Which best explains why graphite is a good lubricant? Carbon atoms form strong bonds within each graphite layer but weak bonds between layers. Carbon atoms in graphite form alternating single and double bonds. Each carbon atom in graphite forms weak covalent bonds with three other carbon atoms.

Question

Anastasia Ramos

Physics

21 September, 22:18

Which best explains why graphite is a good lubricant? Carbon atoms form strong bonds within each graphite layer but weak bonds between layers. Carbon atoms in graphite form alternating single and double bonds. Each carbon atom in graphite forms weak covalent bonds with three other carbon atoms.

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Answers (2)

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Brenda Bond · Answer 1

Carbon atoms form strong bonds within each graphite layer but weak bonds between layers.

Explanation:

Graphite is known as solid lubricant which means it is a lubricant which is in the solid state form.

Here we know that lubricant has function to make the relative movement very smooth or easy.

So here in structure of graphite it is formed in such a way that all carbon atoms in graphite layer are bonded strongly with each other. While two layers of graphite are weakly bonded to each other

So here two layers of graphite can easily slide over each other which is useful for the function of lubricants

So correct answer will be

Carbon atoms form strong bonds within each graphite layer but weak bonds between layers.

Thalia · Answer 2

Graphite is great lubricant because each carbon atom forms weak covalent bonds with three other carbon atoms.

Diamond and graphite both are entirely made up of carbon but both the elements are completely different because of the bonding of carbon atoms. In graphite the carbon atoms form weak covalent with the other three carbon atom due to which there is less or no force between the atoms, and makes the graphite very soft and slippery, and graphite act as lubricant.