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Chemistry 2 Atomic Stuff
Matching
Match each item with the correct statement below.
a. proton
d. electron
b. nucleus
e. neutron
c. atom
____
____
____
____
____
1.
2.
3.
4.
5.
the smallest particle of an element that retains the properties of that element
a positively charged subatomic particle
a negatively charged subatomic particle
a subatomic particle with no charge
the central part of an atom, containing protons and neutrons
Match each item with the correct statement below.
a. mass number
d. atomic mass
b. atomic mass unit
e. isotope
c. atomic number
____ 6.
____ 7.
____ 8.
____ 9.
____ 10.
atoms with the same number of protons, but different numbers of neutrons in the nucleus of an atom
the total number of protons and neutrons in the nucleus of an atom
the number of protons in the nucleus of an element
the weighted average of the masses of the isotopes of an element
one-twelfth the mass of a carbon atom having six protons and six neutrons
Match each item with the correct statement below.
a. atomic orbital
d. Heisenberg Uncertainty Principle
b. aufbau principle
e. Pauli exclusion principle
c. electron configuration
____
____
____
____
____
11.
12.
13.
14.
15.
region of high probability of finding an electron
states the impossibility of knowing both velocity and position of a moving particle at the same time
orbitals contain at most, 2 electrons with opposite spin.
tendency of electrons to enter orbitals of lowest energy first
arrangement of electrons around atomic nucleus
Match each item with the correct statement below.
a. atomic emission spectrum
d. photon
b. frequency
e. quantum
c. wavelength
____
____
____
____
____
16.
17.
18.
19.
20.
electromagnetic energy released when an electron falls to its ground state
energy needed to move an electron from one energy level to another
number of wave cycles passing a point per unit of time
distance between wave crests
separation of light into different wavelengths
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
____ 21. Who was the man who lived from 460B.C.–370B.C. and was among the first to suggest the idea of atoms?
a. Atomos
c. Democritus
b. Dalton
d. Thomson
____ 22. Which of the following was NOT among Democritus’s ideas?
a. Matter consists of tiny particles called atoms.
b. Atoms are indivisible.
c. Atoms retain their identity in a chemical reaction.
d. Atoms are indestructible.
____ 23. The smallest particle of an element that retains the properties of that element is a(n) ____.
a. atom
c. proton
b. electron
d. neutron
____ 24. Dalton's atomic theory included which idea?
a. All atoms of all elements are the same size.
b. Atoms of different elements always combine in one-to-one ratios.
c. Atoms of the same element are always identical.
d. Individual atoms can be seen with a microscope.
____ 25. Which of the following is NOT a part of Dalton's atomic theory?
a. All elements are composed of atoms.
b. Atoms are always in motion.
c. Atoms of the same element are identical.
d. Atoms that combine do so in simple whole-number ratios.
____ 26. Dalton hypothesized that atoms are indivisible and that all atoms of an element are identical. It is now known
that ____.
a. all of Dalton's hypotheses are correct
b. atoms of an element can have different numbers of protons
c. atoms are divisible
d. all atoms of an element are not identical but they must all have the same mass
____ 27. Which of the following is true about subatomic particles?
a. Electrons are negatively charged and are the heaviest subatomic particle.
b. Protons are positively charged and the lightest subatomic particle.
c. Neutrons have no charge and are the lightest subatomic particle.
d. The mass of a neutron nearly equals the mass of a proton.
____ 28. Who conducted experiments to determine the quantity of charge carried by an electron?
a. Rutherford
c. Dalton
b. Millikan
d. Thomson
____ 29. All atoms are ____.
a. positively charged, with the number of protons exceeding the number of electrons
b. negatively charged, with the number of electrons exceeding the number of protons
c. neutral, with the number of protons equaling the number of electrons
d. neutral, with the number of protons equaling the number of electrons, which is equal to the
number of neutrons
____ 30. The particles that are found in the nucleus of an atom are ____.
a. neutrons and electrons
c. protons and neutrons
b. electrons only
d. protons and electrons
____ 31. The nucleus of an atom is ____.
a. the central core and is composed of protons and neutrons
b. positively charged and has more protons than neutrons
____ 32.
____ 33.
____ 34.
____ 35.
____ 36.
____ 37.
____ 38.
____ 39.
c. negatively charged and has a high density
d. negatively charged and has a low density
The atomic number of an element is the total number of which particles in the nucleus?
a. neutrons
c. electrons
b. protons
d. protons and electrons
An element has an atomic number of 76. The number of protons and electrons in a neutral atom of the
element are ____.
