CHAPTER 3
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
____
____
1. Which object(s) would you use to describe the shape of the 2p orbital?
a. a dumb-bell
b. a circle
c. a sphere
d. two perpendicular dumb-bells
e. a doughnut
2. Which situation must be true for two electrons to occupy the same orbital?
a. The electrons must have the same principal quantum number, but the other quantum
numbers must be different.
b. The electrons must have the same spin.
c. The electrons must have identical sets of quantum numbers.
d. The electrons must have low energy.
e. The electrons must have the opposite spin.
____
3. An electron has the following set of quantum numbers: n = 3, l = 1, ml = 1, ms =
____
____
this electron found?
a. 3s
b. 3p
c. 3d
d. 3f
e. 4p
4. Which element contains a full 3s orbital?
a. B
b. Na
c. Mg
d. Be
e. Ne
5. Which set of quantum numbers is not possible?
a.
n = 3, l = 0, ml = 0, ms =
b.
n = 5, l = 3, ml = 2, ms =
c.
n = 4, l = 3, ml = -1, ms =
d.
n = 5, l = 3, ml = -3, ms =
e.
____
n = 4, l = 4, ml = 2, ms =
6. Which set of quantum numbers is not possible?
a.
n = 5, l = 3, ml = 0, ms =
. In which orbital is
b.
n = 1, l = 0, ml = 0, ms =
c.
n = 3, l = 2, ml = 1, ms =
d.
n = 4, l = 3, ml = -3, ms =
e.
____
____
____
____
____
____
n = 5, l = 2, ml = 0, ms =
7. Which scientist postulated that electrons can only move between certain energy levels?
a. Rutherford
b. Dalton
c. Einstein
d. Schodinger
e. Bohr
8. Which element has the ground state electron configuration [Ne] 3s2 3px13py1 for its valence electrons?
a. Mg
b. Al
c. Si
d. P
e. S
9. Which electron configuration represents a reactive non-metallic element?
a. 1s2 2s2 2p6 3s2 3p5
b. 1s2 2s2 2p6 3s2 3p1
c. 1s2 2s2 2p6 3s2
d. 1s2 2s2 2p6 3s2 3p6
e. 1s2 2s2 2p6 3s2 3p6 4s2
10. How many p orbitals are in each energy level, except n = 1?
a. 1
b. 3
c. 5
d. 6
e. 7
11. What is the maximum number of electrons in n = 3?
a. 2
b. 3
c. 6
d. 9
e. 18
12. What is the total number of electrons in the 2p orbitals of a sulfur atom at ground state?
a. 8
b. 6
c. 4
d. 3
e. 2
____ 13. Which sublevel, when full, corresponds to the first row of transition elements?
a. 3d
b. 3f
c. 4d
d. 4f
e. 4p
____ 14. Which sublevel, when full, corresponds to the lanthanide series of elements?
a. 3d
b. 3f
c. 4d
d. 4f
e. 5f
____ 15. Which pair of atoms and/or ions is isoelectronic?
a. O2- and Clb. Ca2+ and Clc. F- and N2d. Li+ and Na+
e. K+ and Kr
____ 16. How does atomic radius change from left to right across a period in the periodic table?
a. It increases.
b. It decreases.
c. It stays the same.
d. It increases and then decreases.
e. It decreases and then increases.
