Question 1

Which of the following best explains why metallic solids are good conductors of electricity?

Accepted Answer

They have a delocalized sea of electrons that can move freely throughout the lattice. $$	ext{Delocalized electrons allow for electrical conductivity.}$$

Question 2

Why are ionic solids typically brittle and likely to shatter when struck?

Accepted Answer

Applying a force causes like-charged ions to align and repel each other, breaking the solid apart. $$	ext{Force causes repulsion between like charges.}$$

Question 3

Which of the following is a property of covalent network solids such as diamond?

Accepted Answer

They have extremely high melting points due to strong covalent bonds throughout the structure.

Question 4

Which of the following best describes the bonding in metallic solids?

Accepted Answer

A lattice of positive metal cations surrounded by a sea of delocalized valence electrons.

Question 5

Why do molecular solids, such as sucrose, generally have lower melting points than ionic or covalent network solids?

Accepted Answer

The intermolecular forces (IMFs) holding the molecules together are much weaker than ionic or covalent bonds.

Question 6

Which of the following is NOT a characteristic property of most metals?

Accepted Answer

They are brittle and shatter easily when struck.

Question 7

Which of the following best explains why ionic solids have high melting and boiling points?

Accepted Answer

The strong electrostatic attraction between oppositely charged ions requires a large amount of energy to break.

Question 8

Which of the following is an example of a covalent network solid?

Accepted Answer

Silicon ($$\mathrm{Si})$$

Question 9

Which of the following best describes the difference between crystalline and amorphous solids?

Accepted Answer

Crystalline solids have a regular, repeating pattern of particles, while amorphous solids lack this order.

Question 10

Which of the following is a correct statement about the electrical conductivity of ionic solids?

Accepted Answer

Ionic solids conduct electricity only when melted or dissolved in water, because ions are free to move.

Question 11

Which of the following best explains why graphite can conduct electricity, but diamond cannot, even though both are forms of carbon?

Accepted Answer

Graphite has delocalized electrons between its layers, allowing for electrical conductivity, while diamond's electrons are localized in covalent bonds.

Question 12

Which of the following is a property of molecular solids?

Accepted Answer

They tend to be soft and have relatively low melting points due to weak intermolecular forces.

Question 13

A sample of glass is classified as which type of solid?

Accepted Answer

Amorphous solid

Question 14

Which of the following best describes the bonding in sodium chloride ($$\mathrm{NaCl}$$)?

Accepted Answer

A regular lattice of alternating positive and negative ions held together by electrostatic attraction.

Question 15

Which of the following is a reason why metals are malleable and ductile?

Accepted Answer

The delocalized electrons allow metal atoms to slide past each other without breaking the metallic bond.

Question 16

Which of the following is an example of a substitutional alloy?

Accepted Answer

Brass (copper and zinc)

Question 17

Which of the following intermolecular forces is NOT present in all molecular solids?

Accepted Answer

Hydrogen bonding

Question 18

Why does sucrose have a much higher melting point than most other molecular solids?

Accepted Answer

Each sucrose molecule has multiple $$-\mathrm{OH}$$ groups, allowing for extensive hydrogen bonding.

Question 19

Which of the following best explains why covalent network solids are much harder than molecular solids?

Accepted Answer

Covalent bonds are much stronger than intermolecular forces.

Question 20

Which of the following is a correct example of an amorphous solid?

Accepted Answer

Obsidian (volcanic glass/rock)

Types of Solids and Their Properties: Metallic, Ionic, Molecular, and Covalent Network Solids

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