Chapter 8 Test Bank

5/24/2018 Chapter 8 Test Bank

1/26

Chapter 8 - Electron Configurations and Periodicity

1. The Pauli exclusion principle states that

A) the wavelength of a photon of light times its frequency is equal to the speed of

light.B) no two electrons in the same atom can have the same set of four quantum numbers.

C) both the position of an electron and its momentum cannot be knownsimultaneously very accurately.

D) the wavelength and mass of a subatomic particle are related by .

E) an electron can have either particle character or wave character.

ANS: B PTS: 1 DIF: easy REF: 8.1

OBJ: State the Pauli exclusion principle.

TOP: atomic theory | electronic structure of atoms

KEY: electron configuration | Pauli exclusion principle MSC: general chemistry

2. What is the maximum number of electrons that can occupy one p orbital?A) 14B) 2

C) 10

D) 1

E) 6


OBJ: State the Pauli exclusion principle.

TOP: atomic theory | electronic structure of atomsKEY: electron configuration | Pauli exclusion principle MSC: general chemistry

3. What is the maximum number of electrons that can be accommodated in the n= 2 shell?

A) 8

B) 4

C) 16

D) 22

E) 24

ANS: A PTS: 1 DIF: easy REF: 8.1OBJ: State the Pauli exclusion principle.


4. Which of the following orbital occupancy designations is incorrect?A) 3d

B) 2p

C) 4f

D) 1sE) 4f

ANS: E PTS: 1 DIF: easy REF: 8.1

OBJ: Apply the Pauli exclusion principle. (Example 8.1)



2/26

5. The maximum number of electrons that can be accommodated in an f subshell is

A) 2.B) 10.

C) 6.

D) 1.

E) 14.


OBJ: Apply the Pauli exclusion principle. (Example 8.1)TOP: atomic theory | electronic structure of atoms


6. What is the maximum number of electrons in an atom that have the set of quantum numbers

n= 1 and l= 0?

A) 6

B) 14

C) 10

D) 18E) 2




7. Which of the following orbital diagrams violates the Pauli exclusion principle?

1s 2s 2p

A)

B)

C)

D)

E)

ANS: D PTS: 1 DIF: easy REF: 8.1



8. Which principle or rule is violated by the following orbital diagram of an atom in its groundstate?

1s 2s 2p

A) Pauli exclusion principleB) Aufbau principle

C) No rules or principles are violated by this orbital diagram.

D) Heisenberg uncertainty principle


3/26

E) Hund's rule

ANS: A PTS: 1 DIF: easy REF: 8.1




9. Which of the following electron configurations is impossible, according to the Pauli

exclusion principle?A)

B)

C)

D)

E)

ANS: C PTS: 1 DIF: easy REF: 8.1



10. Which of the following statements is true concerning the electron configuration [Kr]5p2?

A) This configuration cannot be the ground-state electron configuration for a Sr atom

because it violates the Pauli exclusion principle.

B) This configuration cannot be the ground-state electron configuration for a Sr atom

because it violates Hund's rule.

C) This configuration is the ground-state electron configuration for a Sr atom.

D) This configuration cannot be the ground-state electron configuration for a Sr atom

because it violates the Heisenberg uncertainty principle.E) This configuration cannot be the ground-state electron configuration for a Sr atom

because it violates the Aufbau principle.

ANS: E PTS: 1 DIF: moderate REF: 8.2

OBJ: Define building-up principle.


KEY: electron configuration | aufbau principle MSC: general chemistry

11. Which of the following statements is incorrect?

A) Stern and Gerlach discovered electron spin by passing silver atoms through amagnetic field.

B) Hunds rule states that electrons are placed in the orbitals of a subshell in such away as to give a maximum number of unpaired electrons.

C) The Pauli exclusion principle states that each electron in an atom must have its

own unique set of quantum numbers.

D) Valence electrons consist of those electrons not contained within a noble-gas core

or a pseudo-noble-gas core.

E) The building-up principle states that electrons are added to atoms in order of

increasing principal quantum number.




4/26



12. Which principle or rule is violated by the following orbital diagram of an atom in its ground

state?

1s 2s 2p

A) Pauli exclusion principleB) Hund's rule

C) Heisenberg uncertainty principle

D) No rules or principles are violated by this orbital diagram.

