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chemistry > structure and bonding (paper 1) > Flashcards

structure and bonding (paper 1) Flashcards

1
Q

steps for writing ionic formula

A
  1. write the formula of the ions in the compound
  2. take the numbers down and across
  3. write out the formula
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2
Q

hydroxide ion

A

OH-

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3
Q

nitrate ion

A

NO3-

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4
Q

sulphate ion

A

2-
SO4

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5
Q

carbonate ion

A

2-
CO3

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6
Q

why are metallic substances malleable

A

the layers of metal ions are able to slide

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7
Q

why are metallic substances good thermal conductors

A

when a metal is heated the delocalised electrons gain kinetic energy and move faster

the movement transfers the gained energy through the metal

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8
Q

why can metallic substances conduct electricity

A

the delocalised electrons can carry charge and move freely through the metal

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9
Q

why do metallic substances have a high melting and boiling point

A

strong electrostatic attraction between the metal ion and delocalised electrons
needs a lot of energy to break the bonds

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10
Q

what is metallic bonding

A

when a metal and another metal bonds together to create a metallic compound

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11
Q

what is an allotrope

A

different physical forms of an element

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12
Q

why does graphite have a high melting point

A

lots of strong covalent bonds between the atoms
needs lots of energy to break the bonds

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13
Q

why can graphite conduct electricty

A

has delocalised electrons that can move throughout the whole structure

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14
Q

why is graphite soft and slippery

A

layers that can slide over each other
weak forces between the layers

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15
Q

why do giant covalent compounds have a high melting point

A

many strong covalent bonds between the atoms
need a lot of energy to break

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16
Q

why can giant covalent compounds not conduct electricty

A

no delocalised electrons that can move

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17
Q

why are giant covalent compounds hard

A

giant covalent structure
lots of strong bonds between the atoms

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18
Q

why do covalent compounds (small molecules) not conduct electricty

A

the molecules have no charge and are neutral so the molecules cannot move and conduct electricty

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19
Q

why do covalent compounds (small molecules) have low melting points

A

there are weak intermolecular forces between the molecules so it takes a small amount of energy to break them

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20
Q

explain how covalent bonds form

A

covalent bonding happens in a compound where a non metal is joined to a non metal
____ has __ electrons in its outer shell
___ has __ electrons in its outer shell
to get a full outer shell of electrons, the _____ and _____ share an electron each
this sharing of a pair of electrons is called a covalent bond

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21
Q

why do ionic compounds conduct electricity as a solution

A

because the ions can move so can conduct electricity through a solution

22
Q

why do ionic compounds NOT conduct electricity as a solid

A

because the ions are in a fixed lattice structure and can’t move due to strong electrostatic attraction

23
Q

why are ionic compounds soluble

A

because the ions can separate in water

24
Q

why do ionic compounds have a high melting point

A

the strong electrostatic attraction stops the ions from moving further apart
so a lot of energy is needed to break the bond

25
Q

how would you describe the bonding in an ionic compound

A

_____ atom loses ____ electrons to become a positively charged + ion
____ gains ____ electrons to become a negatively charged - ion
____ transfers ____ electron to _____
there is an electrostatic attraction between the oppositely charged ions
this forms an ionic bond

26
Q

what type of attraction is there between oppositely charged ions

A

electro static attraction

27
Q

why is diamond hard

A

giant covalent structure
carbon is bonded to 4 other carbon atoms
lots of strong bonds

28
Q

why does diamond not conduct electricty

A

no delocalised electrons that can move

29
Q

why does diamond have a high melting point

A

many strong covalent bonds between atoms
carbon is bonded to four other carbon atoms
needs a lot of energy to break

30
Q

why is silicon dioxide hard and doesn’t conduct electricty

A

giant structure
lots of strong covalent bonds
has no delocalised electrons that can move

31
Q

why does silicone dioxide have a high melting point

A

many strong covalent bonds
needs a lot of energy to break these bonds

32
Q

what structure do ionic compounds have

A

a giant ionic lattice

33
Q

what is a polymer

A

long chains of repeating units

34
Q

how do you draw a polymer

A

draw the repeating unit of the molecular formula inside the brackets

pit an ‘n’ outside the bottom right hand corner of the bracket

make sure the arms are sticking outside of the bracket

35
Q

what are properties of polymer molecules

A

the intermolecular forces between polymers are larger than the ones between simple covalent molecules, so more energy is needed tot break them - this means most polymers are solid at room temperature

the intermolecular forces are still weaker than ionic or covalent bonds, so they generally have lower boiling points than ionic of giant molecular compounds

36
Q

describe the structure of diamond

A

each carbon atom forms four covalent bonds in a very rigid giant covalent structure

37
Q

describes the structure of graphite

A

each carbon atom forms three covalent bonds to create layers of hexagons, each carbon atom also has one delocalised electron

38
Q

what is graphene

A

one layer of graphite

39
Q

how thick is a layer of graphene

A

one atom thick

40
Q

describe properties of graphene

A

the network of covalent bonds makes it very strong

is incredibly light , so can be added to composite materials to improve their strength without adding much weight

it contains delocalised electrons so can conduct electricity through the whole structure - which means it has the potential to be used in electronics

41
Q

what do fullerenes form

A

spheres and tubes

42
Q

what shape is a buckminsterfullerene

A

a sphere

43
Q

uses of fullerenes

A

delivering drugs around the body

lubricants

industrial catalysts - have a hue surface area

44
Q

what are nano tubes

A

tiny carbon cylinders

45
Q

describe properties of nanotubes

A

the ratio between the length and the diameter of nanotubes is very high

can conduct both electricity and thermal energy

have a high tensile strength

46
Q

uses of nanotubes

A

electronics

to strengthen materials without adding much weight such as in tennis racket frames

47
Q

describe the arrangement of particles in a solid

A

there are strong forces of attraction between the particles, which holds them close together in fixed positions to form a very regular lattice arrangement

the particles do not move from their positions, so all solids keep a definite shape and volume and do not flow like liquids

the particles vibrate around their fixed positions - the hotter the solid becomes, the more they vibrate ( causing them to expand slightly when they are heated )

48
Q

describe the arrangement of particles in a liquid

A

there is a weak force of attraction between the particles - they are randomly arranged and free to move past each other but tend to stick closely together

liquids have a definite volume but do not keep a definite shape, and will flow to fit the bottom of a container

the particles are constantly moving with random motion , the hotter the liquid gets, the faster they move. this causes liquids to expand slightly when heated

49
Q

describe the arrangement of particles in a gas

A

the forces of attraction between particles is very weak - they are free to move and are far apart. the particles in gases travel in straight lines

gases do not keep a definite shape or volume and will always fill any container

the particles move constantly with random motion, the hotter the gas gets the faster they move. gases either expand when heated, or their pressure increases

50
Q

how can you predict the state of a substance

A

if the temperature is below the melting point of substance , it will be a solid

if it above the boiling point, it will be a gas

if it is between the two points, then it is a liquid

51
Q

uses of nanoparticles

A

have a hue surface area to volume ratio so help make new catalysts

nanomedicine - can help deliver drugs

some can conduct electricity - used in tiny electric circuits for computer chips

cosmetics - can improve moisturisers

silver nanoparticles have antibacterial properties - used in polymer fibres to make surgical masks

52
Q

why are some people against the use of nano particles

A

the way they affect the body is not fully understood

the long term impacts they may have are not known

chemistry (11 decks)

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