A form of carbon that has a regular three-dimensional giant structure and whose atoms each form four covalent bonds to other carbon atoms, making it hard and transparent.
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What is graphite?
A form of carbon. In graphite atoms are covalently bonds to three other carbon atoms in giant flat two-dimensional layers with no covalent bonds between layers, so they slide over each other, making graphite slippery and grey.
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How can graphite conduct electricity?
Because of the delocalised elections in its structure.
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What are giant covalent structures?
Atoms of some elements can form several covalent bonds. These atoms can join together in giant covalent structures. Every atom in the structure is jointed to several other atoms by strong covalent bonds.
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What are giant covalent structures sometimes called?
Macromolecules.
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What compound has a similar structure to diamond?
Silicon dioxide (silica).
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In graphite, what happens to the electrons in each carbon atom?
One electron from each carbon atom is delocalised, rather like electrons in a metal. The delocalised electrons allow granite to conduct heat and electricity.
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How can the layers in graphite slide over each other easily?
There are only weak intermolecular forces between the layers.
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What are fullerenes?
Large molecules formed from hexagonal rings of carbon atoms.
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What do the hexagonal rings of fullerenes do?
Joint together to form cage-like shapes with different numbers of carbon atoms, some of which are nano-sized.
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Why are fullerenes important?
Scientists are finding many applications for fullerenes, including drug delivery into the body, lubricants, catalysts and reinforcing materials.
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Why do substances with giant covalent structures have very high melting points?
Every atom is joined to several other atoms, many strong covalent bonds have to be broken and so it takes a large amount of energy to melt the giant structure.
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What similarities are there between diamond and graphite?
Both forms of carbon; giant covalent structures; covalent bonding.
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What differences are there between diamond and graphite?
What similarities are there between graphite and fullerenes?
Forms of carbon; hexagonal rings of atoms.
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What differences are there between graphite and fullerenes?
Graphite=giant structure/fullerenes=molecules; graphite=two-dimensional/fullerenes=three-dimensional, cage-like; graphite=forms large particles/fullerenes=many are nano-sized.
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Why do diamond and graphite both have very high melting points?
Because they are both giant covalent structures.
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**YOU NEED TO BE ABLE TO EXPLAIN THE DIFFERENCES IN THE PROPERTIES OF GRAPHITE AND DIAMOND IN TERMS OF INTERMOLECULAR FORCES AND DELOCALISED ELECTRONS**
**LOOK AT DIAGRAMS OF GIANT COVALENT STRUCTURES**
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Other cards in this set
Card 2
Front
What is graphite?
Back
A form of carbon. In graphite atoms are covalently bonds to three other carbon atoms in giant flat two-dimensional layers with no covalent bonds between layers, so they slide over each other, making graphite slippery and grey.
Card 3
Front
How can graphite conduct electricity?
Back
Card 4
Front
What are giant covalent structures?
Back
Card 5
Front
What are giant covalent structures sometimes called?
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