E) Building-up principle





13. Which of the following electron configurations represents an excited state of the indicated

atom?

A) Ne: 1s 2s 2p

B) N: 1s 2s 2p

C) P: 1s 2s 2p 3s 3p 4s1

D) Na: 1s 2s 2p 3s 3p 3s1

E) He: 1s

ANS: C PTS: 1 DIF: moderate REF: 8.2

OBJ: Define building-up principle.TOP: atomic theory | electronic structure of atoms


14. Which of the following have one or more filled d subshells in their ground state electron

configuration?

A) Ga

B) ClC) Si

D) He

E) Ar

ANS: A PTS: 1 DIF: easy REF: 8.2OBJ: Define noble-gas core, pseudo-noble-gas core, and valence electron.


15. Two elements that have the same ground-state valence shell configuration of ns2np

2are

A) K and Mg.B) O and Se.

C) Al and Ga.

D) Ge and Pb.

E) Mg and Ca.


5/26


OBJ: Define noble-gas core, pseudo-noble-gas core, and valence electron.TOP: atomic theory | electronic structure of atoms

KEY: electron configuration and the periodic table MSC: general chemistry

16. Which element is found in the s-block of the periodic table?A) HB) Rn

C) Mo

D) Pr

E) none of the above


OBJ: Define noble-gas core, pseudo-noble-gas core, and valence electron.


17. According to the building-up principle or aufbau principle, which subshell is typically filled

next after the 3d subshell?A) 4p

B) 5f

C) 6p

D) 5dE) 1s

ANS: A PTS: 1 DIF: easy REF: 8.2OBJ: Define building-up principle.


18. Which of the following electron configurations corresponds to the ground state of an atomof a transition element?

A) 1s 2s 2p

B) 1s 2s 2p 3s 3p 3d1

4s 4p

C) 1s 2s 2p 3s 3p 3d 4s

D) 1s 2s 2p 3s 3p 4s

E) 1s 2s 2p 3s 3p4

ANS: C PTS: 1 DIF: easy REF: 8.2OBJ: Define main-group element and (d-block and f-block) transition element.



19. The ground-state valence-shell configuration of a particular atom is . The

element to which this atom belongs is a

A) noble gas.

B) inner transition element.

C) p-block main-group element.

D) transition element.

E) s-block main-group element.



6/26

OBJ: Define main-group element and (d-block and f-block) transition element.

TOP: atomic theory | electronic structure of atomsKEY: electron configuration and the periodic table MSC: general chemistry

20. The ground-state valence-shell configuration of a particular atom is . The

element to which this atom belongs is aA) noble gas.B) s-block main-group element.C) p-block main-group element.

D) transition element.

E) inner transition element.





21. The ground-state valence-shell configuration of a particular atom is 5s24d5. This

valence-shell electron configuration identifies the atom as

A) a transition element.

B) an inner transition element.

C) an s-block main-group element.

D) a p-block main-group element.

E) a noble gas.

ANS: A PTS: 1 DIF: easy REF: 8.2OBJ: Define main-group element and (d-block and f-block) transition element.


22. Which of the following statements is incorrect?

A) A p-block main-group element belonging to period nhas a completely filled(n 1)d subshell.

B) All noble gases have completely filled shells.

C) All s-block main-group elements have only one or two valence electrons.

D) Carbon and silicon have the same number of valence electrons.E) All elements in the n= 4 period have a partially or completely filled n= 4 shell.



TOP: atomic theory | electronic structure of atomsKEY: electron configuration and the periodic table MSC: general chemistry

23. Which of the following statements is true concerning the electron configuration [Ne]3s13p

1?

A) It may represent a ground-state electron configuration of a Al+cation.

B) It may represent an excited-state electron configuration of a Mg atom.C) It may represent an excited-state electron configuration of a Neanion.

D) It may represent a ground-state electron configuration of a Mg+cation.

E) It may represent a ground-state electron configuration of a Na+cation.

