Chapter 8 Test Bank

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 known simultaneously 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: OBJ: TOP: KEY:

B PTS: 1 DIF: easy State the Pauli exclusion principle. atomic theory | electronic structure of atoms electron configuration | Pauli exclusion principle

REF: 8.1

MSC: general chemistry

2. What is the maximum number of electrons that can occupy one p orbital? A) 14 B) 2 C) 10 D) 1 E) 6 ANS: OBJ: TOP: KEY:

B PTS: 1 DIF: easy State the Pauli exclusion principle. atomic theory | electronic structure of atoms electron configuration | Pauli exclusion principle

REF: 8.1


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 OBJ: State the Pauli exclusion principle. TOP: atomic theory | electronic structure of atoms

REF: 8.1

4. Which of the following orbital occupancy designations is incorrect? A) 3d7 B) 2p6 C) 4f6 D) 1s2 E) 4f15 ANS: E PTS: 1 DIF: easy OBJ: Apply the Pauli exclusion principle. (Example 8.1) TOP: atomic theory | electronic structure of atoms

REF: 8.1

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. ANS: OBJ: TOP: KEY:

E PTS: 1 DIF: easy Apply the Pauli exclusion principle. (Example 8.1) atomic theory | electronic structure of atoms electron configuration | Pauli exclusion principle

REF: 8.1


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) 18 E) 2 ANS: E PTS: 1 DIF: easy OBJ: Apply the Pauli exclusion principle. (Example 8.1) TOP: atomic theory | electronic structure of atoms

REF: 8.1

7. Which of the following orbital diagrams violates the Pauli exclusion principle? 1s

2s

2p

A) B) C) D) E) ANS: OBJ: TOP: KEY:

D PTS: 1 DIF: easy Apply the Pauli exclusion principle. (Example 8.1) atomic theory | electronic structure of atoms electron configuration | Pauli exclusion principle

REF: 8.1


8. Which principle or rule is violated by the following orbital diagram of an atom in its ground state? 1s A) B) C) D)

2s

2p

Pauli exclusion principle Aufbau principle No rules or principles are violated by this orbital diagram. Heisenberg uncertainty principle

E) Hund's rule ANS: OBJ: TOP: KEY:

A PTS: 1 DIF: easy Apply the Pauli exclusion principle. (Example 8.1) atomic theory | electronic structure of atoms electron configuration | Pauli exclusion principle

REF: 8.1


9. Which of the following electron configurations is impossible, according to the Pauli exclusion principle? A) B) C) D) E) ANS: OBJ: TOP: KEY:

C PTS: 1 DIF: easy Apply the Pauli exclusion principle. (Example 8.1) atomic theory | electronic structure of atoms electron configuration | Pauli exclusion principle

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: OBJ: TOP: KEY:

E PTS: 1 DIF: moderate Define building-up principle. atomic theory | electronic structure of atoms electron configuration | aufbau principle

REF: 8.2


11. Which of the following statements is incorrect? A) Stern and Gerlach discovered electron spin by passing silver atoms through a magnetic field. B) Hund’s rule states that electrons are placed in the orbitals of a subshell in such a way 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. ANS: E PTS: 1 OBJ: Define building-up principle.

DIF:

easy

REF: 8.2

TOP: atomic theory | electronic structure of atoms KEY: electron configuration | aufbau principle


12. Which principle or rule is violated by the following orbital diagram of an atom in its ground state? 1s A) B) C) D) E)

2s

2p

Pauli exclusion principle Hund's rule Heisenberg uncertainty principle No rules or principles are violated by this orbital diagram. Building-up principle

ANS: OBJ: TOP: KEY:

E PTS: 1 DIF: easy Define building-up principle. atomic theory | electronic structure of atoms electron configuration | aufbau principle

REF: 8.2


13. Which of the following electron configurations represents an excited state of the indicated atom? A) Ne: 1s2 2s2 2p6 B) N: 1s2 2s2 2p3 C) P: 1s2 2s2 2p6 3s2 3p2 4s1 D) Na: 1s2 2s2 2p6 3s2 3p2 3s1 E) He: 1s2 ANS: OBJ: TOP: KEY:

