Diamonds and Carbon

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

Tags

NGSS.HS-PS2-6

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.

Tags

NGSS.HS-PS1-3

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

Tags

NGSS.HS-PS2-6

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.

Tags

NGSS.HS-PS2-6