ANS: B PTS: 1 DIF: difficult REF: 8.3

OBJ: Determine the configuration of an atom using the building-up principle. (Example


7/26

8.2) TOP: atomic theory | electronic structure of atoms

KEY: electron configuration and the periodic table | writing electron configurations usingthe periodic table MSC: general chemistry

24. Which of the following may represent an excited-state electron configuration for a cobalt

atom?A) [Ar]3d 4s

1

B) [Ar]3d 4s

C) [Ar]3d 4s

D) [Ar]3d 4s1

E) [Ar]3d 4s

ANS: C PTS: 1 DIF: difficult REF: 8.3



KEY: electron configuration and the periodic table | writing electron configurations using

the periodic table MSC: general chemistry

25. All of the following ground-state electron configurations are correct except

A) .

B) .

C) .

D) .

E) .

ANS: A PTS: 1 DIF: moderate REF: 8.3


8.2) TOP: atomic theory | electronic structure of atomsKEY: electron configuration and the periodic table MSC: general chemistry

26. What is the total number of electrons in p orbitals in a ground-state vanadium atom?

A) 6

B) 18

C) 12

D) 24E) 30

ANS: C PTS: 1 DIF: moderate REF: 8.3OBJ: Determine the configuration of an atom using the building-up principle. (Example


27. Which ground-state electron configuration is incorrect?

A)

B)

C)

D)

E)



8/26


8.2) TOP: atomic theory | electronic structure of atomsKEY: electron configuration | aufbau principle MSC: general chemistry

28. How many valence electrons does an arsenic atom have?

A) 5B) 8C) 7

D) 2

E) 33





29. Which of the following sets of four quantum numbers (n,l, ml,ms) correctly describes one of

the valence electrons in a ground-state radium atom?A) 7 1 0

B) 6 1 1

C) 7 2 0

D) 7 2 0

E) 7 0 0 +

ANS: E PTS: 1 DIF: easy REF: 8.3OBJ: Determine the configuration of an atom using the building-up principle. (Example8.2) TOP: atomic theory | electronic structure of atoms


30. What is the ground-state electron configuration of tantalum (Ta)?

A) 1s 2s 2p 3s 3p 4s 4p 4d 4f 5s 5p

B) 1s 2s 2p 3s 3p 3d1

4s 4p 4d1

5s 5p

C) 1s 2s 2p 3s 3p 3d1

4s 4p 4d1

4f14

5s 5p 5d 6sD) 1s 2s 2p 3s 3p 3d 4s 4p 4d 5s 5p 5d

E) 1s 2s 2p 3s 3p 3d1 4s 4p 4d1 4f


OBJ: Determine the configuration of an atom using the building-up principle. (Example8.2) TOP: atomic theory | electronic structure of atoms


31. What is the ground-state electron configuration of terbium (Tb)?

A) 1s 2s 2p 3s 3p 3d1

4s 4p 4d1

5s 5p 5d 6sB) 1s 2s 2p 3s 3p 3d1 4s 4p 4d1 4f145s 5p

C) 1s 2s 2p 3s 3p 3d1

4s 4p 4d1

5s 5p 5d1

6s1

D) 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 6s

E) 1s 2s 2p 3s 3p 3d1 4s 4p 4d1 4f 5s 5p 6s


9/26


OBJ: Determine the configuration of an atom using the building-up principle. (Example8.2) TOP: atomic theory | electronic structure of atoms


32. What is the ground-state electron configuration of sulfur (S)?A)

B)

C)

D)

E)

ANS: D PTS: 1 DIF: easy REF: 8.3OBJ: Determine the configuration of an atom using the building-up principle. (Example



33. What noble gas core would be used when writing the ground state electron configuration for

tungsten (W)?

A) [Xe]

B) [Rn]C) [Kr]

D) [Ar]

E) [Ne]




34. If the electron could have a third spin state (that is, , , and 0), what would be the

ground-state electron configuration of carbon?

A) 1s 2s4

B) 1s 2s 2p1

C) 1s 2s

D) 1s 2s 2pE) 1s 2s 2p1


OBJ: Determine the configuration of an atom using the building-up principle. (Example8.2) TOP: atomic theory | electronic structure of atomsKEY: electron configuration MSC: general chemistry

35. The elements that are filling the 5f subshell are called

A) alkali metals.

B) transition elements.

C) lanthanides.

D) actinides.

E) main-group elements.


