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CHEMISTRY -EVIE💘 > 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 ions

A

charged particles

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2
Q

what can ions be

A

single atoms or groups of atoms

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3
Q

when atoms lose or gain electron to form ions, what are they trying to do

A

form a full outer shell

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4
Q

what happens when metals form ions

A

they lose electrons from their outer shell to form positive ions

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5
Q

what happens when non metals form ions

A

they gain electrons into their outer shell to form negative ions

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6
Q

if two electrons are lost the charge is…

A

2+

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7
Q

if two electrons are gained the charge is…

A

2-

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8
Q

which groups readily form ions

A

groups 1,2,6,7

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9
Q

are groups 1 and 2 metals or non metals?

A

metals

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10
Q

do metals (groups one and two) lose or gain electrons and what do they form?

A

lose electrons to form positive ions (cations)

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11
Q

are groups 6 and 7 metals or non metals?

A

non metals

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12
Q

elements in the same group have the same number of…

A

electrons on their outer shell

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13
Q

explain what ions each group form

A

1 form 1+
2 form 2+
6 form 2-
7 form 1-

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14
Q

so if a sodium atom (group one) forms an ion, what has happened?

A

its lost one electron to form a positive sodium ion (Na+)

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15
Q

why do simple ions often have noble gas electronic structures

A

because noble gas electronic structures have a full shell of outer electrons which is a very stable structure

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16
Q

name the three types of bonding

A

ionic,metallic, covalent

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17
Q

what is ionic bonding

A

when a metal and non metal react together, the metal atom loses electrons to form a positive ion and teh non metal gains THESE electrons to form a negative ion. these oppositely chatged ions are STRONGLY ATTRACTED to one another by ELECTROSTATIC forces and this force is called ionic bond

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18
Q

in an ionic bonding dot and cross diagram, what happens with the dots and crosses

A

the dots go on one element and crosses on another

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19
Q

describe the structure of an ionic compound

A

giant ionic lattice

the ions form a closely packed regular lattice arrangement and there are very strong electrostatic forces of attraction between oppositely charged ions, in all directions in the lattice

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20
Q

how can you represent an ionic lattice

A

ball and stick diagram

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21
Q

What are ionic compounds boiling and melting points like and why

A

High because the strong bonds between the ions

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22
Q

explain a solid ionic compound

A

ions are in place so compounds can’t conduct electricit

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23
Q

explain ionic compound when it melts

A

ions are free to move and carry electric current

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24
Q

Why do ionic compounds dissolve easily

A

because the Ions separate and are all free to move in solution, so theyll carry an electric current

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25
Q

what is covalent bonding between

A

compounds of nonmetals and nonmetal elements

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26
Q

what happens when elements bond together in covalent bonding

A

they share pairs of electrons to make covalent bond

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27
Q

What makes covalent bonds strong

A

positively charged nucleus of the bonded atoms are attracted to the shared pair of electrons by electrostatic forces making covalent bond is very strong

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28
Q

where do atoms share electrons

A

only in their outer shells (highest energy levels)

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29
Q

what does each single covalent bond provide

A

One extra shared electron for each atom

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30
Q

what are simple molecular substances

A

consist of molecules in which the atoms are joined by strong covalent bonds.

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31
Q

how many electrons does hydrogen need to complete its outer shell

A

2

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32
Q

give the properties of simple molecular substances

A

very strong covalent bonds in the atoms which means by contrast the attraction between these molecules are very weak

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33
Q

are the melting and boiling points high or low

A

low because the molecules are easily parted from each other, because you only have to break the weak intermolecular forces, not the covalent bonds

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34
Q

what are most molecular substances like at room temperature

A

gases or liquids

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35
Q

The bigger the molecules…

A

the strength of the intermolecular forces increases, so more energy is needed to break them and the melting and boiling points increase

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36
Q

don’t simple molecular substances conduct electricity

A

because they aren’t charged so there are no free electrons or irons

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37
Q

what are polymers

A

Long chains of repeating units, which form a long molecule

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38
Q

what all the atoms in a polymer joined by

A

strong covalent bonds

39
Q

how do you draw a repeating unit, for polymers

A 
(H H)
 ( |   | )
-(C-C)-
  ( |  | )
  (H H) n
40
Q

how do you find the molecular formula of a polymer?

