C2 Covalent Bonding Flashcards

1
Q

How are covalent bonds formed?

A

by sharing electrons

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2
Q

Which type of atoms form covalent bonds between them?

A

non-metals

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3
Q

describe the structure and bonding of a giant covalent substance

A

billions of atoms bonded together by strong covalent bonds

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4
Q

properties of simple covalent substances

A

don’t conduct electricity
low melting and boiling
weak intermolecular forces

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5
Q

what are giant covalent substances

A

atoms bonded together in a giant lattice

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6
Q

properties of giant covalent substances

A

high melting and boiling point DUE to it needing lots of energy to break the strong covalent bonds between atoms

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7
Q

3 carbon allotropes

A

diamond
graphite
silicon dioxide

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8
Q

properties of diamond

A

~4 strong covalent bonds
for each C atom
~very strong
~very high melting point
~doesn’t conduct electricity

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9
Q

properties of graphite

A

~3 covalent bonds for each
C atom
~layers of hexagonal rings
~high melting point
~layers free to move / slide
~conduct electricity

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10
Q

Why can graphite conduct electricity?

A

As there is one delocalised electron per atom meaning that it can carry charge in a sea of delocalised electrons

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11
Q

What carbon fullerene has a spherical shape?

A

C60
buckminster fullerene

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12
Q

What are intermolecular forces?

A

forces of attraction that act with neighbouring particles

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13
Q

Why do small molecules have low melting points?

A

only a small amount of energy is needed to break the weak intermolecular forces

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14
Q

Why do large molecules have higher melting point in comparison to small molecules?

A

intermolecular forces are stronger in larger molecules

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15
Q

What is a nanotube?

A

hollow cylinder of carbon atoms

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16
Q

Give 3 uses for fullerenes

A

lubricants
drug delivery
high tech electronics

17
Q

Why does diamond have a high melting point?

A

Many strong covalent bonds which require lots of energy to break