Ch.8 – Electron Configuration And | Test Questions & Answers

Chapter 8 Test Bank

Electron Configuration and Chemical Periodicity

1. “Each electron in an atom must have its own unique set of quantum numbers” is a statement of

A. the aufbau principle.

B. the Pauli exclusion principle.

C. Hund's rule.

D. the periodic law.

E. Heisenberg's principle.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Pauli Exclusion Principle

Topic: Electron Configuration

2. Energy states of atoms containing more than one electron arise from nucleus-electron and electron-electron interactions. Which of the following statements correctly describes these effects?

A. Larger nuclear charge lowers energy, more electrons in an orbital lowers energy.

B. Larger nuclear charge lowers energy, more electrons in an orbital increases energy.

C. Smaller nuclear charge lowers energy, more electrons in an orbital lowers energy.

D. Smaller nuclear charge lowers energy, more electrons in an orbital increases energy.

E. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Energy-Level Splitting (Zeff and Shielding)

Topic: Electron Configuration

3. Which one of the following statements about orbital energies is incorrect?

A. In the hydrogen atom, the energy of an orbital depends only on the value of the quantum number n.

B. In many-electron atoms the energy of an orbital depends on both n and l.

C. Inner electrons shield outer electrons more effectively than do electrons in the same orbital.

D. The splitting of sublevels in many-electron atoms is explained in terms of the penetration effect.

E. The energy of a given orbital increases as the nuclear charge Z increases.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Energy-Level Splitting (Zeff and Shielding)

Topic: Electron Configuration

4. The effective nuclear charge for an atom is less than the actual nuclear charge due to

A. shielding.

B. penetration.

C. paramagnetism.

D. electron-pair repulsion.

E. relativity.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Energy-Level Splitting (Zeff and Shielding)

Topic: Electron Configuration

5. In many-electron atoms, which quantum numbers specify the energy of an electron?

A. n and l

B. n and m_l

C. l and m_l

D. n and m_s

E. n, l, and m_l

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Quantum Numbers

Topic: Quantum Theory and Atomic Structure

6. Which of the following sublevels is filled last? 3d, 4s, 4p, 4d, 5s

A. 3d

B. 4s

C. 4p

D. 4d

E. 5s

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)

Topic: Electron Configuration

7. “Electrons added to atomic orbitals of the same energy will remain unpaired with parallel spins until the subshell is more than half-filled” is a statement of

A. the aufbau principle.

B. Hund's rule.

C. the Pauli exclusion principle.

D. the periodic law.

E. the singularity rule.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Hund's Rule

Topic: Electron Configuration

8. Which one of the following statements about atomic structure and quantum numbers is incorrect?

A. In a given atom, the maximum number of electrons having principal quantum number n = 3, is 18.

B. The number of orbitals in a given f subshell is 7.

C. For n = 4, the largest possible value of l is 3.

D. For n = 4, the largest possible value of m_l is 2.

E. The following set of quantum numbers for a single orbital is not allowed: n = 3, l = 1, ml = –2.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Quantum Numbers

Topic: Quantum Theory and Atomic Structure

9. In a single atom, what is the maximum number of electrons which can have quantum number n = 4?

A. 16

B. 18

C. 32

D. 36

E. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Quantum Numbers

Topic: Quantum Theory and Atomic Structure

10. Select the correct set of quantum numbers (n, l, m_l, m_s) for the highest energy electron in the ground state of potassium, K.

A. 4, 1, –1, ½

B. 4, 1, 0, ½

C. 4, 0, 1, ½

D. 4, 0, 0, ½

E. 4, 1, 1, ½

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Quantum Numbers

Topic: Quantum Theory and Atomic Structure

11. Select the correct set of quantum numbers (n, l, m_l, m_s) for the highest energy electron in the ground state of tin, Sn.

A. 5, 2, –1, ½

B. 5, 2, 0, ½

C. 5, 1, 2, ½

D. 5, 1, 0, ½

E. 5, 2, 1, ½

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Quantum Numbers

Topic: Quantum Theory and Atomic Structure

12. Select the correct set of quantum numbers (n, l, m_l, m_s) for the first electron removed in the formation of a cation for strontium, Sr.