10/26


OBJ: Determine the configuration of an atom using the period and group numbers.(Example 8.3) TOP: atomic theory | electronic structure of atoms

KEY: electron configuration and the periodic table | writing electron configurations using


36. The quantum numbers of an atom's highest-energy valence electrons are n= 5 and l= 1.The element to which this atom belongs could be a

A) inner transition metal.

B) alkali metal.

C) s-block main-group element.

D) transition metal.

E) p-block main-group element.


OBJ: Determine the configuration of an atom using the period and group numbers.

(Example 8.3) TOP: atomic theory | electronic structure of atoms


37. The angular momentum quantum number of the two highest-energy valence electrons in an

atom of germanium is

A) 4.B) 0.

C) 1.

D) 2.

E) 3.




38. Which of the following sets of four quantum numbers (n,l, ml,ms) correctly describes an

electron occupying a d orbital of an element in the third row of the transition metals?

A) 4 2 2 +

B) 5 2 1

C) 5 3 1

D)4 1 0

E) 5 0 0


OBJ: Determine the configuration of an atom using the period and group numbers.

(Example 8.3) TOP: atomic theory | electronic structure of atomsKEY: electron configuration and the periodic table | writing electron configurations using


39. An element that has the same ground state valence-shell electron configuration as indium is

A) boron.


11/26

B) silicon.

C) krypton.D) lithium.

E) barium.



40. What is the valence-shell electron configuration for the fourth-period element in Group VA?

A)

B)

C)

D)

E)

ANS: C PTS: 1 DIF: easy REF: 8.3OBJ: Determine the configuration of an atom using the period and group numbers.

(Example 8.3) TOP: atomic theory | electronic structure of atoms

KEY: electron configuration and the periodic table | writing electron configurations usingthe periodic table MSC: general chemistry

41. The statement that "the lowest-energy configuration for an atom is the one having the

maximum number of unpaired electrons allowed by the Pauli principle in a particular set of

degenerate orbitals" is known as

A) the aufbau principle.

B) Hund's rule.

C) the Pauli exclusion principle.D) Heisenberg uncertainty principle.

E) the quantum model.


OBJ: State Hunds rule.


KEY: electron configuration | Hund's rule MSC: general chemistry

42. Which principle or rule is violated by the following orbital diagram of an atom in its ground

state?

1s 2s 2p

A) Heisenberg uncertainty principle

B) No rules or principles are violated by this orbital diagram.

C) aufbau principle

D) Hund's rule

E) Pauli exclusion principle


OBJ: State Hunds rule.TOP: atomic theory | electronic structure of atoms


12/26


43. The element whose atoms in the ground state have two half-filled orbitals is

A) Na.

B) Be.

C) Tl.D) Po.E) Sb.


OBJ: Apply Hunds rule. (Example 8.4)



44. How many unpaired electrons are found in the ground state electron configuration of

selenium (Se)?

A) 2

B) 3C) 5

D) 0

E) 1




45. Fe has ____ that is(are) unpaired in its d orbitals.A) 2 electrons

B) 3 electronsC) 1 electron

D) 4 electrons

E) none of these





46. An atom of which of the following elements is not diamagnetic in the ground state?

A) Ca

B) Rn

C) All are diamagnetic.

D) Cd

E) Pt

ANS: E PTS: 1 DIF: easy REF: 8.4OBJ: Define paramagnetic substance and diamagnetic substance.

TOP: atomic theory | electronic structure of atomsKEY: electron configuration | magnetic properties of atoms MSC: general chemistry

47. Which of the following orbital diagrams represent(s) a paramagnetic atom?


13/26

1s 2s 3s

1.

2.

3.

A) 3 only

B) 2 and 3

C) 1 only

D) 1 and 2

E) 2 only


OBJ: Define paramagnetic substance and diamagnetic substance.


48. Which of the following orbital diagrams represents a diamagnetic atom?

1s 2s 2p

A)

B)

C)

D)

E)

ANS: A PTS: 1 DIF: easy REF: 8.4OBJ: Define paramagnetic substance and diamagnetic substance.


49. The ground-state electron configuration of a . Therefore,

isA) paramagnetic with four unpaired electrons.

B) diamagnetic.C) paramagnetic with one unpaired electron.

D) paramagnetic with five unpaired electrons.

