Transcript Document
Chem I
Semester 1 Review
All of the following are general characteristics of a substance in the liquid state except
A. definite volume. B. not easily compressed.
C. able to flow.
D. definite shape.
A.
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In the chemical reaction iron plus oxygen →iron oxide,
A. iron oxide is a reactant.
B. oxygen is a product.
C. iron is a reactant. D. iron is a product.
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Which term does not fit with the others listed?
A. Solid B. Gas C. Reactant D. Liquid 0% A.
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The chemical symbol for sodium is
A. NA. B. SO.
C. Na.
D. So.
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A basketball has more mass than a golf ball because:
A. the basketball takes up more space.
B. the basketball contains more matter.
C. the golf ball contains a different kind of matter.
D. the golf ball has an indefinite composition.
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B.
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A gas is a form of matter that
A. has a definite volume.
B. is generally a liquid or solid at room temperature.
C. takes the shape and volume of its container.
D. is difficult to compress.
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Homogeneous mixtures
A. are always liquids.
B. consist of two or more phases.
C. have a composition that is fixed.
D. are known as solutions.
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A compound
A. is a pure substance.
B. has a composition that varies.
C. can be physically separated into its elements.
D. has properties similar to those of its elements.
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Physical properties of a substance include
A. color and odor. B. malleability.
C. melting & boiling points.
D. all of the above.
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When iron and oxygen combine to form iron oxide,
A. a physical change occurs. B. a change of state occurs. C. a change in mass occurs.
D. a chemical change occurs.
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How many significant figures are in the measurement 2103.2 g?
A. 2 B. 4 C. 5 D. 3 0% A.
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Which of these equalities is not correct?
A. 10 kg= 1 g B. 100 cg= 1 g C. 1 cm 3 = 1 mL D. 1000 mm= 1 m 0% A.
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How many of the zeros in the measurement 0.000 040 200 m are significant?
A. 2 B. 7 C. 3 D. 8 0% A.
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How many milligrams are in 2.5 kg?
A. 2.5 x 10 6 mg B. 2.5 x 10 4 mg C. 25 mg D. 2.5 x 10 2 mg 0% A.
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The closeness of a measurement to its true value is a measure of its:
A. usefulness. B. accuracy.
C. precision. D. reproducibility.
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Which of these measurements is expressed to three significant figures?
A. 0.070 mm B. 7007 mg C. 7.30 x 10 7 km D. 0.007 m E. both C and D 0% A.
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A. L.
B. km.
C. mg.
D. K.
A metric unit of volume is the:
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The number of seconds in a 40-hour work week can be calculated as follows: A.
60
s
1min 60
s
1
hr
60min 1
s
B.
1min 60
s
1
hr
60 min C.
40
hr
60min 1
hr
60
s
1min D.
40
hr
60 min 40
hr
60
s
60 min
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The metric prefix kilo- means:
A. 100 times smaller. B. 1000 times smaller.
C. 1000 times larger.
D. 100 times larger.
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What is the volume of 60.0 g of ether if the density of ether is 0.70 g/mL?
A. 86 mL B. 2.4 x10 2 mL C. 1.2 x 10 2 mL D. 42 mL 0% A.
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Concentrated hydrochloric acid has a density of 1.19 g/mL. What is the mass, in grams, of 2.00 liters of this acid?
A. 2.38 x 10 3 g B. 4.20 x 10 -4 g C. 2.38 g D. 4.20 x 10 4 g 0% A.
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A conversion factor:
A. is equal to 1.
B. is a ratio of equivalent measurements.
C. does not change the value of a measurement.
D. all of the above 0% A.
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Which of the following is not a part of Dalton’s atomic theory?
