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iGCSE Chemistry > 4.1 Covalent Bonding > Flashcards

4.1 Covalent Bonding Flashcards

1
Q

Define covalent bonding

A

electrostatic attraction between two positively charge nuclei and a shared pair of electrons

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2
Q

What is a simple molecule?

A

small group of atoms held together by covalent bonds

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3
Q

What does the shared pair of electrons do?

A

pull the nuclei of atoms closer together

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4
Q

Covalent bonding is very…

A

strong

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5
Q

Why does simple molecular substances have low boiling points?

A

the weak intermolecular forces break but not bonds

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6
Q

Intermolecular forces are very…

A

weak

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7
Q

Where do intermolecular forces act?

A

in between the molecules

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8
Q

Where do the covalent bonds act?

A

in the molecules , making the molecules

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9
Q

Why does molecular mass increase with boiling point?

A

strength of intermolecular forces increases
more energy needed

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10
Q

Can simple molecular molecules conduct electricity?

A

cannot conduct because a charge is needed

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11
Q

What is C60 fullerene?

A

simple molecule made of 60 carbon atoms

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12
Q

Why does C60 fullerene have a low boiling point?

A

simple molecule
-> weak intermolecular forces
-> not much energy needed

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13
Q

C60 fullerene has a….

A

low boiling point

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14
Q

What are the properties of C60 fullerene?

A

soft and slippery
electrical insulator

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15
Q

Why is C60 fullerene soft and slippery?

A

molecules can roll over each other

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16
Q

Why is C60 fullerene an electrical insulator?

A

molecules are neutral NOT charged

17
Q

What is diamond?

A

form of pure carbon arranged into giant lattice

18
Q

What structure does diamond have?

A

giant lattice
every Carbon has 4 covalent bonds so no free bonds
tetrahedral shape
strong
grid like shape

19
Q

How many covalent bonds does each carbon have in diamond?

A

4
none free

20
Q

What shape is diamond?

A

tetrahedral

21
Q

Why does diamond sublime at every temperature?

A

covalent bonds are strong
lots of bonds in giant lattice
lots of energy needed to break

22
Q

Why is diamond used for cutting?

A

it is very hard

23
Q

What is diamond used for?

A

cutting glass

24
Q

Why cannot diamond
conduct electricity?

A

no freely moving particles
all atoms neutral
all electrons in atom or bond

25
Q

What is graphite?

A

pure carbon arranged into a giant lattice

26
Q

What is the structure of graphite?

A

layers of hexagons of Carbon atoms
every carbon has 3 covalent bonds
weak intermolecular forces
delocalised electrons inside each layer

27
Q

Why does graphite sublime at a high temperature?

A

covalent bonds are strong
lots of bonds in giant lattice
lots of energy needed to break

28
Q

What are the properties of graphite?

A

soft and slippery
conducts electricity

29
Q

What is graphite used for?

A

solid lubricant

30
Q

Why is graphite used as a solid lubricant?

A

soft and slippery

31
Q

Why can graphite conduct electrcity?

A

delocalised electrons can move freely

32
Q

What is silicon dioxide?

A

giant covalent substance made of silicon and oxygen

33
Q

What is another name for silicon dioxide?

A

silica

34
Q

What is the structure of silicon dioxide?

A

every silicon has 4 covalent bonds
every oxygen has 2 covalent bonds
tetrahedral shape
strong
grid-like arrangement

35
Q

Why does silicon dioxide sublime at high temperatures?

A

covalent bonds are strong
lots of bonds in giant lattice
lots of energy needed to break

36
Q

What elements does covalent bonding occur between?

A

non metal + non metal

37
Q

Are covalent bonds insulators or conductors?

A

insulators

38
Q

Why is Graphite so soft?

A

layers of hexagons can slide

39
Q

Why is Diamond so hard?

A

lots of covalent bonds

iGCSE Chemistry (10 decks)

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