A

write down the repeating unit in brackets and put an n outside e.g polyethene is (C2H4)n

41
Q

why are most polymers solid at room temperature

A

because the intermolecular forces between polymer moecules are larger than between simple covalent molecules so more energy is needed to break them

42
Q

why do polymers have lower boiling points than ionic or giant molecular compounds

A

the intermolecular forces are weaker than ionic or covalent bonds

43
Q

what are the bonds like in giant covalent structures

A

strong

44
Q

why do giant covalent structures have very high melting and boiling points

A

lots of energy is needed to break the covalent bonds between the atoms

45
Q

why dont giant covalent structures conduct electricity

A

they dont contain charged particles

46
Q

give the main examples of giant covalent structures

A

diamond, graphite (made from carbon atoms only) and silicon dioxide (silica)

47
Q

Describe the giant covalent bond in diamond

A

each carbon atom forms four covalent bonds in a very rigid giant covalent structure, which is strong

the strong covalent bonds take lots of energy to break so diamond has a very high melting point

doesnt conduct electricity because it has no free electrons or ions

48
Q

describe the giant covalent bond in graphite

A

each carbon atom forms three covalent bonds to create layers carbon atoms arranged in hexagons. These arent held together by covalent bonds so can slide over each other, making it soft and slippery- lubricating material.

high melting point, covalent bonds need loads of energy to break.

each carbon atom also has one delocalised electron, so conduct electricity and thermal energy

49
Q

describe silicon dioxide

A

one giant structure of silicon and oxygen

50
Q

What are allotropes

A

different structural forms of the same element in the same physical state

51
Q

what is graphene

A

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

52
Q

by being only one atom thick, what is graphene

A

a two dimensional compound

53
Q

features of graphene

A

network of covalent bonds- strong
very light- can be added to composite matericals to improve their strength without adding much weight
contains delocalised electrons, like graphite, so conducts electricity- can be used in electronics

54
Q

what are fullerenes

A

molecules of carbon, shaped like closed tubes or hollow balls

55
Q

what are fullerenes made up of

A

carbon atoms, arranged in hexagons but can also contain pentagons or heptagons

56
Q

what was the first fullerene to be discovered called

A

buckminsterfullerene

57
Q

what can fullerenes be used for

A

to cage other molecules, to deliver drugs into the body

lubricants

58
Q

why are fullerenes great industrial catalysts

A

they have a huge surface area, so individual catalyst molecules can be attached to them

59
Q

what are nanotubes

A

tiny carbon cylinders formed by fullerenes

60
Q

what can nanotubes do

A

conduct electricity and thermal energy
high tensile strength(dont break when stretched)
nanotechnology, strengthen materials without adding weight (ie tenis racket frames) and electronics

61
Q

what does metallic bonding involve

A

delocalised electrons in outer shell of metal atoms

62
Q

what sort of structure do metals consist of

A

giant

63
Q

describe metallic bonding

A

There are strong forces of electrostatic attraction between the positive irons and the shared negative electrons
these forces of attraction hold the atoms together in a regular structure and are known as metalic bonding.
(very strong bonding)

64
Q

name some structures held together by metallic bonding

A

metallic elements and alloys

65
Q

what produces ALL the properties of metals

A

delocalised electrons

66
Q

what state are most metals at room temp

A

solid

67
Q

describe the forces between metal atoms and delocalised sea of electrons

A

strong, so need lots of energy to be broken-> metalic compounds have high melting and boiling points

68
Q

why are metals good conductors of heat and electricity

A

delocalised electrons carry current through structure

69
Q

why are most metals malleable

A

the layers of atoms can slide over each other

70
Q

whats an alloy

A

a metal made by combining two or more metallic elements, especially to give greater strength or resistance to corrosion.