____ 17. Which atom or ion is isoelectric with Ar?
a. Ca2+
b. K
c. Sd. P2e. Cl
____ 18. Which element has the highest electron affinity?
a. Li
b. N
c. O
d. F
e. Ni
____ 19. Which metal is the most reactive?
a. Al
b. K
c. Cu
d. Zn
e. Ca
____ 20. Which element has the largest atomic radius?
a. Mg
b. Be
c. F
d. Cl
e. Si
____ 21. Which element has the smallest effective nuclear charge?
a. Al
b. S
c. I
d. Be
e. Na
____ 22. Which element has the lowest first ionization energy?
a. Ca
b. Cs
c. Br
d. O
e. Ba
____ 23. The arrangement of electrons around the nucleus of an atom is known as
a. the Bohr model
d. the diagonal rule
b. the ground state
e. the electron configuration
c. the principal quantum number
____ 24. The 3p atomic orbital has the shape of
a. a sphere
d. two perpendicular dumb-bells
b. a torus
e. an egg
c. a dumb-bell
____ 25. Which of the following elements would have the lowest first ionization energy?
a. sodium
d. chlorine
b. aluminum
e. argon
c. nitrogen
____ 26. How does atomic radius change from left to right across a period of the Periodic Table?
a. it tends to decrease
b. it tends to increase
c. it does not change
d. it first increases, and then decreases
e. it first decreases and then it increases
____ 27. Energy released when "excited" electrons return to lower energy levels produce...
a. line spectra
d. all of the above
b. ionization energies
e. none of the above
c. electron affinities
____ 28. Rutherford's gold foil experiment showed that the atom is mostly empty space because
a. some of the alpha particles were reflected right back
b. some of the alpha particles were deflected
c. most of the alpha particles went straight through the foil
d. all of the alpha particles went straight through the foil
e. all of the alpha particles were deflected
____ 29. The lines in the line spectrum of an atom results from
a. energy absorbed by electrons dropping back down to a lower energy level
b. energy absorbed by electrons jumping to a higher energy level
c. energy released by electrons jumping to a higher energy level
d. energy released by electrons dropping back down to a lower energy level
e. none of the above
____ 30. Why do energy levels exist in atoms?
a. electrons are negatively charged
b. electrons are attracted to certain numbers of neutrons
c. electrons are able to possess any range of energy
d. electrons will only display certain colours
e. electrons are only able to possess quanta of energy
____ 31. What was Planck's contribution to the quantum mechanical model of the atom?
a. the uncertainty principle
b. the concept of quanta of energy
c. the idea that every mass has a wave with which it is associated
d. the wave equation
e. a relationship between energy and mass
____ 32. What was de Broglie's contribution to the quantum mechanical model of the atom?
a. the uncertainty principle
b. concept of quanta of energy
c. the idea that every mass has a wave with which is it associated
d. the wave equation
e. a relationship between energy and mass
____ 33. What did Einstein contribute to the quantum mechanical model of the atom?
a. uncertainty principle
b. concept of quanta of energy
c. the idea that every mass has a wave with which it is associated
d. the wave equation
e. a relationship between energy and mass
____ 34. What did Heisenberg contribute to the quantum mechanical model of the atom?
a. the uncertainty principle
b. concept of quanta of energy
c. the idea that every mass has a wave with which it is associated
d. the wave equation
e. a relationship between energy and mass
____ 35. What did Schrodinger contribute to the quantum mechanical model of the atom?
a. the uncertainty principle
b. concept of quanta of energy
____ 36.
____ 37.
____ 38.
____ 39.
c. the idea that every mass has a wave with which it is associated
d. the wave equation
e. a relationship between energy and mass
"A region of space in which there is a high probability of finding an electron" is the definition of
a. orbital
d. photon
b. absorption spectrum
e. dipole
c. quantum
"A packet of energy that can be absorbed or released by an electron" is a description of
a. orbital
d. photon
b. absorption spectrum
e. dipole
c. quantum
"A particle of light" is one way of describing
a. orbital
d. photon
b. absorption spectrum
e. dipole
c. quantum
Which of the following is the electron configuration for the valence shell of oxygen?
a.
d.
b.
e.
c.
____ 40. Which of the following is the electron configuration for the valence shell of nitrogen?
a.
d.
b.
e.
c.
____ 41. Which of the following is the electron configuration for magnesium?
a. 1s2 2s2 2p8
d. 1s3 2s3 2p3 3s2
3
3
4
2
b. 1s 2s 2p 3s
e. 1s2 2s2 2p6 3s2
2
2
7
1
c. 1s 2s 2p 3s
____ 42. Which of the following is the electron configuration for neon?
a. 1s22s22p43s2
d. 1s32s32p4
b. 1s12s12p63s2
e. 1s22s22p8
2
2
6
c. 1s 2s 2p
____ 43. Which of the following is the electron configuration for sodium?
a. 1s2 2s3 2p5 3s1
d. 1s2 2s2 2p6 3s1
3
3
3
2
b. 1s 2s 2p 3s
e. 1s22s22p7
2
2
5
2
c. 1s 2s 2p 3s
____ 44. What experimental evidence led Bohr to believe that electrons can possess only specific amounts of
energy?