C PTS: 1 DIF: moderate Define building-up principle. atomic theory | electronic structure of atoms electron configuration | aufbau principle

REF: 8.2


14. Which of the following have one or more filled d subshells in their ground state electron configuration? A) Ga B) Cl C) Si D) He E) Ar ANS: A PTS: 1 DIF: easy REF: 8.2 OBJ: Define noble-gas core, pseudo-noble-gas core, and valence electron. TOP: atomic theory | electronic structure of atoms 15. Two elements that have the same ground-state valence shell configuration of ns2np2 are A) K and Mg. B) O and Se. C) Al and Ga. D) Ge and Pb. E) Mg and Ca.

ANS: OBJ: TOP: KEY:

D PTS: 1 DIF: easy REF: 8.2 Define noble-gas core, pseudo-noble-gas core, and valence electron. atomic theory | electronic structure of atoms electron configuration and the periodic table MSC: general chemistry

16. Which element is found in the s-block of the periodic table? A) H B) Rn C) Mo D) Pr E) none of the above ANS: A PTS: 1 DIF: easy REF: 8.2 OBJ: Define noble-gas core, pseudo-noble-gas core, and valence electron. TOP: atomic theory | electronic structure of atoms 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) 5d E) 1s ANS: A PTS: 1 DIF: easy OBJ: Define building-up principle. TOP: atomic theory | electronic structure of atoms

REF: 8.2

18. Which of the following electron configurations corresponds to the ground state of an atom of a transition element? A) 1s22s22p5 B) 1s22s22p63s23p63d104s24p2 C) 1s22s22p63s23p63d64s2 D) 1s22s22p63s23p64s2 E) 1s22s22p63s23p4 ANS: OBJ: TOP: KEY:

C PTS: 1 DIF: easy REF: 8.2 Define main-group element and (d-block and f-block) transition element. atomic theory | electronic structure of atoms electron configuration and the periodic table MSC: general chemistry

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

PTS:

1

DIF:

easy

REF: 8.2

. The

OBJ: Define main-group element and (d-block and f-block) transition element. TOP: atomic theory | electronic structure of atoms KEY: electron configuration and the periodic table MSC: general chemistry 20. The ground-state valence-shell configuration of a particular atom is element to which this atom belongs is a A) noble gas. B) s-block main-group element. C) p-block main-group element. D) transition element. E) inner transition element. ANS: OBJ: TOP: KEY:

. The

D PTS: 1 DIF: easy REF: 8.2 Define main-group element and (d-block and f-block) transition element. atomic theory | electronic structure of atoms electron configuration and the periodic table MSC: general chemistry

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: 8.2 OBJ: Define main-group element and (d-block and f-block) transition element. TOP: atomic theory | electronic structure of atoms 22. Which of the following statements is incorrect? A) A p-block main-group element belonging to period n has 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. ANS: OBJ: TOP: KEY:

E PTS: 1 DIF: moderate REF: 8.2 Define main-group element and (d-block and f-block) transition element. atomic theory | electronic structure of atoms electron configuration and the periodic table MSC: general chemistry

23. Which of the following statements is true concerning the electron configuration [Ne]3s13p1? 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 Ne– anion. 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

8.2) TOP: atomic theory | electronic structure of atoms KEY: electron configuration and the periodic table | writing electron configurations using the periodic table MSC: general chemistry 24. Which of the following may represent an excited-state electron configuration for a cobalt atom? A) [Ar]3d54s1 B) [Ar]3d64s2 C) [Ar]3d84s1 D) [Ar]3d64s1 E) [Ar]3d74s2 ANS: C PTS: 1 DIF: difficult REF: 8.3 OBJ: Determine the configuration of an atom using the building-up principle. (Example 8.2) TOP: atomic theory | electronic structure of atoms 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: OBJ: 8.2) KEY:

A PTS: 1 DIF: moderate REF: 8.3 Determine the configuration of an atom using the building-up principle. (Example TOP: atomic theory | electronic structure of atoms 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) 24 E) 30 ANS: C PTS: 1 DIF: moderate REF: 8.3 OBJ: Determine the configuration of an atom using the building-up principle. (Example 8.2) TOP: atomic theory | electronic structure of atoms 27. Which ground-state electron configuration is incorrect? A) B) C) D) E) ANS: C

