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Chemistry Paper 1 > Structure and Bonding > Flashcards

Structure and Bonding Flashcards

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1
Q

what is ionic bonding between?

A

a metal and a non-metal

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2
Q

what is the aim of ionic bonding?

A

both elements achieve a full outer energy level

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3
Q

what are giant ionic lattices? (2)

A
  • where every positive ion is surrounded by negative ions
  • have strong forces of attraction between the positive and negative ions (electrostatic forces)
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4
Q

the two key points about ionic compounds:

A
  1. have very high melting and boiling points

because the strong electrostatic forces require a great deal of energy to break

  1. can not conduct electricity when they are solids

because the ions can not move - they are locked in place by the strong electrostatic forces of attraction

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5
Q

what is covalent bonding between?

A

a non-metal and a non-metal

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6
Q

define covalent bonding

A

sharing an electron, or electrons, to achieve a full outer energy level

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7
Q

two key properties of small covalent molecules:

A
  1. have low melting and boiling points

because there are weak intermolecular forces between the molecules that do not require a great deal of energy to break

  1. they are usually gases or liquids at room temperature
  2. do not conduct electricity

because the molecules do not have an overall electric charge

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8
Q

two key properties of giant covalent molecules:

A
  1. always solids at room temperature

because they have millions of strong covalent bonds

  1. always have high melting and boiling points
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9
Q

which element is diamond formed from?

A

carbon

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10
Q

key properties of diamond: (3)

A
  1. each carbon atom forms four strong covalent bonds
  2. diamonds have a huge number of strong covalent bonds and these have to be broken when diamond is melted

this requires a great deal of energy

  1. diamond can not conduct electricity

there are no free electrons to carry electrical charge

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11
Q

key properties of silicon dioxide:

A
  1. has a very high melting and boiling point

because it has a huge number of strong covalent bonds that need to be broken and this requires a great deal of energy

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12
Q

two examples of giant covalent molecules?

A

diamond
silicon dioxide

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13
Q

what are the three properties of graphite?

A
  • has a high melting and a boiling point
  • soft and slippery
  • an excellent conductor of both electricity and heat
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14
Q

which element is graphite formed from?

A

carbon

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15
Q

how many bonds does each carbon atom form in graphite?

A

three covalent bonds

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16
Q

why does graphite have a high melting and boiling point?

A

because it has many strong covalent bonds and so it takes a great deal of energy to break these

17
Q

why is graphite slippery? (2)

A
  • the hexagonal rings are in layers
  • there are no covalent bonds between the layers and so they can slide
18
Q

why is graphite a good conductor of heat and electricity?

A

because it has a sea of delocalised electrons that can move freely

19
Q

what is graphene? (2)

A
  • a single layer of graphite
  • one atom thick
20
Q

what are the properties of graphene? (2)

A
  • excellent conductor of electricity because it has delocalised electrons
  • graphene is extremely strong
21
Q

what are fullerenes? (3)

A
  • molecules of carbon atoms with hollow shapes
  • usually have hexagonal rings of carbon atoms
  • can also have rings with five or seven carbon atoms
22
Q

what was the name of the first fullerene to be discovered?

A

buckminsterfullerene

23
Q

what are the uses of fullerenes? (3)

A
  • pharmaceutical delivery
  • lubricants
  • catalysts
24
Q

what are the properties of carbon nanotubes? (2)

A
  • have high tensile strength ( can be stretched without breaking)
  • excellent conductors of heat and electricity
25
Q

what are the uses of carbon nanotubes?

A
  • used to reinforce materials e.g. in tennis rackets
26
Q

what are polymers?

A

very large molecules - made by joining together thousands of small, identical molecules (monomers)

27
Q

what are the key properties of polymers?

A
  • most are solids at room temperature because the intermolecular forces of attraction between polymer molecules are relatively strong
28
Q

what is the key property of a metal?

A
  • they can be bent and shaped because in metals, the layers of atoms are able to slide over each other
29
Q

what is an alloy?

A

a mixture of metals

30
Q

what is the key property of of alloys? (2)

A
  • the different sizes of atoms distorts the layers, making it more difficult for them to slide over each other
  • alloys are harder than pure metals

Chemistry Paper 1 (5 decks)

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