Name: ____________________________________ Class Period:________ October 19, 2012
THERE are 110 Total Points; You May Write On This Test. Good Luck
Test Copy: A
CHEM TEST: Introduction to Matter and Energy
Multiple Choice (1 pt each) Identify the choice that best completes the statement or answers the question and print the
corresponding letter, using only CAPITAL LETTERS, on the blank to the left of the question number .
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1. Study of the composition and structure of materials and the changes that materials undergo best describes the
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2.
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3.
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4.
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5.
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6.
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7.
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8.
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9.
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10.
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11.
science of
A) chemistry.
C) physics.
B) biology.
D) engineering.
Matter includes all of the following EXCEPT
A) air.
C) smoke.
B) light.
D) water vapor.
A physical property may be investigated by
A) melting ice.
C) allowing silver to tarnish.
B) letting milk turn sour.
D) burning wood.
Chemical properties
A) include changes of state of a substance.
B) include mass and color.
C) include changes that alter the identity of a substance.
D) can be observed without altering the identity of a substance.
Two features that distinguish matter are
A) mass and velocity.
C) mass and volume.
B) weight and velocity.
D) weight and volume.
One chemical property of matter is
A) boiling point.
C) reactivity.
B) texture.
D) density.
Which of the following is an intensive physical property?
A) volume
C) color
B) length
D) mass
A chemical change occurs when
A) dissolved minerals solidify to form a crystal.
B) ethanol is purified through distillation.
C) salt deposits form from evaporated sea water.
D) a leaf changes color.
The melting of candle wax is classified as a physical change because it
A) produces no new substances.
B) transfers energy.
C) absorbs heat.
D) changes the chemical properties of wax.
The particles in a solid are
A) packed closely together.
C) constantly in motion.
B) very far apart.
D) able to slide past each other.
The state of matter in which a material has neither a definite shape nor a definite volume is the
A) gaseous state.
C) elemental state.
B) liquid state.
D) solid state.
1
ID: A
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12. A list of pure substances could include
A) bread dough.
B) vinegar (5% acetic acid).
C) vitamin C (ascorbic acid).
D) sea water.
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13. The homogeneous mixture in the illustration above is in container
A) a.
C) c.
B) b.
D) d.
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14. The substances that are chemically bound together are
A) the gases in the air.
C) dust particles in air.
B) the elements that compose water.
D) substances in blood.
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15. Physical means can be used to separate
A) elements.
B) pure substances.
C) mixtures.
D) compounds.
2
ID: A
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16. Which part of the illustration above shows the particles in a heterogeneous mixture?
A) a
C) c
B) b
D) d
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17. Group ____ in the figure above contains only metals.
A) 2
C) 17
B) 13
D) 18
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18. A vertical column of blocks in the periodic table is called a(n)
A) group.
C) property.
B) period.
D) octet.
3
ID: A
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19. All of the following statements are true EXCEPT
A) of the 113 known elements, 91 occur naturally.
B) an element cannot be broken down into two or more pure substances.
C) a compound is a substance that contains two or more elements.
D) a pure compound always contains the same elements in the same mass percentages.
E) another name for a heterogeneous mixture is a solution.
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20. Which term best describes calcium at room temperature?
A) gas
B) element
C) compound
D) homogeneous mixture
E) heterogeneous mixture
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21. All of the following statements are true EXCEPT
A) potassium is represented by the symbol K.
B) zinc is represented by the symbol Zn.
C) argon is represented by the symbol Ar.
D) iron is represented by the symbol Fe.
E) nitrogen is represented by the symbol Ni.
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22. All of the following statements are false EXCEPT
A) lithium is represented by the symbol Li.
B) oxygen is represented by the symbol Ox.
C) potassium is represented by the symbol P.
D) bromine is represented by the symbol B.
E) copper is represented by the symbol Co.
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23. Which method is best for separating a mixture of ethyl alcohol and water?
A) distillation
B) light absorption
C) electrolysis
D) gas-liquid chromatography
E) filtration
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24. Which method is best for removing the pulp from orange juice?