PTS:

1

DIF:

easy

REF: 8.3

OBJ: Determine the configuration of an atom using the building-up principle. (Example 8.2) TOP: atomic theory | electronic structure of atoms KEY: electron configuration | aufbau principle MSC: general chemistry 28. How many valence electrons does an arsenic atom have? A) 5 B) 8 C) 7 D) 2 E) 33 ANS: OBJ: 8.2) KEY:

A PTS: 1 DIF: easy REF: 8.3 Determine the configuration of an atom using the building-up principle. (Example TOP: atomic theory | electronic structure of atoms electron configuration and the periodic table MSC: general chemistry

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: OBJ: 8.2) KEY:

E PTS: 1 DIF: easy REF: 8.3 Determine the configuration of an atom using the building-up principle. (Example TOP: atomic theory | electronic structure of atoms electron configuration and the periodic table MSC: general chemistry

30. What is the ground-state electron configuration of tantalum (Ta)? A) 1s22s22p63s23p64s24p64d104f145s25p3 B) 1s22s22p63s23p63d104s24p64d105s25p3 C) 1s22s22p63s23p63d104s24p64d104f145s25p65d36s2 D) 1s22s22p63s23p63d104s24p64d105s25p65d3 E) 1s22s22p63s23p63d104s24p64d104f3 ANS: OBJ: 8.2) KEY:

C PTS: 1 DIF: easy REF: 8.3 Determine the configuration of an atom using the building-up principle. (Example TOP: atomic theory | electronic structure of atoms electron configuration and the periodic table MSC: general chemistry

31. What is the ground-state electron configuration of terbium (Tb)? A) 1s22s22p63s23p63d104s24p64d105s25p65d96s2 B) 1s22s22p63s23p63d104s24p64d104f145s25p3 C) 1s22s22p63s23p63d104s24p64d105s25p65d106s1 D) 1s22s22p63s23p63d104s24p64d94f105s25p66s2 E) 1s22s22p63s23p63d104s24p64d104f95s25p66s2

ANS: OBJ: 8.2) KEY:

E PTS: 1 DIF: moderate REF: 8.3 Determine the configuration of an atom using the building-up principle. (Example TOP: atomic theory | electronic structure of atoms electron configuration and the periodic table MSC: general chemistry

32. What is the ground-state electron configuration of sulfur (S)? A) B) C) D) E) ANS: OBJ: 8.2) KEY:

D PTS: 1 DIF: easy REF: 8.3 Determine the configuration of an atom using the building-up principle. (Example TOP: atomic theory | electronic structure of atoms electron configuration and the periodic table MSC: general chemistry

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] ANS: A PTS: 1 DIF: easy REF: 8.3 OBJ: Determine the configuration of an atom using the building-up principle. (Example 8.2) TOP: atomic theory | electronic structure of atoms 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) 1s22s4 B) 1s22s32p1 C) 1s32s3 D) 1s22s22p2 E) 1s32s22p1 ANS: OBJ: 8.2) KEY:

C PTS: 1 DIF: difficult REF: 8.3 Determine the configuration of an atom using the building-up principle. (Example TOP: atomic theory | electronic structure of atoms 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.

ANS: D PTS: 1 DIF: easy REF: 8.3 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 the periodic table MSC: general chemistry 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. ANS: E PTS: 1 DIF: moderate REF: 8.3 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 MSC: general chemistry 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. ANS: C PTS: 1 DIF: difficult REF: 8.3 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 MSC: general chemistry 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 – ANS: B PTS: 1 DIF: easy REF: 8.3 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 the periodic table MSC: general chemistry 39. An element that has the same ground state valence-shell electron configuration as indium is A) boron.

B) C) D) E)

silicon. krypton. lithium. barium.

