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Advanced Chemistry
Chapter 13 Review
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Wave Properties
1) Which one of the following is correct?
A) ν + λ = c
B) ν ÷ λ = c
C) ν = cλ
D) λ = c ν
E) νλ = c
2) The energy of a photon of light is __________ proportional to its frequency and __________
proportional to its wavelength.
A) directly, directly
B) inversely, inversely
C) inversely, directly
D) directly, inversely
E) indirectly, not
3) The wavelength of light that has a frequency of 1.66 × 109s-1 is __________ m.
A) 0.181
B) 5.53
C) 2.00 x 10-9
D) 5.53 x 108
E) none of the above
4) The wavelength of light emitted from a traffic light having a frequency of 5.75 × 1014 Hz is
__________.
A) 702 nm
B) 641 nm
C) 674 nm
D) 522 nm
E) 583 nm
5) The energy of a photon that has a frequency of 8.21 × 1015 s-1 is __________ J.
A) 8.08 × 10-50
B) 1.99 × 10-25
C) 5.44 × 10-18
D) 1.24 × 1049
E) 1.26 × 10-19
6) What is the frequency (s-1) of a photon that has an energy of 4.38 × 10-18 J?
A) 436
B) 6.61 × 1015
C) 1.45 × 10-16
D) 2.30 × 107
E) 1.31 × 10-9
7) Electromagnetic radiation with a wavelength of 525 nm appears as green light to the human
eye. The frequency of this light is __________ sl.
A) 5.71 × 1014
B) 5.71 × 105
C) 1.58 × 102
D) 1.58 × 1011
E) 1.75 × 10-15
8) Electromagnetic radiation with a wavelength of 525 nm appears as green light to the human
eye. The energy of one photon of this light is __________ J.
A) 1.04 × 10-31
B) 3.79 × 10-28
C) 3.79 × 10-19
D) 1.04 × 10-22
E) 2.64 × 1018
9) Of the following, __________ radiation has the shortest wavelength.
A) X-ray
B) radio
C) microwave
D) ultraviolet
E) infrared
10) How does the speed of visible light compare with the speed of gamma rays, when both
speeds are measured in a vacuum?
A) The speeds are the same.
B) The speed of visible light is greater.
C) The speed of gamma rays is greater.
D) No definite statement can be made on this question.
11) The amplitude of a wave is the measure of the _____.
A) number of particles in a wave front
B) number of cycles per unit time
C) height from origin to crest
D) distance between crests
12) Which of the following electromagnetic waves have the highest frequencies?
A) ultraviolet light waves
B) gamma rays
C) x-rays
D) infrared light waves
E) microwaves
13) The photoelectric effect is __________.
A) the total reflection of light by metals giving them their typical luster
B) the production of current by silicon solar cells when exposed to sunlight
C) the ejection of electrons by a metal when struck with light of sufficient energy
D) the darkening of photographic film when exposed to an electric field
E) a relativistic effect
Bohr Model/Line Spectra
14) In the Bohr model of the atom, __________.
A) electrons travel in circular paths called orbitals
B) electrons can have any energy
C) electron energies are quantized
D) electron paths are controlled by probability
E) both A and C
15) In Bohr's model of the atom, where are the electrons and protons located?
A) The electrons orbit the protons, which are at the center of the atom.
B) The electrons and protons move throughout the atom.
C) The electrons and protons are located throughout the atom, but they are not free to move.
D) The electrons occupy fixed positions around the protons, which are at the center of the atom.
16) In the Bohr model of the atom, an electron in an orbit has a fixed _____.
A) position
B) energy
C) color
17) When an electron moves from a lower to a higher energy level, the electron _____.
A) absorbs a continuously variable amount of energy
B) always doubles its energy
C) moves closer to the nucleus
D) absorbs a quantum of energy
18) The lowest energy state of an atom is called the _____.
A) configurational state
B) ground state
C) dependent state
D) independent state
E) excited state
19) Emission of light from an atom occurs when the electron _____.
62) ______
A) drops from a higher to a lower energy level
B) falls into the nucleus
C) jumps from a lower to a higher energy level
D) moves within its atomic orbital
20) Which of the following quantum leaps would be associated with the greatest energy of
emitted light? 64) ______
A) n = 1
B) n = 2
C) n = 5
D) n = 5
E) n = 5
to
to
to
to
to
n=5
n=5
n=1
n=3
n=2
21) Calculate the energy (J) change associated with an electron transition from n = 2 to n = 5 in a
Bohr hydrogen atom.
