrons, and 10 electrons. The symbol for the ion is __________.
A) 17O2B) 17O2+
C) 19F+
D) 19FE) 17Ne2+
120) How many protons does the Br- ion possess?
A) 34
B) 36
C) 6
D) 8
E) 35
121) Predict the charge of the most stable ion of fluorine.
A) +2
B) +1
C) +3
D) -1
E) -2
122) Predict the charge of the most stable ion of potassium.
A) +3
B) -1
C) +2
D) -2
E) +1
123) 420 ppm is the same as __________ Angstroms.
A) 4200
B) 42
C) 420
D) 4.2
E) 0.42