ANS: A PTS: 1 DIF: easy REF: 8.3 OBJ: Determine the configuration of an atom using the period and group numbers. (Example 8.3) TOP: atomic theory | electronic structure of atoms 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: 8.3 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 the 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. ANS: OBJ: TOP: KEY:

B PTS: 1 DIF: easy State Hund’s rule. atomic theory | electronic structure of atoms electron configuration | Hund's rule

REF: 8.4


42. Which principle or rule is violated by the following orbital diagram of an atom in its ground state? 1s A) B) C) D) E)

2s

2p

Heisenberg uncertainty principle No rules or principles are violated by this orbital diagram. aufbau principle Hund's rule Pauli exclusion principle

ANS: D PTS: 1 DIF: easy OBJ: State Hund’s rule. TOP: atomic theory | electronic structure of atoms

REF: 8.4

KEY: electron configuration | Hund's rule


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. ANS: OBJ: TOP: KEY:

D PTS: 1 DIF: easy Apply Hund’s rule. (Example 8.4) atomic theory | electronic structure of atoms electron configuration | Hund's rule

REF: 8.4


44. How many unpaired electrons are found in the ground state electron configuration of selenium (Se)? A) 2 B) 3 C) 5 D) 0 E) 1 ANS: A PTS: 1 DIF: easy OBJ: Apply Hund’s rule. (Example 8.4) TOP: atomic theory | electronic structure of atoms

REF: 8.4

45. Fe has ____ that is(are) unpaired in its d orbitals. A) 2 electrons B) 3 electrons C) 1 electron D) 4 electrons E) none of these ANS: OBJ: TOP: KEY:

D PTS: 1 DIF: easy Apply Hund’s rule. (Example 8.4) atomic theory | electronic structure of atoms electron configuration | Hund's rule

REF: 8.4


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: OBJ: TOP: KEY:

E PTS: 1 DIF: easy REF: 8.4 Define paramagnetic substance and diamagnetic substance. atomic theory | electronic structure of atoms electron configuration | magnetic properties of atoms MSC: general chemistry

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

1s

2s

3s

1. 2. 3. A) B) C) D) E)

3 only 2 and 3 1 only 1 and 2 2 only

ANS: B PTS: 1 DIF: easy REF: 8.4 OBJ: Define paramagnetic substance and diamagnetic substance. TOP: atomic theory | electronic structure of atoms 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: 8.4 OBJ: Define paramagnetic substance and diamagnetic substance. TOP: atomic theory | electronic structure of atoms 49. The ground-state electron configuration of a is A) 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: OBJ: TOP: KEY:

. Therefore,

A PTS: 1 DIF: easy REF: 8.4 Define paramagnetic substance and diamagnetic substance. atomic theory | electronic structure of atoms electron configuration | magnetic properties of atoms MSC: general chemistry

50. Which of the following orbital diagrams represents a paramagnetic atom? 1s 2s 2p A)

B) C) D) E) ANS: OBJ: TOP: KEY:

E PTS: 1 DIF: easy REF: 8.4 Define paramagnetic substance and diamagnetic substance. atomic theory | electronic structure of atoms 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) ANS: A PTS: 1 DIF: easy REF: 8.4 OBJ: Define paramagnetic substance and diamagnetic substance. TOP: atomic theory | electronic structure of atoms 52. Who was the first chemist to recognize patterns in chemical properties of the elements? A) Bohr B) Dobereiner C) Meyer D) Mendeleev E) Newlands ANS: OBJ: TOP: KEY:

B PTS: 1 DIF: easy REF: 8.5 Describe how Mendeleev predicted the properties of undiscovered elements. atomic theory | periodicity of the elements 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 atomic numbers. 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. ANS: OBJ: TOP: KEY:

C PTS: 1 DIF: easy REF: 8.5 Describe how Mendeleev predicted the properties of undiscovered elements. atomic theory | periodicity of the elements 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?