a. 152 protons and 76 electrons
c. 38 protons and 38 electrons
b. 76 protons and 0 electrons
d. 76 protons and 76 electrons
The sum of the protons and neutrons in an atom equals the ____.
a. atomic number
c. atomic mass
b. nucleus number
d. mass number
All atoms of the same element have the same ____.
a. number of neutrons
c. mass numbers
b. number of protons
d. mass
Isotopes of the same element have different ____.
a. numbers of neutrons
c. numbers of electrons
b. numbers of protons
d. atomic numbers
Isotopes of the same element have different ____.
a. positions on the periodic table
c. atomic numbers
b. chemical behavior
d. mass numbers
In which of the following sets is the symbol of the element, the number of protons, and the number of
electrons given correctly?
a. In, 49 protons, 49 electrons
c. Cs, 55 protons, 132.9 electrons
b. Zn, 30 protons, 60 electrons
d. F, 19 protons, 19 electrons
The mass number of an element is equal to ____.
a. the total number of electrons in the nucleus
b. the total number of protons and neutrons in the nucleus
c. less than twice the atomic number
d. a constant number for the lighter elements
____ 40. Using the periodic table, determine the number of neutrons in O.
a. 4
c. 16
b. 8
d. 24
____ 41. How many protons, electrons, and neutrons does an atom with atomic number 50 and mass number 125
contain?
a. 50 protons, 50 electrons, 75 neutrons
c. 120 neutrons, 50 protons, 75 electrons
b. 75 electrons, 50 protons, 50 neutrons
d. 70 neutrons, 75 protons, 50 electrons
____ 42. Which of the following statements is NOT true?
a. Atoms of the same element can have different masses.
b. Atoms of isotopes of an element have different numbers of protons.
c. The nucleus of an atom has a positive charge.
d. Atoms are mostly empty space.
____ 43. How is the number of neutrons in the nucleus of an atom calculated?
a. Add the number of electrons and protons together.
b. Subtract the number of electrons from the number of protons.
c. Subtract the number of protons from the mass number.
d. Add the mass number to the number of electrons.
____ 44. How do the isotopes hydrogen-1 and hydrogen-2 differ?
____ 45.
____ 46.
____ 47.
____ 48.
____ 49.
____ 50.
____ 51.
____ 52.
____ 53.
____ 54.
____ 55.
____ 56.
a. Hydrogen-2 has one more electron than hydrogen-1.
b. Hydrogen-2 has one neutron; hydrogen-1 has none.
c. Hydrogen-2 has two protons; hydrogen-1 has one.
d. Hydrogen-2 has one proton; hydrogen-1 has none.
What unit is used to measure weighted average atomic mass?
a. amu
c. angstrom
b. gram
d. nanogram
Which of the following equals one atomic mass unit?
a. the mass of one electron
b. the mass of one helium-4 atom
c. the mass of one carbon-12 atom
d. one-twelfth the mass of one carbon-12 atom
Which of the following statements is NOT true?
a. Protons have a positive charge.
b. Electrons are negatively charged and have a mass of 1 amu.
c. The nucleus of an atom is positively charged.
d. Neutrons are located in the nucleus of an atom.
The atomic mass of an element is the ____.
a. total number of subatomic particles in its nucleus
b. weighted average of the masses of the isotopes of the element
c. total mass of the isotopes of the element
d. average of the mass number and the atomic number for the element
The atomic mass of an element depends upon the ____.
a. mass of each electron in that element
b. mass of each isotope of that element
c. relative abundance of protons in that element
d. mass and relative abundance of each isotope of that element
In Bohr's model of the atom, where are the electrons and protons located?
a. The electrons move around the protons, which are at the center of the atom.
b. The electrons and protons move throughout the atom.
c. The electrons occupy fixed positions around the protons, which are at the center of the
atom.
d. The electrons and protons are located throughout the atom, but they are not free to move.
In the Bohr model of the atom, an electron in an orbit has a fixed ____.
a. position
c. energy
b. color
d. size
How does the energy of an electron change when the electron moves closer to the nucleus?
a. It decreases.
c. It stays the same.
b. It increases.
d. It doubles.
