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CHEMSITRY > CHAPTER 3 > Flashcards

CHAPTER 3 Flashcards

1
Q

What is it called when atoms share electrons

A

covalent bonding

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2
Q

what is it called when atoms transfer electrons

A

ionic bonding

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3
Q

what arrangement is formed when ionic bonding occurs

A

giant structure/ giant lattice

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4
Q

characteristics of ionic compounds

A

high melting points

conduct electricity

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5
Q

characteristics of simple molecules

A

weak intermolecular forces forces

cant carry electricity

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6
Q

why can graphite conduct electricity

A

delocalised electrons carry charge

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7
Q

what are fullerenes

A

hollow shapes molecules of carbon

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8
Q

uses of fullerenes

A

transport drugs
catalyst
reinforcement

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9
Q

what is graphene

A

1 atom thick

graphite

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10
Q

what is metallic bonding

A

when the negative electrons holds the positive nuclei in position

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11
Q

what is an alloy

A

mixture of two elements at least one of which is metal

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12
Q

why can metals bend

A

the layers slide over eachother

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13
Q

why do nano particles have different properties

A

large SA to volume ratio

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14
Q

uses of nano particles

A

sun cream
glass
cosmetics

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15
Q

what is it called when a solid changes directly to a gas

A

sublimation

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16
Q

what is a compound

A

something that contains two or more elements

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17
Q

when electrons have been gained what is the charge of the ion

A

negative

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18
Q

what arrangement do ionic bonds give

A

giant lattice

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19
Q

why do lattices have such high boiling points

A

the ionic bonds act in all directions on an atom

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20
Q

why will molten or dissolved ionic compounds conduct electricity

A

ions free to move

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21
Q

what are the three states of matter

A

solid, liquid, gas

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22
Q

characteristics of particles in solid

A

packed closely together vibrate in fixed positions

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23
Q

characteristics of liquid

A

close together but can slide round

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24
Q

characteristics of gas

A

lots of empty space of particles to move around

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25
Q

what energy changes happen when something melts or boils

A

energy is transferred to the substance

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26
Q

limitations of the simple particle model

A

atoms aren’t all solid spheres with o forces between them

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27
Q

why do different substances have different melting points

A

depends on the strength of the bonds between them

28
Q

what is covalent

A

when two atoms share electrons

29
Q

what is ionic bonding

A

when atoms transfer electrons to each other and become ions

30
Q

how do ionic compounds stay together

A

the forces of attraction between the oppositely charged ions

31
Q

what is formed with ionic bonds

A

a giant structure or giant lattice

32
Q

why do ionic compounds have such high melting and boiling points

A

the strong electrostatic forces of attraction

33
Q

how to work out the charge of an ionic compound

A

look at the charges of the ions

the overall charge must be 0 so there must be enough of each to cancel out

34
Q

why will ionic compounds only conduct electricity when dissolved or molten

A

the ions become mobile and can carry the charge through the liquid

35
Q

what are covalent bonds

A

the strong bonds between atoms that are sharing electrons

36
Q

what is a macromolecule

A

a giant covalent structure

37
Q

how do a shared pair of electrons bond the atoms together

A

the positive nuclei are attracted to the negative pair of electrons

38
Q

what are the three ways of representing covalent bonding

A

dot and cross
displayed formula
the 3d model

39
Q

why is it easy to break apart a simple molecular compound

A

weak intermolecular forces

40
Q

why don’t molecular compounds conduct electricity

A

they aren’t charged so there are no free electrons

41
Q

what is a polymer

A

a long chain made up of smaller molecules

42
Q

why does diamond have such a high melting point

A

very strong intermolecular forces

43
Q

what are intermolecular forces

A

the forces between the covalently bonded molecules

44
Q

why do macromolecules have such high melting points

A

all the atoms are bonded to eachother by strong covalent bonds

45
Q

why can layers in graphite slide off eachother

A

very weak intermolecular forces

46
Q

what are delocalised electrons

A

spare electrons that don’t belong to an atom so can move through out graphite

47
Q

why does graphite conduct electricity

A

delocalised electrons

48
Q

what is a fullerene

A

a large hollow cage made of carbon

49
Q

how many carbon atoms are in a fullerene

A

60

50
Q

what are carbon nanotubes

A

cylindrical fullerenes

51
Q

what is graphene

A

a single layer of carbon atoms

52
Q

three uses of fullerenes

A

can cage other molecules

deliver drug catalyst

53
Q

what type of bonding occurs in metals

A

metallic bonding

54
Q

how are metallic bonds so strong

A

the positive metal ions are attracted to the negative delocalised electrons

55
Q

what is an alloy

A

a mixture of two elements at least one of which is a metal

56
Q

why are metals solid at room temperature

A

strong electrostatic bonds

57
Q

why are metals good conductors of electricity and heat

A

delocalised electrons carry change and energy

58
Q

why are metals malleable

A

layers of atoms can slide over eachother

59
Q

why are alloys harder than normal metals

A

the different sizes atoms mean its harder for the layers to slide over eachother

60
Q

what is a nanoparticle

A

a very small particle

61
Q

what is important about nanoparticles

A

large surface area to volume ratio

62
Q

what is the size range for a nanoparticle

A

between 10-9 and 10-7 metres

63
Q

uses of nanoparticles

A 
catalyst 
nanomedicine 
magic bullet 
sun creams
cosmetics
64
Q

risk of nanoparticle

A

large sa = flammable
breathing them in could damage bloodstream
affecting environment

65
Q

what are silver nanoparticles used for

A

inhibit growth of microorganisms
textiles
sanitation as they protect against bacteria

66
Q

how are nanocages used to deliver drugs

A

can get into leaky walls of tumours and carry drugs at the same time

67
Q

what are nanowires

A

very small wires used in electronic circuit

CHEMSITRY (13 decks)

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