a. most alpha particles went straight through the gold foil
b. some alpha particles were deflected by the gold foil
c. the line spectra produced by excited atoms
d. atoms are electrically neutral
e. none of the above
____ 45. What led Rutherford to believe that atoms contain a positive nucleus?
a. most alpha particles went straight through the gold foil
b. some alpha particles were deflected by the gold foil
c. the line spectra of excited atoms
d. atoms are electrically neutral
e. none of the above
____ 46. What made Rutherford believe that atoms are mostly empty space?
a. most alpha particles went straight through the gold foil
b. some alpha particles were deflected by the gold foil
c. the line spectra of excited atoms
d. atoms are electrically neutral
e. none of the above
____ 47. What made scientists believe that atoms contain equal numbers of protons and neutrons?
a. most alpha particles went straight through the gold foil
b. some alpha particles were deflected by the gold foil
c. the line spectra of excited atoms
d. atoms are electrically neutral
e. none of the above
____ 48. How was Bohr able to discover the energies of each energy level in the hydrogen atom?
a. using the fact that most alpha particles went straight through the gold foil
b. using the fact that some alpha particles were deflected by the gold foil
c. using the line spectrum of hydrogen when it is excited
d. using the fact that atoms are electrically neutral
e. none of the above
____ 49. Bohr's model of the atom can be termed a "quantum" model of the atom because
a. electrons and protons are equal
b. it is based on the solar system
c. the nucleus is positive
d. each electron can possess only specific amounts of energy
e. the potential energy of electrons is measurable
____ 50. Unlike Bohr's model of the atom, the quantum mechanical model of the atom treats the electron like
a. a tiny particle
d. a wave
b. a proton
e. a photon
c. a positive particle
____ 52.
____ 53.
____ 54.
____ 55.
____ 56.
____ 57.
___
51.
Which of the following is true of orbitals?
a. They are three-dimensional
b. They can contain maximum of two electrons
c. Their shapes are predicted by Schrodinger's equation
d. all of the above
e. none of the above
Which of the following is always true of all electrons in the same principal energy level.
a. they possess the same energy
d. all of the above
b. they have opposite spins
e. none of the above
c. they are in identical orbitals
Which of the following are properties of alkali metals?
I.
They have one valence electron.
II.
They have high first ionization energies.
III.
They are very reactive.
IV.
Their most easily removed electron is in an s orbital.
a. I and II only
d. III only
b. I and IV only
e. I only
c. I, III and IV only
Which of the following are characteristics of transition metals?
I.
Their most easily removed electron is in a d or s orbital.
II.
They are highly reactive.
III.
They have low electron affinities
IV.
Their most easily removed electron is in a p orbital.
a. I and IV only
d. II and III only
b. I and III only
e. I only
c. I, II and III only
Why do halogens have high electron affinities?
a. their electron configurations are close to noble gases
b. they have low electronegativities
c. they have high ionization energies
d. all of the above
e. none of the above
Why is the first ionization energy of arsenic higher than the first ionization energy of selenium?
a. arsenic wants to be iso-electronic with a noble gas
b. arsenic is larger than selenium
c. arsenic's 4p orbitals are half full
d. selenium needs only two electrons to be iso-electronic with a noble gas
e. none of the above
Why is phosphorus able to have a valence of 5+?
a. it is in group 5
b. it has five valence electrons
c. its most easily removed electron is in a p orbital
d. it has empty d orbitals
e. none of the above
____ 58. Why do non-metals have high electronegativities?
a. they are very small atoms and thus have a stronger hold on their electrons
b. they are on the left side of the periodic table
c. they contain many protons therefore they have a stronger hold on their electrons
