AQA A-LEVEL CHEMISTRY PAPER 1 INORGANIC AND PHYSICAL
CHEMISTRY QP 2020
Please write clearly in block capitals.
Centre number Candidate number
Surname
Forename(s)
Candidate signatu re
I declare this is my own work.
A-level
CHEMISTRY
Paper 1 Inorganic and Physical Chemistry
Tuesday 2 June 2020 Afternoon Time allowed: 2 hours
Materials For Examiner’s Use
For this paper you must have:
the Periodic Table/Data Booklet, provided as an insert (enclosed) Question Mark
a ruler with millimetre measurements 1
a scientific calculator, which you are expected to use where appropriate.
2
Instructions 3
Use black ink or black ball-point pen. 4
Fill in the boxes at the top of this page. 5
Answer all questions.
6
You must answer the questions in the spaces provided. Do not write outside
the box around each page or on blank pages. 7
If you need extra space for your answer(s), use the lined pages at the end of 8
this book. Write the question number against your answer(s).
9
All working must be shown.
Do all rough work in this book. Cross through any work you do not 10
want to be marked. 11
TOTAL
Information
The marks for questions are shown in brackets.
The maximum mark for this paper is 105.
*JUN207405101*
IB/M/Jun20/E7 7405/1
, 2
Do not write
outside the
Answer all questions in the spaces provided. box
0 1 This question is about enthalpy changes.
0 1 . 1 Figure 1 shows a Born–Haber cycle for the formation of strontium chloride, SrCl2
Figure 1
Table 1 shows some thermodynamic data.
Table 1
Enthalpy change
/ kJ mol–1
First ionisation energy of strontium +548
Second ionisation energy of strontium +1060
Enthalpy of atomisation of chlorine +121
Enthalpy of atomisation of strontium +164
Enthalpy of formation of strontium chloride –828
Enthalpy of lattice formation of strontium chloride –2112
*02*
IB/M/Jun20/7405/1
, 3
Do not write
outside the
Use the data in Table 1 to calculate a value for the electron affinity of chlorine. box
[3 marks]
Electron affinity kJ mol–1
0 1 . 2 Draw a line from each substance to the enthalpy of lattice formation of that substance.
[1 mark]
Substance Enthalpy of lattice
formation / kJ mol–1
MgCl2 –2018
MgO –2493
BaCl2 –3889
Question 1 continues on the next page
Turn over ►
*03*
IB/M/Jun20/7405/1
, 4
Do not write
outside the
box
Table 2 shows the theoretical lattice enthalpy, based on a perfect ionic model, and an
experimental value for the enthalpy of lattice formation of silver chloride.
Table 2
Theoretical Experimental
Enthalpy of lattice formation / kJ mol –1
–770 –905
0 1 . 3 State why there is a difference between the theoretical and experimental values.
[1 mark]
0 1 . 4 Table 3 shows enthalpy of hydration values for ions of some Group 1 elements.
Table 3
Li+(g) Na+(g) K+(g)
Enthalpy of hydration / kJ mol–1 –519 –406 –322
Explain why the enthalpy of hydration becomes less exothermic from Li+ to K+
[2 marks]
*04*
IB/M/Jun20/7405/1
CHEMISTRY QP 2020
Please write clearly in block capitals.
Centre number Candidate number
Surname
Forename(s)
Candidate signatu re
I declare this is my own work.
A-level
CHEMISTRY
Paper 1 Inorganic and Physical Chemistry
Tuesday 2 June 2020 Afternoon Time allowed: 2 hours
Materials For Examiner’s Use
For this paper you must have:
the Periodic Table/Data Booklet, provided as an insert (enclosed) Question Mark
a ruler with millimetre measurements 1
a scientific calculator, which you are expected to use where appropriate.
2
Instructions 3
Use black ink or black ball-point pen. 4
Fill in the boxes at the top of this page. 5
Answer all questions.
6
You must answer the questions in the spaces provided. Do not write outside
the box around each page or on blank pages. 7
If you need extra space for your answer(s), use the lined pages at the end of 8
this book. Write the question number against your answer(s).
9
All working must be shown.
Do all rough work in this book. Cross through any work you do not 10
want to be marked. 11
TOTAL
Information
The marks for questions are shown in brackets.
The maximum mark for this paper is 105.
*JUN207405101*
IB/M/Jun20/E7 7405/1
, 2
Do not write
outside the
Answer all questions in the spaces provided. box
0 1 This question is about enthalpy changes.
0 1 . 1 Figure 1 shows a Born–Haber cycle for the formation of strontium chloride, SrCl2
Figure 1
Table 1 shows some thermodynamic data.
Table 1
Enthalpy change
/ kJ mol–1
First ionisation energy of strontium +548
Second ionisation energy of strontium +1060
Enthalpy of atomisation of chlorine +121
Enthalpy of atomisation of strontium +164
Enthalpy of formation of strontium chloride –828
Enthalpy of lattice formation of strontium chloride –2112
*02*
IB/M/Jun20/7405/1
, 3
Do not write
outside the
Use the data in Table 1 to calculate a value for the electron affinity of chlorine. box
[3 marks]
Electron affinity kJ mol–1
0 1 . 2 Draw a line from each substance to the enthalpy of lattice formation of that substance.
[1 mark]
Substance Enthalpy of lattice
formation / kJ mol–1
MgCl2 –2018
MgO –2493
BaCl2 –3889
Question 1 continues on the next page
Turn over ►
*03*
IB/M/Jun20/7405/1
, 4
Do not write
outside the
box
Table 2 shows the theoretical lattice enthalpy, based on a perfect ionic model, and an
experimental value for the enthalpy of lattice formation of silver chloride.
Table 2
Theoretical Experimental
Enthalpy of lattice formation / kJ mol –1
–770 –905
0 1 . 3 State why there is a difference between the theoretical and experimental values.
[1 mark]
0 1 . 4 Table 3 shows enthalpy of hydration values for ions of some Group 1 elements.
Table 3
Li+(g) Na+(g) K+(g)
Enthalpy of hydration / kJ mol–1 –519 –406 –322
Explain why the enthalpy of hydration becomes less exothermic from Li+ to K+
[2 marks]
*04*
IB/M/Jun20/7405/1