A) distillation
B) light absorption
C) electrolysis
D) gas-liquid chromatography
E) filtration
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25. Vinegar is a homogeneous mixture of two liquids: acetic acid and water. Which method is best for separating
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the components of vinegar?
A) distillation
B) filtration
C) electrolysis
D) gas-liquid chromatography
E) light absorption
26. All of the following relationships are true EXCEPT
A) 0.328 g = 328 mg.
B) 23 km < 4.5 × 107 mm.
C) 0.84 kg > 8.4 × 104 mg.
D) 41.3 mL > 8.72 × 10-2 L.
E) 1.3 nm = 1.3 × 10-6 mm.
4
ID: A
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27. All of the following are examples of chemical change EXCEPT
A) the fermentation of wine.
B) the tarnishing of silver.
C) the condensation of steam.
D) the combustion of butane gas
E) the rusting of iron.
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28. All of the following are examples of a physical property EXCEPT
A) the density of oxygen.
B) the boiling point of dry ice.
C) the color of copper.
D) the electrical conductivity of aluminum.
E) the rusting of iron.
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29. At 25°C, nitrogen has a density of 0.895 g/L. What mass of nitrogen will occupy a room of the following
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30.
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31.
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32.
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33.
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34.
____
35.
dimensions: 5.00 m × 5.00 m × 2.50 m?
A) 1.43 × 10-2 g
B) 5.59 × 101 g
C) 6.98 × 101 g
D) 1.43 × 101 g
E) 5.59 × 104 g
The measure of the average kinetic energy of the particles of a substance is the ____.
A) temperature
C) thermal energy
B) heat
D) kinetic energy
The freezing point of a substance is ____ the melting point of the same substance.
A) greater than
C) equal to
B) less than
D) unrelated to
Kinetic energy is the ____ of motion.
A) temperature
C) heat
B) energy
D) state
All of the following statements are true EXCEPT
A) a proton carries a +1 charge and an electron carries a -1 charge.
B) the nucleus of an atom has a negative charge.
C) an alpha particle is a helium atom minus its electrons.
D) a neutron is an uncharged particle with a mass slightly greater than a proton.
E) more than 99.9% of an atom's mass is concentrated in the nucleus.
Rank the subatomic particles from least to greatest mass.
A) electrons = neutrons = protons
B) electrons = protons < neutrons
C) electrons < neutrons = protons
D) electrons < protons < neutrons
E) electrons < neutrons < protons
All of the following statements are true EXCEPT
A) all atoms of a given element have the same mass number.
B) for any neutral element, the number of electrons is equal to the number of protons.
C) the mass number is the sum of the number of protons and neutrons.
D) isotopes of atoms contain the same number of protons but a different number of neutrons.
E) the atomic number equals the number of protons in an atom.
5
ID: A
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36. All atoms of the same element have the same number of __________ .
A) neutrons
B) protons
C) protons and neutrons
D) electrons and neutrons
E) protons, neutrons, and electrons
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37. Which nuclear symbol describes oxygen-15, a radioactive element used in positron emission tomography?
A)
B)
C)
D)
E)
____
15
7
16
8
15
8
16
15
15
16
O
O
O
O
O
38. Which of the following atoms contains the largest number protons?
A)
B)
C)
D)
E)
14
6
14
7
16
8
18
8
19
9
C
N
O
O
F
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39. Which description most accurately describes neptunium-239?
A) mass number = 93, atomic number = 239
B) mass number = 93, number of neutrons = 146
C) mass number = 146, atomic number = 93
D) number of protons = 93, number of neutrons = 146
E) number of protons = 93, atomic number = 239
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40. F-20, a radioactive isotope of fluorine, has
A) 9 protons, 10 neutrons, and 1 electron.
B) 9 protons, 10 neutrons, and 9 electrons.
C) 9 protons, 11 neutrons, and 9 electrons.
D) 10 protons, 9 neutrons, and 1 electron.
E) 10 protons, 10 neutrons, and 10 electrons.
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41. Which two atoms below have the same number of neutrons?
