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1
Q

whats an element

A

all atoms are the same

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2
Q

whats a compound

A

contains 2 or more different elements that are chemically combined

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3
Q

whats a mixture

A

different elements or compounds that are not chemically combined

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4
Q

what is filtration used for

A

is used to separate an insoluble solid from a liquid

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5
Q

what is crystallisation used for

A

used to separate a soluble solid from a liquid

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6
Q

what is simple distillation

A

used to separate a dissolved solid from a liquid but keeps the liquid

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7
Q

what must mixtures have in fractional distillation

A

different boiling points

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8
Q

what does chromatography allow

A

allows us to separate substances based on their different solubilities

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9
Q

what does the plum pudding model consist of

A

ball of positive charge
negative electrons embedded in it

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10
Q

what happens in the plum pudding model

A

scientists took a piece of gold foil
then fired tiny particles at the gold foil
alpha particles have a positive charge
most of the alpha particles passed straight through the gold foil without changing direction
some alpha particles bounced back
this told scientists atoms are mainly empty space
and showed plum pudding model was wrong

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11
Q

what happens in the nuclear model

A

-scientists proposed that electrons orbit the nucleus at specific distances
-backed up by experiments by scientists
-proton determines amount of positive charge in the nucleus
-chadwick discovers nucleus also contains neutrons

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12
Q

relative charge

A

proton=+1
neutrons=0
electrons=-1

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13
Q

relative mass

A

protons=1
neutrons=1
electrons=very small

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14
Q

What is mass number

A

the big number/top number

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15
Q

what is the atomic number

A

bottom/smaller number

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16
Q

how to work out protons neutrons and electrons

A

protons=atomic number
electrons=atomic number
neutrons=mass number-atomic number

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17
Q

what are isotopes

A

isotopes are atoms of the same element with different numbers of neutrons

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18
Q

what are ions

A

atoms which have an overall charge because ions have lost or gained electrons

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19
Q

where are metals found in the periodic table

A

left

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20
Q

where are non-metals found in the periodic table

A

right

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21
Q

when happens when metals react

A

they lose electrons to achieve a full outer shell

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22
Q

what is the relative atomic mass

A

(mass of isotope 1 x percent abundance of isotope 1) + (mass number of isotope 2 x percent abundance of isotope 2) divided by 100

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23
Q

how is the modern periodic table arranged

A

elements with similar properties occur at regular intervals
all the elements in a group have similar chemical properties

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24
Q

mendeleevs periodic table

A

-arranged all elements in order of increasing atomic weight
-Mendeleev would switch the order if specific elements so they fitted patterns of other elements in the same group
-left gaps for undiscovered elements
-predicted properties of undiscovered elements

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25
Q

group 0 (noble gases)

A

-very unreactive because they have a full outer shell
-as you go down group 0 boiling point increases

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26
Q

group 1 (alkali metals)

A

1 electron in outer shell
group 1 metals are soft
as you move down group 1 the metals are more reactive
reacts rapidly with oxygen and chlorine
reacts rapidly with water - fizzes which means a gas is being produced

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27
Q

group 7 (the halogens)

A

7 electrons in outer shell
2 atoms join together to form a covalent bond
melting and boiling point increases as you go down group
relative molecular mass increases as you go down group 7
group 7 elements form covalent compounds when they react with other non metals
-halogens get less reactive as you move down group 7
a more reactive halogen can displace a less reactive halogen to form a aqueous solution

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28
Q

Transition elements/metals

A

all metals
hard/strong metals
all have high melting points
high density
much less reactive than group 1 metals
useful as catalysts

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29
Q

what can copper be used for

A

pipes that carry water

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30
Q

Solids

A

-hard to compress
-packed together with no spaces
-fixed shape
-particles vibrate

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31
Q

Liquids

A

-hard to compress
-take the shape of container
-they can move

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32
Q

gases

A

-easy to compress
-widely spaced
-move quickly and randomly

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33
Q

limitations of gas , liquid , solid diagrams

A

-simple particle model assumes that all particles are solid spheres
-assumes that there are no forces between the particles

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34
Q

what is metallic bonding

A

is the electrostatic attraction between positive metal ions and delocalised electrons

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35
Q

what is a solid to liquid called

A

melting

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36
Q

what is a liquid to solid called

A

freezing

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37
Q

what is liquid to gas called

A

boiling

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38
Q

what is a gas to liquid called

A

condensing

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39
Q

what do coarse particles contain

A

thousands of atoms

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40
Q

what do fine particles contain

A

several thousand atoms

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41
Q

what do nanoparticles contain

A

a few hundred atoms

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42
Q

what is ionic bonding

A

when a metal and a non-metal react

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43
Q

what do ionic compounds form

A

giant ionic lattices

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44
Q

what happens with surface area : volume ratio

A

as the particle size decreases by 10 times the surface area:volume ratio increases by 10 times

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45
Q

what did nano particles have

A

a huge surface area:volume ratio

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46
Q

uses of nanoparticles

A

suncream
catalysts
cosmetics
electronics

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47
Q

risk of nanoparticles

A

can be absorbed into body and enter our cells

48
Q

what happens in a giant ionic lattice

A

every positive ion is surrounded by negative ions

49
Q

features of giant ionic lattices

A

-3d structures
very strong electrostatic forces

50
Q

features of ionic compounds

A

-very high melting and boiling points
-strong electrostatic forces require a large amount of energy to break
-cannot conduct electricity when they are solids
-

51
Q

what is an alloy

A

an alloy is a mixture of metals
-harder than pure metals

52
Q

how are polymers made

A

are made by joining together thousands of small identical molecules (monomers)