E) paramagnetic with three unpaired electrons.ANS: A PTS: 1 DIF: easy REF: 8.4



KEY: electron configuration | magnetic properties of atoms MSC: general chemistry

50. Which of the following orbital diagrams represents a paramagnetic atom?

1s 2s 2p

A)


14/26

B)

C)

D)

E)

ANS: E PTS: 1 DIF: easy REF: 8.4OBJ: Define paramagnetic substance and diamagnetic substance.


KEY: electron configuration | magnetic properties of atoms MSC: general chemistry

51. Which of the following atoms is paramagnetic in its ground state?

A) tin (Sn)

B) barium (ba)C) cadmium (Cd)D) ytterbium (Yb)

E) argon (Ar)




52. Who was the first chemist to recognize patterns in chemical properties of the elements?

A) Bohr

B) DobereinerC) Meyer

D) Mendeleev

E) NewlandsANS: B PTS: 1 DIF: easy REF: 8.5

OBJ: Describe how Mendeleev predicted the properties of undiscovered elements.

TOP: atomic theory | periodicity of the elementsKEY: Mendeleev's predictions MSC: general chemistry

53. Which of the following statements concerning the periodic table is incorrect?A) The elements in a given group or family have similar chemical properties.

B) The chemical characteristics of the elements are periodic functions of their atomicnumbers.

C) All the elements are arranged in order of increasing atomic weight.

D) Mendeleev left spaces in his periodic table for undiscovered elements.E) Mendeleev received most of the credit for the early development of the periodic

table.


OBJ: Describe how Mendeleev predicted the properties of undiscovered elements.TOP: atomic theory | periodicity of the elements

KEY: Mendeleev's predictions MSC: general chemistry

54. Which of the following species would be expected to have chemical properties most similar

to those of the nitrogen atom?


15/26

A) nitride ion

B) nitrite ionC) phosphate ion

D) phosphide ion

E) phosphorus atom

ANS: E PTS: 1 DIF: easy REF: 8.6OBJ: State the periodic law.

TOP: atomic theory | periodicity of the elementsKEY: periodicity in main group elements | group VA elements MSC: general chemistry

55. Which of the following elements would be expected to have chemical and physical

properties most similar to those of the bromine (Br)?

A) chlorine (Cl)

B) neon (Ne)

C) gallium (Ga)

D) calcium (Ca)

E) lead (Pb)


OBJ: State the periodic law.

TOP: atomic theory | periodicity of the elements

56. When arranged in order of increasing atomic number, the elements exhibit periodicity for all

the following properties exceptA) electron affinity.

B) color.C) ionization energy.

D) electron configuration.E) atomic radius.


OBJ: State the periodic law.


KEY: periodic properties MSC: general chemistry

57. In general, atomic radiiA) decrease from left to right in a period and increase down a group.

B) increase from left to right in a period and decrease down a group.

C) do not change across a period or a group.

D) decrease from left to right and decrease down a group.

E) increase from left to right in a period and increase down a group.


OBJ: State the general periodic trends in size of atomic radii.

TOP: atomic theory | periodicity of the elementsKEY: periodic properties | atomic radius MSC: general chemistry

58. Which of the following statements is true?

A) The krypton 1s orbital is smaller than the helium 1s orbital because krypton's

nuclear charge draws the electrons closer.


16/26

B) The krypton 1s orbital is smaller than the helium 1s orbital because krypton's p and

d orbitals crowd the s orbitals.C) The krypton 1s orbital and the helium 1s orbital are the same size because both s

orbitals can have only two electrons.

D) The krypton 1s orbital is larger than the helium 1s orbital because krypton contains

more electrons.E) The krypton 1s orbital is larger than the helium 1s orbital because krypton's

ionization energy is lower so it's easier to remove electrons.


OBJ: Define effective nuclear charge.

TOP: atomic theory | periodicity of the elements KEY: atomic radii

MSC: general chemistry

59. A section of the periodic table with all identification features removed is shown below.

V W X

Y Z

Which element has the smallest atomic radius?

