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Chemistry > 2. Bonding, structure and the properties of matter (covalent bonding and the structure and bonding of carbon) > Flashcards

2. Bonding, structure and the properties of matter (covalent bonding and the structure and bonding of carbon) Flashcards

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1
Q

What is covalent bonding?

A

The sharing of electrons between non-metals

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2
Q

Why do non-metals gain electrons?

A

Because it is energetically unfavourable for them to lose electrons, so they gain electrons

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3
Q

What do covalent bonds form?

A

Covalent compounds

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4
Q

What 2 types of molecules can be formed as a result of covalent bonding?

A
  • Simple covalent molecules
  • Giant covalent structures/lattices
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5
Q

What are simple covalent molecules?

A

Molecules containing few atoms which are covalently bonded. Like H2, 02

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6
Q

What are examples of simple molecular covalent structures?

A

(H2, O2, Cl2, CH4)

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7
Q

What are the properties of simple molecular covalent substances?

A
  • low melting and boiling points
  • they are gases at room temperature
  • cannot conduct electricty
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8
Q

Why do simple molecular substances have low melting and boiling points?

A
  • The intermolecular forces between the molecules are very weak
  • So not a lot of energy is required to overcome them
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9
Q

Why do simple covalent molecules not conduct electricity?

A

Because there are no free electrons or ions to carry charge

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10
Q

What are examples of giant covalent structures/lattices?

A
  • Diamond
  • Graphite
  • Silicon dioxide
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11
Q

What does allotrope mean?

A

Different forms of something

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12
Q

What are the 3 giant covalent structures allotropes of?

A

Carbon

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13
Q

How many bonds can carbon atoms make in diamond?

A

4 bonds

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14
Q

What is diamond made up of?

A

Carbon atoms covalently bonded 4 times

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15
Q

What are the properties of diamond?

A
  • High melting and boiling points due to incredibly strong covalent bonds
  • Found as a solid
  • Very rigid structure
  • Does not conduct electricity because there are no free electrons or ions to carry charge
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16
Q

What is formed in graphite?

A

hexagonal structures

17
Q

What does graphite have?

A

A free, delocalised electron

18
Q

Why is graphite similar to metals?

A

Because it has a delocalised electron

19
Q

What are the properties of graphite?

A
  • High melting and boiling points because of the strong covalent bonds
  • Can conduct electricity because of the free delocalised electrons
  • It is arranged in layers of graphene that can be used as a lubricant, such as the lead in pencils
20
Q

Why can graphite be used as a lubricant (such as, led in pencils)?

A

As the layers slide off of each other as it made up of layers that are one atom thick

21
Q

What is graphene?

A

A single layer of graphite

22
Q

Does graphene have the same properties as graphite?

A

Yes

23
Q

What are fullerenes?

A

Carbon atoms arranged in hollow balls or closed tubes

24
Q

What can fullerenes be used for?

A
  • Drug delivery
  • Catalysts due to huge surface area
  • Lubricants
25
Q

What can graphene be used for?

A
  • Electronics
  • Improving strength of composite materials
26
Q

What is each grain of sand made out of?

A

Silicon dioxide

27
Q

How many times is the carbon atom bonded in graphite?

A

3 times

28
Q

What was the first fullerene to be discovered?

A

Buckminister fullerene (C60)

29
Q

What shape does buckminister fullerene have?

A

a spherical shape

30
Q

What is the structure of fullerenes?

A

hexagonal rings of carbon atoms

31
Q

What are nanotubes?

A
  • fullerenes which are tiny carbon cylinders
  • they are good conductor of heat and electricity
32
Q

What is this?

A

Nanotube

33
Q

What is this?

A

Buckminsterfullerene

34
Q

How do intermolecular forces change as the mass/size of the molecule increases?

A
  • they increase, so melting and boiling points also increase

Chemistry (34 decks)

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