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Chemistry > T2 - Bonding, structure and the properties of matter > Flashcards

T2 - Bonding, structure and the properties of matter Flashcards

1
Q

what is ionic bonding?

A

metal reacts with non metal

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2
Q

What happens when a metal atom looses electrons in ionic bonding?

A

become positively charged ions

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3
Q

what happens when a non metal gains electrons?

A

becomes negatively charged

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4
Q

what is an ion?

A

an atom with an overall charge

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5
Q

what is an ionic compound?

A

a giant structure of ions

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6
Q

what are ionic compounds held together by?

A

electrostatic forces/ ionic bonds

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7
Q

which direction do electrostatic forces work in ionic compound?

A

all directions

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8
Q

properties of ionic compounds? X3

A

-high melting and boiling point
-cannot conduct electricity when solid
-can conduct electricity when melted or dissolved in water

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9
Q

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

A

electrostatic force require lots of heat energy to break

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10
Q

why can’t ionic compounds conduct electricity when solid?

A

ions cant move due to electrostatic forces

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11
Q

Why can ionic compounds conduct electricity when melted or dissolved in water?

A

Ions are free to move and can carry charge

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12
Q

What is covalent bonding?

A

when atoms share electrons

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13
Q

strength of covalent bond?

A

Very strong

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14
Q

Properties of small covalent molecules? x2

A

-low melting and boiling points
-Do not conduct electricity

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15
Q

what is the state of small covalent molecules at room temperature?

A

gas or liquid

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16
Q

What is the name of the force between 2 molecules in a small covalent molecule?

A

intermolecular force

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17
Q

Why do small covalent molecules have low melting and boiling points?

A

weak intermolecular forces between molecules that are easy to break

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18
Q

What happens when size of small covalent molecule increases?

A

intermolecular forces increase

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19
Q

Why don’t small covalent molecules conduct electricity?

A

No overall charge

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20
Q

What state do giant covalent molecule take at room temperature?

A

solid

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21
Q

Why are giant covalent molecule solids at room temperature?

A

Lots of strong covalent bonds

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22
Q

what is diamond formed from?

A

carbon

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23
Q

Properties of giant covalent molecule? x1

A

High melting and boiling points

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24
Q

Why cant diamonds conduct electricity?

A

-no free electrons to carry charge

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25
Q

Properties of graphite? x3

A

-HIgh melting and boiling point
-soft and slippery
-good conductor of heat and electricity

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26
Q

Properties of diamond? x3

A
  • hard
    -high melting and boiling point
  • do not conduct electricity
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27
Q

How many covalent bonds does each carbon atoms form in diamond?

A

four covalent bonds

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28
Q

How many covalent bonds does each carbon atoms form in graphite?

A

three covalent bonds

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29
Q

What shape do carbon atoms in graphite form?

A

Hexagonal rings

30
Q

Why does graphite have a high melting and boiling point?

A

lots of covalent bonds

31
Q

Why is graphite slippery?

A

no covalent bonds between layers of hexagonal rings

32
Q

Why is graphite a good conductor of heat and electricity?

A

Has delocalised electrons

33
Q

What is graphene?

A

a single layer of graphite

34
Q

properties of graphene? x2

A

-good conductor of electricity
-strong

35
Q

What is graphene useful for? X2

A

electronics and making new materials

36
Q

What is fullerenes?

A

molecules of carbon atoms with hollow shapes

37
Q

How many carbon atoms form rings in fullerene? x3

A

5,6,7

38
Q

What was the first fullerene to be discovered?

A

Buckminsterfullerene

39
Q

What shape does Buckminsterfullerene have?

A

Spherical shape

40
Q

Uses of fullerenes? X3

A

-Pharmaceutical delivery into body
-lubricants
-catalysts

41
Q

What are carbon nanotubes?

A

fullerenes shaped as cylinders

42
Q

Properties of carbon nanotubes? x2

A

-high tensile strength
good conductors of heat and electricity

43
Q

Uses of carbon nanotubes? x1

A

To reinforce materials

44
Q

Size of polymers?

A

large molecules

45
Q

What are polymers made from?

A

Monomers (small molecules)

46
Q

What are monomers in polymers linked by?

A

strong covalent bonds

47
Q

Properties of polymers? x1

A
48
Q

Why are polymers solids at room temperatre?

A

intermolecular forces between polymer molecules are strong

49
Q

size of structure of metals?

A

giant structures of atoms

50
Q

Why are metals good conductors of heat and electricity?

A

-delocalised electrons with charge

51
Q

Why do metals have high melting and boiling points?

A

Strong metallic bonds

52
Q

What is the bond between delocalised electrons and metal ions?

A

metallic bonds

53
Q

Why are metals malleable?

A

Layers of atoms slide over each other

54
Q

What is an alloy?

A

mixture of metals

55
Q

Why are alloys harder than pure metals?

A

Different size atoms stop layer of atoms from sliding

56
Q

Diameter of coarse particles?

A

2500 to 10,000 nm

57
Q

Diameter of fine particles?

A

100 to 2,500 nm

58
Q

Diameter of nanoparticles?

A

between 1–100 nm

59
Q

What happens when the side of cube decreases by 10 times?

A

Surface area to volume ratio increases by 10 times

60
Q

Main feature of nanoparticles?

A

High surface area to volume ratio

61
Q

Benefit of nanoparticles?

A

only small quantity needed

62
Q

Risks of nanoparticles? x2

A

-can enter body
-not studied much

63
Q

Uses of nano particles? x4

A

-sun cream
-deodorant
-electronics
-catalyst

64
Q

Advantage of dot and cross diagrams?

A

Easy to tell where electron comes from

65
Q

disadvantage of dot and cross diagrams?

A

dont tell us shape of moleculce

66
Q

disadvantage of stick diagram? x3

A

-cant tell where electron am from
-doesnt tell us about outer electrons not in bonds
-dont tell us shape of moleculce

67
Q

advantage of 3D stick diagram?

A

-shows shape of molecule

68
Q

advantage of ball and stick diagram?

A

allows us to see ions in 3D

69
Q

disadvantage of ball and stick diagram?

A

ions shown as spaced instead of together

70
Q

advantage of space filling diagram?

A

shows how close ions are

71
Q

disadvantage of ball and stick diagram?

A

hard to see 3D packing

72
Q

disadvantage of both ball and stick diagram and space filling diagram?

A

doesnt show size of structure

Chemistry (4 decks)

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