LT 6.2 Practice Test

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1. The __________ quantum number defines the shape of an orbital.

spin

magnetic

principal

azimuthal

psi

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2. There are __________ orbitals in the third shell.

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3. The __________ subshell contains only one orbital.

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4. There are __________ orbitals in the second shell.

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5. The n = 1 shell contains __________ p orbitals. All the other shells contain __________ p orbitals.

3; 6

0; 3

6; 2

3; 3

0; 6

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6. The lowest energy shell that contains f orbitals is the shell with n = __________.

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7. The principal quantum number of the first d subshell is __________.

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8. The total number of orbitals in a shell is given by __________.

l²

n²

2n + 1

2l + 1

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9. The uncertainty principle states that __________.

matter and energy are really the same thing

it is impossible to know anything with certainty

it is impossible to know the exact position and momentum of an electron

there can only be one uncertain digit in a reported number

it is impossible to know how many electrons there are in an atom

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10. All of the orbitals in a given electron shell have the same value of the __________ quantum number.

principal

azimuthal

magnetic

spin

psi

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11. Which of the subshells below do not exist due to the constraints upon the azimuthal quantum number?

all of the above

none of the above

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12. An electron cannot have the quantum numbers n = __________, l = __________, mℓ = __________.

2; 0; 0

2; 1; -1

3; 1; -1

1; 1; 1

3; 2; 1

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13. An electron cannot have the quantum numbers n = __________, l = __________, mℓ = __________.

6; 1; 0

3; 2; 3

3; 2; -2

1; 0; 0

3; 2; 1

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14. Which one of the following is an incorrect subshell notation?

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15. Which one of the following is an incorrect orbital notation?

3py

4dxy

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16. How many p-orbitals are occupied in a Ne atom?

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17. Each p-subshell can accommodate a maximum of __________ electrons.

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18. How many quantum numbers are necessary to designate a particular electron in an atom?

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19. Which set of three quantum numbers (n, l, mℓ) corresponds to a 3d orbital?

3; 2; 2

3; 3; 2

3; 2; 3

2; 1; 0

2; 3; 3

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20. At maximum, an f-subshell can hold __________ electrons, a d-subshell can hold __________ electrons, and a p-subshell can hold __________ electrons.

14; 10; 6

2; 8; 18

14; 8; 2

2; 12; 21

2; 6; 10

Clear selection

21. If an electron has a principal quantum number (n) of 3 and an azimuthal quantum number (l) of 2, the subshell designation is _________.

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22. Which one of the following represents an acceptable set of quantum numbers for an electron in an atom? (arranged as n, l, mℓ, and ms)

2; 2; -1; -1/2

1; 0; 0; 1/2

3; 3; 3; 1/2

5; 4;- 5; 1/2

3; 3; 3;-1/2

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23. Which one of the following represents an acceptable possible set of quantum numbers (in the order n, l, mℓ, ms) for an electron in an atom?

2; 1; -1; 1/2

2; 1; 0; 0

2; 2; 0; 1/2

2; 0; 1; -1/2

2; 0; 2; +1/2

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23. Which one of the following represents an acceptable possible set of quantum numbers (in the order n, l, mℓ, ms) for an electron in an atom?

2; 1; -1; -1/2

1; 0; 0; 1/2

3; 3; 3; 1/2

5; 4; - 3; 1/2

5; 4; -3; -1/2

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25. Which of the following is not a valid set of four quantum numbers? (n, l, mℓ, ms)

2; 0; 0; +1/2

2; 1; 0; -1/2

3; 1; -1; -1/2

1; 0; 0; +1/2

1; 1; 0; +1/2

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26. [Ar]4s²3d¹⁰4p³ is the electron configuration of a(n) __________ atom.

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27. There are __________ unpaired electrons in a ground state phosphorus atom.

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28. There are __________ unpaired electrons in a ground state fluorine atom.

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29. In a ground-state manganese atoms, the __________ subshell is partially fille,

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30. The principal quantum number for the outermost electrons in a Br atom in the ground state is __________.

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31. Which of the following is a valid set of four quantum numbers? (n, l, mℓ, ms)

2; 1; 0; +1/2

2; 2; 1; -1/2

1; 0; 1; +1/2

2; 1; +2; +1/2

1; 1; 0; -1/2

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32. Which electron configuration represents a violation of the Pauli exclusion principle?

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33. Which electron configuration represents a violation of the Pauli exclusion principle?

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34. Which electron configuration represents a violation of the Pauli exclusion principle?

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35. Which one of the following is the correct electron configuration for a ground-state nitrogen atom?

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36. Which electron configuration denotes an atom in its ground state?

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37. The ground state electron configuration of Fe is __________.

