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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
group 0 (noble gases)
-very unreactive because they have a full outer shell -as you go down group 0 boiling point increases
26
group 1 (alkali metals)
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
27
group 7 (the halogens)
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
28
Transition elements/metals
all metals hard/strong metals all have high melting points high density much less reactive than group 1 metals useful as catalysts
29
what can copper be used for
pipes that carry water
30
Solids
-hard to compress -packed together with no spaces -fixed shape -particles vibrate
31
Liquids
-hard to compress -take the shape of container -they can move
32
gases
-easy to compress -widely spaced -move quickly and randomly
33
limitations of gas , liquid , solid diagrams
-simple particle model assumes that all particles are solid spheres -assumes that there are no forces between the particles
34
what is metallic bonding
is the electrostatic attraction between positive metal ions and delocalised electrons
35
what is a solid to liquid called
melting
36
what is a liquid to solid called
freezing
37
what is liquid to gas called
boiling
38
what is a gas to liquid called
condensing
39
what do coarse particles contain
thousands of atoms
40
what do fine particles contain
several thousand atoms
41
what do nanoparticles contain
a few hundred atoms
42
what is ionic bonding
when a metal and a non-metal react
43
what do ionic compounds form
giant ionic lattices
44
what happens with surface area : volume ratio
as the particle size decreases by 10 times the surface area:volume ratio increases by 10 times
45
what did nano particles have
a huge surface area:volume ratio
46
uses of nanoparticles
suncream catalysts cosmetics electronics
47
risk of nanoparticles
can be absorbed into body and enter our cells
48
what happens in a giant ionic lattice
every positive ion is surrounded by negative ions
49
features of giant ionic lattices
-3d structures very strong electrostatic forces
50
features of ionic compounds
-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
what is an alloy
an alloy is a mixture of metals -harder than pure metals
52
how are polymers made
are made by joining together thousands of small identical molecules (monomers)
53
what are monomers often
alkene molecules
54
what bond are monomers
double covalent bonds
55
what bond is poly(ethene)
single covalent bond
56
what state are polymers at room temperature
solid
57
features of metals
high boiling and melting point melting can be bent or shaped because the layers of atoms are able to slide over each other
58
what is covalent bonding
when non metals bond together
59
are covalent bonds strong
yes
60
what type of bond us a shared pair of electrons
single covalent bond
61
what type of bond is 2 shared pairs of electrons
double covalent bond
62
what type of bond is 3 shared pairs of electrons
triple covalent bond
63
small covalent molecules
-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
what thing about dot and cross diagram
do not tell us about the shape of the molecule
65
bad thing about 2d stick diagram
cannot tell which electron in the bond came from which atom
66
what are giant covalent bonds at room temperature
solids
67
what do giant covalent bonds have
high melting and boiling points
68
features of diamond
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
can diamond conduct electricity
no because all of the outer electrons are in covalent bonds
70
Silicon dioxide
contains oxygen and silicon covalently bonded together -has a very high boiling and melting point because it has lots of covalent bonds
71
what is graphite
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
what is graphene
is a single layer of graphite graphene is one atom thick excellent conductor of electricity because it has delocalised electrons is very strong
73
what are fullerenes
molecules of carbon atoms with hollow shapes used for -pharmaceutical delivery -lubricants -catalysts
74
carbon nanotubes
high tensile strength excellent conductors of heat and electricity reinforce materials
75
benefits of 3d stick diagrams
shows us the shape of the molecule
76
what is the conservation of mass
no atoms are lost or made during a chemical reactions so the mass of products equals the mass of reactants
77
what do most metals form
positive ions
78
what do most non metals form
negative ions
79
what happens in an ionic compound
the charges on the ions have to cancel out to leave an overall charge of 0
80
equation for percentage by mass of an element
total relative atomic mass of the atoms of element divided by relative formula mass
81
equations for moles in element
moles=mass/relative atomic mass
82
moles equation for compound
moles=mass/relative formula mass
83
equation for mass
number of moles x relative formula mass
84
avogadros constant
6.02x10^23
85
what is a solute
a chemical that is dissolved in a solvent
86
concentration equation
concentration =mass/volume
87
mass equation
concentration x volume
88
equation for volume
mass/concentration
89
why is it not possible to achieve 100% yield
-some reactants may react in a different way than thought -reversible reactions may not go to completion
90
percentage yield equation
percentage yield=mass of product actually made / maximum theoretical mass of product x 100
91
why is atom economy useful
-minimises the production of unwanted products so we save money -increases sustainability by not wasting recources
92
atom economy equation
atom economy = relative formula mass of desired products /sum of relative formula mass of reactants x100
93
concentration equation
moles/volume
94
volume equation
moles/concentration
95
moles equation
concentration x volume
96
volume
number of moles x 24
97
exothermic
transfer energy from the reacting molecules to the surroundings
98
exothermic reactions
neutralisation and combustion
99
endothermic reactions
take in energy from their surroundings
100
endothermic reactions
thermal decomposition
101
what happens if we take 2 different metals and place them into an electrolyte
we can produce electricity
102
what is an electrolyte
a solution that can conduct electricity
103
what can a cell do
only produce electricity for a certain amount of time -chemicals runs out
104
what does a battery contain
two or more cells connected in series to produce a greater voltage
105
what is gaining oxygen called
oxidation
106
what is losing oxygen called
reduction
107
reactivity series
potassium sodium lithium calcium magnesium carbon zinc iron hydrogen copper
108
what happens when metals react
they lose electrons and form a positive ion
109
oxidation (electrons)
the loss of electrons
110
reduction (electrons)
gain of electrons
111
what are bases
chemicals that can neutralise acids producing salt + water
112
acid + alkali
water
113
acid + metal
salt + hydrogen
114
solid ionic compounds (electrolysis)
cannot conduct electricity because the ions are locked in place and are not to free to move
115
how do we extract metals
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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