AQA A-Level Chemistry Paper 1
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1. how do van der waals random movement of electrons in one molecule creates a dipole, which
forces arise? (3 marks) induces a dipole in a neighbouring molecule, and these temporary
dipoles attract.
2. describe the structure - large macromolecular structure
and bonding in mag- - strong metallic bonds between magnesium ions and delocalised elec-
nesium. (2 marks) trons
3. how are ions detected they hit a detector plate and each ion gains an electron
in a TOF mass spec-
trometer?
4. how is the abundance they hit the detector plate and the size of the current produced is propor-
of ions measured in a tional to their abundance
TOF mass spectrome-
ter?
5. name and explain the -four bonding pairs and two lone pairs
shape of XeF₄. state -the lone pairs repel more than the bonding pairs, so they are opposite
the bond angle. (3 each other
marks) -bond angle 90°
6. name and explain the -four bonding pairs and no lone pairs
shape of CF₄. state the -the electron pairs all repel each other equally
bond angle. (3 marks) -bond angle 109.5°
7. explain why the elec- the atoms become larger and so there is less attraction between the
tronegativity of the nucleus and the bonding pair of electrons
halogens decreases
down the group. (2
marks)
8.
, AQA A-Level Chemistry Paper 1
Study online at https://quizlet.com/_fy93qd
state the type of in- - van der waals forces
termolecular forces in - movement of electrons in a molecule creates a dipole which induces a
SiF₄. explain how this dipole in a neighbouring molecule
type of intermolecular - the dipoles cancel
force arises and why
no other type of inter-
molecular force exists
in a sample of SiF₄. (3
marks)
9. explain why the boil- - bromine has a simple molecular structure
ing point of bromine - magnesium is metallic
is different to that - bromine has weak van der waals forces between the molecules
of magnesium. sug- - more energy is required to overcome the (stronger) metallic bonds
gest why magnesium - magnesium has a greater liquid range because forces of attraction in
is a liquid over a molten metals are stronger
much greater temper-
ature range compared
to bromine. (5 marks)
10. explain the difference covalent character, so the forces holding the lattice together are stronger
between the text-
book/theoretical value
(based on a perfect
ionic model) for en-
thalpy of lattice forma-
tion and the experi-
mental/calculated val-
ue.
11. identify a reagent that silver nitrate, yellow precipitate forms
could be used to iden-
, AQA A-Level Chemistry Paper 1
Study online at https://quizlet.com/_fy93qd
tify iodide ions in a
solution and describe
the observation made.
12. suggest why pure wa- pure water always has equal concentrations of H+ and OH- ions
ter is not acidic or alka-
line even when its pH
is not 7.
13. state the types of crys- sulfur dioxide - giant covalent structure
tal structures shown in sulfur trioxide - molecular
silicon dioxide and sul-
fur trioxide.
14. explain why silicon silicon dioxide has covalent bonds between its atoms, sulfur trioxide has
dioxide has a higher van der waals forces, covalent bonds are stronger than van der waals
melting point than sul- forces, so more energy is required to overcome the covalent bonds
fur trioxide.
15. platinum acts as a het- - reactant(s) adsorbed onto the platinum provides a surface for the reac-
erogeneous catalyst in tion
the reaction between - reaction occurs on the surface
ammonia and oxygen. - product is desorbed
it provides an alter-
native reaction route
with a lower activation
energy. describe the
stages of this alterna-
tive route.
16. explain why the sec- the outer electrons in calcium are futher from the nucleus, so there is more
ond ionisation ener- shielding than in potassium
gy of calcium is low-
, AQA A-Level Chemistry Paper 1
Study online at https://quizlet.com/_fy93qd
er than the second
ionisation energy of
potassium.
17. why do isotopes of el- they all have the same electronic configuration
ements have identical
chemical properties?
18. state the meaning of completely ionises
the term strong acid.
19. explain how the salt ions can move through it
bridge in an electro-
chemical cell provides
an electrical connec-
tion between the two
solutions.
20. explain why sodium sodium, sodium bromide and sodium iodide all have a lattice structure.
bromide has a high- sodium has metallic bonding and sodium bromide and sodium iodide
er melting point than have ionic bonding. the ionic bonds are stronger than the metallic bonds.
that of sodium and there is stronger attraction between the positive and negative ions in NaBr
sodium iodide. than NaI, since the Br- ion is smaller than the I- ion.
21. describe the shape of two bonding pairs and two lone pairs. bond angle 104.5°. the electrons
the NH2⁻ ion. predict pairs all repel to be as far apart as possible. the repulsion between lone
the bond angle. justify pairs is stronger than the repulsion between a lone pair and a bonding
your prediction. pair.
22. describe the process sample is dissolved, then injected through a fine needle at high voltage,
of electrospray ionisa- so a proton is gained
tion.