1s²2s²3s²3p⁶3d⁶

1s²2s²2p⁶3s²3p⁶3d⁶4s²

1s²2s²2p⁶3s²3p⁶4s²

1s²2s²2p⁶3s²3p⁶4s²4d⁶

1s²2s²3s²3p¹⁰

Clear selection

38. The ground state electron configuration of Ga is __________.

1s²2s²3s²3p⁶3d¹⁰4s²4p¹

1s²2s²2p⁶3s²3p⁶4s²4d¹⁰4p¹

1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p¹

1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4d¹

[Ar]4s²3d¹¹

Clear selection

39. The ground-state electron configuration of the element __________ is [Kr]5s¹4d⁵.

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40. The ground-state electron configuration of __________ is [Ar]4s¹3d⁵.

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41. Which one of the following configurations depicts an excited oxygen atom?

1s²2s²2p²

1s²2s²2p²3s²

1s²2s²2p¹

1s²2s²2p⁴

[He]2s²2p⁴

Clear selection

42. Which one of the following configurations depicts an excited carbon atom?

1s²2s²2p¹3s¹

1s²2s²2p³

1s²2s²2p¹

1s²2s²3s¹

1s²2s²2p²

Clear selection

43. Which electron configuration represents a violation of Hund's rule for an atom in its ground state?

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44. Which electron configuration represents a violation of Hund's rule for an atom in its ground state?

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45. Which electron configuration represents a violation of Hund's rule for an atom in its ground state?

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46. The ground state configuration of fluorine is __________.

[He]2s²2p²

[He]2s²2p³

[He]2s²2p⁴

[He]2s²2p⁵

[He]2s²2p⁶

Clear selection

47. The ground state configuration of tungsten is __________.

[Ar]4s²3d³

[Xe]6s²4f¹⁴5d⁴

[Ne]3s¹

[Xe]6s²4f⁷

[Kr]5s²4d¹⁰5p⁵

Clear selection

48. The lowest orbital energy is reached when the number of electrons with the same spin is maximize, This statement describes __________.

Pauli Exclusion Principle

Planck's constant

deBroglie hypothesis

Heisenberg Uncertainty Principle

Hund's rule

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49. The element that has a valence configuration of 4s¹ is _________.

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50. Which of the following elements has a ground-state electron configuration different from the predicted one?

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51. Which two elements have the same ground-state electron configuration?

Pd and Pt

Cu and Ag

Fe and Cu

Cl and Ar

No two elements have the same ground-state electron configuration.

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52. The element that corresponds to the electron configuration 1s²2s²2p⁶ is __________.

sodium

magnesium

lithium

beryllium

neon

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53. The complete electron configuration of argon, element 18, is __________.

1s²2s²2p⁶3s²3p⁶

1s²2s²2p¹⁰3s²3p²

1s⁴2s⁴2p⁶3s⁴

1s⁴2s⁴2p¹⁰

1s⁶2s⁶2p²3s⁴

Clear selection

54. The complete electron configuration of gallium, element 31, is __________.

1s²2s²2p¹⁰3s²3p¹⁰4s²3d³

1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p¹

1s⁴2s⁴2p⁶3s⁴3p⁶4s⁴3d³

1s⁴2s⁴2p¹⁰3s⁴3p⁹

1s⁴2s⁴2p⁸3s⁴3p⁸4s³

Clear selection

55. The condensed electron configuration of silicon, element 14, is __________.

[He]2s⁴2p⁶

[Ne]2p¹⁰

[Ne]3s²3p²

[He]2s⁴

[He]2s⁶2p²

Clear selection

56. The condensed electron configuration of krypton, element 36, is __________.

[Kr]4s²3d⁸

[Ar]4s⁴

[Kr]4s⁴3d⁸

[Ar]3d¹⁰4s²4p⁶

[Ar]4s⁴3d⁴

Clear selection

57. The electron configuration of a ground-state Ag atom is __________.

[Ar]4s²4d⁹

[Kr]5s1⁴d¹⁰

[Kr]5s²3d⁹

[Ar]4s1⁴d¹⁰

[Kr]5s²4d¹⁰

Clear selection

58. The ground state electron configuration for Zn is __________.

[Kr]4s²3d¹⁰

[Ar]4s²3d¹⁰

[Ar]4s13d¹⁰

[Ar]3s²3d¹⁰

[Kr]3s²3d¹⁰

Clear selection

59. Which is the correct ground-state electron configuration for silver?

[Kr]5s²4d⁹

[Kr]5s¹4d¹⁰

[Kr]5s²4d¹⁰

[Xe]5s²4d⁹

[Xe]5s¹4d¹⁰

Clear selection

60. What is the correct ground-state electron configuration for molybdenum?

[Kr]5s¹4d¹⁰

[Kr]5s²4d⁴

[Kr]5s¹4d⁵

[Kr]5s²4d⁵

[Kr]5s²4d⁹

Clear selection

61. All of the __________ have a valence shell electron configuration ns¹.

noble gases

halogens

chalcogens

alkali metals

alkaline earth metals

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62. The elements in the __________ period of the periodic table have a core-electron configuration that is the same as the electron configuration of neon.

first

second

third

fourth

fifth

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63. Elements in group __________ have a np⁶ electron configuration in the outer shell.

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