15
8
O,
A)
B)
C)
D)
E)
16
8
15
8
16
8
20
9
20
9
20
10
O,
20
9
F,
20
10
Ne,
22
11
Na
O and 168 O
O and 22
Na
11
F and 20
Ne
10
F and 22
Na
11
Ne and 22
Na
11
6
ID: A
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42. How many electrons, protons, and neutrons are found in a Cl - ion formed from Cl-35?
A) 17 electrons, 16 protons, 19 neutrons
B) 17 electrons, 17 protons, 18 neutrons
C) 18 electrons, 18 protons, 18 neutrons
D) 18 electrons, 17 protons, 18 neutrons
E) 18 electrons, 18 protons, 17 neutrons
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43. Which species has 63 neutrons?
A)
B)
C)
44.
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45.
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46.
____
47.
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48.
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49.
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50.
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51.
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52.
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53.
Cd
In
Zn
Eu
E) none of the above
A molecule of water (H2O) is made from _____ combining two hydrogen atoms and one oxygen atom.
A) physically
C) thermally
B) ionically
D) chemically
You put 1 spoonful of salt into 1 liter of water and stir. The resulting liquid is an example of a(n)
A) pure substance.
C) heterogeneous mixture.
B) homogeneous mixture.
D) immiscible mixture.
Which of the following is not a potential sign of chemical change?
A) release of gas
C) change of color
B) evaporation of water
D) production of gas
The smallest unit of an element that maintains the properties of that element is a(n)
A) molecule.
C) substance.
B) atom.
D) compound.
Which of the following is not a pure substance?
A) element
C) compound
B) molecule
D) mixture
The different substances in a mixture
A) keep their properties.
C) form new molecules.
B) combine chemically.
D) cannot be separated.
Which of the following is not a potential sign of chemical change?
A) change in odor
C) change in color
B) fizzing
D) boiling
A chemical change occurs whenever
A) substances are mixed.
C) hot objects melt.
B) objects change shape.
D) new substances form.
Which tool is best for separating a mixture of sand and water?
A) tweezers
C) centrifuge
B) magnet
D) filter
Chemical changes can affect physical and chemical properties whereas physical changes can affect
A) chemical properties.
B) physical properties.
C) both chemical and physical properties.
D) None of the above
D)
____
112
48
112
49
63
29
152
63
7
ID: A
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54. Which of the following is made of at least two different types of atoms?
A) element
C) compound
B) molecule
D) matter
____
55. Unlike a mixture, a pure substance has
A) atoms
B) molecules
C) a specific size.
D) a fixed composition.
____
56. Which of the following is not an example of a physical property?
A) freezing point
C) boiling point
B) reactivity
D) density
____
57. A substance that cannot be broken down into simpler substances is a(n)
A) compound.
C) element.
B) mixture.
D) atom.
____
58. You put a spoonful of salt into 1 liter of water and stir. The resulting liquid is an example of a(n)
A) pure substance.
C) heterogeneous mixture.
B) homogeneous mixture.
D) immiscible mixture.
____
59. Knowing the chemical properties of a substance will tell you how the substance
A) looks.
C) smells.
B) can be broken down into atoms.
D) reacts with other substances.
____
60. The ability of an apple to change color when exposed to air is a ____.
A) physical property
C) physical change
B) chemical property
D) chemical change
____
61. The ability of a pond to freeze over in winter is a ____.
A) physical property
C) physical change
B) chemical property
D) chemical change
____
62. Which of the following is NOT a possible sign of a chemical change?
A) a change in state
C) the release of a gas
B) a change in color
D) the release of energy
____
63. When a newspaper is left in direct sunlight for a few days, the paper begins to turn yellow. The yellow color
____
____
____
is evidence of a ____.
