CIE AS Chemistry

Topic Questions

ASChemistryCIETopic Questions1. Physical Chemistry1.1 Atomic Structure

Syllabus Edition

First teaching 2020

Last exams 2024

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1.1 Atomic Structure

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1a4 marks

Complete Table 1.1 to show the relative charge and mass of the subatomic particles.

Table 1.1

Subatomic particle Relative Charge Relative Mass
Proton   1
Neutron    

Electron

   1 over 1836

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1b
Sme Calculator3 marks

Using the Periodic Table, complete Table 1.2 to show the number of protons, neutrons and electrons in each of the given species.

Table 1.2

Species Number of protons Number of neutrons Number of electrons 
31P      
24Na+      
37Cl–      

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1c2 marks

State why the physical properties of isotopes are different.

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1d2 marks

Explain why the chemical properties of 35Cl and 37Cl are similar.

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2a1 mark

An isotope of element X has two more protons and two more neutrons than an atom of 41K. Use the Periodic Table to identify element X.

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2b3 marks

Give the full electronic configuration of the following species:

 
K+ .........................................................................................
 
Ti ..........................................................................................
 
Co ........................................................................................

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2c3 marks

Ionisation energy reactions are endothermic processes.

i)
Write the equations for the first ionisation energy of K and the second ionisation energy of Sc
[2]
 
ii)
Give the full electronic configuration of the Sc2+ 
[1]

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2d5 marks

Table 2.1 shows successive ionisation energies of element Z in Period 3. 

Table 2.1

  1 2 3 4 5

Ionisation energy
(kJ mol-1)

 786 1576 3232 4356 16091

i)
State why the first ionisation energy generally increases from left to right across the Periodic Table. 
[2]
ii)
Using the data of successive ionisation energies in table 2.1, state which group of the Periodic Table element Z belongs to. 

Group .........................

Explanation .........................................................................................................
[3]

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3a1 mark

Aluminium is a metal in Group 13

Complete the electron configuration in Fig. 3.1 for an aluminium atom using box notation.

1-1-atomic-structure-2c-a
Fig. 3.1

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3b1 mark

Draw the orbital of the 2s orbital on the axis in Fig. 3.2.

1-1-3b-e-orbital-axis
Fig. 3.2

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3c1 mark

The first ionisation energy values of Li, Mg and Na are shown in Table 3.1

Table 3.1

Element First ionisation energy (kJ mol-1)
  496
Li 520
  738


Complete the table.

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3d2 marks

Explain why the first ionisation energy of aluminium is lower than the first ionisation energy of magnesium.

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4a2 marks

Give the electron configuration of the following species:


Mg .................................................................

Mg2+ .................................................................

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4b2 marks

Write an equation including state symbols to show the first ionisation energy of Mg.

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4c2 marks

Explain why the second ionisation energy of Mg is higher that the first ionisation energy.

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5a1 mark

Fig. 5.1 shows how protons, neutrons and electrons behave differently when they move at the same velocity in an electric field.

Label the positive and negative plates in Fig. 5.1.

129c5fc8-2d7a-4e7d-be1d-139c459aad6d
 
Fig. 5.1

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5b3 marks

Using the Periodic Table, complete Table 5.1 to show the number of protons, neutrons and electrons in each of the given species.

Table 5.1
 
Symbol Protons Neutrons Electrons
23Na      
32S2–      
86Sr2+      
 

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5c1 mark

Write the electronic configuration for the 32S2– atom.

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1a5 marks

Fig. 1.1 shows the elements from the first three periods of the Periodic Table.

first-three-periods-of-pt

Fig. 1.1

Identify an element that fits each of the following descriptions:

i)
An element that forms a 2- ion with the same electronic configuration as Ne 
[1]
ii)
The Period 3 element with the highest boiling point 
[1]
iii)
The element from the first three periods with the largest atomic radius 
[1]
iv)
The element from the first three periods with the highest first ionisation energy
[1]
v)
The Period 3 element with the successive ionisation energies shown in Table 1.1

Table 1.1 

Ionisation number

1st

2nd

3rd

4th

Ionisation energy / kJ mol−1

738

1451

7733

10541
[1]

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1b5 marks

Fig. 1.2 shows the first ionisation energies for six consecutive elements labelled A-F. 

ionisation-energy-graph-

Fig. 1.2 

Complete the graph to show the first ionisation energies of elements G-K.

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1c2 marks

Explain why the value of the first ionisation energy for D is greater than for C.