A) 6.5 × 10-19
B) 5.5 × 10-19
C) 8.7 × 10-20
D) 4.6 × 10-19
E) 5.8 × 10-53
22) When the electron in a hydrogen atom moves from n = 4 to n = 2, light with a wavelength of
__________ nm is emitted.
A) 93.8
B) 434
C) 410
D) 657
E) 486
Quantum Model/Quantum Numbers
23) Which one of the following represents an acceptable set of quantum numbers for an electron
in an atom? (arranged as n, l, ml, and ms)
A) 2, 2, -1, -1/2
B) 1, 0, 0, 1/2
C) 3, 3, 3, 1/2
D) 5, 4,- 5, 1/2
E) 3, 3, 3, -1/2
24) An electron cannot have the quantum numbers n = __________, l = __________, ml =
__________.
A) 6, 1, 0
B) 3, 2, 3
C) 3, 2, -2
D) 1, 0, 0
E) 3, 2, 1
25) According to the uncertainty principle, if the position of a moving particle is known, what
other quantity cannot be known?
A) temperature
B) spin
C) mass
D) charge
E) velocity
26) All of the orbitals in a given electron shell have the same value of the __________ quantum
number.
A) principal
B) angular momentum
C) magnetic
D) spin
E) psi
27) According to the Heisenberg Uncertainty Principle, it is impossible to know precisely both
the position and the __________ of an electron.
A) mass
B) color
C) momentum
D) shape
E) charge
28) Which of the following energy levels has the lowest energy?
A) 4f
B) 4s
C) 4p
D) 3d
29) The letter "p" in the symbol 4p3 indicates the _____.
A) principle energy level
B) spin of an electron
C) orbital shape
D) speed of an electron
30) Which one of the following is an incorrect subshell notation?
A) 4f
B) 2d
C) 3s
D) 2p
E) 3d
Electron Configurations/Oribital Diagrams
31) If the spin of one electron in an orbital is clockwise, what is the spin of the other electron in
that orbital?
A) clockwise
B) counterclockwise
C) zero
32) Which of the following states that no more than two electrons can occupy an atomic orbital
and that two electrons in the same orbital must have opposite spins?
A) the Aufbau principle
B) Hund's rule
C) the Pauli exclusion principle
D) Dalton's theory
33) In order to occupy the same orbital, two electrons must have _____.
A) the same direction of spin
B) opposite spin
C) a high quantum number
D) low energy
34) Which electron configuration represents a violation of the Pauli exclusion principle?
A)
B)
C)
D)
E)
35) Which electron configuration represents a violation of Hund's rule for an atom in its ground
state?
A)
B)
C)
D)
E)
36) According to the Aufbau principle _____.
A) electrons enter orbitals of highest energy first
B) electrons in the same orbital must have opposite spins
C) electrons enter orbitals of lowest energy first
D) an orbital may be occupied by only two electrons
37) The element that has a valence configuration of 4s1 is __________.
A) Li
B) Na
C) K
D) Rb
E) Cs
38) What is the electron configuration of potassium?
A) 1s22s22p103s23p3
B) 1s22s23s23p63d1
C) 1s22s22p23s23p24s1
D) 1s22s22p63s23p64s1
39) [Ar]4s23d104p3 is the electron configuration of a(n) __________ atom.
A) As
B) V
C) P
D) Sb
E) Sn
40) The complete electron configuration of gallium, element 31, is __________.
A) 1s22s22p103s23p104s23d3
B) 1s22s22p63s23p63d104s24p1
C) 1s42s42p63s43p64s43d3
D) 1s42s42p103s43p9
E) 1s42s42p83s43p84s3
41) The lowest energy state of an atom is called the________.
A) excited state
B) dependent state
C) independent state
D) ground state
E) configurational state
42) The highest energy state of an atom is called the________.
A) excited state
B) dependent state
C) independent state
D) ground state
E) configurational state
43) Which one of the following is the correct electron configuration for a ground-state nitrogen
atom?
A)
B)
C)
D)
E) None of the above is correct.
Historical Figures
44) Who predicted that all matter can behave as waves as well as particles?
A) Albert Einstein
B) Erwin Schrodinger
C) Louis de Broglie
D) Max Planck
E) Niels Bohr
45) Who developed the uncertainty principle?
A) Louis de Broglie
B) Albert Einstein
C) Werner Heisenberg
D) Erwin Schrodinger
E) Niels Bohr
46) Who related energy (E) to frequency (v)?
A) Louis de Broglie
B) Max Planck
C) Werner Heisenberg
D) Erwin Schrodinger
E) Niels Bohr
47) Who solved the wave function (Ψ) showing a region of electron probability (orbitals shapes)
as a solution?
A) Louis de Broglie
B) Max Planck
C) Werner Heisenberg
D) Erwin Schrodinger
E) Niels Bohr