d. they can easily become iso-electronic with noble gases by accepting electrons
e. none of the above
____ 59. Which element is the most electronegative?
a. helium
d. hydrogen
b. fluorine
e. sodium
c. francium
____ 60. Which is true of all p-block elements?
a. they are all metals
b. they have relatively low electron affinities
c. they are all non-metals
d. they have relatively high electronegativities
e. none of the above
____ 61. Which atoms could have the valence electron configuration shown below?
­¯
s
­¯ ­¯ ­¯
p
a. N3d. Cl12b. O
e. all of the above
c. Ar
____ 62. Which of the atoms could have the following valence electron configuration?
­¯
­ ­¯ ­
s
p
a. carbon
d. sulfur
b. nitrogen
e. none of the above
c. boron
____ 63. Which of the following is the electron configuration for a halogen?
a. 1s2 2s2 2p4
d. 1s2 2s2
2
2
6
1
b. 1s 2s 2p 3s
e. 1s22s22p6
2
2
5
c. 1s 2s 2p
____ 64. Which of the following is the electron configuration for calcium, Ca?
a. 1s22s22p63s23p64s2
d. 1s22s22p63s23p6
2
2
6
2
b. 1s 2s 2p 3s
e. 1s2 2s2
c. 1s2 2s2 2p6
____ 65. Which of the following is the electron configuration for fluoride, F1-?
a. 1s22s22p4
d. 1s22s22p6
2
6
b. 1s 1p
e. 1s2 2s2 2p6 3s1
2
2
5
c. 1s 2s 2p
____ 66. Which of the following are characteristics of light produced by lasers?
a. it is monochromatic
d. all of the above
b. it contains coherent waves
e. none of the above
c. it contains parallel waves
____ 67. Why does a laser produce a narrow beam of light?
a. the light produced is monochromatic
b. the light produced contains coherent waves
c. the light produced contains parallel waves
d. all of the above
e. none of the above
____ 68. Which statement is true of absorption spectrophotometers?
a. they excite electrons using photons
b. they excite electrons using different types of energy
c. they produce electricity
d. the intensity of the output photons is inversely proportional to the number of specific
species present
e. none of the above
____ 69. Which device uses electrons accelerated to high speeds to bombard a target material?
a. MRI
d. laser
b. spectrophotometer
e. none of the above
c. X-ray
____ 70. Which technology uses superconductors?
a. MRI
d. laser
b. spectrophotometer
e. none of the above
c. X-ray
____ 71. Which technology uses light amplification by stimulated emission of radiation?
a. laser
d. MRI
b. spectrophotometer
e. all of the above
c. X-rays
____ 72. Which technology demonstrates the principles of quantum mechanics?
a. laser
d. MRI
b. spectrophotometer
e. all of the above
c. X-ray machine
____ 73. In which of the following situations is a spectrophotometer a useful instrument?
a. producing new substances
d. microsurgery
b. producing high energy photons
e. all of the above
c. detecting trace amounts of substances
____ 74. How is the X-ray image of an object produced?
I.
X-rays being absorbed by parts of the object.
II.
X-rays bouncing off of parts of the object.
III.
X-rays hitting a photographic plate.
IV.
X-rays causing the production of photons.
a. IV only
d. I and IV only
b. I, II and III only
e. I, III and IV only
c. I and III only
____ 75. The "cat scan", computerized axial tomography, is a modification of which technology?
a. laser
d. MRI
b. spectrophotometer
e. combination of all of the above
c. X-ray
____ 76. How are CT scans an improvement on X-rays?
I.
They produce three dimensional images
II.
They are in colour
III.
They have higher resolution
IV.
They use microwaves
a. I, III and IV only
d. I and III only
b. II and IV only
e. I and II only
c. III and IV only
____ 77. Which technology seems to challenge our understanding of quantum mechanics?
a. superconductors
d. semi-conductors
b. lasers
e. X-ray machines
c. spectrophotometers
____ 78. What is the definition of a superconductor?
a. contains iron and conducts electricity very well
b. contains helium and conducts electricity
c. conducts electricity only at low temperatures
d. conducts electricity at room temperature
e. conducts electricity with a resistance near zero
____ 79. Which of the following is the configuration of carbon?
a. 1s22s22p2
d. 1s22s12p4
2
2
4
b. 1s 2s 2p
e. none of the above
2
1
3
c. 1s 2s 2p
____ 80. Which of the following does not apply to the quantum mechanical model of the atom?
a. it is three dimensional
b. it treats electrons as wave/particles
c. it has protons and neutrons trapped in the nucleus
d. it has electrons travelling in orbits
e. none of the above