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Chemistry > C3: Structure and Bonding > Flashcards

C3: Structure and Bonding Flashcards

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1
Q

Solids:

A

-fixed shape and volume, cannot be compressed, vibrate in fixed positions.

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2
Q

Liquids:

A

-fixed volume, can flow, more space than when solid.
-particles slide over one another.

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3
Q

Gases:

A

-no fixed shape or volume, compressed easily
-random and rapid movements.

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4
Q

What does particle theory describe?

A

-movement of particles
-average distance between particles

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5
Q

Liquid to solid

A

freezing

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6
Q

solid to liquid

A

melting

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7
Q

liquid to gas

A

evaporation

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8
Q

gas to liquid

A

condensation

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9
Q

solid to gas

A

sublimation

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10
Q

gas to solid

A

depostion

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11
Q

Why doesn’t the temperature increase when changing state?

A

All energy is going towards breaking the particles apart from one another.

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12
Q

What are the limitations of the particle model?

A

-No electrostatic attractions
-Solid spheres, not atoms

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13
Q

What is the bonding that shares electrons?

A

Covalent

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14
Q

What is the bonding that transfers electrons?

A

Ionic

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15
Q

What charge ions do metals form?

A

Positive

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16
Q

What charge ion do non-metals form?

A

Negative

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17
Q

What do we use to represent ionic bonding?

A

dot and cross diagrams

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18
Q

What charge ion do group 5 form?

A

3-

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19
Q

What charge ion do group 4 create

A

Don’t make ions silly (other than tin and lead)

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20
Q

How are ionic compounds held together?

A

Strong forces of attraction between oppositely charged ions.

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21
Q

What can ionic bonds create (if there are lots of them)

A

-giant ionic structures
-giant ionic lattices

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22
Q

What is a lattice?

A

arranged in a regular pattern

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23
Q

main property of ionic compounds?

A

high melting and boiling points

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24
Q

why can molten ionic COMPOUND then conduct electricity when dissolved in water?

A

Attracted to oppositely charged electrodes and carry their electrical charge through the liquid.

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25
Q

why can ionic compound IN SOLUTION conduct electricity?

A

ions (+delocalised electrons) can move around freely within the solution.

26
Q

Covalent bonding - what is it between?

A

non metal and non metal

27
Q

what does covalent bonding entail?

A

two non metals sharing electrons to fill their outer shells.

28
Q

What are giant covalent structures also known as?

A

Macromolecules

29
Q

What is diamond an example of?

A

Giant covalent structure

30
Q

What is diamond made of

A

Carbon atoms forming four covalent bonds with its neighbours.

31
Q

How do we express covalent bonds?

A

Dot and cross (but with circles!)

32
Q

Intermolecular forces _____ with the size of the molecules.

A

Increase (higher b+m points but thats easy.)

33
Q

What is a polymer

A

made up of many small reactive molecules that bond to each other to form long chains.

34
Q

example of polymer

A

poly(ethene)

35
Q

Long polymers can be expressed like:

A

( H H )
-(-C—-C-)- (poly(ethene))
( H H ) n

36
Q

Can compounds made of simple molecules conduct electricity?

A

NO, no overall charge, neutral molecules can’t carry charge.

37
Q

Properties of diamond

A

-very hard
-high boiling point
-insoluble in water.

38
Q

can giant covalent structures conduct?

A

NO, other than GRAPHITE

39
Q

Why can graphite conduct electricity?

A

It has layers, and delocalised electrons run between the layers.

40
Q

What do the layers in graphite form?

A

hexagons

41
Q

What is graphite arranged in?

A

layers

42
Q

why is graphite soft and slippery?

A

it’s in layers

43
Q

what is a fullerene?

A

hollow-shaped molecules of carbon

44
Q

Shape of fullerenes:

A

hexagon

45
Q

Example of a fullerene:

A

carbon nanotube

46
Q

Properties of fullerenes:

A

-high tensile strength
-high electrical and thermal conductivity.

47
Q

What can fullerenes be used for?

A

drug delivery into the body.

48
Q

What is graphene?

A

a single sheet of carbon atoms from graphite

49
Q

How thick is graphene?

A

1 atom thick.

50
Q

Properties of graphene?

A

-excellent conductor of thermal energy and electricity.
-low density
-strong

51
Q

Metals can form what, even though not visible to the naked eye?

A

crystals

52
Q

What is metallic bonding between?

A

two metals

53
Q

How do the outer electrons move in metallic bonding?

A

Move freely throughout the structure (delocalised)

54
Q

What do the delocalised electrons in metallic bonding do?

A

Make them conduct electricity.

55
Q

What is an alloy?

A

mixture of two or more elements, at least one of which is a metal.

56
Q

Why are metals used as cooking utensils?

A

Cook conductors of thermal energy, high melting points.

57
Q

Why do metals have high melting points?

A

giant structures, lots of energy to break apart electrostatic attraction.

58
Q

1nm=?m

A

1x10 (-9) m

59
Q

What do nanoparticles have that makes them useful?

A

high surface area :volume

60
Q

uses of nanoparticles (materials):

A

-glass (breaks down dirt)
-Sunscreen (effective blockers)
-cosmetics (deeper into skin)

61
Q

uses of nanoparticles (medical)

A

-nanocages delivering drugs
-can potentially change the proteins in a cancer cell and destroy it.

62
Q

risks of nanoparticles:

A

-can cause explosion of catalysts
-finding way into atmosphere, can breathe in and damage lungs.
-affect wildlife

Chemistry (6 decks)

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