Properties and uses Graphite has delocalised electrons, just like metals. These electrons are free to move between the layers in graphite, so graphite can conduct electricity. This makes graphite useful for electrodes in batteries and for electrolysis. The forces between the layers in graphite are weak.
What are the properties of graphite BBC Bitesize?
high melting and boiling points. Graphite’s many covalent bonds are strong and substantial energy is needed to break them. good electrical conductivity.
What is graphite GCSE?
Graphite is a giant covalent substance in which: each carbon atom is joined to three other carbon atoms by covalent bonds. the carbon atoms form a hexagonal layered network structure. the layers have weak forces between them and can slide over each other.
What are the uses of graphene BBC Bitesize?
Like graphite, graphene conducts electricity well because it has delocalised electrons that are free to move across its surface. These properties make graphene useful in electronics and for making composites .
Why is graphite used in pencils GCSE?
Graphite is used to make the core or ‘lead’ in pencils because it is soft. The layers are easily rubbed off to leave a mark on paper.
What are uses of graphite?
Graphite is used in pencils and lubricants. It is a good conductor of heat and electricity. Its high conductivity makes it useful in electronic products such as electrodes, batteries, and solar panels.
Why is graphite used as a lubricant BBC Bitesize?
The forces between the layers in graphite are weak. This means that the layers can slide over each other. This makes graphite slippery, so it is useful as a lubricant .
Why is graphite a good conductor of electricity GCSE?
Each carbon atom is bonded into its layer with three strong covalent bonds. This leaves each atom with a spare electron, which together form a delocalised ‘sea’ of electrons loosely bonding the layers together. These delocalised electrons can all move along together – making graphite a good electrical conductor.
Why is graphite a good conductor of electricity?
In a graphite molecule, one valence electron of each carbon atom remains free. Due to the free electrons in its framework, graphite can perform electricity. Therefore, graphite is said to be a good conductor of electricity.
Why is graphite used in pencils?
Graphite molecules are flat groups of carbon atoms that are stacked in layers. The layers slide against each other and allow the lead to slide off the pencil point and onto the paper. When you erase with a rubber eraser, the graphite in the lead sticks to the rubber better than it does to the paper.
What is graphene and graphite?
In very basic terms graphene could be described as a single, one atom thick layer of the commonly found mineral graphite; graphite is essentially made up of hundreds of thousands of layers of graphene.
What are nanotubes used for BBC Bitesize?
Nanotubes have high tensile strength , so they are strong in tension and resist being stretched. Like graphene, nanotubes are strong and conduct electricity because they have delocalised electrons. These properties make nanotubes useful for nanotechnology, electronics and specialised materials.
What is graphene BBC Bitesize?
Graphene is a single-atom thick layer of graphite with strong covalent bonds between each carbon atom. The atoms are arranged in hexagons. Its properties include: high melting and boiling points. Graphene’s many covalent bonds are strong and substantial energy is needed to break them.
What are the uses of graphite and diamond?
The atoms in graphite and diamond are strongly bonded with covalent bonds, forming different arrangements with each other. Diamonds are used in Jewelry making, construction, minor industrial applications, and surgeries. Graphites are used in stationery, lubricants, industries, or nuclear reactors.
Why is graphite soft GCSE?
This means that each carbon atom has a ‘spare’ electron (as carbon has four outer electrons) which is delocalised between layers of carbon atoms. These layers can slide over each other, so graphite is much softer than diamond.
Why graphite can be used as a solid lubricant and also as electrodes?
Graphite has delocalised electrons, just like metals. These electrons are free to move between the layers in graphite, so graphite can conduct electricity. This makes graphite useful for electrodes in batteries and for electrolysis.This makes graphite slippery, so it is useful as a lubricant .
What was graphite first used for?
The first documented use of graphite as a pencil occurred in 1565. The use of graphite as an art material became popular, sold by Flemish merchants throughout Europe.
How is graphite used in sports?
Graphene Technology
Such a rolled sheet is also referred to as graphene, and this derivative of graphite is the world’s strongest identified material and has been used to make super-strength, lightweight sports equipment.
Where is graphite used the most?
In pencils and lubricants, graphite is used. It is a strong heat and energy conductor. In electrical devices such as electrodes, batteries, and solar panels, its high conductivity makes it useful.
Why is graphite used as electrode in the process of electrolysis?
Graphite rods are used as electrodes in electrolysis because graphite’s structure enables it to be an excellent conductor. The high number of delocalized electrons allows electricity to pass through graphite rapidly.
Why does graphite have delocalised electrons?
Graphite form a giant covalent structure in which each carbon atom joined to three others carbon atoms by covalent bonds. So, each carbon atom has one free electron which are known as delocalised electrons. Due to these free electrons graphite conduct electricity.
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