Question 1

Which of the following best explains why ionic bonds are generally stronger than covalent bonds when comparing compounds with similar atomic sizes and charges?

Accepted Answer

Ionic bonds are non-directional and result from strong electrostatic attractions between oppositely charged ions.

Question 2

Which of the following compounds is expected to have the highest melting point based on lattice energy considerations?

Accepted Answer

MgF$$_2$$

Question 3

A molecule of NO$$_2^-$$ has how many total valence electrons?

Accepted Answer

$$18$$

Question 4

Which of the following best describes the bonding in metallic solids such as sodium metal?

Accepted Answer

A sea of delocalized electrons shared among a lattice of cations

Question 5

Which of the following statements about the octet rule is FALSE?

Accepted Answer

Hydrogen typically forms bonds to achieve an octet of electrons.

Question 6

Which of the following best explains why ionic solids are brittle?

Accepted Answer

When struck, like charges are forced next to each other, causing repulsion and shattering.

Question 7

Which of the following bonds is the most polar, based on electronegativity differences?

Accepted Answer

Na–Cl

Question 8

What is the formal charge on the central nitrogen atom in the best Lewis structure of HNO$$_3$$?

Accepted Answer

$$+1$$

Question 9

Which of the following compounds contains both ionic and covalent bonds?

Accepted Answer

CaCO$$_3$$

Question 10

Which of the following best describes the trend in lattice energy as the size of the ions increases?

Accepted Answer

Lattice energy decreases as ion size increases.

Question 11

Which of the following is a correct statement about resonance structures?

Accepted Answer

Resonance structures have the same number of electrons and atom connectivity.

Question 12

Which of the following best explains why molecular compounds generally have lower melting points than ionic compounds?

Accepted Answer

Molecular compounds have weaker intermolecular forces compared to the strong electrostatic forces in ionic compounds.

Question 13

Which of the following is the correct formula unit for the ionic compound formed between calcium and bromine?

Accepted Answer

CaBr$$_2$$

Question 14

Which of the following best describes the relationship between bond order and bond length in covalent bonds?

Accepted Answer

As bond order increases, bond length decreases.

Question 15

Which of the following elements is the most electronegative?

Accepted Answer

Fluorine

Question 16

A diatomic molecule has a bond length of $$145 pm $$and a dipole moment of $$5.2 D. $$What is the percent ionic character if the maximum possible dipole moment is $$6.7 D$$?

Accepted Answer

$$77.6\%$$

Question 17

Which of the following best explains why solid NaCl does not conduct electricity, but molten NaCl does?

Accepted Answer

In the solid state, ions are locked in place and cannot move; in the molten state, ions are free to move and carry charge.

Question 18

Which of the following is the correct Lewis structure for arsenic (As)?

Accepted Answer

Five dots around the As symbol, with one pair and three single electrons.

Question 19

Which of the following best describes the effect of increasing ion charge on lattice energy?

Accepted Answer

Lattice energy increases as ion charge increases.

Question 20

Which of the following is a valid exception to the octet rule?

Accepted Answer

Boron forming compounds with six valence electrons.

Chemical Bonding and Lewis Structures: Mini-Textbook Study Notes

Study Guide - Practice Questions

Study Guide - Flashcards