Question 1

Which of the following best explains why NaCl is an ionic compound while HCl is a molecular compound?

Accepted Answer

Na and Cl form a crystal lattice, while HCl forms discrete molecules.

Question 2

Which of the following statements about Lewis symbols is correct?

Accepted Answer

Lewis symbols show only the valence electrons as dots around the chemical symbol.

Question 3

According to the octet rule, how do atoms typically achieve a complete outer shell?

Accepted Answer

By sharing or transferring electrons to achieve eight valence electrons.

Question 4

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

Accepted Answer

Their ionization energies and electron affinities.

Question 5

Why is the formation of NaCl from its elements exothermic, even though the sum of the ionization energy of Na and the electron affinity of Cl is positive?

Accepted Answer

Because the lattice energy released when the crystal forms is large and exothermic.

Question 6

Which factor has the greatest effect on the magnitude of lattice energy according to Coulomb's law?

Accepted Answer

The charge of the ions.

Question 7

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

Accepted Answer

CsI \u003c NaF \u003c CaO

Question 8

Which of the following best describes a coordinate covalent bond?

Accepted Answer

A bond where both electrons in the bond are donated by one atom.

Question 9

Which statement about multiple bonds is correct?

Accepted Answer

The distance between atoms decreases as the number of bonds increases.

Question 10

What is the correct sequence of steps for drawing a Lewis structure?

Accepted Answer

Sum valence electrons, make skeleton, complete octets, place remaining electrons, form multiple bonds if needed.

Question 11

Which of the following is true about bond energies?

Accepted Answer

Bond energies are always positive because energy is required to break a bond.

Question 12

Given the reaction $$2\ \mathrm{H}_2\mathrm{O}_2 \rightarrow 2\ \mathrm{H}_2\mathrm{O} + \mathrm{O}_2$$ and the following bond enthalpies: $$\Delta H (\mathrm{O}-\mathrm{O}) = 146\ \mathrm{kJ\ mol}^{-1}$$, $$\Delta H (\mathrm{O}-\mathrm{H}) = 463\ \mathrm{kJ\ mol}^{-1}$$, $$\Delta H (\mathrm{O}=\mathrm{O}) = 495\ \mathrm{kJ\ mol}^{-1}$$, what is the enthalpy change for the reaction?

Accepted Answer

$$-203\ \mathrm{kJ\ mol}^{-1}$$

Question 13

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.

Question 14

Which of the following is a feature of lattice energy?

Accepted Answer

It is always exothermic and generally large.

Question 15

Which of the following compounds would you expect to have the highest lattice energy?

Accepted Answer

CaO

Question 16

What is the main reason noble gases are generally unreactive?

Accepted Answer

They have filled outer shells of s and p electrons.

Question 17

Which of the following best describes a metallic bond?

Accepted Answer

Metal nuclei floating in a sea of electrons.

Question 18

Which of the following is true about the relationship between bond length and bond strength?

Accepted Answer

Shorter bonds are generally stronger than longer bonds.

Question 19

Which of the following is the correct formula for the potential energy between two interacting charged particles according to Coulomb's law?

Accepted Answer

$$E = \frac{1}{4\pi\$$varepsilon_0$$} \frac{q_1$ q_2$}{r}$$

Chapter 9: Chemical Bonding I – Lewis Theory (General Chemistry II Study Notes)

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