Chapter 6 B

Rank the following atoms in order of decreasing size (i.e., largest to smallest): Rb, F, Mg, B, N. A) Rb > Mg > B > N > F B) N > F > B > Mg > Rb C) Rb > Mg > F > N > B D) Mg > Rb > B > N > F E) Rb > Mg > N > B > F

A

Which of the following electron configurations is incorrect? A) S [Ne]3s³3p⁴ B) Sn [Kr]5s²4d¹⁰5p² C) Rb [Kr]5s¹ D) V [Ar]4s²3d³ E) I [Kr]5s²4d¹⁰5p⁵

A

Which of the following elements would have a very different electron affinity value compared to the others? A) Ne B) Al C) O D) F E) Na

A

Which of the following is the electron configuration for Ba? A) [Xe]6s² B) [Rn]6s² C) [Xe]6s¹ D) [Xe]7s² E) [Rn]7s²

A

The energy released in the reaction F(g) + e⁻ → F⁻(g) is known as the A) Ionization energy B) Electron affinity C) Enthalpy of ionization D) Electronegativity E) Enthalpy of electronegativity

B

What is the electron configuration of K⁺? A) 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶ B) 1s²2s²2p⁶3s²3p⁶ C) 1s²2s²2p⁶3s²3p⁶4s² D) 1s²2s²2p⁶ E) 1s²2s²2p⁶3s²3p⁵

B

Which of the following is not a property affected by the effective nuclear charge, Zeff? A) Ionization energy. B) Color. C) Electron affinity. D) Atomic radius. E) Ionic radius.

B. Color

Which element has the electron configuration 1s²2s²2p⁶3s²3p⁶4s¹3d⁵? A) V B) Cr C) Mo D) Mn E) No element has this configuration

B. Cr

Which element has the ground state electron configuration [Kr]5s²4d¹⁰5p³? A) Te B) Pb C) Sb D) Bi E) Sn

C

Which of the following states that no two electrons can have the same set of four quantum numbers? A) Hund's rule B) de Broglie wave equation C) Pauli exclusion principle D) Bohr equation E) Schrödinger equation

C. Pauli exclusion principle

Rank the following atoms in order of increasing first ionization energies (i.e., lowest to highest): Rb, F, Mg, B, N. A) F < N < B < Mg < Rb B) Rb < Mg < F < N < B C) Mg < Rb < F < N < B D) Rb < Mg < B < N < F E) Rb > B > N > F > Mg

D

Which electron configuration violates Hund's rule? A) [He]2s²2px²2py²2pz¹ B) [He]2s²2px²2py¹2pz² C) [He]2s²2px¹2py²2pz² D) [He]2s²2px²2py² E) [He]2s²2px¹2py¹2pz²

D

Which of the following electron configurations represent a transition metal atom? A) 1s²2s²2p⁶ B) 1s²2s²2p⁶3s²3p⁴ C) 1s²2s²2p⁶3s²3p⁶4s² D) 1s²2s²2p⁶3s²3p⁶4s²3d⁷ E) 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p¹

D

Which of the following series of isoelectronic ions (Mg²⁺, N³⁻, F⁻, Si⁴⁺) has the ionic radii in order of largest to smallest? A) Mg²⁺ > N³⁻ > F⁻ > Si⁴⁺ B) Mg²⁺ > Si⁴⁺ > F⁻ > N³⁻ C) N³⁻ > F⁻ > Si⁴⁺ > Mg²⁺ D) N³⁻ > F⁻ > Mg²⁺ > Si⁴⁺ E) F⁻ > N³⁻ > Si⁴⁺ > Mg²⁺

D

Which of these statements is true concerning the following reaction? Na(g) → Na⁺(g) + e⁻. A) The energy required is the electron affinity B) The reaction is exothermic C) Na⁺(g) is an anion D) This is an ionization process.

D

Which of the following orbitals cannot exist? A) 2p B) 3d C) 4d D) 3f E) 162p

D. 3f

In a multi-electron atom, which orbital will have the highest energy? A) 4s B) 4p C) 4d D) 4f E) All are equal

D. 4f

Which of the following has the electron configuration 1s²2s²2p⁶3s²3p⁶3d³? A) V³⁺ B) Mn³⁺ C) Cr²⁺ D) Sc²⁺ E) V²⁺

E

Which of the following is the electron configuration of a neutral K atom? A) 1s²2s²2p⁶3s² B) 1s²2s²2p⁶3s¹ C) 1s²2s²2p⁶3s²3p⁶4s² D) 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s¹ E) 1s²2s²2p⁶3s²3p⁶4s¹

E