A. 5, 1 , 0, –½

B. 5, 1, 0, ½

C. 5, 0, 1, ½

D. 5, 1, 1, ½

E. 5, 0, 0, –½

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Quantum Numbers

Topic: Quantum Theory and Atomic Structure

13. Which of the following electron configurations is impossible?

A. 1s²2s²2p⁶3s²3p⁴

B. 1s²2s²2p⁵3s¹3p⁴

C. 1s²2s²2p⁶3s²3p⁶3d¹⁰4s²

D. 1s²2s²2p⁶3s³3p⁴

E. 1s¹2s²2p⁶3s²3p⁴

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)

Topic: Electron Configuration

14. Select the correct electron configuration for sulfur (Z = 16).

A. 1s²1p⁶2s²2p⁶

B. 1s²2s²2p⁸3s²3p⁴

C. 1s²2s²2p⁸3s²3p²

D. 1s²2s²2p⁶3s²3p⁴

E. 1s²2s²2p⁶3s²3d⁴

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)

Topic: Electron Configuration

15. Select the correct electron configuration for Cu (Z = 29).

A. [Ar]4s²3d⁹

B. [Ar]4s¹3d¹⁰

C. [Ar]4s²4p⁶3d³

D. [Ar]4s²4d⁹

E. [Ar]5s²4d⁹

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)

Topic: Electron Configuration

16. Select the correct electron configuration for Te (Z = 52).

A. [Kr]5s²5p⁶4d⁸

B. [Kr]5s²5d¹⁰5p⁴

C. [Kr]5s²4d¹⁰5p⁶

D. [Kr]5s²4f¹⁴

E. [Kr]5s²4d¹⁰5p⁴

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)

Topic: Electron Configuration

17. The electronic structure 1s²2s²2p⁶3s²3p⁶4s²3d⁸ refers to the ground state of

A. Kr.

B. Ni.

C. Fe.

D. Pd.

E. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)

Topic: Electron Configuration

18. In the ground state of an atom of silver (Ag), how many electrons will there be with the quantum number l = 1? (The n, m_l, and m_s quantum numbers may have any appropriate values.)

A. 9

B. 12

C. 18

D. 24

E. 36

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Quantum Numbers

Topic: Quantum Theory and Atomic Structure

19. An atom of element number 33 (As) is in its ground electronic state. Which one of the following sets quantum numbers could not apply to any of its electrons?

A. n = 2 l = 1 ml = –1 m_s = +½

B. n = 3 l = 0 ml = 0 m_s = –½

C. n = 3 l = 2 ml = –2 m_s = –½

D. n = 4 l = 0 ml = 0 m_s = –½

E. n = 4 l = 2 ml = 1 m_s = +½

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Quantum Numbers

Topic: Quantum Theory and Atomic Structure

20. How many valence electrons are there in an atom with the electron configuration [noble gas]ns²(n –1)d¹⁰np³?

A. 2

B. 3

C. 5

D. 10

E. 15

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)

Topic: Electron Configuration

21. How many valence electrons are there in an atom with the electron configuration [noble gas]ns²(n – 1)d⁸?

A. 2

B. 6

C. 8

D. 10

E. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)

Topic: Electron Configuration

22. Which of the following electron configurations represents the ground state of an element?

A. [Ne]3s¹3p¹

B. [He]2s¹2p³

C. [Ne]3s²3p²3d¹

D. [Ne]3s²3p³3d¹

E. [Ne]3s²3p³

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)

Topic: Electron Configuration

23. Which of the following sets of elements have the [noble gas]ns²np² valence electron configuration?

A. O, S, Se, Te, Po

B. N, P, As, Sb, Bi

C. F, Cl, Br, I, At

D. C, Si, Ge, Sn, Pb

E. Ti, Zr, Hf

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)

Topic: Electron Configuration

24. In the electron configuration [Ar]4s²3d¹⁰4p⁴, which are valence electrons?

A. all of the electrons after the [Ar]

B. only the 4s² electrons

C. only the 3d¹⁰ electrons

D. only the 4p⁴ electrons

E. both the 4s² and the 4p⁴ electrons

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)

Topic: Electron Configuration

25. Which of the following electron configurations is correct for the excited state of an element?

A. [He]2s²2p⁵

B. [Ne]3s²3p¹

C. [Ar]4s¹4p¹

D. [Kr]5s²4d⁷

E. [He]1p¹

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)

Topic: Electron Configuration

26. Which of the following electron configurations is not possible for an atom in an excited state?

A. 1s²2s²2p⁶3s²3p⁶3d¹⁰4s¹4p¹

B. 1s²2s²2p⁶3s¹3p⁵

C. 1s²2s²2p⁶3s²3p²3d²

D. 1s²2s²2p⁶3s²3p⁶3d¹⁰4s²

E. 1s²2s²2p⁶3s²3p⁶3d¹⁰4s¹4p³

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)