A) B) C) D) E)

nitride ion nitrite ion phosphate ion phosphide ion phosphorus atom

ANS: OBJ: TOP: KEY:

E PTS: 1 DIF: easy State the periodic law. atomic theory | periodicity of the elements periodicity in main group elements | group VA elements

REF: 8.6


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) ANS: A PTS: 1 DIF: easy OBJ: State the periodic law. TOP: atomic theory | periodicity of the elements

REF: 8.5

56. When arranged in order of increasing atomic number, the elements exhibit periodicity for all the following properties except A) electron affinity. B) color. C) ionization energy. D) electron configuration. E) atomic radius. ANS: OBJ: TOP: KEY:

B PTS: 1 DIF: easy REF: 8.6 State the periodic law. atomic theory | periodicity of the elements periodic properties MSC: general chemistry

57. In general, atomic radii A) 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. ANS: OBJ: TOP: KEY:

A PTS: 1 DIF: easy REF: 8.6 State the general periodic trends in size of atomic radii. atomic theory | periodicity of the elements 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.

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. ANS: OBJ: TOP: MSC:

A PTS: 1 DIF: moderate Define effective nuclear charge. atomic theory | periodicity of the elements general chemistry

REF: 8.6 KEY: atomic radii

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

W Y

X Z

Which element has the smallest atomic radius? A) W B) Y C) X D) Z E) V ANS: OBJ: TOP: KEY:

C PTS: 1 DIF: moderate REF: 8.6 Determine relative atomic sizes from periodic trends. (Example 8.5) atomic theory | periodicity of the elements periodic properties | atomic radius MSC: general chemistry

60. An atom of which of the following elements has the smallest atomic radius? A) Sb B) I C) Te D) Rb E) Sn ANS: OBJ: TOP: KEY:

B PTS: 1 DIF: easy REF: 8.6 Determine relative atomic sizes from periodic trends. (Example 8.5) atomic theory | periodicity of the elements periodic properties | atomic radius MSC: general chemistry

61. An atom of which of the following elements has the largest atomic radius? A) Cl B) P C) Na D) S E) Si ANS: C PTS: 1 DIF: easy REF: 8.6 OBJ: Determine relative atomic sizes from periodic trends. (Example 8.5)

TOP: atomic theory | periodicity of the elements KEY: periodic properties | atomic radius MSC: general chemistry 62. An atom of which of the following elements has the smallest atomic radius? A) At B) F C) I D) Br E) Cl ANS: OBJ: TOP: KEY:

B PTS: 1 DIF: easy REF: 8.6 Determine relative atomic sizes from periodic trends. (Example 8.5) atomic theory | periodicity of the elements periodic properties | atomic radius MSC: general chemistry

63. An atom of which of the following elements has the largest atomic radius? A) As B) Sb C) P D) Bi E) N ANS: OBJ: TOP: KEY:

D PTS: 1 DIF: easy REF: 8.6 Determine relative atomic sizes from periodic trends. (Example 8.5) atomic theory | periodicity of the elements periodic properties | atomic radius MSC: general chemistry

64. An atom of which of the following elements has the smallest atomic radius? A) Cl B) Rb C) Ca D) Si E) As ANS: OBJ: TOP: KEY:

A PTS: 1 DIF: moderate REF: 8.6 Determine relative atomic sizes from periodic trends. (Example 8.5) atomic theory | periodicity of the elements periodic properties | atomic radius MSC: general chemistry

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: OBJ: TOP: KEY:

B PTS: 1 DIF: moderate REF: 8.6 Determine relative atomic sizes from periodic trends. (Example 8.5) atomic theory | periodicity of the elements periodic properties | atomic radius MSC: general chemistry

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, Cr E) B, Si, As, Te ANS: OBJ: TOP: KEY:

D PTS: 1 DIF: moderate REF: 8.6 Determine relative atomic sizes from periodic trends. (Example 8.5) atomic theory | periodicity of the elements periodic properties | atomic radius MSC: general chemistry

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 > K E) K > P > Al > Cl ANS: A 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 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: OBJ: TOP: KEY:

D PTS: 1 DIF: difficult State the general periodic trends in ionization energy. atomic theory | periodicity of the elements periodic properties | ionization energy

REF: 8.6


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 radius C) density D) ionization energy

E) metallic character ANS: OBJ: TOP: KEY:

D PTS: 1 DIF: easy State the general periodic trends in ionization energy. atomic theory | periodicity of the elements periodic properties | ionization energy

