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Paper1- 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 elements do covalent bonding

A

2 non metals

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2
Q

what does bonding mean

A

atoms share electrons with each other to get full outer shells

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3
Q

what is a covalent bond

A

a shared pair of electrons between non metal atoms

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4
Q

how many covalent bonds does nitrogen need to make with hydrogen

A

3
NH3
it needs 3 covalent bonds to make up the extra 3 electrons needed (2.5)

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5
Q

how do you draw a displayed formula for NH3

A

H
(
H - N - H
the lines represent the covalent bond

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6
Q

what is it called when an element has 3 pairs of covalent bonds between another element(eg N2)

A

a triple bond

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7
Q

what is a simple molecular substance

A

substance made up of a few atoms of non metals joined by covalent bonds

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8
Q

what are the properties of simple molecular substances

A
  • usually have simple molecular structures
  • very low melting and boiling points
  • most are gas or liquid at room temperature
  • don’t conduct electricity
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9
Q

why do the simple molecular substances have very low melting and boiling points

A

weak intermolecular forces

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10
Q

why the simple molecular substances not conduct electricity

A

there are no free electrons to carry charge

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11
Q

what happens as simple molecular structures get bigger

A

as the molecules get bigger, the strengths of the IMFs increase, so melting and boiling points increase

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12
Q

what can be used to show bonding

A
  • dot and cross diagrams
  • displayed formula
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13
Q

what does a dot and cross diagram show

A

show the arrangement of electrons in an atom or ion
- they can show which atom of the electron in an ion originally came from

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14
Q

what are the four state symbols
what do they mean

A

(s) solid
(L) liquid
(G) gas
(Aq) aqueous

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15
Q

what does aqueous mean

A

dissolved in water

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16
Q

ESQ ethanol melts at
-114 C and boils at 78 C. Predict the state at
a) -150 C
b) 0 C
c) 25C
d) 100 C

A

a)solid
b)liquid
c)liquid
d)gas

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17
Q

how do gases move

A

move constantly with random motion

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18
Q

what is the force between the particles

A

very weak

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19
Q

what happens when the particles in a gas get hotter

A

the hotter they get the more they move- so expand or increase in pressure

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20
Q

how do the particles in a gas move

A

free to move, far apart and move in straight lines

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21
Q

do gases fill the container

A

always- don’t keep a definite shape or volume

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22
Q

how doe a solid become liquid

A

melting

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23
Q

how does a liquid become a solid

A

freezing

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24
Q

how does a gas become a liquid

A

condensing

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25
Q

how does a liquid become a gas

A

boiling

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26
Q

how does a solid become a gas

A

sublimation

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27
Q

what happens as the forces become stronger

A

more energy is needed to break them

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28
Q

how are the particles in a solid arranged

A
  • regular arrangement, vibrate in fixed positions
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29
Q

what happens as solids become hotter

A

they vibrate more and expand slightly

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30
Q

what are the forces like in a solid

A

strong forces of attraction and hold them close in fixed positions

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31
Q

do they keep a definite shape and volume

A

yes

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32
Q

what happens when a liquid gets hotter

A

they get faster and they move- expand slightly

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33
Q

how does a liquid move

A

constantly moving randomly, free to move past each other

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34
Q

how is a liquid arranged

A

tend to stick close together, constantly changing shape

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35
Q

what are the forces between particles in a liquid

A

weak forces so free to move

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36
Q

do liquids have a definite volume and/or shape

A

volume- yes
shape- no

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37
Q

do liquids flow to fill the container

A

yes

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38
Q

how many covalent bonds does each carbon atom in diamond make

A

each atom makes 4 atoms

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39
Q

what is diamond made out of

A

carbon

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40
Q

why is diamond very hard

A

because each carbon atom makes 4 covalent bonds

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41
Q

what are the properties of diamond

A
  • very high melting point
  • doesn’t conduct electricity
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42
Q

why does diamond have a very high melting point

A

because it needs lots of energy to break the 4 covalent bonds

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43
Q

why does diamond not conduct electricity

A

it has no free electrons or ions to carry the charge

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44
Q

what is graphite made of

A

carbon

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45
Q

what are the structures of carbon

A
  • fullerenes
  • diamond
  • graphene
  • graphite
46
Q

how many covalent bonds does graphite make

A

3

47
Q

what does graphite’s 3 covalent bonds create

A

create shells arranged in hexagons - layers

48
Q

why are the layers free to move over each other

A

the layers are only held together by weak forces so free to move over each other- makes them soft and slippy

49
Q

what are the properties of graphite

A
  • high melting point
  • conducts thermal energy and electricity
50
Q

why does graphite have a high melting point

A

needs lots of energy to break

51
Q

why does graphite conduct thermal energy and electricity

A

it has a free delocalised electron to carry charge through the whole structure

52
Q

what is graphite ideally used for

A

used for lubricating material

53
Q

what are fullerenes shaped like

A

shaped like closed tubes or hollow balls

54
Q

what is an example of a fullerene

A

Buckminster fullerene

55
Q

what are fullerenes made of

A

carbon

56
Q

what can fullerenes be used for

A
  • good lubricant
  • good industrial catalyst
  • can be used to deliver drugs into the body
57
Q

what is good about fullerenes

A

they have a huge surface area

58
Q

what is graphene

A

one layer of graphite , a sheet of carbon atoms joined together in hexagons

59
Q

how big is graphene

A

one atom thick- 2D

60
Q

what make graphene strong

A

the covalent bonds

61
Q

what are the properties of graphene

A
  • very light
  • conduct electricity
62
Q

because graphene is so light, what can it be used for

A

can be added to composite materials to improve their strengths without adding weight

