Question 1

Which of the following best explains why NaCl is a solid at room temperature while HCl is a gas, despite both containing chlorine?

Accepted Answer

NaCl forms ionic bonds, which are stronger than the covalent bonds in HCl.

Question 2

According to Lewis theory, what is the primary reason noble gases are generally unreactive?

Accepted Answer

They have a filled outer shell of s and p electrons.

Question 3

Which of the following best describes the process of ionic bond formation between sodium and chlorine?

Accepted Answer

Sodium transfers an electron to chlorine, resulting in oppositely charged ions that attract each other.

Question 4

What is the significance of lattice energy in the formation of ionic solids?

Accepted Answer

It is the energy released when gaseous ions form a crystal lattice.

Question 5

Given the following steps for the formation of NaCl from its elements, which step is exothermic?

Accepted Answer

$$\mathrm{Cl}(g) + e^- \rightarrow \mathrm{Cl}^-(g)$$

Question 6

Which of the following compounds has the highest lattice energy?

Accepted Answer

CaO

Question 7

Using Coulomb’s law, which factor has the greatest effect on lattice energy?

Accepted Answer

Charge

Question 8

Which statement best describes the octet rule as it applies to chemical bonding?

Accepted Answer

Atoms tend to achieve a complete outer shell by losing, gaining, or sharing electrons.

Question 9

Why does the formation of NaCl(s) from Na(s) and $$\frac{1}{2}Cl$_2(g) $$have a large negative enthalpy change ($$\Delta H^\circ = -411 kJ $$mol$$^{-1}$$)?

Accepted Answer

Because the lattice energy released when Na$$^+$$ and Cl$$^-$$ form a crystal is very large and exothermic.

Question 10

Arrange the following ionic compounds in order of increasing lattice energy: NaF, CsI, CaO.

Accepted Answer

CsI \u003c NaF \u003c CaO

Question 11

Which of the following best describes a metallic bond?

Accepted Answer

Metal nuclei floating in a sea of delocalized electrons.

Question 12

What is the Lewis symbol for nitrogen?

Accepted Answer

N with 5 dots around it

Question 13

Which property of sodium and chlorine makes electron transfer favorable in forming NaCl?

Accepted Answer

Their ionization energies and electron affinities.

Question 14

Which of the following is NOT a feature of lattice energy?

Accepted Answer

It is always endothermic.

Question 15

Which step in the Born-Haber cycle for NaCl formation is associated with the largest energy release?

Accepted Answer

Formation of the crystal lattice from gaseous ions.

Question 16

Why are Lewis diagrams not useful for elements with d electrons?

Accepted Answer

Because Lewis diagrams only represent s and p valence electrons.

Question 17

Which of the following best explains why lattice energy increases as ion charge increases?

Accepted Answer

The electrostatic force between ions increases with charge, as shown by $$E = \frac{1}{4\pi\$$varepsilon_0$$} \frac{q_1$ q_2$}{r}.$$

Question 18

Which of the following is a correct Lewis symbol for fluorine?

Accepted Answer

F with 7 dots around it

Question 19

Which of the following best describes the difference between intramolecular and intermolecular forces?

Accepted Answer

Intramolecular forces are within a molecule, while intermolecular forces are between molecules.

Chapter 9: Chemical Bonding I – The Lewis Model and Ionic Bonding

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