REF: 8.6


70. The statement that the first ionization energy for an oxygen atom is lower than the first ionization energy for a nitrogen atom is A) 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. ANS: OBJ: TOP: KEY:

A PTS: 1 DIF: moderate State the general periodic trends in ionization energy. atomic theory | periodicity of the elements periodic properties | ionization energy

REF: 8.6


71. The change in energy for which of the following processes corresponds to the first ionization energy of calcium? A) B) C) D) E) ANS: OBJ: TOP: KEY:

A PTS: 1 DIF: easy Define first ionization energy. atomic theory | periodicity of the elements periodic properties | ionization energy

REF: 8.6


72. The change in energy for which of the following processes represents the first ionization energy of bromine? A) B) C) D) E)

ANS: OBJ: TOP: KEY:

D PTS: 1 DIF: easy Define first ionization energy. atomic theory | periodicity of the elements periodic properties | ionization energy

REF: 8.6


73. The change in energy for which of the following processes corresponds to the second ionization energy of barium? A) B) C) D) E) ANS: OBJ: TOP: KEY:

C PTS: 1 DIF: moderate Define first ionization energy. atomic theory | periodicity of the elements periodic properties | ionization energy

REF: 8.6


74. An atom of which of the following elements has the highest fourth ionization energy? A) Al B) Se C) Si D) Ga E) As ANS: OBJ: TOP: KEY:

A PTS: 1 DIF: moderate REF: 8.6 Determine relative ionization energies from periodic trends. (Example 8.6) atomic theory | periodicity of the elements periodic properties | ionization energy MSC: general chemistry

75. An atom of which of the following elements has the smallest ionization energy? A) I B) Sb C) Sn D) Rb E) Te ANS: OBJ: TOP: KEY:

D PTS: 1 DIF: easy REF: 8.6 Determine relative ionization energies from periodic trends. (Example 8.6) atomic theory | periodicity of the elements periodic properties | ionization energy MSC: general chemistry

76. An atom of which of the following elements has the largest ionization energy? A) Te B) Sn C) Sb D) I E) Rb

ANS: OBJ: TOP: KEY:

D PTS: 1 DIF: easy REF: 8.6 Determine relative ionization energies from periodic trends. (Example 8.6) atomic theory | periodicity of the elements periodic properties | ionization energy MSC: general chemistry

77. An atom of which of the following elements has the smallest first ionization energy? A) Sn B) Pb C) Ge D) C E) Si ANS: OBJ: TOP: KEY:

B PTS: 1 DIF: easy REF: 8.6 Determine relative ionization energies from periodic trends. (Example 8.6) atomic theory | periodicity of the elements periodic properties | ionization energy MSC: general chemistry

78. An atom of which of the following elements has the largest first ionization energy? A) N B) Sb C) As D) P E) Bi ANS: OBJ: TOP: KEY:

A PTS: 1 DIF: easy REF: 8.6 Determine relative ionization energies from periodic trends. (Example 8.6) atomic theory | periodicity of the elements periodic properties | ionization energy MSC: general chemistry

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: OBJ: TOP: KEY:


80. An atom of which of the following elements has the largest first ionization energy? A) Ca B) Rb C) Ge D) Cl E) P ANS: D PTS: 1 DIF: moderate REF: 8.6 OBJ: Determine relative ionization energies from periodic trends. (Example 8.6) TOP: atomic theory | periodicity of the elements

KEY: periodic properties | ionization energy


81. An atom of which of the following elements has the largest second ionization energy? A) Na B) Cl C) S D) Si E) Mg ANS: OBJ: TOP: KEY:


82. Which of the following ground-state electron configurations corresponds to an atom having the largest ionization energy? A) [Ar]3d104s24p3 B) [Ne]3s23p3 C) [Ne]3s23p2 D) [Kr]4d105s25p3 E) [Xe]4f145d106s26p3 ANS: OBJ: TOP: KEY:

B PTS: 1 DIF: moderate REF: 8.6 Determine relative ionization energies from periodic trends. (Example 8.6) atomic theory | periodicity of the elements periodic properties | ionization energy MSC: general chemistry

