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chemistry spec > c2 bonding, structure and properties of matter > Flashcards

c2 bonding, structure and properties of matter Flashcards

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1
Q

what are the three types of chemical bonding?

A

ionic, covalent and metallic bonding

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2
Q

what is ionic bonding?

A

the transfer of electrons

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3
Q

what is covalent bonding?

A

the sharing of electrons

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4
Q

what is metallic bonding?

A

the sharing of delocalised electrons

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5
Q

between what types of elements does ionic bonding take place in?

A

metals and non metals

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6
Q

between what types of elements does covelant bonding take place in?

A

non metals

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7
Q

between what types of element does metallic bonding take place in?

A

metals and alloys

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8
Q

explain ionic bonding

A

When a metal atom reacts with a non-metal atom electrons in the
outer shell of the metal atom are transferred. Metal atoms lose
electrons to become positively charged ions. Non-metal atoms gain electrons to become negatively charged ions. The ions produced by metals in Groups 1 and 2 and by non-metals in Groups 6 and 7
have the electronic structure of a noble gas

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9
Q

what is an ionic compound?

A

An ionic compound is a giant structure of ions. Ionic compounds are held together by strong electrostatic forces of attraction between oppositely charged ions. These forces act in all directions in the lattice and this is called ionic bonding.

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10
Q

properties of ionic compounds?

A

1) all have high melting and boiling points due to their strong electrostatic forces between oppositely charged ions. it takes a lot of energy to overcome this
2) cant conduct electricity when solid because the ions are held into place and cant carry the charge
3) some can easily be dissolved in water, ions separate and are all free to move in the solution

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11
Q

pros and cons of three-dimensional diagrams? (ionic bonding)

A

pros- shows the relative size of the ions as well as the regular pattern of an ionic crystal
cons- only lets you see the outside layer

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12
Q

explain covalent bonding

A

when two non metals share an electron they form strong covalent bonds.
- they may consist of small molecules
- they may have large molecules (eg polymers)
- some may have giant covalent structures ( eg diamonds and silicon dioxide)

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13
Q

how to deduce the formula of a substance given from a model// diagram?

A

count how many of each element there is

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14
Q

pros and cons of three dimensional diagrams? (covelant bonding)

A

pros- shows atoms and arrangements
cons- do not show which atom the electron has come from and can get confusing with larger structures

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15
Q

pros and cons of ball and stick diagrams? (covalent bonding)

A

pros- shows how atoms are connected in large molecules
cons- dont show a 3d structure and doesnt show which atoms the electron has come from

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16
Q

pros and cons of ball and stick diagrams? (ionic bonding)

A

pros- shows the regular pattern of an ionic crystal and how they are arranged
cons- isnt drawn to scale and there arent really gaps between the ions

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17
Q

explain metallic bonding

A

metals consist of giant structures of atoms arranged in a regular pattern, the electrons in the outer shell of each atom is delocalised and are free to move around the whole structure. the sharing of these delocalised electrons forms a strong metallic bond

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18
Q

what are the three states of matter?

A

solid, liquid and gas

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19
Q

what can the particle theory help to explain?

A

boiling, melting, freezing, condensing

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20
Q

what does the amount of energy needed to change a substance’s state depend on?

A

the strength of the electrostatic forces between each particle

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21
Q

what does the nature of the particles depend on?

A

the type of bonding and the structure of the substance

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22
Q

what is the relationship between electrostatic forces and melting/ boiling points?

A

the stronger the forces, the higher the mp and bp are as more energy is required to break those forces

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23
Q

what are the limitations of particle theory?

A

the particles arent solid, spheres or inelastic. and it doesnt show the the forces between the particles so we dont know how strong they really are

24
Q

what are the state symbols solid, liquid, gas and aqueous?

A

solid (s)
liquid (l)
gas (g)
aqueous (aq)

25
Q

explain the properties of ionic compounds

A

1) ionic compounds have giant ionic structures (giant ionic lattices). in which there are strong electrostatic forces acting on the oppositely charged ions and because of this, they have high bps and mps
2) when melted or dissolved in water, they can conduct electricity as their ions are free to move around and carry the charge flow

26
Q

explain the properties of small molecules

A

1) substances that contain small molecules tend to have lower mps and bps as the intermolecular forces between them are weak, intermolecular forces strengthen with the size of the molecule
2) they cannot conduct electricity because the molecules dont have an overall charge
3)

27
Q

what are polymers?

