Honors Chemistry
Chapter 6 Review 2016-2017
Name______________________________________ Per______
Equations
c = λν
E=hv
∆E= -2.18x10-18 ( 1/nf2 -1/ni2)
8
-34
c = 3.00x10 m/s
h = 6.63x10 js
λ = hc/E
1m = 109 nm
6.1 The Wave Nature of Light
1. All electromagnetic radiation travels through a vacuum at a speed of _____ m/s.
(A) 186,000
(B) 125
(C) 3.00 x 108
(D) 10,000
(E) it depends on wavelength
2. 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
3. What color of visible light has the highest energy?
(A)
(B)
(C)
(D)
(E)
Violet
Blue
Red
Green
Yellow
4. 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
5. Of the following, __________ radiation has the shortest wavelength.
(A) X-ray
(B) radio
(C) microwave
(D) ultraviolet
(E) infrared
6. 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
Use the following answer choices for questons 7-11.
(A) Molecular vibrations
(B) Molecular bond rotation
(C) Electron transitions
(D) Electron emissions
(E) Nuclear decay
7. UV-VIS radiation results in this type of interaction with matter.
8. Gamma radiation results in this type of interaction with matter.
9. X-Ray radiation results in this type of interaction with matter.
10. Microwave radiation results in this type of interaction with matter.
11. IR radiation results in this type of interaction with matter.
12. The wavelength of light (in nm) 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
13. What is the frequency (s-1) of electromagnetic radiation that has a wavelength of 0.53 m?
(A) 5.7 x 108
(B) 1.8 x 10-9
(C) 1.6 x 108
(D) 1.3 x 10-33
(E) 1.3 x 1033
6.2 Quantized Energy and Photons
14. 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
15. 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
16. 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
17. A mole of photons of wavelength 725 nm has ______ kJ of energy.
(A) 2.74 x 10-19
(B) 4.56 x 10-46
(C) 6.05 x 10-3
(D) 165
(E) 227
6.3 Line Spectra and the Bohr Model
18. 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
19. In the Bohr model of the atom, an electron in an orbit has a fixed _____.
(A) position
(B) energy
(C) color
20. Emission of light from an atom occurs when the electron _____.
(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
21. Which of the following quantum leaps would be associated with the greatest energy of emitted light?
(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
22. Calculate the energy (J) change associated with an electron transition from n = 5 to n = 2 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
23. The n = 2 to n = 6 transition in the Bohr hydrogen atom corresponds to the _________ of a photon with a
wavelength of ______ nm.
(A) emission, 411
(B) absorption, 411
(C) absorption, 657
(D) emission, 93.8
(E) emission, 389
6.4 The Wave Behavior of Matter
24. The de Broglie wavelength of an electron is 8.7 x 10-11 m. The mass of this electron is 9.1 x 10-31 kg. The
velocity of this electron is _____ m/s.
(A) 8.4 x 103
(B) 1.2 x 10-7
(C) 6.9 x 10-54
(D) 8.4 x 106
(E) 8.4 x 10-3
6.5 Quantum Mechanics and Atomic Orbitals
25. According to the Heisenberg 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. Which one of the following is an incorrect subshell notation?
(A) 4f
(B) 2d
(C) 3s
(D) 2p
(E) 3d
27. Which of the following energy levels has the lowest energy?
(A) 4f
(B) 4s
(C) 4p
(D) 3d
28. The letter "p" in the symbol 4p3 indicates the _____.
(A) principle energy level
(B) spin of an electron
(C) subshell (orbital shape)
(D) speed of an electron
6.6 Representations of Orbitals
29. In a px orbital, the subscript x denotes the __________ of the electron.
(A) energy
(B) spin of the electrons
(C) probability of the shell
(D) size of the orbital
(E) axis along which the orbital is aligned
30. The __________ orbital is degenerate with 5py in a many-electron atom.
(A) 5s
(B) 5px
(C) 4py
(D) 5dxy
(E) 5d2
31. __________-orbitals are spherically symmetrical.
(A) s
(B) p
(C) d
(D) f
(E) g
6.7 Many Electron Atoms
32. At maximum, an f-subshell can hold __________ electrons, a d-subshell can hold __________ electrons,
and a p-subshell can hold __________ electrons.
(A) 14, 10, 6
(B) 2, 8, 18
(C) 14, 8, 2
(D) 2, 12, 21
(E) 2, 6, 10
33. Which electron configuration represents a violation of the Pauli Exclusion Principle?
(A)
(B)
(C)
(D)
(E)
6.8 Electron Configurations
34. Which electron configuration represents a violation of Hund's rule for an atom in its ground state?
(A)
(B)
(C)
(D)
(E)
35. 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
36. What is the electron configuration of potassium?
(A) 1s22s22p103s23p3
(B) 1s22s23s23p63d1
(C) 1s22s22p23s23p24s1
(D) 1s22s22p63s23p64s1
37. The ground state electron configuration of Fe is __________.
(A) 1s22s23s23p63d6
(B) 1s22s22p63s23p64s23d6
(C) 1s22s22p63s23p64s2
(D) 1s22s22p63s23p64s24d6
(E) 1s22s23s23p10
38. [Ar]4s23d104p3 is the electron configuration of a(n) __________ atom.
(A) As
(B) V
(C) P
(D) Sb
(E) Sn
39. The complete electron configuration of gallium, element 31, is __________.
(A) 1s22s22p103s23p104s23d3
(B) 1s22s22p63s23p63d104s24p1
(C) 1s42s42p63s43p64s43d3
(D) 1s42s42p103s43p9
(E) 1s42s42p83s43p84s3
40. 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
41. The ground-state electron configuration of the element __________ is [Kr]5s14d5.
(A) Nb
(B) Mo
(C) Cr
(D) Mn
(E) Tc
42. Which one of the following configurations depicts an excited carbon atom?
(A) 1s22s22p13s1
(B) 1s22s22p3
(C) 1s22s22p1
(D) 1s22s23s1
(E) 1s22s22p2
43. There are _____ unpaired electrons are there in a ground state phosphorus atom.
(A) 0
(B) 1
(C) 2
(D) 3
(E) 4
44. What is the correct, ground-state electron configuration for molybdenum?
(A) [Kr]5s14d10
(B) [Kr]5s24d4
(C) [Kr]5s14d5
(D) [Kr]5s24d5
(E) [Kr]5s24d9
45. The electron configuration of the sulfide ion (S2-) is __________.
(A) [Ne]3s2
(B) [Ne]3s23Pl
(C) [Ne]3s23P4
(D) [Ne]3P2
(E) [Ne]3s23P6
46. What species has the electron configuration [Ar]3d2
(A) Mn2+
(B) Cr2+
(C) V3+
(D) Fe3+
(E) K+
47. What is the electron configuration for the Fe3+ ion?
(A) [Ar]4s13d6
(B) [Ar]4s03d7
(C) [Ar]4s03d5
(D) [Ar]4s23d9
(E) [Ne]3s23p10
6.9 Electron Configurations and the Periodic Table
48. Elements in group __________ have a np6 electron configuration in the outer shell.
(A) 4A
(B) 6A
(C) 7A
(D) 8A
(E) 5A
49. All of the __________ have a valence shell electron configuration ns2.
(A) noble gases
(B) halogens
(C) chalcogens
(D) alkali metals
(E) alkaline earth metals
50. The element that has a valence configuration of 4s1 is __________.
(A) Li
(B) Na
(C) K
(D) Rb
(E) Cs