A) physical property
C) physical change
B) chemical property
D) chemical change
64. The substance being dissolved to form a solution is the ____.
A) solvent
C) precipitate
B) solute
D) mixture
65. The atmosphere of Earth is an example of a ____ solution.
A) liquid-liquid
C) gas-gas
B) gas-liquid
D) solid-liquid
66. A solution that contains all the solute it can hold under the given conditions is ____.
A) saturated
C) dilute
B) unsaturated
D) supersaturated
8
ID: A
____
67. Which is the type of separation technique being demonstrated in the figure?
A) crystallization
B) distillation
C) filtration
D) chromatography
____
68. Which is the separation technique that relies on the different boiling points of the parts of the mixture?
A) filtration
C) chromatography
B) distillation
D) crystallization
____
69. Matter that has a uniform and unchanging composition is known as a(n) ____.
A) compound
C) mixture
B) element
D) substance
____
70. Bromine element occurs in the ____ state at room temperature.
A) gaseous
C) plasma
B) liquid
D) solid
____
71. The box for an element from the periodic table is shown. Which is the atomic mass?
A) A
B) B
____
C) C
D) D
72. The box for an element from the periodic table is shown. Which is the atomic number?
A) A
C) C
B) B
D) D
9
ID: A
____
73. Which scientist developed the model of the atom shown?
A) Chadwick
B) Thomson
____
C) Rutherford
D) Bohr
74. Which scientist developed the model of the atom shown?
A) Chadwick
B) Thomson
____
____
75. Which one is comprised of the other three?
A) proton
B) atom
C) electron
D) neutron
76. Which has a charge of +1?
A) proton
B) atom
C) electron
D) neutron
Atom
1
2
3
4
____
C) Rutherford
D) Bohr
Protons
8
10
9
8
Atoms
Neutrons
10
9
9
11
77. Which two are isotopes of one another?
A) Atoms 1 & 2
B) Atoms 2 & 3
Electrons
8
10
9
8
C) Atoms 1 & 3
D) Atoms 1 & 4
10
ID: A
____
78. Which two have the same mass?
A) Atoms 1 & 2
B) Atoms 2 & 4
Atom
Sodium
Chlorine
Protons
C) Atoms 1 & 4
D) Atoms 2 & 3
Atoms
Neutrons
12
17
Electrons
17
____
79. How many neutrons are in an atom of chlorine?
A) 17
C) 34
B) 18
D) 35
____
80. How many electrons are in an neutral atom of sodium?
A) 22
C) 12
B) 11
D) 23
____
81. What is the mass number of the atom shown?
A) 11
B) 18
C) 19
D) 20
82. Which element does this atom represent?
A) potassium
B) neon
C) fluorine
D) sodium
____
____
83. Which is the correct symbol for this atom?
A)
B)
____
Mass Number
23
35
11
9
20
11
F
C)
F
D)
18
11
20
9
F
F
84. Which is the correct symbol for the atom with 42 protons and 49 neutrons?
A)
B)
49
42
91
42
In
C)
Mo
D)
11
91
49
91
42
Mo
In
ID: A
____
85. According to modern atomic theory, it is nearly impossible to determine an electron’s exact
A) color.
C) charge
B) position.
D) mass.
____
86. Which of the following statements not true?
A) Protons have a positive charge.
B) A nucleus has a positive charge.
C) Neutrons have no charge.
D) Neutrons have a negative charge.
____
87. What is an atom’s nucleus made of?
A) protons and neutrons
B) only protons
____
C) only neutrons
D) anodes
88. An iron atom has an atomic mass of 56. Its atomic number is 26. How many neutrons does the iron atom
____
89.
____
90.
____
91.
____
92.
____
93.
____
94.
____
95.
____
96.
have?
A) 30
C) 26
B) 56
D) 82
How much effect do commonly found isotopes have on the average atomic mass of an element?
A) less than rarely found isotopes
C) same as rarely found isotopes
B) no effect on atomic mass
D) more than rarely found isotopes
A mole is an SI base unit that describes the
A) mass of a substance.
C) volume of a substance.
B) amount of a substance.
D) electric charge of a substance.
An atom’s mass number equals the number of
A) protons plus the number of electrons.
B) protons plus the number of neutrons.
C) protons.
D) neutrons.