63
Q

why can graphene conduct electricity

A

it had delocalised electrons so conduct though the whole structure

64
Q

what can fullerenes form

A

nanotubes( tiny carbon cylinders)

65
Q

what is the ratio between the length and diameter of nanotubes

A

very high

66
Q

what are the properties of nanotubes

A
  • can conduct electricity and thermal energy
  • high tensile strengths
67
Q

what can nanotubes be used for

A
  • in electronics
  • strengthen material
68
Q

what are the properties of giant covalent structures

A
  • high melting and boiling points(lots of energy needed to break them)
  • don’t conduct electricity(don’t contain charged particles)
69
Q

how are the atoms in giant covalent structures bonded

A

bonded to each other by strong covalent bonds

70
Q

what are examples of giant covalent structures

A
  • diamond
  • graphite
  • silicon dioxide
71
Q

what is sand made of

A

silicon dioxide- each grain of sand is one giant structure of silicon and oxygen

72
Q

what are polymers

A

long chains of repeating units- joined by strong covalent bonds

73
Q

how do you draw a polymer

A

draw the shortest repeating section called the repeating unit

74
Q

what is an example of how a polymer is drawn

A

( H H )
( [ [ )
-( C C )-
( [ [ )
( H H) N

75
Q

how do you find the molecular formula from a repeating unit

A
  • write down the repeating unit formula
  • add N
    ex. (C2 H4) N
76
Q

what does the N mean in the repeating unit

A

tells us that the unit repeats a lot of times

77
Q

what are the properties of polymers

A
  • solid at room temperatures
  • have lower boiling points
78
Q

why are polymers solid at room temperatures

A

the IMFs are larger than between simple covalent molecules, more energy is needed to break them

79
Q

why do polymers have lower boiling points

A

the IMFs are still weaker that ionic or covalent bonds

80
Q

what is an ionic compound

A

any compound that only contains ionic bonds

81
Q

what is the structure of ionic compounds

A

called a giant ionic lattice

82
Q

why do atoms lose or gain electrons

A

to try and get a full outer shell- form ions

83
Q

what happens when a metal and a non metal react together

A
  • the metal atom loses electrons to form positively charged ions
  • the non metal gain these electrons to form a negatively charged ion
84
Q

what are the oppositely charged ions strongly attracted to

A

by electrostatic forces, the attraction is called ionic bonding

85
Q

what elements react together in ionic bonding

A

metal and non metal

86
Q

when using nano particles in science what is in it known as

A

nanoscience

87
Q

how are particles put into catogries

A

depending on diameter

88
Q

what are the 3 types of particles

A
  • coarse
  • fine
  • nano
89
Q

what are the size of coarse particles

A

between 2500nm and 10000 nm

90
Q

what are the size of fine particles

A

between 100nm and 2500nm

91
Q

what are the size if nano particles

A

between 1nm and 100nm

92
Q

do nanoparticles have a large surface area to volume ration

A

yes

93
Q

what can affect the way a particle behaves

A

the surface area: volume

94
Q

what happens as a particle decreases in size?
what can this cause?

A
  • the size of their surface arear increases in relation to volume
  • this can cause the properties of a material to be different depending on whether its a nanoparticle or whether its in bulk
95
Q

what can nanoparticles be used for

A
  • make new catalysts- huge sa:v
  • nano medicine- tiny particles are absorbed easier by body
  • some conduct electricity so can be used in circuits
    -can be used in cosemetics
  • silver nanoparticles have antibacterial properties(surgical masks etc)
96
Q

what is the problem about nanoparticles on health

A

effects of nanoparticles on health aren’t fully understood
- new products are tested thoroughly
- some people say we don’t know the long term impacts on health, uses it too early and they should be clearly labelled

97
Q

why are nanoparticles used in sun cream

A

better at protecting the skin but could damage cells if gets into the body or damage environment

98
Q

what do the ions form in a compound

A

form a close regular lattice arrangement

99
Q

what are the forces in ionic compounds

A

there are strong electrostatic forces of attraction between oppostiely charged ions in all directions

100
Q

what are the properties of ionic compounds

A
  • all have high melting and boiling points
  • when solid, can conduct electricity
  • when they melt, they carry charge
  • some dissolve easily in water and carry electric charge
101
Q

why can ionic compounds not conduct electricity when solid?
when liquid?

A
  • the ions are held in place
  • ions are free to move
102
Q

why can ionic compounds carry charge when dissolved easily in water

A

ion separate and are free to move in solution

103
Q

what is an empirical formula

A

eg. K 2O

104
Q

how do you work out the empirical formula from a diagram

A

1) work out what ions are in the compound
2) work out what charges the ions will form
3)balance the charge so the empirical formula charge is 0

105
Q

ESQ what’s the empirical formula of the ionic compound

+ * + ** + *
* * + * +++

A
  • is potassium ion
    Group 1 (+1)

+ is oxide ion
Group 6 (2-)

we need 2 potassium ions to balance the oxide ion so…
K2 O

106
Q

what elements are bonded in metallic bonding

A

metal and metal

107
Q

what are the properties of metallic bonding

A
  • solid at room temperature
  • good conductors of electricity and heat
  • most are malleable
108
Q

what are the strong forces between in metallic bonding

A

strong electrostatic forces of attraction between positive metal ions and the shared negative electrons

109
Q

what is an alloy

A

a mixture of two or more elements

110
Q

what is good about alloys

A

they are harder and more useful than pure metals

111
Q

how is an alloy different

A

different elements have different sized atoms, when another element is mixed the new metal atom will distort the layers, making it harder and less easy for it to slide over each other

Paper1- Chemistry (4 decks)

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