53
Q

what are monomers often

A

alkene molecules

54
Q

what bond are monomers

A

double covalent bonds

55
Q

what bond is poly(ethene)

A

single covalent bond

56
Q

what state are polymers at room temperature

A

solid

57
Q

features of metals

A

high boiling and melting point
melting can be bent or shaped because the layers of atoms are able to slide over each other

58
Q

what is covalent bonding

A

when non metals bond together

59
Q

are covalent bonds strong

A

yes

60
Q

what type of bond us a shared pair of electrons

A

single covalent bond

61
Q

what type of bond is 2 shared pairs of electrons

A

double covalent bond

62
Q

what type of bond is 3 shared pairs of electrons

A

triple covalent bond

63
Q

small covalent molecules

A

-low melting and boiling points
-gases at room temperature
-weak intermolecular forces which do not require a lot of energy to break
-do not conduct electricity because they do not have an overall charge

64
Q

what thing about dot and cross diagram

A

do not tell us about the shape of the molecule

65
Q

bad thing about 2d stick diagram

A

cannot tell which electron in the bond came from which atom

66
Q

what are giant covalent bonds at room temperature

A

solids

67
Q

what do giant covalent bonds have

A

high melting and boiling points

68
Q

features of diamond

A

formed by carbon
contains lots if carbon atoms joined by covalent bonds
extremely hard
breaking covalent bonds takes a huge amount of energy because they have strong intermolecular forces

69
Q

can diamond conduct electricity

A

no because all of the outer electrons are in covalent bonds

70
Q

Silicon dioxide

A

contains oxygen and silicon covalently bonded together
-has a very high boiling and melting point because it has lots of covalent bonds

71
Q

what is graphite

A

made of carbon atoms
soft and slippery because layers can slide over each other
high melting and boiling point
good conductor of both electricity and of heat
often used as lubricant in machines
delocalised electrons can move and carry thermal energy and conduct electricity

72
Q

what is graphene

A

is a single layer of graphite
graphene is one atom thick
excellent conductor of electricity because it has delocalised electrons
is very strong

73
Q

what are fullerenes

A

molecules of carbon atoms with hollow shapes
used for
-pharmaceutical delivery
-lubricants
-catalysts

74
Q

carbon nanotubes

A

high tensile strength
excellent conductors of heat and electricity
reinforce materials

75
Q

benefits of 3d stick diagrams

A

shows us the shape of the molecule

76
Q

what is the conservation of mass

A

no atoms are lost or made during a chemical reactions so the mass of products equals the mass of reactants

77
Q

what do most metals form

A

positive ions

78
Q

what do most non metals form

A

negative ions

79
Q

what happens in an ionic compound

A

the charges on the ions have to cancel out to leave an overall charge of 0

80
Q

equation for percentage by mass of an element

A

total relative atomic mass of the atoms of element divided by relative formula mass

81
Q

equations for moles in element

A

moles=mass/relative atomic mass

82
Q

moles equation for compound

A

moles=mass/relative formula mass

83
Q

equation for mass

A

number of moles x relative formula mass

84
Q

avogadros constant

A

6.02x10^23

85
Q

what is a solute

A

a chemical that is dissolved in a solvent

86
Q

concentration equation

A

concentration =mass/volume

87
Q

mass equation

A

concentration x volume

88
Q

equation for volume

A

mass/concentration

89
Q

why is it not possible to achieve 100% yield

A

-some reactants may react in a different way than thought
-reversible reactions may not go to completion

90
Q

percentage yield equation

A

percentage yield=mass of product actually made / maximum theoretical mass of product x 100

91
Q

why is atom economy useful

A

-minimises the production of unwanted products so we save money
-increases sustainability by not wasting recources

92
Q

atom economy equation

A

atom economy = relative formula mass of desired products /sum of relative formula mass of reactants x100

93
Q

concentration equation

A

moles/volume

94
Q

volume equation

A

moles/concentration

95
Q

moles equation

A

concentration x volume

96
Q

volume

A

number of moles x 24

97
Q

exothermic

A

transfer energy from the reacting molecules to the surroundings

98
Q

exothermic reactions

A

neutralisation and combustion

99
Q

endothermic reactions

A

take in energy from their surroundings

100
Q

endothermic reactions

A

thermal decomposition

101
Q

what happens if we take 2 different metals and place them into an electrolyte

A

we can produce electricity

102
Q

what is an electrolyte

A

a solution that can conduct electricity

103
Q

what can a cell do

A

only produce electricity for a certain amount of time
-chemicals runs out

104
Q

what does a battery contain

A

two or more cells connected in series to produce a greater voltage

105
Q

what is gaining oxygen called

A

oxidation

106
Q

what is losing oxygen called

A

reduction

107
Q

reactivity series

A

potassium
sodium
lithium
calcium
magnesium
carbon
zinc
iron
hydrogen
copper

108
Q

what happens when metals react

A

they lose electrons and form a positive ion

109
Q

oxidation (electrons)

A

the loss of electrons

110
Q

reduction (electrons)

A

gain of electrons

111
Q

what are bases

A

chemicals that can neutralise acids producing salt + water

112
Q

acid + alkali

A

water

113
Q

acid + metal

A

salt + hydrogen

114
Q

solid ionic compounds (electrolysis)

A

cannot conduct electricity because the ions are locked in place and are not to free to move

115
Q

how do we extract metals

A

zinc iron copper are extracted by reduction with copper
everything above carbon is extracted using electrolysis

chemistry paper 1 (1 decks)

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