Question 1

Which of the following ions is isoelectronic with argon (Ar)?

Accepted Answer

$$\mathrm{K^+}$$

Question 2

What is the ground-state electron configuration for the ion $$\mathrm{Fe$$^{2+}$$}$$?

Accepted Answer

$$[\mathrm{Ar}]\ 3d^6$

Question 3

Which of the following statements best explains why the first ionization energy of magnesium is higher than that of aluminum?

Accepted Answer

Magnesium has a filled $$3s$$ subshell, which is more stable than the partially filled $$3p$$ subshell of aluminum.

Question 4

Which of the following ions has the largest ionic radius?

Accepted Answer

$$\mathrm{I^-}$$

Question 5

Which of the following pairs of ions are isoelectronic with krypton ($$\mathrm{Kr}$$)?

Accepted Answer

$$\mathrm{As$$^{3-}$$}$$ and $$\mathrm{Sr$$^{2+}$$}$$

Question 6

Which of the following best describes the trend in first ionization energy across a period from left to right?

Accepted Answer

It increases due to increasing nuclear charge and decreasing atomic radius.

Question 7

Which of the following compounds has the highest lattice energy?

Accepted Answer

$$\mathrm{MgO}$$

Question 8

What is the correct ground-state electron configuration for $$\mathrm{Ti$$^{2+}$$}$$?

Accepted Answer

$$[\mathrm{Ar}]\ 3d^2$

Question 9

Which of the following elements is most likely to form a $$2-$$ ion to achieve a noble gas configuration?

Accepted Answer

Oxygen

Question 10

Which of the following best explains why the lattice energy of $$\mathrm{MgO} is $$much greater than that of $$\mathrm{NaCl}$$?

Accepted Answer

The charges on $$\mathrm{Mg$$^{2+}$$}$$ and $$\mathrm{O$$^{2-}$$}$$ are higher than those on $$\mathrm{Na^+}$$ and $$\mathrm{Cl^-}.$$

Question 11

Which of the following ions has the smallest radius?

Accepted Answer

$$\mathrm{Na^+}$$

Question 12

Which of the following elements has the most negative electron affinity?

Accepted Answer

Fluorine

Question 13

Which of the following best describes the octet rule?

Accepted Answer

Atoms tend to gain, lose, or share electrons to achieve a filled $$s$$ and $$p$$ subshell in their valence shell.

Question 14

Which of the following ions is isoelectronic with $$\mathrm{Ne}$$?

Accepted Answer

$$\mathrm{F^-}$$

Question 15

Which of the following steps in the Born-Haber cycle for NaCl formation is most exothermic?

Accepted Answer

Formation of solid NaCl from gaseous Na$$^+$$ and Cl$$^-$$ ions

Question 16

Which of the following ions would have the same electron configuration as $$\mathrm{Ca$$^{2+}$$}$$?

Accepted Answer

$$\mathrm{Ar}$$

Question 17

Which of the following elements would require the most energy to remove a second electron from a neutral atom?

Accepted Answer

Na

Question 18

Which of the following best explains why noble gases have very low (or positive) electron affinities?

Accepted Answer

Their valence shells are already full, so adding another electron is energetically unfavorable.

Question 19

Which of the following ions would you expect to have the smallest ionic radius?

Accepted Answer

$$\mathrm{F^-}$$

Question 20

Which of the following best describes the removal of electrons in the formation of transition metal ions?

Accepted Answer

Valence $$s$$ electrons are removed before $$d$$ electrons.

Chapter 6: Ionic Compounds – Electron Configurations, Ionization Energies, and Lattice Energies

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