Topic: Electron Configuration

27. Which of the following fourth-period elements has the smallest atomic radius?

A. K

B. Ti

C. Cu

D. Ge

E. Kr

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

28. Which of the following elements has the largest atomic size?

A. S

B. Ca

C. Ba

D. Po

E. Rn

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

29. Which of the following elements has the smallest atomic size?

A. Na

B. Ar

C. K

D. Ca

E. Kr

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

30. Which of the following elements has the smallest atomic radius?

A. Li

B. Ne

C. Rb

D. Sr

E. Xe

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

31. Which of the following elements has the greatest atomic radius?

A. Li

B. Ne

C. Rb

D. Sr

E. Xe

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

32. Which one of the following equations correctly represents the process relating to the ionization energy of X?

A. X(s) → X⁺(g) + e^–

B. X2(g) → X⁺(g) + X^–(g)

C. X(g) + e^– → X^–(g)

D. X^–(g) → X(g) + e^–

E. X(g) → X⁺(g) + e^–

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Hard

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

33. Which of the following elements has the largest first ionization energy?

A. Na

B. Cl

C. Ca

D. Te

E. Br

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

34. Which of the following elements has the smallest first ionization energy?

A. Rb

B. Mg

C. I

D. As

E. F

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

35. When comparing the successive ionization energies of an element, an unusually big increase in ionization energy is seen when

A. the first valence electron is removed.

B. the second valence electron is removed.

C. the eighth electron of is removed.

D. the first core electron is removed.

E. the last valence electron is removed.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

36. Identify the element of Period 2 which has the following successive ionization energies, in kJ/mol.

IE₁, 1314 IE₂, 3389 IE₃, 5298 IE₄, 7471

IE₅, 10992 IE₆, 13329 IE₇, 71345 IE₈, 84087

A. Li

B. B

C. O

D. Ne

E. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

37. Which of the following elements has the largest second ionization energy (IE₂)?

A. Li

B. B

C. O

D. F

E. Na

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

38. Elements with the highest first ionization energies are found in the ___________ region of the periodic table.

A. lower left

B. upper left

C. center

D. lower right

E. upper right

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

39. Which one of the following equations correctly represents the process involved in the electron affinity of X?

A. X(g) → X⁺(g) + e^–

B. X⁺(g) → X⁺(aq)

C. X⁺(g) + e^– → X(g)

D. X(g) + e^– → X^–(g)

E. X⁺(g) + Y^–(g) → XY(s)

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Hard

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

40. Select the element with the most negative electron affinity (i.e., accepts an electron most readily).

A. H

B. Li

C. C

D. F

E. Ne

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

41. Which of the following has the most negative electron affinity?

A. H

B. Li

C. Na

D. K

E. Rb

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

42. Elements with ________________ first ionization energies and ___________ electron affinities generally form cations.

A. low; very negative

B. high; positive or slightly negative

C. low; positive or slightly negative

D. high; very negative

E. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Hard

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

43. Elements with _______________ first ionization energies and ___________ electron affinities generally form anions.

A. low; very negative

B. high; positive or slightly negative

C. low; positive or slightly negative

D. high; very negative

E. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Hard

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

44. Select the element with the greatest metallic character.

A. Li

B. Ca

C. Al

D. Pb

E. Cs

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

45. Select the element with the least metallic character.

A. Sn

B. Sr

C. Tl

D. Ge

E. Ga

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

46. Metallic behavior is generally associated with

A. elements with very negative electron affinities.

B. elements with low ionization energies.

C. elements with small atomic radii.

D. elements with unpaired electrons.

E. elements with partially filled p orbitals.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

47. The most acidic oxides are formed from elements found in the _________________ region of the periodic table.

A. upper right

B. upper left

C. center

D. lower right

E. lower left

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Trends in Chemical Reactivity

Topic: Chemical Periodicity

48. The most basic oxides are formed from elements found in the __________________ region of the periodic table.

A. upper right

B. upper left

C. center

D. lower right

E. lower left

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Trends in Chemical Reactivity

Topic: Chemical Periodicity

49. Select the most acidic compound from the following.

A. SO₂

B. Al₂O₃

C. CaO

D. PbO

E. H₂O

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Chemical Reactivity

Topic: Chemical Periodicity

50. Select the most basic compound from the following.

A. Bi₂O₃

B. SiO₂

C. Cs₂O

D. Na₂O

E. H₂O

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Chemical Reactivity

Topic: Chemical Periodicity

51. Which of the following elements will form a cation with a +2 charge?

A. Si

B. Sr

C. Ga

D. Cs

E. S

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Molecules and Ions

Topic: Components of Matter

52. Which of the following ions will be most likely to form when selenium ionizes?

A. Se⁶⁺

B. Se⁴⁺

C. Se²⁺

D. Se^2–

E. Se^4–

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Molecules and Ions

Topic: Components of Matter

53. Which of the following atoms will be diamagnetic?

A. Cr

B. Ru

C. Fe

D. Pt

E. Cd

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Diamagnetism and Paramagnetism

Topic: Chemical Periodicity

54. Which of the following elements is paramagnetic?

A. Kr

B. Zn

C. Sr

D. V

E. Ar

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Diamagnetism and Paramagnetism

Topic: Chemical Periodicity

55. Select the paramagnetic ion.

A. Cu⁺

B. Ag⁺

C. Fe³⁺

D. Cd²⁺

E. Ca²⁺

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Diamagnetism and Paramagnetism

Topic: Chemical Periodicity

56. Select the diamagnetic ion.

A. Cu²⁺

B. Ni²⁺

C. Cr³⁺

D. Sc³⁺

E. Cr²⁺

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Diamagnetism and Paramagnetism

Topic: Chemical Periodicity

57. Consider the set of isoelectronic atoms and ions A^2–, B^–, C, D⁺, and E²⁺. Which arrangement of relative radii is correct?