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2a4 marks

Successive ionisation energies provide evidence for the arrangement of electrons in atoms. In Table 2.1, the successive ionisation energies of oxygen are given.

Table 2.1

Ionisation number 1 2 3 4 5 6 7 8
Ionisation energy / kJ mol-1 1314 3388 5301 7469 10989 13327 71337 84080

 

i)
Give the equation, including state symbols, for the third ionisation energy of oxygen. 
 
[2]

ii)
Explain how this data shows evidence of two energy shells in oxygen.
 
[2]

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2b3 marks

Give the full electron configuration of the following atoms and ions.

 
i)
Te
 
[1]
 
ii)
Zn2+
 
[1]
 
iii)
Cu2+
 
[1]

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2c
Sme Calculator2 marks

Palladium is a transition metal that is primarily used in a catalytic converter.

 
i)
Give the electron configuration for the Zirconium 2+ ion, Zr2+, starting with [Kr]. 
 
[1]
 
ii)
Give the equation including state symbols to represent the third ionisation energy of Zirconium, Zr.
 
[1]

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3a
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Copper is an easily moulded base metal that is often added to precious metals to improve their elasticity, flexibility, hardness, colour, and resistance to corrosion.

Table 3.1 shows the number of protons, neutrons and electrons of different isotopes and ions of copper.

 
Table 3.1
 
Species Protons Neutrons Electrons
    34 27
65Cu+ 29    
 
i)
Complete Table 3.1.
 
[2]
 
ii)
Give the full electron configuration of the Cu+ ion. 
 
[1]

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3b
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Calculate the percentage abundance of 63Cu with a mass of 62.9296 and 65Cu with a mass of 64.9278, when the average mass of the Cu isotope is 63.546.

 

Express your answer to an appropriate number of significant figures.

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3c2 marks

Explain why the isotopes of copper exhibit the same chemical reactions but their densities differ.

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3d2 marks

Copper can form a salt with chlorine to form copper(II) chloride. This reacts with sodium phosphate to form two different salts only.

 

Write a balanced equation for this reaction.

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4a6 marks

Table 4.1 below shows the atomic radii for the elements of Period 2, Li to F.

Table 4.1 

Element

 Li Be B C N O F
Atomic radius / pm 152 112 88 77 70 66 68

 

i)
Explain the variation in atomic radius.
 
[4]
 
ii)
The value for neon is missing in Table 4.1. Explain why the atomic radius of neon cannot be measured in the same way as the other Period 2 elements.
 
[2]

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4b1 mark

Complete Fig. 4.1 to show the electronic configuration of boron in the excited state.

 
1-1-atomic-structure-2c-a
 
Fig. 4.1

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4c2 marks

Explain why the first ionisation energy of boron is lower than the first ionisation of beryllium.

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4d1 mark

The successive ionisation energies for another element, J, are shown in Table 4.2.

 
Table 4.2
 

Energy number

1st

2nd

3rd

4th

5th

Ionisation energy value / kJ mol−1 

738

1450

7733

10543

13630
 

State the formula of the compound when element J reacts with chlorine. 

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5a2 marks

In the blast furnace, carbon can react with oxygen to form carbon dioxide and carbon monoxide.

Write one equation for the this reaction. 

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5b2 marks

Identify and draw the subshell on Fig. 5.1 which has the highest occupied energy level in an oxygen atom.

 
Subshell …………………………….
 
[1]
 
Diagram
1-1-3b-e-orbital-axis
Fig. 5.2

[1]

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5c5 marks
i)
Complete Fig. 5.2 to show the excited state of a carbon atom.
 
1-1-atomic-structure-2c-a
 
Fig. 5.2 
 
[1]
 
ii)
Identify the type of hybridisation that arises in a molecule of carbon monoxide for both atoms and explain how this hybridisation occurs

Hybridisation ………….

Explanation
[4]

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1a2 marks

The composition of atoms and ions can be determined from knowledge of atomic number, nucleon number and charge.

Complete Table 1.1.

Table 1.1 

Atomic number Nucleon number Number of electrons Number of protons Number of neutrons Symbol 
9   10     straight F presubscript 9 presuperscript 19 superscript minus
    23 26 32  

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1b2 marks

Lithium and potassium are Group 1 metals. 

State the following for the potassium 1+ ion with a nucleon number of 39.

Symbol .......................................

[1] 

Full electronic configuration .................................................

[1] 

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1c3 marks

Beams of protons, neutrons and electrons behave differently in an electric field due to their differing properties.


Fig. 1.1 shows the path of a beam of electrons in an electric field.