The organization that is responsible for establishing the rules for naming chemicals as well as overseeing the
verification of new man-made elements is
A) IUC
C) IUPAC
B) CSA
D) Not Listed
A group of chemistry students at Scott high school discovered a new man-made element that was finally
recognized by the IUPAC and they decided to name it after their home state. The resulting symbol would be
A) KY
C) Kyy
B) Ky
D) Ken
While a man-made element is being verified, the IUPAC will give it a designation that
A) uses there letters that represent the
C) actually there isn’t one as it is premature
assigned prefixes for the atomic number
and the IUPAC does not want to look
of the new element
foolish
B) has the finders selecting the two letter
designation that they want
The number of naturally occurring elements is
A) 92
C) 113
B) 115
D) 90
The elements in the last column of the classroom Periodic Table has their symbols written in red which means
A) those elements are dangerous
C) those elements are gases
B) those elements are liquids
D) those elements are solids
12
ID: A
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97. There are many different ways to classify matter, but one way is to use only two categories for ALL
____
98.
____
99.
____ 100.
____ 101.
____ 102.
____ 103.
____ 104.
matter. All matter can be classified as either:
A) solids or liquids.
B) mixtures or substances.
C) atoms or molecules.
D) elements or compounds.
A substance made of two or more elements that cannot be separated by physical means is called a:
A) compound.
B) homogeneous mixture.
C) heterogeneous mixture.
D) multi-element.
Which of the following is true of a heterogeneous mixture?
A) It is not possible to separate the various parts of the mixture.
B) Taking one sample will enable you to determine what it is made of.
C) Different samples may not be exactly alike.
D) The density is the same throughout the entire mixture.
A compound:
A) is made of more than one kind of element.
B) cannot be separated by physical means.
C) is classified as a substance.
D) All of the above are true.
Condensation occurs when:
A) a gas changes to a liquid.
B) a solid changes to a liquid.
C) a liquid changes to a gas.
D) a gas changes to a solid.
Evaporation occurs when:
A) a solid changes to a gas.
B) a gas changes to a liquid.
C) a liquid changes to a solid.
D) a liquid changes to a gas.
Which ONE of the following is a true statement?
A) In the gas state, molecules move around freely.
B) Liquids do not change shape easily.
C) Gas molecules move more slowly as they are heated.
D) Plasma is the most common state of matter found on Earth.
Density is the ratio:
A) mass/weight
B) mass/volume
C) volume/area
D) mass/area
13
ID: A
Short Answer (6 pts.) Answer ONLY one of the two questions - YOUR CHOICE; answer on the ACCOMPANYING
ANSWER SHEET. Failure to follow this direction will result in a 10 point deduction.
105. Explain in detail how you would separate and isolate a mixture of equal volumes of following three liquids
using the properties given below. Make sure you specify what equipment you would use in their isolation and
recovery.
HEXANE- a brown liquid with a density of 2.34 g/mL, miscible in water and kerosene but immiscible in
42 oC; reacts with silver
benzene, methanol and toulene, boiling point of 68 oC and a melting point of
nitrate solution to produce a white precipitate;
BENZENE- a clear liquid with a density of 1.89 g/mL, miscible in water, kerosene and methanol, boiling
point of 76 oC and a melting point of 36 oC; does not react with silver nitrate
METHANOL- a clear liquid with a density of 1.46 g/mL, miscible in water, kerosene and benzene; boils at 92
oC and has a melting point of 36 oC, does not react with silver nitrate
106. You are given a misture containing three solids- you are to explain in detail how you will separate and isolate
each of the solids. Make sure to include the equipment that you will use as part of your detailed answer:
Iron filings- soplid black color, insoluble in water, reacts with hydrochloric cid to produce iron chloride a
yellow precipitate; is attracted by a magnet
Sodium chloride- a white crystalline solid, soluble in water, does not react with hydrochloric acid nor sodium
hydroxide nor is it soluble in either the acid or the hydroxide
Silver chloride- a white crystalline solid that is insoluble in water, reacts with hydrochloric acid to form the
yellow precipitate hexachloro silver chloride.
