Types of substances

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What are the properties of ionic compounds?
•Strong electrostatic forces of attraction in all directions between oppositely charged ions. •High melting and boiling points. •Conduct electricity as a liquid because they have delocalised electrons. •Don't conduct electricity as a solid.
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What are the properties of simple molecular compounds?
•low boiling and melting points. •weak intermolecular forces between the molecules. •Don't conduct electricity.
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What are the properties of giant covalent structures?
•High melting points. •linked to other atoms by strong covalent bonds.
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What are the properties of metals?
•Regular pattern •Delocalised electrons •High melting and boiling points •Conduct heat and electricity • Can be bent and shaped
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Recall that graphite and diamond are different forms of carbon and that they are examples of giant covalent substances
Diamond:joined to 4 other carbons covalently, has a very high melting point and does not conduct electricity. Graphite: covalently bonded to 3 other carbons,slide over each other, One electron from each carbon atom is delocalised.
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Why is graphite used to make electrodes and as a lubricant?
Electrodes – graphite can conduct electricity. Lubricant – weak intermolecular forces and no covalent bonds between the layers, therefore it is soft and slippery
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Why is diamond used in cutting tools?
Cutting tools – very hard, due to its rigid structure so won't break easily.
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Other cards in this set

Card 2

Front

What are the properties of simple molecular compounds?

Back

•low boiling and melting points. •weak intermolecular forces between the molecules. •Don't conduct electricity.

Card 3

Front

What are the properties of giant covalent structures?

Back

Preview of the front of card 3

Card 4

Front

What are the properties of metals?

Back

Preview of the front of card 4

Card 5

Front

Recall that graphite and diamond are different forms of carbon and that they are examples of giant covalent substances

Back

Preview of the front of card 5
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