83. Rank the following ions in order of increasing first ionization energy: O2–, Mg2+, F–, Na+. A) Mg2+ < Na+ < F– < O2– B) Mg2+ < O2– < Na+ < F– C) O2– < F– < Mg2+ < Na+ D) O2– < F– < Na+ < Mg2+ E) O2– < Mg2+ < F– < Na+ ANS: OBJ: TOP: KEY:

D PTS: 1 DIF: difficult REF: 8.6 Determine relative ionization energies from periodic trends. (Example 8.6) atomic theory | periodicity of the elements periodic properties | ionization energy MSC: general chemistry

84. The electron affinity value expected for the process A) a small negative number. B) a large positive number. C) a small positive number. D) a large negative number. E) zero. ANS: OBJ: TOP: KEY:

D PTS: 1 DIF: easy Define electron affinity. atomic theory | periodicity of the elements periodic properties | electron affinity

would be

REF: 8.6


85. The change in energy for which of the following processes corresponds to the electron affinity of iodine? A) B) C) D) E) ANS: OBJ: TOP: KEY:

B PTS: 1 DIF: easy Define electron affinity. atomic theory | periodicity of the elements periodic properties | electron affinity

REF: 8.6


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 Mg2+. D) It will be equal to the ionization energy of Li. E) none of the above ANS: OBJ: TOP: KEY:

C PTS: 1 DIF: moderate Define electron affinity. atomic theory | periodicity of the elements periodic properties | electron affinity

REF: 8.6


87. An atom of which of the following elements has the most negative electron affinity? A) Rb B) As C) Cl D) Br E) Se ANS: OBJ: TOP: KEY:

C PTS: 1 DIF: easy REF: 8.6 State the broad general trend in electron affinity across any period. atomic theory | periodicity of the elements periodic properties | electron affinity MSC: general chemistry

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 ANS: B PTS: 1 DIF: easy REF: 8.6 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?

A) B) C) D) E)

Br (electron affinity = -325 kJ/mol) I (electron affinity = -295 kJ/mol) Te (electron affinity = -190 kJ/mol) C (electron affinity = -122 kJ/mol) As (electron affinity = -77 kJ/mol)

ANS: A PTS: 1 DIF: easy REF: 8.6 OBJ: State the broad general trend in electron affinity across any period. TOP: atomic theory | periodicity of the elements 90. Which of the following ground-state electron configurations corresponds to an atom that has the most negative value of the electron affinity? A) 1s22s22p63s1 B) 1s22s22p63s23p5 C) 1s22s22p63s23p2 D) 1s22s22p63s23p63d54s2 E) 1s22s22p6 ANS: OBJ: TOP: KEY:

B PTS: 1 DIF: moderate REF: 8.6 State the broad general trend in electron affinity across any period. atomic theory | periodicity of the elements periodic properties | electron affinity MSC: general chemistry

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. ANS: OBJ: TOP: KEY:

A PTS: 1 DIF: easy Define basic oxide, acidic oxide, and amphoteric oxide. atomic theory | periodicity of the elements periodicity in main group elements | group IA elements

REF: 8.7


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 ANS: D PTS: 1 DIF: easy REF: 8.7 OBJ: State the main group corresponding to an alkali metal, an alkaline earth metal, and a chalcogen. TOP: atomic theory | periodicity of the elements KEY: 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.

B) C) D) E)

have low relative atomic masses. are in Period 1 of the periodic table. have relatively low first ionization energies. are active metals.

ANS: A PTS: 1 DIF: moderate REF: 8.7 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 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: 8.7 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 95. A few atoms of the new element 113 were created in 2004 by a team of Russian and American 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. ANS: E PTS: 1 DIF: easy REF: 8.7 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 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 VA elements


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) ANS: C PTS: 1 DIF: moderate REF: 8.7 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 VIA elements MSC: general chemistry 98. An unknown element, X, reacts with oxygen to form two oxides with the general formula X2O3 and 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) Na C) Bi D) S E) Sb ANS: E PTS: 1 DIF: moderate REF: 8.7 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 VA elements MSC: general chemistry

Chapter 8 Test Bank

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