14
ID: A
CHEM TEST: Introduction to Matter and Energy
Answer Section
MULTIPLE CHOICE
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A
B
A
C
C
C
C
D
A
A
A
C
A
B
C
A
A
A
E
B
E
A
A
E
A
D
C
E
E
A
C
SC-07-1.1.1
B
SC-08-4.6.3
B
D
A
B
C
E
D
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I
I
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I
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1-1.1
1-2.1
1-2.1
1-2.1
1-2.1
1-2.1
1-2.1
1-2.2
1-2.2
1-2.3
1-2.3
1-2.4
1-2.4
1-2.4
1-2.4
1-2.4
1-3.2
1-3.3
DIF: B
DIF: B
OBJ: 3/2
OBJ: 3/2
DIF: B
OBJ: 3/2
1
1
1
1
1
1
1
1
ID: A
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OBJ:
ANS:
OBJ:
ANS:
OBJ:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
NAT:
ANS:
NAT:
C
D
D
B
D
3
C
4
B
2
B
1
D
4
A
3
D
1
D
2
D
3
B
1|2
C
3
D
4
B
1
C
2
B
4
D
2
B
A
A
D
B
C
A
C
UCP.2
B
UCP.2
PTS:
PTS:
PTS:
PTS:
PTS:
1
1
1
1
1
DIF: 1
REF: 1
PTS: 1
DIF: 1
REF: 1
PTS: 1
DIF: 1
REF: 3
PTS: 1
STA: SC.HS.1.1.1
PTS: 1
DIF: 1
REF: 1
DIF: 1
REF: 1
PTS: 1
DIF: 1
REF: 3
PTS: 1
DIF: 1
REF: 3
PTS: 1
DIF: 1
REF: 3
PTS: 1
DIF: 1
REF: 3
PTS: 1
DIF: 1
REF: 3
PTS: 1
DIF: 1
REF: 1
PTS: 1
DIF: 1
REF: 1
PTS: 1
DIF: 1
STA: SC.HS.1.1.1| SC.HS.1.1.5
PTS: 1
DIF: 1
REF: 2
PTS: 1
REF: 1
PTS:
STA:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
STA:
PTS:
STA:
DIF: 1
REF: 1
1
DIF: 1
REF:
SC.HS.1.1.1| SC.HS.1.1.5
1
DIF: B
OBJ:
1
DIF: B
OBJ:
1
DIF: B
OBJ:
1
DIF: B
OBJ:
1
DIF: B
OBJ:
1
DIF: B
OBJ:
1
DIF: B
OBJ:
1
DIF: Bloom's Level 3
SC-HS-1.1.1
1
DIF: Bloom's Level 2
SC-HS-1.1.1
2
2
1/1
1/1
4/2
3/2
3/1
4/1
7/2
ID: A
69. ANS: D
An element is a substance that cannot be broken down into simpler substances by chemical or physical means.
Feedback
A
B
C
D
A compound is a chemical composition of two or more elements.
An element is a substance that cannot be broken down into simpler substances by
chemical or physical means.
A mixture is a physical blend of two or more pure substances in any proportion.
Correct!
PTS: 1
DIF: 1
REF: Page 55
OBJ: 3.1.1 Identify the characteristics of a substance.
NAT: B.2
STA: SC-HS-1.1.1 TOP: Identify the characteristics of a substance.
KEY: Substance
MSC: 1
70. ANS: B
Bromine is the only nonmetallic element that occurs in the liquid state at room temperature.
Feedback
A
B
C
D
71.
72.
73.
74.
75.
76.
77.
78.
79.
Bromine is a nonmetallic element and does not occur in the gaseous state at room
temperature.
Correct!
The plasma state does not occur naturally on Earth except in the form of lightning bolts.
Bromine is a nonmetallic element and does not occur in the solid state at room
temperature.
PTS:
OBJ:
STA:
KEY:
ANS:
NAT:
ANS:
NAT:
ANS:
NAT:
ANS:
NAT:
ANS:
NAT:
ANS:
NAT:
ANS:
NAT:
ANS:
NAT:
ANS:
NAT:
1
DIF: 1
REF: Page 59
3.1.3 Differentiate among the physical states of matter.
NAT: B.2
SC-HS-1.1.1 TOP: Differentiate among the physical states of matter.
