C2 - Giant Covalent Structures

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What are the properties of simple covalent molecules?
Low melting and boiling points, usually soft and brittle, shatter when hit, does not conduct electricity.
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Why do simple covalent molecules have the properties they do?
Weak intermolecular forces.
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What is covalent bonding?
The bonding of NON METALS.
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Name some giant covalent structures.
Silicone Dioxide (Sand), Diamond (Carbon), Graphite (carbon) Fullerines (carbon)
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What are different forms of the same element called?
Allotropes (Diamond and Graphite are allotropes)
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What is diamond made of?
Carbon
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In diamond, each carbon is bonded to how many other atoms?
4/4
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What are the properties of diamond?
Strong, high melting and boiling points, very hard, can't conduct, because of strong covalent bonds
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Why is graphite soft and slippery?
Weak intermolecular forces. Bonded to 3 instead of four. Arranged in layers.
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Can graphite conduct?
Yes, due to having delocalized electrons.
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Describe the structure of fullerenes (double covalent bonds)
Carbon, with each carbon bonded to 3 others, strong covalent bonds, will not conduct, HMP, HBP.
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Describe the structure and properties of Silicone Dioxide.
Giant, made of silicon and oxygen, each silicon bonded to 4 oxygens, strong covalent bonds, does not conduct, HMP, HBP, hard.
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Why is silicon dioxide a suitable material for lining furnaces?
HMP HBP, strong covalent bonds, does not conduct, giant lattice structure
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Other cards in this set

Card 2

Front

Why do simple covalent molecules have the properties they do?

Back

Weak intermolecular forces.

Card 3

Front

What is covalent bonding?

Back

Preview of the front of card 3

Card 4

Front

Name some giant covalent structures.

Back

Preview of the front of card 4

Card 5

Front

What are different forms of the same element called?

Back

Preview of the front of card 5
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