A

a substance composed of very large molecules

28
Q

how are atoms in a polymer linked to other atoms?

A

strong covalent bonds

29
Q

how strong are intermolecular forces between molecules?

A

relatively strong, therefore they are solids at room temp

30
Q

examples of giant covalent structures?

A

1) diamond
2) graphite
3) silicon dioxide

31
Q

properties of giant covalent structures?

A

1) solids with very high melting points as it requires a big amount of energy to break the covalent bonds between the atoms
2) all atoms are bonded together via strong covalent bonds

32
Q

what is an alloy?

A

a mixture of metals to make the arrangement of atoms less regular (distortion) so that they become less soft and have many more uses.

33
Q

why do alloys have more uses?

A

as pure metals have a regular atom arrangement in layers, the layers can slide over eachother, meaning that it can bend and shaped, making them too soft for other uses. Alloys fixes this problem while still maintaining the useful metal properties such as conductivity

34
Q

why are metals good conductors?

A

the delocalised
electrons in the metal carry electrical charge through the metal. Metals are good conductors of thermal energy because energy is transferred by the delocalised electrons

35
Q

structure of diamond?

A

each carbon atom forms four covalent bonds with other
carbon atoms in a giant covalent structure

36
Q

properties of diamond?

A

very hard
very high melting point
does not conduct electricity

37
Q

structure of graphite?

A

each carbon atom forms three covalent bonds with three other carbon atoms, forming layers of hexagonal rings which
have no covalent bonds between the layers. each atom has one delocalised electron

38
Q

properties of graphite?

A

1) soft and smooth (due to the layers that can slide over one another as there are no covalent bonds between the layers)
2) can conduct electricity ( due to the delocalised electrons)
3) good lubricant

39
Q

structure of silicon dioxide?

A

many silicon and oxygen bonded together in a giant covalent structure

40
Q

properties of silicon dioxide?

A

hard
high melting point

41
Q

what is graphene?

A

a single layer of graphite, the sheet is just one atom thick therefore it is 2D

42
Q

properties graphene?

A

1) very strong because of the network of covalent bonds
2) very light so it can be added to composite materials to improve their strength withoutadding much weight
3) conducts electricity due to their delocalised electrons so it can be used for electronics

43
Q

what are fullerenes?

A

molecules of carbon atoms with hollow shapes

44
Q

whate are the structure of fullerenes based on?

A

hexagonal rings of carbon atoms
but they may also contain rings with five or seven carbon atoms

45
Q

what was the first fullerene discovered called?

A

blackminsterfullerene (C60)

46
Q

what is the shape of blackminsterfullerene?

A

spherical shape containing 20 hexagons and 12 pentagons

47
Q

properties of fullerenes?

A

1) huge surface area (so they can be great catalysts)
2) smooth and slippery (so they can make great lubricants)

48
Q

what can fullerenes do?

A

1) can be used to ‘cage’ other molecules as they can form fullerene structures around other molecules and atoms, this can then be used to deliver a drug into the body
2) catalyse reactions
3) lubricate

49
Q

what can fullerenes form?

A

nanotubes - tiny carbon cylinders

50
Q

properties of nano tubes?

A

1) ratio between length and diameter is very high
2) can conduct both heat and electricity
3) have high tensile strength

51
Q

what is the technology that uses nanotubes called?

A

nanotechnology

52
Q

what can nanotubes be used for?

A

1) electronics
2) to strengthen materials without adding much weight (eg tennis racket frames)

53
Q

why might nanoparticles have different properties to ‘bulk’ materials?

A

because of their surface area to volume ratio.It may also mean that smaller quantities are needed
to be effective than for materials with normal particle sizes

54
Q

uses of nanoparticles?

A

1) medicine - some may have anti bacterial properties so they can be added to polymer fibres to be applied to surgical masks or wound dressings
2) electronics - some can conduct electricity so they can be used in tiny circuits
3) catalysts - due to their high surface area to volume ratio
4) nano medicine - some may be absorbed more easily so they can deliver drugs into the body
4) sun creams

55
Q

equation for surface area to volume ratio?

A

SA to V= SA // V

56
Q

disadvantages of nanoparticles?

A

1) not fully understood on how they affect health
2) highly penetrating so it could cause damage to cells

chemistry spec (9 decks)

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