Giant covalent structures

What is a giant covalent structure?

A giant covalent structure is a network of atoms bonded together by strong covalent bonds in a continuous, repeating pattern.

What is the structure of diamond?

In diamond, each carbon atom is covalently bonded to four other carbon atoms in a tetrahedral 3D structure, forming a rigid network.

Why is diamond hard?

Diamond is extremely hard because it has a strong 3D network of covalent bonds that are very difficult to break.

What is the structure of graphite?

Graphite consists of layers of carbon atoms arranged in hexagonal rings, with weak forces between the layers.

Why does graphite conduct electricity?

Graphite conducts electricity because it has delocalised electrons within the layers that can move freely, allowing the flow of electricity.

What is the structure of silicon dioxide (SiO₂)?

Silicon dioxide has a 3D lattice structure where each silicon atom is covalently bonded to four oxygen atoms, creating a very strong network.

Why does silicon dioxide have a high melting point?

Silicon dioxide has a strong covalent bond network, meaning a large amount of energy is needed to break the bonds, resulting in a high melting point.

What are the properties of giant covalent structures?

Giant covalent structures typically have high melting points, are hard, and do not conduct electricity (except for graphite).

What is the difference between diamond and graphite?

Diamond has a rigid 3D structure with strong bonds in all directions, while graphite has layers with weak forces between them, allowing layers to slide over each other.

Why is graphite used as a lubricant?

Graphite is used as a lubricant because its layers can slide over each other easily due to the weak forces between them, reducing friction.

What is an example of a giant covalent structure?

Diamond, graphite, and silicon dioxide are all examples of giant covalent structures.

What is the bonding in a giant covalent structure?

In a giant covalent structure, atoms are bonded by strong covalent bonds that extend throughout the entire structure.

Why do giant covalent structures not conduct electricity?

Most giant covalent structures do not conduct electricity because they do not have free electrons or ions to carry charge (except graphite, which has delocalised electrons).

Why is graphite soft compared to diamond?

Graphite is soft because its layers can easily slide over one another, whereas diamond has a rigid 3D structure that makes it very hard.

What is a key difference in the atomic arrangement between diamond and silicon dioxide?

In diamond, each carbon atom is bonded to four other carbon atoms, forming a strong 3D structure, while in silicon dioxide, each silicon atom is bonded to four oxygen atoms, forming a tetrahedral network.