Question 1

Which of the following statements best describes the difference between ionic and covalent bonding?

Accepted Answer

Ionic bonding involves the transfer of electrons from a metal to a nonmetal, resulting in the formation of ions, while covalent bonding involves the sharing of electrons between two nonmetals.

Question 2

According to the octet rule, atoms tend to gain, lose, or share electrons until they are surrounded by how many valence electrons?

Accepted Answer

Eight

Question 3

Which of the following best explains why ionic compounds, such as NaCl, have high melting points?

Accepted Answer

They have a well-defined three-dimensional lattice structure with strong electrostatic attractions between oppositely charged ions.

Question 4

Which step in the Born-Haber cycle is typically exothermic?

Accepted Answer

Formation of the ionic solid from gaseous ions

Question 5

What is lattice energy, and how is it defined?

Accepted Answer

The energy required to convert a solid ionic compound into its gaseous ions.

Question 6

Which factor increases the lattice energy of an ionic compound?

Accepted Answer

Increasing the charge on the ions

Question 7

Which of the following electron configurations would you expect for a sodium ion ($\mathrm{Na^+}$)?

Accepted Answer

$[\mathrm{Ne}]$

Question 8

Which statement about transition metal ions is correct?

Accepted Answer

Transition metals lose their highest $n$ valence electrons first, then lose $d$ electrons as needed for the ion charge.

Question 9

Which of the following molecules contains a triple bond?

Accepted Answer

$\mathrm{N_2}$

Question 10

Which of the following best describes a polar covalent bond?

Accepted Answer

Electrons are shared unequally, with one atom attracting the electrons more strongly.

Question 11

Which compound would you expect to have the most ionic character based on electronegativity difference?

Accepted Answer

$\mathrm{LiF}$

Question 12

What is the formula for calculating the dipole moment ($\mu$) of a molecule?

Accepted Answer

$\mu = Q 	imes r$

Question 13

Which of the following is true regarding resonance structures?

Accepted Answer

Resonance structures are used when a single Lewis structure cannot accurately depict the molecule, and the actual structure is a hybrid of all resonance forms.

Question 14

Which molecule is an example of an exception to the octet rule due to having fewer than eight valence electrons?

Accepted Answer

$\mathrm{BF_3}$

Question 15

Which of the following molecules is hypervalent (has more than eight electrons around the central atom)?

Accepted Answer

$\mathrm{PF_5}$

Question 16

Given the following reaction: $\mathrm{CH_4 (g) + Cl_2 (g) \rightarrow CH_3Cl (g) + HCl (g)}$, and the average bond enthalpies: $D(C-H) = 413\ \mathrm{kJ/mol}$, $D(Cl-Cl) = 242\ \mathrm{kJ/mol}$, $D(C-Cl) = 328\ \mathrm{kJ/mol}$, $D(H-Cl) = 431\ \mathrm{kJ/mol}$, calculate $\Delta H_{rxn}$.

Accepted Answer

$-104\ \mathrm{kJ}$

Question 17

Which statement about bond length and bond strength is correct?

Accepted Answer

As the number of bonds between two atoms increases, the bond length decreases and the bond strength increases.

Question 18

Which of the following is the dominant Lewis structure for a molecule?

Accepted Answer

The structure in which atoms have formal charges closest to zero and negative charges are on the most electronegative atoms.

Question 19

Which of the following molecules contains delocalized electrons as depicted by a resonance structure?

Accepted Answer

$\mathrm{C_6H_6}$ (benzene)

Chapter 8: Basic Concepts of Chemical Bonding – Study Notes

Study Guide - Practice Questions

Study Guide - Flashcards