Liquids
MSC: 3
D
PTS: 1
DIF: Bloom's Level 3
UCP.2 | B.1 STA: SC-HS-1.1.1 | SC-HS-1.1.2
B
PTS: 1
DIF: Bloom's Level 3
UCP.2 | B.1 STA: SC-HS-1.1.1 | SC-HS-1.1.2
B
PTS: 1
DIF: Bloom's Level 4
UCP.2 | B.1 | G.3
STA: SC-HS-1.1.1 | SC-HS-1.1.2
C
PTS: 1
DIF: Bloom's Level 4
UCP.2 | B.1 | G.3
STA: SC-HS-1.1.1 | SC-HS-1.1.2
B
PTS: 1
DIF: Bloom's Level 2
B.1
STA: SC-HS-1.1.1 | SC-HS-1.1.2
A
PTS: 1
DIF: Bloom's Level 1
B.1
STA: SC-HS-1.1.1 | SC-HS-1.1.2
D
PTS: 1
DIF: Bloom's Level 4
UCP.2 | B.1 STA: SC-HS-1.1.1 | SC-HS-1.1.2
B
PTS: 1
DIF: Bloom's Level 4
UCP.2 | B.1 STA: SC-HS-1.1.1 | SC-HS-1.1.2
B
PTS: 1
DIF: Bloom's Level 3
B.1
STA: SC-HS-1.1.1 | SC-HS-1.1.2
3
ID: A
80. ANS: B
81.
82.
83.
84.
85.
86.
87.
88.
89.
90.
91.
92.
93.
94.
95.
96.
97.
98.
99.
100.
101.
102.
103.
104.
NAT:
ANS:
NAT:
ANS:
NAT:
ANS:
NAT:
ANS:
NAT:
ANS:
OBJ:
ANS:
OBJ:
ANS:
OBJ:
ANS:
OBJ:
ANS:
OBJ:
ANS:
OBJ:
ANS:
OBJ:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
B.1
D
B.1
C
UCP.2 | B.1
D
UCP.2 | B.1
B
UCP.2 | B.1
B
1
D
4
A
4
A
3
D
3
B
4
B
2
C
B
A
D
C
B
A
C
D
A
D
A
B
PTS:
STA:
PTS:
STA:
PTS:
STA:
PTS:
STA:
PTS:
STA:
PTS:
1
DIF: Bloom's Level 3
SC-HS-1.1.1 | SC-HS-1.1.2
1
DIF: Bloom's Level 3
SC-HS-1.1.1 | SC-HS-1.1.2
1
DIF: Bloom's Level 3
SC-HS-1.1.1 | SC-HS-1.1.2
1
DIF: Bloom's Level 3
SC-HS-1.1.1 | SC-HS-1.1.2
1
DIF: Bloom's Level 3
SC-HS-1.1.1 | SC-HS-1.1.2
1
DIF: 1
REF: 3
PTS: 1
DIF: 1
REF: 1
PTS: 1
DIF: 1
REF: 1
PTS:
STA:
PTS:
STA:
PTS:
1
DIF: 1
SC.HS.1.1.1| SC.HS.1.1.2
1
DIF: 1
SC.HS.1.1.1| SC.HS.1.1.2
1
DIF: 1
REF: 2
PTS:
STA:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
1
SC.HS.1.1.1
1
1
1
1
1
1
1
1
1
1
1
1
1
DIF: 1
REF: 2
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
basic
basic
basic
basic
basic
basic
intermediate
basic
REF: 2
REF: 2
chapter 16 | section 16.1
chapter 16 | section 16.1
chapter 16 | section 16.1
chapter 16 | section 16.1
chapter 16 | section 16.3
chapter 16 | section 16.3
chapter 16 | section 16.3
chapter 17 | section 17.1
SHORT ANSWER
105. ANS:
separatory funnel to draw off the lower level hexane; heat the remaining two on a hot plate collecting the
boiling flask to a condenser; heat to a temperature between 80 and 85 oC thereby causing the benzene to boil
off as a vapor leaving the methanol behind. The benzene is recovered as the vapor is changed back to a liquid
as the temperature is lowered in the condenser.
PTS: 1
4
ID: A
106. ANS:
use a magnet to separate the iron from the other two crystals. Add water to the crystals and filter- collect the
insoluble silver chloride in the filter paper; take the filtrate and evaporate to dryness thereby recovering the
sodium chloride
PTS: 1
5