Add and label lines to Fig. 1.1 to represent the paths of beams of protons and neutrons in the same field.

screen-shot-2023-01-09-at-12-07-30
Fig. 1.1 

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1d6 marks

The fifth to eighth ionisation energies of three elements in the third period of the Periodic Table are given. The symbols used for reference are not the actual symbols of the elements.

  Ionisation energies, kJ mol-1
  fifth sixth seventh eighth
X 6274 21 269 25 398 29 855
Y 7012 8496 27 107 31 671
Z 6542 9362 11 018 33 606

i)
State and explain the group number of element Y.
 
Group number ...............................
 
Explanation ..............................
[1]
 
ii)
State and explain the general trend in first ionisation energies across the third period.
[2]
 
iii)
Explain why the first ionisation energy of element Y is less than that of element X.
[2]
 
iv)
Complete the electronic configuration of element Z.
1s2 .................
[1]

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2a4 marks

The model of the nuclear atom was first proposed by Ernest Rutherford. He developed this model on the basis of results obtained from an experiment using gold metal foil.

Complete the Table 2.1 with information for two of the particles in an atom of 197Au.

Table 2.1
 
Particle Relative mass Relative charge Location within atom Total number in an atom of 197Au
electron 0.0005 -1   79
neutron     nucleus   

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2b3 marks

A sample of gold found in the earth consists of only one isotope.

i)
Explain what is meant by the term isotopes
[2]

ii)
A different sample of gold contains more than one isotope.

Suggest why this different sample of gold has the same chemical properties as the sample found in the earth.
[1]

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2c1 mark

Gold(III) chloride, traditionally called auric chloride, is one of the most common compounds of gold.

It has the formula AuCl3.

Complete the electron configuration for the chloride ion using box notation.

1-1-atomic-structure-2c-a

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2d3 marks

On the axes shown in Fig. 2.1, draw a sketch diagram of one of each different type of orbital that is occupied by the electrons in a Period 3 element. 

Label each type of orbital. 

1-1-atomic-structure-2d-a

Fig. 2.1

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3a3 marks

All elements have a value for a first ionisation energy. 

i)
Define the term first ionisation energy of an element.
[2]
ii)
Write the equation for the first ionisation energy of aluminium.
[1]

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3b2 marks

Table 3.1 shows successive ionisation energies of an element A, found in period 3 of the Periodic Table.

Table 3.1

Number of electrons 1 2 3 4 5 6 7 8

Ionisation energy (kJ mol-1)

 1012 1904 2914 4964 6274 21 268 25 431 29 872

Identify element A. Explain your answer using data from Table 3.1.

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3c6 marks

Fig. 3.1 shows the trend in ionisation energy for Period 3 of the Periodic Table.

period-3-ionisation-energies

Fig. 3.1

i) 
Explain why the first ionisation energy increases across Period 3.
[3]
ii)
Explain the deviations in the trend. 
[3]

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3d1 mark

Explain why the second ionisation energy of aluminium is a larger value than the first ionisation energy.

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4a2 marks

Iron and cobalt are adjacent elements in the Periodic Table. Iron has three main naturally occurring isotopes, cobalt has one.

Explain the meaning of the term isotope.

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4b
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Isotopes of polonium, proton number 84, are produced by the radioactive decay of several elements including thorium, proton number 90. The isotope 213Po is produced from the thorium isotope 232Th.

Complete Table 4.1 below to show the atomic structures of the isotopes 213Po and 232Th.

Table 4.1 

Isotope Protons Neutrons  Electrons
213Po      
232Th      

 

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4c2 marks

Polonium has twenty five different isotopes.

Explain why the isotopes of polonium exhibit the same chemical reactions but their boiling points differ slightly.  

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5a2 marks

The first six ionisation energies of an element X are given below in Table 5.1.

Table 5.1

  First Second Third Fourth Fifth Sixth

Ionisation energy 

(kJ mol-1)

 950  1800 2700 4800 6000 12 300

Write an equation, with state symbols, for the second ionisation energy of element X.

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5b3 marks

Use the data given above to deduce in which group of the Periodic Table element X is placed. Explain your answer.

Group ........................................................

Explanation ............................................................ 

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5c4 marks

The first ionisation energies (I.E.) for the elements of Group 4 are given below in Table 5.2.

Table 5.2

Element  C Si Ge Sn Pb
1st I.E (kJ mol-1) 1090 786 762 707 716

Explain the trend shown by these values in terms of the atomic structure of the elements.

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5d1 mark

Write the full electronic configuration for germanium.

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