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Chemistry Paper 1 > C2 - Bonding, Structure and Properties of Matter > Flashcards

C2 - Bonding, Structure and Properties of Matter Flashcards

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1
Q

Define Covalent bond.

A

A shared pair of electrons between two non-metals.

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2
Q

What are the properties of diamond?

A

4 covalent bonds for each carbon atom.
High melting point.
Hard (strong bonds).
Doesn’t conduct (no delocalized electrons).

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3
Q

What are Electrostatic forces?

A

The strong forces of attraction between oppositely charged ions.

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4
Q

What is Graphene?

A

A single layer of graphite.

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5
Q

Define gas.

A

The state of matter where the particles have the most energy. The particles in a gas are relatively spread out and move randomly in all directions.

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6
Q

What are polymers?

A

Large molecules made by linking together large numbers of smaller molecules called monomers.

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7
Q

What are Nanoparticles?

A

Nanoparticles have diameters between 1 nm to 100 nm in size.

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8
Q

What are the properties of Graphite?

A
  • A giant covalent structure of carbon atoms.
  • Three covalent bonds.
  • Layers of hexagonal rings held together by weak intermolecular forces
  • Which means that layers are free to slide and can be used as a lubricant.
  • High melting point due to strong covalent bonds.
  • Conducts heat and electricity due to one delocalised electron per carbon atom.
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9
Q

What is an ion?

A

An atom or molecule with an electric charge due to the loss or gain of electrons.

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10
Q

What is an ionic compound?

A

A giant structure of ions held together by strong electrostatic forces.

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11
Q

What are intermolecular forces?

A

The forces which exist between molecules. The strength of the intermolecular forces in covalent bonds impact physical properties like the boiling/melting point.

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12
Q

What is a lattice?

A

A repeating regular arrangement of atoms/ions/molecules. This arrangement occurs in crystal structures.

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13
Q

What is ionic bonding?

A

Electrostatic attraction between positive and negative ions.

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14
Q

How are ionic compounds held together?

A

Held together in a giant lattice.
Strong electrostatic attractions holds the structure together.

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15
Q

State the properties of ionic substances.

A

High melting point and boiling point.
Do not conduct electricity when solid.
Conduct electricity when molten or dissolved in water- ions are free to move.

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16
Q

How are ionic compounds formed? In the MgO case.

A

The reaction of a metal and a non-metal. Magnesium is in group 2 so can give away 2 electrons. Oxygen is in group 6 so can gain two electrons to get a full outer shell.
Mg becomes Mg 2+.
O becomes O 2-.

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17
Q

What is a covalent bond?

A

The electrostatic attraction between a shared pair of electrons and the nuclei of the atoms, between two non-metals.

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18
Q

What are the properties of molecular covalent substances?

A

Doesn’t conduct - no ions.
Low melting and boiling points because of the weak inter-molecular forces.

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19
Q

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

A

Inter-molecular forces increase as well.

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20
Q

Define monomer.

A

A molecule that can be bonded to other identical molecules to form a polymer.

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21
Q

Name 5 allotropes of carbon.

A

Graphite
Graphene
Diamond
Fullerenes
Nanotubes

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22
Q

What are Fullerenes?

A
  • Fullerenes are molecules of carbon atoms with hollow shapes.
  • Their structures are based on hexagonal rings of carbon atoms joined by covalent bonds.
  • Some fullerenes include rings with five or seven carbon atoms.
  • Two examples of fullerenes are buckminsterfullerene and nanotubes .
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23
Q

What is a Nanotube?

A

High length to diameter ratio.
Layer of graphene rolled into a cylindrical shape.
High tensile strength (strong bonds).
Conductivity due to delocalised electrons.
Fullerene.

24
Q

What is metallic bonding?

A

Electrostatic attraction between positive nuclei of metal ions and delocalised electrons.

25
Q

Describe the properties of metals.

A

High melting/boiling points (strong forces of attraction).
Conduct electricity and heat due to mobile electrons which can move through the structure.
Malleable as layers of ions can slide over each other.