A. All elements are composed of atoms.
B. Atoms of the same element are alike.
C. Atoms are always in motion.
D. Atoms that combine do so in simple whole number ratios.
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The nucleus of an atom is
A. negatively charged and has a low density.
B. negatively charged and has a high density.
C. positively charged and has a low density.
D. positively charged and has a high density.
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Dalton theorized that atoms are indivisible and that all atoms of an element are identical. Scientists now know that
A. Dalton’s theories are completely correct.
B. atoms of an element can have different numbers of protons.
C. atoms are all divisible.
D. all atoms of an element are not identical but they all have the same
mass.
A.
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The number of neutrons in the nucleus of an atom can be calculated by A. adding together the numbers of electrons and protons.
B. subtracting the number of protons from the mass number.
C. subtracting the number of protons from the number of electrons.
D. adding the mass number to the number of protons.
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The sum of the protons and neutrons in an atom equals the
A. atomic number.
B. atomic mass.
C. number of electrons.
D. mass number.
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All atoms of the same element have the same:
A. number of protons.
B. mass number.
C. number of neutrons.
D. mass.
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Which of these statements is false?
A. Electrons have a negative charge.
B. Electrons have a mass of 1 amu.
C. The nucleus of an atom is positively charged.
D. The neutron is found in the nucleus of an atom.
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An atom of an element with atomic number 48 and mass number 120 contains A. 48 protons, 48 electrons, and 72 neutrons.
B. 72 protons, 48 electrons, and 48 neutrons.
C. 120 protons, 48 electrons, and 72 neutrons.
D. 72 protons, 72 electrons, and 48 neutrons.
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The number 80 in the name bromine-80 represents
A. the atomic number.
B. the mass number.
C. the sum of protons and electrons.
D. none of the above 0% A.
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Which of these statements is not true?
A. Atoms of the same elements can have different masses.
B. The nucleus of an atom has a positive charge.
C. Atoms of isotopes of an element have different numbers of protons.
D. Atoms are mostly empty space.
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If E is the symbol for an element, which two of the following symbols represent isotopes of the same element?
24 1.
12
E
24 2.
13
E
25 3.
11
E
25 4.
12
E
A. 1 and 2 B. 3 and 4 C. 1 and 4 D. 2 and 3
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The fourth principal energy level has
A. 4 orbitals.
B. 32 orbitals.
C. 16 orbitals.
D. 9 orbitals.
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If the electron configuration of an element is 1s
2 2s 2 2p 6 3s 2 3p 5
, the element is
A. iron.
B. chlorine.
C. bromine.
D. phosphorus.
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The electron configuration of calcium is
A. 1s
2 2s 2 2p 2 3s 2 3p 3 4s 2 .
B. 1s
2 2s 2 2p 10 3s 2 3p 4 . C. 1s 2 2s 2 3s 2 3p 6 3d 8 .
D. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 .
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The maximum number of electrons that can occupy the third principal energy level is
A. 18. B. 2.
C. 32.
D. 8.
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As the frequency of light increases, the wavelength
A. increases. B. remains the same. C. decreases.
D. approaches the speed of light.
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In order to occupy the same orbital, two electrons must have
A. the same direction of spin.
B. low energy. C. opposite charge.
D. opposite spin.
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Stable electron configurations are likely to contain
A. high-energy electrons.
B. unfilled s orbitals. C. fewer electrons than unstable configurations.
D. filled energy sublevels.
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According to Hund’s rule, when electrons occupy orbitals of equal energy, one electron enters each orbit until
A. all the orbitals contain one electron, with spins parallel.
B. all the orbitals contain one electron, with opposite spins.
C. there are two electrons in each orbital.
D. electron velocities become constant.
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In the periodic table, there is a periodic pattern in the physical and chemical properties of elements when they are arranged in order of
A. increasing atomic mass.
B. increasing electronegativity.
C. increasing atomic number.
D. increasing atomic radius.
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Which sublevel corresponds to the transition metals in the periodic table?
A. s B. p C. d D. f
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Which of the following elements is a metalloid?
