Question 1

Which of the following elements is most likely to form an expanded octet in a stable compound?

Accepted Answer

Phosphorus (P)

Question 2

A patient is given a saline solution containing NaCl. Which type of chemical bond holds the Na and Cl atoms together in this compound, and what is the primary electron behavior?

Accepted Answer

Ionic bond; transfer of electrons

Question 3

Which of the following molecules has the most polar bond?

Accepted Answer

HF

Question 4

Which statement best explains why metals are good conductors of electricity?

Accepted Answer

Their electrons are delocalized and can move freely throughout the lattice.

Question 5

Given the following Lewis Dot Symbol: [P] with 8 dots and a 3− charge, which ion does this represent and why?

Accepted Answer

P3−, because phosphorus gains three electrons to achieve a noble gas configuration

Question 6

Which of the following best describes the trend in electronegativity across the periodic table?

Accepted Answer

It increases from left to right and decreases from top to bottom.

Question 7

A molecule of CO (carbon monoxide) has a triple bond between C and O. Using the formal charge formula, what is the formal charge on the carbon atom in CO?

Accepted Answer

+1

Question 8

Which of the following compounds is most likely to have a high melting point and conduct electricity when molten, but not when solid?

Accepted Answer

Sodium chloride (NaCl)

Question 9

Which of the following is an exception to the octet rule due to having an incomplete octet?

Accepted Answer

Beryllium chloride (BeCl2)

Question 10

Arrange the following molecules in order of increasing dipole moment: HI, HF, HBr, HCl.

Accepted Answer

HI \u003c HBr \u003c HCl \u003c HF

Question 11

A transition metal ion, Co+, is formed. Which of the following statements about its Lewis Dot Symbol is correct?

Accepted Answer

The number of valence electrons is less straightforward due to d-orbital involvement.

Question 12

Which of the following best describes the electron behavior in a covalent bond?

Accepted Answer

Electrons are shared between two nonmetal atoms.

Question 13

In the thiocyanate ion (SCN−), which atom carries the negative formal charge in the most stable Lewis structure?

Accepted Answer

Sulfur (S)

Question 14

Which of the following best explains why ionic bond formation is generally exothermic?

Accepted Answer

The electrostatic attraction between oppositely charged ions releases energy.

Question 15

A student is asked to draw the Lewis Dot Symbol for Cd2+. Which of the following is correct?

Accepted Answer

Cd2+ has no valence electrons shown as dots.

Question 16

Which of the following bonds is best classified as nonpolar covalent?

Accepted Answer

Br–Br

Question 17

A molecule has a bond with an electronegativity difference (ΔEN) of 1.6. How would you classify this bond?

Accepted Answer

Polar covalent

Question 18

Which property is NOT typically associated with metallic bonding?

Accepted Answer

Poor thermal conductivity

Question 19

Which of the following statements about formal charge is correct?

Accepted Answer

It helps identify the most stable Lewis structure for a molecule.

Question 20

Which of the following best explains why chlorine (Cl) has more valence electrons than calcium (Ca)?

Accepted Answer

Chlorine is in group 7A, so it has 7 valence electrons, while calcium is in group 2A with 2 valence electrons.

Chemical Bonding and Lewis Structures: Study Notes

Study Guide - Practice Questions

Study Guide - Flashcards