A. A^2– > B^– > C > D⁺ > E²⁺

B. E²⁺ > D+ > C > B^– > A^2–

C. A^2– > B^– > C < D⁺ < E²⁺

D. A^2– < B^– < C > D⁺ > E²⁺

E. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

58. What is the correct order of decreasing size of the following ions?

A. P^3– > Cl^– > K⁺ > Ca²⁺

B. Ca²⁺ > K⁺ > Cl^– > P^3–

C. K⁺ > Cl^– > Ca²⁺ > P^3–

D. K⁺ > Cl^– > P^3– > Ca²⁺

E. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

59. In Mendeleev's version of the periodic table, the elements were arranged in order of increasing atomic number.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Development of the Periodic Table

Topic: Chemical Periodicity

60. Moseley's measurements of nuclear charges of the elements provided the basis for arranging the elements of the periodic table in order of increasing atomic number.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Development of the Periodic Table

Topic: Chemical Periodicity

61. According to the exclusion principle, two is the maximum number of electrons in an atom which can share the same four quantum numbers.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Pauli Exclusion Principle

Topic: Electron Configuration

62. The difference in energies between the 1s and 2s orbitals is due to the penetration effect.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Energy-Level Splitting (Zeff and Shielding)

Topic: Electron Configuration

63. In neutral atoms, the 3d orbitals have higher energy than the 4s orbitals.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)

Topic: Electron Configuration

64. Hund's rule is used to predict the electron configuration of atoms in excited states.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Hund's Rule

Topic: Electron Configuration

65. Elements in which the outermost electron has the same principal quantum number n, show similar chemical properties.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Chemical Reactivity

Topic: Chemical Periodicity

66. The maximum number of electrons in an atom with the same value of n is 2n².

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Quantum Numbers

Topic: Quantum Theory and Atomic Structure

67. Elements in the same period of the periodic table have similar valence shell electron configurations.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)

Topic: Electron Configuration

68. Atomic size decreases across a period due to an increase in the effective nuclear charge, Zeff.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

69. First ionization energies of neutral atoms may be positive or negative.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

70. Bigger atoms generally have smaller ionization energies.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

71. Electron affinities of neutral atoms may be positive or negative.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

72. Electron affinities become increasingly positive toward the right hand end of a period.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

73. A negative electron affinity implies that the atom repels an approaching electron.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity)

Topic: Chemical Periodicity

74. In moving down a group in the periodic table, the oxides of the elements become more acidic in nature.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Trends in Chemical Reactivity

Topic: Chemical Periodicity

75. In forming ions of the first series of transition metals, the 4s electrons are lost before the 3d electrons.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Electron Configurations of Cations and Anions

Topic: Electron Configuration

76. Which one of the following oxides does not react with water to form acid solutions?

A. CO₂

B. SO₃

C. BaO

D. NO₂

E. Cl₂O₇

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Trends in Chemical Reactivity

Topic: Chemical Periodicity

77. Consider the element with the electron configuration: [Rn]7s25f7. How would you classify this element?

A. a representative element

B. a transition metal

C. a nonmetal

D. an actinide element

E. a noble gas

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Trends in Chemical Reactivity

Topic: Chemical Periodicity

Category # of Questions

Accessibility: Keyboard Navigation 77

Bloom's: 1. Remember 26

Bloom's: 2. Understand 33

Bloom's: 3. Apply 18

Difficulty: Easy 23

Difficulty: Hard 10

Difficulty: Medium 44

Gradable: automatic 77

Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle) 15

Subtopic: Development of the Periodic Table 2

Subtopic: Diamagnetism and Paramagnetism 4

Subtopic: Electron Configurations of Cations and Anions 1

Subtopic: Energy-Level Splitting (Zeff and Shielding) 4

Subtopic: Hund's Rule 2

Subtopic: Molecules and Ions 2

Subtopic: Pauli Exclusion Principle 2

Subtopic: Quantum Numbers 9

Subtopic: Trends in Chemical Reactivity 8

Subtopic: Trends in Physical Properties (Atomic Radius, Ionization Energy, Ionic Radius, Electron Affinity) 28

Topic: Chemical Periodicity 42

Topic: Components of Matter 2

Topic: Electron Configuration 24

Topic: Quantum Theory and Atomic Structure 9