A) WB) Y

C) X

D) ZE) V


OBJ: Determine relative atomic sizes from periodic trends. (Example 8.5)


KEY: periodic properties | atomic radius MSC: general chemistry

60. An atom of which of the following elements has the smallest atomic radius?

A) Sb

B) IC) Te

D) Rb

E) Sn





61. An atom of which of the following elements has the largest atomic radius?A) Cl

B) P

C) Na

D) S

E) Si




17/26




A) At

B) FC) ID) Br

E) Cl





63. An atom of which of the following elements has the largest atomic radius?

A) As

B) SbC) P

D) Bi

E) N





A) ClB) Rb

C) Ca

D) Si

E) As




65. An atom of which of the following elements has the largest atomic radius?

A) Ge

B) K

C) Cl

D) Ca

E) As

ANS: B PTS: 1 DIF: moderate REF: 8.6

OBJ: Determine relative atomic sizes from periodic trends. (Example 8.5)TOP: atomic theory | periodicity of the elements



18/26

66. In which of the series of elements listed below would the elements have most nearly the

same atomic radius?A) Na, K, Rb, Cs

B) F, Cl, Br, I

C) Na, Mg, Al, Si

D) Sc, Ti, V, CrE) B, Si, As, Te

ANS: D PTS: 1 DIF: moderate REF: 8.6OBJ: Determine relative atomic sizes from periodic trends. (Example 8.5)



67. Rank the following atoms in order of the largest to smallest atomic radius: Al, P, Cl, K.

A) K > Al > P > Cl

B) Al > K > P > Cl

C) P > Al > K > Cl

D) Al > P > Cl > KE) K > P > Al > Cl




68. Below are data on the first four ionization energies for a fictitious element X.

First ionization energy = 500 kJ/mol

Second ionization energy = 2000 kJ/mol

Third ionization energy = 3500 kJ/mol

Fourth ionization energy = 25000 kJ/mol

From the data, which of the following statements is incorrect?A) The third ionization energy is greater than the second ionization energy because

X2+has a bigger charge than X+.

B) X could belong to Group IIIA.

C) X could belong to Group IIIB.

D) X could belong to group VA.

E) The fourth ionization energy is much greater than the third ionization energy

because X3+

consists of a noble-gas core or a pseudo-noble-gas core.

ANS: D PTS: 1 DIF: difficult REF: 8.6

OBJ: State the general periodic trends in ionization energy.TOP: atomic theory | periodicity of the elements

KEY: periodic properties | ionization energy MSC: general chemistry

69. Which of the following properties, in general, increases from left to right across a period in

the periodic table?

A) ionic charge

B) atomic radiusC) density

D) ionization energy


19/26

E) metallic character


OBJ: State the general periodic trends in ionization energy.



70. The statement that the first ionization energy for an oxygen atom is lower than the first

ionization energy for a nitrogen atom isA) inconsistent with the general trend relating changes in ionization energy across a

period from left to right and due to the fact that oxygen has one doubly occupied

2p orbital and nitrogen does not.

B) consistent with the general trend relating changes in ionization energy across a

period from left to right because it is harder to take an electron from an oxygen

atom than from a nitrogen atom.

C) consistent with the general trend relating changes in ionization energy across a

period from left to right because it is easier to take an electron from an oxygen

atom than from a nitrogen atom.D) incorrect.

E) inconsistent with the general trend relating changes in ionization energy across a

period from left to right and due to the fact that the oxygen atom has two doubly

occupied 2p orbitals and nitrogen has only one.


OBJ: State the general periodic trends in ionization energy.TOP: atomic theory | periodicity of the elements


71. The change in energy for which of the following processes corresponds to the firstionization energy of calcium?

A)

B)

C)

D)

E)

ANS: A PTS: 1 DIF: easy REF: 8.6OBJ: Define first ionization energy.

TOP: atomic theory | periodicity of the elementsKEY: periodic properties | ionization energy MSC: general chemistry

72. The change in energy for which of the following processes represents the first ionization

energy of bromine?

A)

B)

C)

D)

E)


20/26


OBJ: Define first ionization energy.



73. The change in energy for which of the following processes corresponds to the secondionization energy of barium?

A)

B)

C)

D)

E)

ANS: C PTS: 1 DIF: moderate REF: 8.6OBJ: Define first ionization energy.


