Question 1

Which of the following best explains why sodium (Na) forms a cation while chlorine (Cl) forms an anion in the formation of NaCl?
Correct answer: Sodium loses electrons to achieve a noble gas configuration, while chlorine gains electrons to achieve an octet.

Accepted Answer

Sodium loses electrons to achieve a noble gas configuration, while chlorine gains electrons to achieve an octet.

Question 2

Which of the following molecules contains both sigma (σ) and pi (π) bonds?
Correct answer: O2

Accepted Answer

O2

Question 3

A molecule of carbon dioxide (CO2) is nonpolar, even though it contains polar bonds. Which concept best explains this observation?
Correct answer: The dipole moments of the two polar bonds cancel each other due to the linear geometry.

Accepted Answer

The dipole moments of the two polar bonds cancel each other due to the linear geometry.

Question 4

Which of the following elements is most likely to form an expanded octet in a stable compound?
Correct answer: Phosphorus (P)

Accepted Answer

Phosphorus (P)

Question 5

Given the Lewis structure for the nitrate ion (NO3−), what is the formal charge on each oxygen atom if the structure is drawn with one double bond and two single bonds to the central nitrogen?
Correct answer: The double-bonded oxygen has a formal charge of 0; each single-bonded oxygen has a formal charge of -1.

Accepted Answer

The double-bonded oxygen has a formal charge of 0; each single-bonded oxygen has a formal charge of -1.

Question 6

Which of the following best describes the bonding in metallic solids such as copper (Cu)?
Correct answer: Atoms are surrounded by a 'sea' of delocalized valence electrons, allowing for conductivity and malleability.

Accepted Answer

Atoms are surrounded by a 'sea' of delocalized valence electrons, allowing for conductivity and malleability.

Question 7

Which of the following statements about electronegativity is correct?
Correct answer: Electronegativity increases across a period and up a group.

Accepted Answer

Electronegativity increases across a period and up a group.

Question 8

A molecule of boron trifluoride (BF3) is known to violate the octet rule. Which type of octet exception does it represent?
Correct answer: Incomplete octet

Accepted Answer

Incomplete octet

Question 9

Which of the following best describes the difference between a sigma (σ) bond and a pi (π) bond?
Correct answer: A sigma bond is the first bond formed between two atoms and is stronger than a pi bond, which is formed by the side-to-side overlap in double or triple bonds.

Accepted Answer

A sigma bond is the first bond formed between two atoms and is stronger than a pi bond, which is formed by the side-to-side overlap in double or triple bonds.

Question 10

Which of the following molecules contains a free radical?
Correct answer: NO

Accepted Answer

NO

Question 11

A student draws the Lewis structure for the sulfate ion $$(SO4^2$$−) and assigns all single bonds between sulfur and oxygen. What is the formal charge on the sulfur atom in this structure?
Correct answer: +2

Accepted Answer

+2

Question 12

Which of the following best explains why metals are good conductors of electricity?
Correct answer: Their valence electrons are free to move throughout the lattice.

Accepted Answer

Their valence electrons are free to move throughout the lattice.

Question 13

Which of the following pairs of atoms would form a bond with the greatest ionic character?
Correct answer: Na and F

Accepted Answer

Na and F

Question 14

How many sigma (σ) and pi (π) bonds are present in a molecule of ethyne (C2H2)?
Correct answer: 3 sigma, 2 pi

Accepted Answer

3 sigma, 2 pi

Question 15

Which of the following is the correct Lewis dot symbol for the chloride ion (Cl−)?
Correct answer: Cl with 8 dots and a negative sign

Accepted Answer

Cl with 8 dots and a negative sign

Question 16

Which of the following statements about lone pairs is correct?
Correct answer: Lone pairs are nonbonding pairs of electrons localized on an atom.

Accepted Answer

Lone pairs are nonbonding pairs of electrons localized on an atom.

Question 17

Which of the following molecules is expected to have the largest dipole moment?
Correct answer: H2O

Accepted Answer

H2O

Question 18

A student is asked to draw the Lewis structure for the ammonium ion (NH4+). How many valence electrons should be used in the structure?
Correct answer: 8 (5 from N + 4 from H − 1 for the positive charge)

Accepted Answer

8 (5 from N + 4 from H − 1 for the positive charge)

Question 19

Which of the following best describes the process of assigning formal charges in a Lewis structure?
Correct answer: Subtract the sum of nonbonding electrons and bonds from the number of valence electrons for each atom.

Accepted Answer

Subtract the sum of nonbonding electrons and bonds from the number of valence electrons for each atom.

Question 20

Which of the following is a real-world example of a molecule with an expanded octet, and what property does this confer?
Correct answer: SF6, which allows sulfur to form six bonds and act as a potent greenhouse gas.

Accepted Answer

SF6, which allows sulfur to form six bonds and act as a potent greenhouse gas.

Chemical Bonding and Lewis Dot Structures Overview

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