A. Br B. Se C. As D. Kr 0% A.
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The element iodine, I, is a
A. period 5 alkali metal. B. period 4 halogen. C. period 5 halogen.
D. period 5 transition metal.
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The subatomic particle that plays the greatest role in determining the physical and chemical properties of an element is the
A. proton.
B. electron.
C. neutron. D. photon.
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Which of the following atoms would you expect to have the largest atomic radius?
A. I B. K C. Rb D. Ca 0% A.
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From left to right across the second period of the periodic table,
A. first ionization energy increases. B. atomic radii increase. C. electronegativity decreases.
D. atomic mass decreases.
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The category of elements that is characterized by the filling of f orbitals is the
A. inner transition metals. B. alkali metals. C. alkali earth metals.
D. transition metals.
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Electronegativity
A. generally decreases from left to right across a period.
B. is the energy change that accompanies the loss of an electron from a gaseous atom.
C. generally decreases from top to bottom within a group.
D. is generally higher for metals than for nonmetals.
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Atomic size generally
A. increases from left to right across a period.
B. decreases from top to bottom within a group.
C. remains constant within a period.
D. decreases from left to right across a period.
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A. Li. B. Na.
C. Ca. D. Rb.
The alkali metals do not include
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How many valence electrons does an atom of any element in Group 16 have?
A. 2 B. 6 C. 4 D. 8 0% A.
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The electron dot structure for an atom of phosphorus is A.
B.
C.
D.
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When an aluminum atom loses its valence electrons, what is the charge on the resulting ion?
A. 2+ B. 3+ C. 2 D. 1+ 0% A.
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15 • • • • • The high surface tension of water is due to the: a. small size of water molecules.
b. low mass of water molecules.
c. hydrogen bonding between water molecules.
d. covalent bonds in water molecules.
c.
The electron configuration of a fluoride ion, F , is
A. 1s
2 2s 2 2p 5 .
B. the same as that of the neon atom.
C. 1s
2 2s 2 2p 6 3s 1 .
D. the same as that of a potassium ion.
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In forming chemical bonds, atoms tend to attain A. the electron configuration of noble gas atoms.
B. a state of higher energy.
C. the electron configuration of halogen atoms.
D. all of the above
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C.
D.
An ionic compound is A. electrically neutral. B. held together by ionic bonds. C. composed of anions and cations.
D. all of the above
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A cation is any atom or group of atoms with A. a positive charge.
B. no charge.
C. a negative charge.
D. more electrons than the corresponding atoms.
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The cation Fe 3+ is formed when A. an atom of iron loses two electrons.
B. an atom of zinc loses two electrons.
C. an atom of iron loses three electrons.
D. an atom of iron gains three electrons.
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Which of these elements does not exist as
a diatomic molecule?
A. H B. F C. He D. I 0% A.
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Which one of the following compounds is
not covalent?
A. HCl B. KCl C. SCl 2 D. S 2 Cl 2 0% A.
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How many valence electrons does an atom of any halogen have?
A. 4 B. 2 C. 1 D. 7 0% A.
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If a bonding pair of electrons is unequally shared between two atoms, the bond is
A. ionic. B. coordinate covalent.
C. nonpolar covalent. D. polar covalent.
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A covalent bond forms A. when an element becomes a noble gas.
B. when atoms share electrons.
C. between metals and nonmetals.
D. when electrons are transferred from one atom to another.
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The correct name for the N 3 ion is the:
A. nitrate ion. B. nitride ion.
C. nitric ion. D. nitrite ion.
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A molecular formula: A. gives information about molecular geometry.
B. can be written for ionic compounds.
C. shows the number and kinds of atoms in a molecule of a compound.
D. uses superscripts to show the number of atoms of each kind.
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The metals in Groups 1A, 2A, and 3A:
A. gain electrons when they form ions.
B. form ions with a charge found by subtracting 8 from the group number.
C. all form ions with a 1 charge.
D. lose electrons when they form ions.
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Which of the following is not an empirical formula?
A. Na 2 SO 4 B. N 2 H 4 C. C 6 H 5 Cl D. Sn 3 (PO 4 ) 4
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