74. An atom of which of the following elements has the highest fourth ionization energy?

A) Al

B) Se

C) SiD) Ga

E) As

ANS: A PTS: 1 DIF: moderate REF: 8.6OBJ: Determine relative ionization energies from periodic trends. (Example 8.6)



75. An atom of which of the following elements has the smallest ionization energy?A) I

B) Sb

C) Sn

D) Rb

E) Te


OBJ: Determine relative ionization energies from periodic trends. (Example 8.6)TOP: atomic theory | periodicity of the elements


76. An atom of which of the following elements has the largest ionization energy?

A) Te

B) SnC) Sb

D) I

E) Rb


21/26


OBJ: Determine relative ionization energies from periodic trends. (Example 8.6)TOP: atomic theory | periodicity of the elements


77. An atom of which of the following elements has the smallest first ionization energy?A) SnB) Pb

C) Ge

D) C

E) Si


OBJ: Determine relative ionization energies from periodic trends. (Example 8.6)



78. An atom of which of the following elements has the largest first ionization energy?A) N

B) Sb

C) As

D) PE) Bi

ANS: A PTS: 1 DIF: easy REF: 8.6OBJ: Determine relative ionization energies from periodic trends. (Example 8.6)


79. An atom of which of the following elements has the smallest first ionization energy?

A) Rb

B) Si

C) F

D) As

E) Ca

ANS: A PTS: 1 DIF: moderate REF: 8.6OBJ: Determine relative ionization energies from periodic trends. (Example 8.6)



80. An atom of which of the following elements has the largest first ionization energy?

A) Ca

B) Rb

C) GeD) ClE) P

ANS: D PTS: 1 DIF: moderate REF: 8.6




22/26


81. An atom of which of the following elements has the largest second ionization energy?

A) Na

B) Cl

C) SD) SiE) Mg





82. Which of the following ground-state electron configurations corresponds to an atom having

the largest ionization energy?

A) [Ar]3d1

4s 4p

B) [Ne]3s 3pC) [Ne]3s 3p

D) [Kr]4d1

5s 5p

E) [Xe]4f 5d 6s 6p

ANS: B PTS: 1 DIF: moderate REF: 8.6



83. Rank the following ions in order of increasing first ionization energy: O2, Mg2+,F, Na+.

A) Mg+

< Na+

< F

< O

B) Mg

+< O

< Na

+< F

C) O< F

< Mg

+< Na

+

D) O< F

< Na

+< Mg

+

E) O< Mg

+< F

< Na

+

ANS: D PTS: 1 DIF: difficult REF: 8.6



84. The electron affinity value expected for the process would beA) a small negative number.

B) a large positive number.

C) a small positive number.

D) a large negative number.

E) zero.

ANS: D PTS: 1 DIF: easy REF: 8.6OBJ: Define electron affinity.


KEY: periodic properties | electron affinity MSC: general chemistry


23/26

85. The change in energy for which of the following processes corresponds to the electron

affinity of iodine?A)

B)

C)

D)

E)


OBJ: Define electron affinity.TOP: atomic theory | periodicity of the elements


86. Which of the following statements is true about the ionization energy of Mg+?

A) It will be equal to and opposite in sign to the electron affinity of Mg +.

B) It will be equal to and opposite in sign to the electron affinity of Mg.

C) It will be equal to and opposite in sign to the electron affinity of Mg +.

D) It will be equal to the ionization energy of Li.E) none of the above


OBJ: Define electron affinity.



87. An atom of which of the following elements has the most negative electron affinity?

A) Rb

B) AsC) Cl

D) Br

E) Se


OBJ: State the broad general trend in electron affinity across any period.



88. According to the general trend in electron affinities, which group (or family) of elements

tend to form the most stable anions in the gas phase?A) noble gases

B) halogens

C) transition metals

D) alkaline earth metals

E) alkali metals


OBJ: State the broad general trend in electron affinity across any period.TOP: atomic theory | periodicity of the elements

89. Which of the following forms the most stable anion in the gas phase?


24/26

A) Br (electron affinity = -325 kJ/mol)

B) I (electron affinity = -295 kJ/mol)C) Te (electron affinity = -190 kJ/mol)

D) C (electron affinity = -122 kJ/mol)

E) As (electron affinity = -77 kJ/mol)

ANS: A PTS: 1 DIF: easy REF: 8.6OBJ: State the broad general trend in electron affinity across any period.


