giant covalent molecules Flashcards

1
Q

What state are giant covalent molecules in room temp, and why?

A

they are always solid, as they have a high melting and boiling point (millions of strong covalent bonds)

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2
Q

what is a diamond formed from

A

the element carbon

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3
Q

how many covalent bonds does each carbon atom form in diamond

A

4 strong covalent bonds, meaning they have many covalent bonds, meaning they have a high melting and boiling point

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4
Q

can diamonds conduct electricity, and why

A

diamonds cannot conduct electricity, there are no free electrons to carry a charge

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5
Q

silicon dixoide is what and waht combined

A

silicon and oxygen

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6
Q

silicon dioxide, all properties

A
  • has a very high melting and boiling point
  • huge number of strong covalent bonds must be broken, takes a great deal of energy
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7
Q

graphite properties

A
  • has high melting and boiling point (due to many strong covalent bonds)
  • graphite is soft and slippery

-graphite is an excellent conductor of both electricity and of heat

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8
Q

what does graphite form from, and how many covalent bonds does each element form

A
  • graphite formed from element carbon
  • each carbon atom forms 3 covalent bonds

the carbon atoms form hexagonal rings

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9
Q

why is graphite slippery

A

as the hexagonal rings are in layers, and there are no covalent bonds in between them, meaning the layers can slide

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10
Q

why is graphite good for conducting heat and electricity

A

as they have de localised electrons (they can move)

each carbon atom has a single electron thats not in the covalent bond

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