The principal quantum number indicates what property of an electron?
a. position
c. energy level
b. speed
d. electron cloud shape
How many energy sublevels are in the second principal energy level?
a. 1
c. 3
b. 2
d. 4
What is the maximum number of f orbitals in any single energy level in an atom?
a. 1
c. 5
b. 3
d. 7
What is the maximum number of d orbitals in a principal energy level?
a. 1
c. 3
b. 2
d. 5
____ 57. What is the maximum number of orbitals in the p sublevel?
a. 2
c. 4
b. 3
d. 5
____ 58. What is the maximum number of electrons in the second principal energy level?
a. 2
c. 18
b. 8
d. 32
____ 59. When an electron moves from a lower to a higher energy level, the electron ____.
a. always doubles its energy
b. absorbs a continuously variable amount of energy
c. absorbs a quantum of energy
d. moves closer to the nucleus
____ 60. The letter "p" in the symbol 4p indicates the ____.
a. spin of an electron
c. principle energy level
b. orbital shape
d. speed of an electron
____ 61. If the spin of one electron in an orbital is clockwise, what is the spin of the other electron in that orbital?
a. zero
c. counterclockwise
b. clockwise
d. both clockwise and counterclockwise
____ 62. What types of atomic orbitals are in the third principal energy level?
a. s and p only
c. s, p, and d only
b. p and d only
d. s, p, d, and f
____ 63. What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p?
a. 2d
c. 3f
b. 3d
d. 4s
____ 64. According to the aufbau principle, ____.
a. an orbital may be occupied by only two electrons
b. electrons in the same orbital must have opposite spins
c. electrons enter orbitals of highest energy first
d. electrons enter orbitals of lowest energy first
____ 65. What is the number of electrons in the outermost energy level of an oxygen atom?
a. 2
c. 6
b. 4
d. 8
____ 66. What is the electron configuration of potassium?
a. 1s 2s 2p 3s 3p 4s
c. 1s 2s 3s 3p 3d
b. 1s 2s 2p 3s 3p
d. 1s 2s 2p 3s 3p 4s
____ 67. If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in
the three orbitals?
a. one electron in each orbital
b. two electrons in one orbital, one in another, none in the third
c. three in one orbital, none in the other two
d. Three electrons cannot fill three empty 2p atomic orbitals.
____ 68. How many unpaired electrons are in a sulfur atom (atomic number 16)?
a. 0
c. 2
b. 1
d. 3
____ 69. How many half-filled orbitals are in a bromine atom?
a. 1
c. 3
b. 2
d. 4
____ 70. Stable electron configurations are likely to contain ____.
a. filled energy sublevels
b. fewer electrons than unstable configurations
c. unfilled s orbitals
d. electrons with a clockwise spin
____ 71. Which electron configuration of the 4f energy sublevel is the most stable?
a. 4f
c. 4f
b. 4f
d. 4f
____ 72. How does the speed of visible light compare with the speed of gamma rays, when both speeds are measured
in a vacuum?
a. The speed of visible light is greater.
b. The speed of gamma rays is greater.
c. The speeds are the same.
d. No answer can be determined from the information given.
____ 73. Which color of visible light has the shortest wavelength?
a. yellow
c. blue
b. green
d. violet
____ 74. Which of the following electromagnetic waves have the highest frequencies?
a. ultraviolet light waves
c. microwaves
b. X-rays
d. gamma rays
____ 75. How are the frequency and wavelength of light related?
a. They are inversely proportional to each other.
b. Frequency equals wavelength divided by the speed of light.
c. Wavelength is determined by dividing frequency by the speed of light.
d. They are directly proportional to each other.
____ 76. What is the wavelength of an electromagnetic wave that travels at 3
MHz? (1 MHz = 1,000,000 Hz)
a.
b. 60 MHz
c.
10 m/s and has a frequency of 60
300,000,000 m/s
d. No answer can be determined from the information given.
____ 77. Emission of light from an atom occurs when an electron ____.
a. drops from a higher to a lower energy level
b. jumps from a lower to a higher energy level
c. moves within its atomic orbital
d. falls into the nucleus
____ 78. The atomic emission spectra of a sodium atom on Earth and of a sodium atom in the sun would be ____.
a. the same
b. different from each other
c. the same as those of several other elements
d. the same as each other only in the ultraviolet range
____ 79. Which variable is directly proportional to frequency?
a. wavelength
c. position
b. velocity
d. energy
____ 80. How do the energy differences between the higher energy levels of an atom compare with the energy
differences between the lower energy levels of the atom?
a. They are greater in magnitude than those between lower energy levels.
b. They are smaller in magnitude than those between lower energy levels.
c. There is no significant difference in the magnitudes of these differences.
d. No answer can be determined from the information given.
____ 81. What are quanta of light called?
a. charms
c. muons
b. excitons
d. photons
____ 82. Which scientist developed the quantum mechanical model of the atom?
a. Albert Einstein
c. Niels Bohr
b. Erwin Schrodinger
d. Ernest Rutherford
____ 83. Who predicted that all matter can behave as waves as well as particles?
a. Albert Einstein
c. Max Planck
b. Erwin Schrodinger
d. Louis de Broglie