90. Which of the following ground-state electron configurations corresponds to an atom that has

the most negative value of the electron affinity?

A) 1s 2s 2p 3s

B) 1s 2s 2p 3s 3p

C) 1s 2s 2p 3s 3p

D) 1s 2s 2p 3s 3p 3d 4s

E) 1s 2s 2p

ANS: B PTS: 1 DIF: moderate REF: 8.6OBJ: State the broad general trend in electron affinity across any period.



91. Which of the following statements is true concerning a concentrated solution of lithium

oxide in water?A) The resulting solution is strongly basic.

B) The resulting solution is weakly acidic.C) The resulting solution is neither acidic nor basic.

D) The resulting solution is weakly basic.E) The resulting solution is strongly acidic.


OBJ: Define basic oxide, acidic oxide, and amphoteric oxide.


KEY: periodicity in main group elements | group IA elements MSC: general chemistry

92. Which of the following are incorrectly paired?A) Group IIA, alkaline earth metals

B) Group IA, alkali metals

C) Group VIIIA, noble gases

D) Group IVA, halogens

E) Group VIA, chalcogens


OBJ: State the main group corresponding to an alkali metal, an alkaline earth metal, and a

chalcogen. TOP: atomic theory | periodicity of the elementsKEY: periodicity in main group elements MSC: general chemistry

93. Sodium and potassium have similar chemical and physical properties. This is best explained

by the fact that both elements

A) have the same ground-state valence-electron configuration.


25/26

B) have low relative atomic masses.

C) are in Period 1 of the periodic table.D) have relatively low first ionization energies.

E) are active metals.


OBJ: Describe the change in metallic/nonmetallic character (or reactivities) in goingthrough any main group of elements.

TOP: atomic theory | periodicity of the elementsKEY: periodicity in main group elements | group IA elements MSC: general chemistry

94. Which element forms the most acidic oxide?

A) B

B) Tl

C) Al

D) In

E) Ga

ANS: A PTS: 1 DIF: easy REF: 8.7OBJ: Describe the change in metallic/nonmetallic character (or reactivities) in going

through any main group of elements.


KEY: periodicity in main group elements | group IIIA elements MSC: general chemistry

95. A few atoms of the new element 113 were created in 2004 by a team of Russian andAmerican scientists. It has been given the temporary name "ununtrium" and the temporary

symbol "Uut." Based on ununtrium's position on the periodic table, what type of oxide(s)should it form?

A) Ununtrium should form a basic oxide with the formula Uut2O3.B) Ununtrium should form an amphoteric oxide with the formula UutO.

C) Ununtrium should form an acidic oxide with the formula Uut2O3.

D) Ununtrium should form two acidic oxides having the formulas Uut2O and Uut2O3.

E) Ununtrium should form two basic oxides having the formulas Uut2O and Uut2O3.


OBJ: Describe the change in metallic/nonmetallic character (or reactivities) in going

through any main group of elements.TOP: atomic theory | periodicity of the elements

KEY: periodicity in main group elements | group IIIA elements MSC: general chemistry

96. The element antimony is in the same group as phosphorus. Which of the following is the

formula of antimonous acid?

A)

B)

C)

D)

E)

ANS: D PTS: 1 DIF: moderate REF: 8.7



26/26


TOP: atomic theory | periodicity of the elementsKEY: periodicity in main group elements | group VA elements MSC: general chemistry

97. The element selenium is in the same group as sulfur. Which of the following is the formula

of selenous acid?A)

B)

C)

D)

E)





KEY: periodicity in main group elements | group VIA elements MSC: general chemistry

98. An unknown element, X, reacts with oxygen to form two oxides with the general formula

X2O3and X2O5. The pure element is strongly paramagnetic, and the oxides are amphoteric.Which of the following elements could be represented by X?

A) Sc

B) NaC) Bi

D) S

E) Sb

ANS: E PTS: 1 DIF: moderate REF: 8.7OBJ: Describe the change in metallic/nonmetallic character (or reactivities) in going



KEY: periodicity in main group elements | group VA elements MSC: general chemistry

Chapter 8 Test Bank

Documents

Transcript of Chapter 8 Test Bank