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Chemistry > Topic 2 - Bonding, Structure And Properties Of Matter > Flashcards

Topic 2 - Bonding, Structure And Properties Of Matter Flashcards

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1
Q

What are the three types of chemical bond?

A

Ionic
Covalent
Metallic

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2
Q

When does ionic bonding occur?

A

In compounds formed of oppositely charged ions of metals combined with non-metals

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3
Q

When does covalent bonding occur?

A

Between atoms which share pairs of electrons. This happens in most non-metallic elements and in compounds of non-metals.

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4
Q

When does metallic bonding occur?

A

Between atoms which share delocalised electrons and occurs in metallic elements and alloys

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5
Q

What happens in ionic bonding?

A

A metal atom reacts with a non-metal atoms and electrons in the outer shell of the metal atom are transferred

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6
Q

In ionic bonding what do the atoms become?

A

Metals become positively charged ions

Non-metals become negatively charged ions

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7
Q

How do you represent ionic bonding?

A

Dot and cross diagrams

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8
Q

What is an ionic compound?

A

A giant structure of ions held together by strong electrostatic forces of attraction in all directions in the lattice between oppositely charged ions

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9
Q

How can ionic compounds be represented?

A

A ball and stick model or a 3D model

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10
Q

What are the limitations of dot and cross diagrams for ionic bonding?

A

Don’t show structure of compound, size or arrangement

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11
Q

What are the limitations of ball and stick diagrams for ionic bonding?

A

Doesn’t show size of ions

Presents gaps but there isn’t gaps in the bonds

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12
Q

What are the limitations of 3-D models for ionic bonding?

A

Only shows outer layer of compound

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13
Q

What are the properties of ionic compounds?

A

High melting and boiling points – strong bonds
When solid they can’t conduct electricity – ions held in place
When liquid ions are free to move and carry electric current
Dissolve easily – separate and free to move

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14
Q

What is covalent bonding?

A

When atoms share pairs of electrons to form strong bonds

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15
Q

How large are covalent bond is?

A

Consist of small molecules but some have very large molecules such as polymers

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16
Q

Give examples of giant covalent structures.

A

Diamond and silicon dioxide

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17
Q

How can covalent bonds and giant structures be represented?

A

Dot and cross diagrams
Displayed formulas
3D models

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18
Q

What are the limitations of dot and cross diagrams for covalent bonding?

A

Don’t show size or arrangement

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19
Q

What are the limitations of representing covalent bonding by the displayed formula?

A

Don’t show structure or which atoms the elements came from

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20
Q

What are the limitations of using a 3-D model to represent covalent bonding?

A

Confusing

Don’t show where electrons have come from

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21
Q

What are the properties of simple molecular substances?

A

Strong covalent bonds but weak forces of attraction
Very low melting and boiling points – easy to break intermolecular forces
Gases or liquids
Don’t conduct electricity – no free electrons

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22
Q

What are polymers?

A

Small units linked together to form a long molecule that has repeating sections joined by covalent bonds

23
Q

How are polymers represented?

A

Displayed formula of the repeating unit in brackets to the number of repetitions

24
Q

What are the properties of polymers?

A

Large intermolecular forces so more energy is needed to break them
Solid
Low boiling points

25
Q

What are giant covalent structures??

A

All atoms are bonded to each other by strong covalent bonds

26
Q

What are the properties of a giant covalent structures?

A

Very high melting and boiling points

Don’t conduct electricity

27
Q

Describe diamond

A

Each carbon atom forms for covalent bonds with other carbon atoms

28
Q

What are the properties of diamond?

A

Very hard
Doesn’t conduct electricity
High melting point

29
Q

Describe graphite

A

Each carbon atom forms three covalent bond with three other carbon atoms forming layers of hexagonal rings which have no covalent bonds between layers
One electron from each carbon atom is delocalised

30
Q

Describe Graphene

A

A single layer of graphite with a strong network of covalent bond

31
Q

What are the properties of graphene?

A

Strong
Light
Good electrical conductors - delocalised electrons

32
Q

Describe Fullerenes

A

Molecules of carbon atoms with hollow shapes.

33
Q

What are the properties of graphite?

A

High melting point – lots of energy needed to break covalent bonds
Soft and slippery - no forces between layers
Conducts electricity and thermal energy

34
Q

What is significant about the structure of fullerenes?

A

Based on hexagonal rings of carbon atoms but may also contain rings with five or seven carbon atoms

35
Q

What was the first fullerene to be discovered?

A

Buckminsterfullerene - forms hollow sphere

36
Q

How are fullerenes used?

A

Cage other molecules - deliver drugs to body
Industrial catalysts - large surface area
Lubricants

37
Q

What are carbon nanotubes?

A

Cylindrical fullerenes with high length to diameter ratios

38
Q

What are the properties of nanotubes?

A

Conduct electricity and thermal energy

Can be stretched without breaking

39
Q

What are nanotubes used for?

A

Electronics, nanotechnology and materials

40
Q

What is metallic bonding?

A

Sharing of delocalised electrons between metal atoms arranged in regular patterns

41
Q

What are the properties of metals?

A

Giant structures with strong metallic bonds

High melting and boiling points

42
Q

How are pure metals arranged?

A

Arranged in layers which allows them to be bent and shaped

43
Q

Why are alloys made?

A

Because pure metals are too soft for many users

44
Q

What are alloys?

A

A mixture of metals or a metal and another element to make them harder

45
Q

How are alloys harder than pure metals?

A

When another element is mixed with a pure metal the new metal atoms will distort the layers making it more difficult for them to slide over each other

46
Q

Describe a solid

A

Strong forces of attraction
Fixed, regular arrangement
Vibrate around fixed positions
High density

47
Q

Describe a liquid

A

Weaker forces of attraction
Particles close together but can move past each other
Irregular arrangements
More energy than solid - move at random directions slowly
Less dense than solids

48
Q

Describe a gas

A

No forces of attraction between particles
More energy than solids and liquids
Free to move in random directions at high speeds
Low density

49
Q

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

A

The strength of the forces between the particles

50
Q

What are the limitations of the state models?

A

Doesn’t show forces
All particles are represented as spheres
Spheres are solid

51
Q

What does aq stand for?

A

Aqueous solutions

52
Q

How are nano particles used for medicine?

A

Tiny particles are absorbed more easily by the body
Silver nanoparticles have antibacterial properties and used to make surgical masks and wound dressing
Cosmetics - deodorant, moisturisers

53
Q

What are the effects of nano particles of health?

A

Not fully understood so tested thoroughly

Chemistry (11 decks)

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