Understanding Molecular Solids

The video tutorial discusses molecular solids, comparing them with ionic and metallic solids. It explains how non-metals form molecular solids through covalent bonds and are held together by weak dispersion forces, resulting in low melting points. Examples like iodine and dry ice illustrate these concepts. The video also compares the melting points of molecular iodine and chlorine, highlighting the role of dispersion forces in determining melting points.

What type of bond holds the atoms together in molecular solids?

• Hydrogen bonds

• Ionic bonds

• Covalent bonds

• Metallic bonds

What forces hold the molecules together in a molecular solid?

• Ionic forces

• Covalent bonds

• London dispersion forces

• Metallic bonds

Why do molecular solids generally have low melting points?

• They have a sea of electrons.

• They are held together by strong ionic bonds.

• They are held together by weak dispersion forces.

• They are composed of heavy atoms.

What is the melting point of solid iodine?

• 101.5 degrees Celsius

• 113.7 degrees Celsius

• 78.5 degrees Celsius

• 0 degrees Celsius

Which of the following is a characteristic of molecular solids?

• Strong metallic bonds

• Weak intermolecular forces

• High melting points

• High electrical conductivity

Why are molecular solids poor conductors of electricity?

• They have high melting points.

• They have a sea of electrons.

• They lack free-moving charged particles.

• They are composed of metals.

What happens to solid carbon dioxide when it is heated?

• It sublimes directly into a gas.

• It melts into a liquid.

• It remains solid.

• It decomposes into carbon and oxygen.

What is the process called when a solid turns directly into a gas?

• Sublimation

• Freezing

• Condensation

• Melting

Why does iodine have a higher melting point than chlorine?

• Chlorine has more electrons.

• Iodine has stronger dispersion forces.

• Iodine has stronger ionic bonds.

• Chlorine has a larger atomic size.

What type of intermolecular force is primarily responsible for holding molecular solids together?

• London dispersion forces

• Dipole-dipole interactions

• Ionic interactions

• Hydrogen bonding