Study online at https://quizlet.com/_fy93qd
1. how do van der waals random movement of electrons in one molecule creates a dipole, which
forces arise? (3 marks) induces a dipole in a neighbouring molecule, and these temporary
dipoles attract.
2. describe the structure - large macromolecular structure
and bonding in mag- - strong metallic bonds between magnesium ions and delocalised elec-
nesium. (2 marks) trons
3. how are ions detected they hit a detector plate and each ion gains an electron
in a TOF mass spec-
trometer?
4. how is the abundance they hit the detector plate and the size of the current produced is propor-
of ions measured in a tional to their abundance
TOF mass spectrome-
ter?
5. name and explain the -four bonding pairs and two lone pairs
shape of XeF₄. state -the lone pairs repel more than the bonding pairs, so they are opposite
the bond angle. (3 each other
marks) -bond angle 90°
6. name and explain the -four bonding pairs and no lone pairs
shape of CF₄. state the -the electron pairs all repel each other equally
bond angle. (3 marks) -bond angle 109.5°
7. explain why the elec- the atoms become larger and so there is less attraction between the
tronegativity of the nucleus and the bonding pair of electrons
halogens decreases
down the group. (2
marks)
8.
, AQA A-Level Chemistry Paper 1
Study online at https://quizlet.com/_fy93qd
state the type of in- - van der waals forces
termolecular forces in - movement of electrons in a molecule creates a dipole which induces a
SiF₄. explain how this dipole in a neighbouring molecule
type of intermolecular - the dipoles cancel
force arises and why
no other type of inter-
molecular force exists
in a sample of SiF₄. (3
marks)
9. explain why the boil- - bromine has a simple molecular structure
ing point of bromine - magnesium is metallic
is different to that - bromine has weak van der waals forces between the molecules
of magnesium. sug- - more energy is required to overcome the (stronger) metallic bonds
gest why magnesium - magnesium has a greater liquid range because forces of attraction in
is a liquid over a molten metals are stronger
much greater temper-
ature range compared
to bromine. (5 marks)
10. explain the difference covalent character, so the forces holding the lattice together are stronger
between the text-
book/theoretical value
(based on a perfect
ionic model) for en-
thalpy of lattice forma-
tion and the experi-
mental/calculated val-
ue.
11. identify a reagent that silver nitrate, yellow precipitate forms
could be used to iden-
, AQA A-Level Chemistry Paper 1
Study online at https://quizlet.com/_fy93qd
tify iodide ions in a
solution and describe
the observation made.
12. suggest why pure wa- pure water always has equal concentrations of H+ and OH- ions
ter is not acidic or alka-
line even when its pH
is not 7.
13. state the types of crys- sulfur dioxide - giant covalent structure
tal structures shown in sulfur trioxide - molecular
silicon dioxide and sul-
fur trioxide.
14. explain why silicon silicon dioxide has covalent bonds between its atoms, sulfur trioxide has
dioxide has a higher van der waals forces, covalent bonds are stronger than van der waals
melting point than sul- forces, so more energy is required to overcome the covalent bonds
fur trioxide.
15. platinum acts as a het- - reactant(s) adsorbed onto the platinum provides a surface for the reac-
erogeneous catalyst in tion
the reaction between - reaction occurs on the surface
ammonia and oxygen. - product is desorbed
it provides an alter-
native reaction route
with a lower activation
energy. describe the
stages of this alterna-
tive route.
16. explain why the sec- the outer electrons in calcium are futher from the nucleus, so there is more
ond ionisation ener- shielding than in potassium
gy of calcium is low-
, AQA A-Level Chemistry Paper 1
Study online at https://quizlet.com/_fy93qd
er than the second
ionisation energy of
potassium.
17. why do isotopes of el- they all have the same electronic configuration
ements have identical
chemical properties?
18. state the meaning of completely ionises
the term strong acid.
19. explain how the salt ions can move through it
bridge in an electro-
chemical cell provides
an electrical connec-
tion between the two
solutions.
20. explain why sodium sodium, sodium bromide and sodium iodide all have a lattice structure.
bromide has a high- sodium has metallic bonding and sodium bromide and sodium iodide
er melting point than have ionic bonding. the ionic bonds are stronger than the metallic bonds.
that of sodium and there is stronger attraction between the positive and negative ions in NaBr
sodium iodide. than NaI, since the Br- ion is smaller than the I- ion.
21. describe the shape of two bonding pairs and two lone pairs. bond angle 104.5°. the electrons
the NH2⁻ ion. predict pairs all repel to be as far apart as possible. the repulsion between lone
the bond angle. justify pairs is stronger than the repulsion between a lone pair and a bonding
your prediction. pair.
22. describe the process sample is dissolved, then injected through a fine needle at high voltage,
of electrospray ionisa- so a proton is gained
tion.