26
Q

What are alloys and why are they harder than pure metals?

A

Alloys are mixtures of metals with other elements (usually metals).
They are harder because the different sized atoms distort the layers found in pure metals, so they can’t slide over each other.

27
Q

What does the amount of energy needed to change state depend on?

A

The strength of the bonds.

28
Q

What is nanoscience?

A

Science that studies particles that are 1 - 100 nm in size.

29
Q

State the uses of nanoparticles.

A

Medicine
Electronics
Deodorant
Sun cream (better skin coverage and more effective protection against cell damage)

30
Q

Why are ionic structures always giant?

A

Because each ion attracts several ions of the opposite charge.

31
Q

Why do ionic compounds have a high melting and boiling point?

A

Many strong ionic bonds holding them together.

32
Q

Properties of giant covalent substances.

A

High melting and boiling point due to many strong covalent bonds holding them together.

33
Q

What does high tensile strength mean?

A

They are strong in tension and resist being stretched.

34
Q

What are buckyballs?

A

Buckyballs are spheres or squashed sphered of carbon atoms.
Made up of large molecules.
They do not have a giant covalent structure.
And have weak intermolecular forces exist in between each individual buckyball.

35
Q

What is an ionic lattice?

A
  • giant structure
  • formed by ions
  • held together by electrostatic forces acting in all directions
36
Q

What is the difference in the boiling points of simple molecular substances and giant covalent substances?

A

Simple molecular - low boiling point as weak intermolecular forces
Giant covalent - high boiling points, lots of strong bonds need to be broken.

37
Q

Boiling/melting point of simple molecular.

A

Low - weak intermolecular forces.

38
Q

Boiling/melting point of ionic.

A

High - Giant lattice of ions with strong electrostatic forces between oppositely charged ions.

39
Q

Boiling/melting point of giant covalent.

A

High - strong covalent bonds between atoms in a giant structure.

40
Q

Boiling/melting point of metallic.

A

High - strong electrostatic forces between delocalised electrons and positive ions.

41
Q

What type of structure does graphite have?

A

A giant covalent structure of carbon atoms.

42
Q

What type of bonds do graphite have?

A

3 covalent bonds.

43
Q

What are the layers of hexagonal rings in graphite held together by?

A

Weak intermolecular forces.

44
Q

Why can graphite be used as a lubricant?

A

Because of the weak intermolecular forces in between the layers meaning the layers are free to slide over each other.

45
Q

How does graphite bonds affect its boiling point?

A

It has strong covalent bonds so it has a high melting point.

46
Q

Why does graphite conduct heat and electricity?

A

Because it has one delocalised electron per carbon atom.

47
Q

What structure does Graphite have?

A

A giant covalent structure of carbon atoms.

48
Q

How many bonds do the carbon atoms have in Graphite?

A

Three covalent bonds each with other carbon atoms.

49
Q

Why can layers of Graphite easily slide over each other?

A

The layers of hexagonal rings are held together by weak intermolecular forces.

50
Q

Why can Graphite be used as a lubricant?

A

The layers of hexagonal rings are held together by weak intermolecular forces so they can slide over each other easily.

51
Q

Does Graphite have a high or low melting point?

A

High melting point due to strong covalent bonds.

52
Q

Does Graphite conduct electricity and heat?

A

Yes. Because of one delocalised electron per carbon atom.

53
Q

Why would you expect metal chlorines to be solid at room temperature?

A

Usually ionic.
Ionic bonds have strong electrostatic forces between ions.

54
Q

Why is Buckminsterfullerene a good lubricant?

A

Molecules are spherical so they will role.

55
Q

Why is using nano particles cheaper than using larger particles?

A

Have a large surface area to volume ratio.
So less can be used for the same effect.

56
Q

Why is it not correct to say that the boiling point of a single bromine atom is 59 degrees Celsius?

A

Boiling point is a bulk property. It is to do with intermolecular forces between molecules.

Chemistry Paper 1 (6 decks)

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