71
Q

why are alloys harder than pure metals

A

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

72
Q

name the three states of matter

A

solid liquid gas

73
Q

what does the state of something depend on

A

how strong the forces of attraction are between the particles of the material

74
Q

what does the strength of forces are in states depend on

A

material
temperature
the pressure

75
Q

describe a solid

A

1) strong forces of attraction, holding them in a fixed position to form very regular lattice arrangement
2) particles dont move around, keep definite shape and volume
3) particles vibrate in positions- the hotter it becomes, the more they vibrate, causing a slight expansion

76
Q

describe a liquid

A

1) weak forces of attraction between particles
2) randomly arranges and free to move past each other
3) stick together fairly closely when moving
4) definite volume, dont keep definite shape
5) flow to fill a container
6) constantly moving with random motion
7) hotter- faster movement of particles
8) expand slightly when heated

77
Q

describe a gas

A

1) force of attraction is very weak
2) free to move, far apart
3) particles travel in straight lines
4) dont keep definite shape or volume
5) fill any container
6) move constantly, random motion, hotter= faster movement
7) gases expand when heated, or pressure increases

78
Q

what does aqueous mean

A

dissolved in water

79
Q

what do physical changes do to a substance

A

dont change the particles- just their arrangement or energy

80
Q

solid to liquid?

A

melting
WHEN HEATED,ITS PARTICLES GAIN MORE ENERGY, WHICH MAKES THEM VIBRATE MORE, WHICH WEAKENS THE FORCES THAT HOLD THE SOLID TOGETHER.
AT MELTING POINT, PARTICLES HAVE ENOUGH ENERGY TO BREAK FREE FROM POSITIONS

81
Q

liquid to gas?

A

boiling
PARTICLES GAIN ENERGY WHEN HEATED, PARTICLES MOVE FASTER, WHICH WEAKENS AND BREAKS THE BONDS HOLDING THE LIQUID TOGETHER.
AT BOILING POINT, PARTICLES HAVE ENOUGH ENERGY TO BREAK BONDS (EVAPORATING) AND LIQUID BECOMES A GAS

82
Q

gas to liquid?

A

condensing
AS GAS COOLS, PARTICLES NO LONGER HAVE ENOUGH ENERGY TO OVERCOME THE FORCES OF ATTRACTION BETWEEN THEM.
BONDS FORM BETWEEN THE PARTICLES
AT BOILING POINT, SO MANY BONDS HAVE FORMED BETWEEN THE GAS PARTICLES, THAT THE GAS BECOMES A LIQUID

83
Q

liquid to solid?

A

freezing
WHEN A LIQUID COOLS, THE PARTICLES HAVE LESS ENERGY, SO MOVE AROUND LESS
NOT ENOUGH ENERGY TO OVERCOME ATTRACTION BETWEEN PARTICLES SO MORE BONDS FORM BETWEEN THEM.
AT MELTING POINT, SO MANY BONDS HAVE FORMED BETWEEN THE PARTICLES THAT THEY’RE HELD IN PLACE. LIQUID BECOMES A SOLID

84
Q

the stronger the forces…

A

the more energy is needed to break them, and so the higher the melting and boiling points of the substance

85
Q

how can you predict the state of a substance

A

temp below melting point- solid
above boiling point- gas
between two points- liquid

86
Q

name the three types of particles and their size

A

coarse- diameter between 2500nm and 10 000nm (dust)
fine- diameter between 100nm and 2500nm
nanoparticles- diameter between 1nm and 100nm (contain only a few atoms)

87
Q

give the surface area to volume ratio equation

A

SA divided by volume

88
Q

as particles decrease in size…

A

the size of their surface area increases in relation to their volume, so the Sa to volume ratio increases

89
Q

as you decrease the size of any cube by a factor of ten…

A

the surface area to volume ratio will always increase by a factor of ten

90
Q

describe a nano particle

A

have very high surface area to volume ratio, which means the surface area is very large compared to the volume

91
Q

how much of a material will you need for a catalyst if its made up of nanoparticles

A

youll need less compared to a material made up of normal sized particles

92
Q

give some uses of nano particles

A

high surface area to volume ratio- catalysts
absorbed more easily by the body- nanomedicine- deliver drugs to the cells that need them
some conduct electricity- electric circuits for computer chips
silver ones have antibacterial properties- can be added to polymer fibres and then used to make surgical masks and wound dressing. can also be added to deodorants
improve moisterisers without making them really oily and other cosmetics.

93
Q

give one use and a potential risk of nanoparticles

A

used in suncreams, protecting skin from harmful UV rays
give better coverage

not clear if they might damage cells
when washed away, could damage environment

-> things are clearly labelled if contain nanoparticles

CHEMISTRY -EVIE💘 (9 decks)

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