Chemistry: Covalent Structures and Properties

Different structural forms of the same element.

A giant covalent structure with strong covalent bonds throughout, resulting in a very hard and strong material.

A giant covalent structure with strong covalent bonds within layers, but weak attraction forces between layers, making it a good lubricant.

A simple molecular structure containing 60 carbon atoms arranged in a spherical shape, with strong covalent bonds within the molecule and weak intermolecular forces between molecules.

A type of structure where atoms are held together by strong covalent bonds, forming a large network extending in all directions.

A very strong bond between atoms where they share electrons.

A material that has a very high melting and boiling point because the strong covalent bonds require a lot of energy to break.

A material that is very hard and resistant to scratching because the strong covalent bonds prevent atoms from sliding past each other easily.

A material that does not conduct electricity because all its electrons are locked into strong bonds, making it difficult for them to flow easily.

A material that is insoluble in most solvents because the strong covalent bonds are too strong to be broken apart by the solvent.

A naturally occurring compound found in sand, quartz, and many minerals.

Each silicon atom is connected to four oxygen atoms, and each oxygen atom is connected to two silicon atoms, forming a vast, three-dimensional network.

Diamond has strong covalent bonds throughout its giant structure, making it very hard and requiring a large amount of energy to melt or boil.

Graphite has layered structures with weaker forces between the layers, which allows the material to be soft and conduct electricity.

Fullerenes have weaker intermolecular forces, causing lower melting/boiling points and lower hardness compared to diamond.

Diamond does not conduct electricity due to its rigid structure and the absence of free electrons.

Graphite's structure allows for the movement of electrons between its layers, enabling electrical conductivity.