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Chemistry > 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

Properties of a diamond.

A

4 covalent bonds for each carbon atom
High melting point
Hard (strong bonds)
Does not conduct (no delocalised 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

Nanoparticles

A

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

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8
Q

Properties of Graphite.

A

A giant covalent structure which is made up of carbon atoms
each of which form three covalent bonds with three other carbon atoms.
This forms layers of hexagonal rings held together by weak inter molecular forces which means that layers are free to slide and can be used as a lubricant.
High melting point due to strong covalent bonds.
Conduct thermal and electricity due to one delocalised electron per carbon atom.

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9
Q

Ion

A

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

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10
Q

Ionic compound

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 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 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

Reaction with a metal with 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 become 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

Properties of molecular covalent substances.

A

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

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19
Q

How do inter molecular 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.

21
Q

Name 5 allotropes of carbon.

A

Graphite
Graphene
Diamond
Fullerenes
Nanotubes

22
Q

What are Fullerenes?

A

Hollow shaped molecule
C60 has spherical shape, simple molecular structure (Buckminsterfullerene) means it has a low boiling point as there are weak intermolecular forces

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 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 a 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 nonoscience?

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 spheres of carbon atoms. They do not have a giant covalent structure. And have weak intermolecular forces between atoms.

35
Q

What is an ionic lattice?

A

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

What are the uses of nanoparticles?

A

Sun cream (better skin coverage)
Medicine
Electronics
Deoderant

38
Q

Boiling/melting point of simple molecular.

A

Low - weak intermolecular forces.

39
Q

Boiling/melting point of ionic.

A

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

40
Q

Boiling/melting point of giant covalent.

A

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

41
Q

Boiling/melting point of metallic.

A

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

42
Q

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

A

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

43
Q

Why is Buckminsterfullerene a good lubricant?

A

Molecules are spherical so thy will roll.

44
Q

Why is using nanoparticles cheaper than using larger particles?

A

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

45
Q

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

A

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

46
Q

What is a nanotube?

A

Layer of graphene with high tensile strength.
Has a high length to diameter ratio.
Good for electronics.

47
Q

2 types of fullerenes

A

Nanotubes
Buckminster fullerene

48
Q

What is graphene useful for?

A

Composites and electronics

Chemistry (10 decks)

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