Chemistry Quiz: Diamond and Graphite Properties

What is the structure of diamond in terms of its covalent bonding?

• Octahedral

• Tetrahedral

• Trigonal planar

• Linear

How does the structure of diamond contribute to its hardness and high melting point?

• The structure of diamond is composed of alternating layers of carbon atoms

• The structure of diamond is made up of weak metallic bonds

• Diamond has a structure with no covalent bonds

• The structure of diamond consists of a network of carbon atoms bonded together by strong covalent bonds in a tetrahedral arrangement.

Explain the electrical conductivity of diamond based on its giant covalent properties.

• Diamond's electrical conductivity is high due to its giant covalent properties.

• Diamond's electrical conductivity is moderate due to its giant covalent properties.

• Diamond's electrical conductivity is variable due to its giant covalent properties.

• Diamond's electrical conductivity is low due to its giant covalent properties.

What is the structure of graphite in terms of its covalent bonding?

• Spherical structure with weak covalent bonds

• Layered structure with strong covalent bonds within the layers

• Linear structure with ionic bonds

• Amorphous structure with metallic bonds

How does the structure of graphite contribute to its ability to conduct electricity?

• Graphite has a linear structure that prevents electron movement

• The structure of graphite is made of non-conductive materials

• Graphite has a closed structure that traps electrons

• The structure of graphite consists of layers of carbon atoms arranged in hexagonal rings, allowing delocalized electrons to move freely between the layers.

Compare the physical properties of diamond and graphite in terms of hardness, density, and transparency.

• Diamond is softer, less dense, and less transparent than graphite.

• Graphite is harder, less dense, and more transparent than diamond.

• Graphite is harder, denser, and more transparent than diamond.

• Diamond is harder, denser, and more transparent than graphite.

Explain the thermal conductivity of graphite based on its giant covalent properties.

• High thermal conductivity due to lack of free electrons

• Low thermal conductivity due to strong metallic bonds

• High thermal conductivity due to delocalized electrons between layers

• Low thermal conductivity due to absence of covalent bonds

Describe the lubricating properties of graphite based on its structure and bonding.

• Graphite has lubricating properties due to its spherical structure and strong intermolecular forces.

• Graphite has lubricating properties due to its linear structure and covalent bonding.

• Graphite has lubricating properties due to its layered structure and weak intermolecular forces.

• Graphite has lubricating properties due to its cubic structure and metallic bonding.