Syllabus Edition

First teaching 2014

Last exams 2024

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The Periodic Table & Periodic Trends (DP IB Chemistry: SL)

Exam Questions

3 hours44 questions
1a1 mark

Define the term first ionisation energy and state what is meant by the term periodicity.

1b1 mark

Distinguish between the terms group and period.

1c1 mark

State the property that determines the order in which elements are arranged in the periodic table.

1d2 marks
State the relationship between the electron arrangement of an element and its group and period in the periodic table.

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2a2 marks

Explain the following statement.

The first ionisation energy of potassium is smaller than the first ionisation energy of calcium.

2b2 marks

Explain the following statement.

The first ionisation energy of potassium is larger in value than rubidium

2c3 marks

Using section 8 of the data booklet, explain the trend of decreasing electronegativity values of the Group 17 elements from F to I.

2d1 mark

Define the term electronegativity.

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3a1 mark

Define what is meant by the term electron affinity.

3b1 mark

State whether first electron affinity is an exothermic or endothermic process.

3c2 marks

Write an equation, including state symbols, for the first electron affinity of bromine.

3d1 mark

State whether the first electron affinity of I is more or less exothermic than Br.

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4a2 marks

An element has the following electron configuration.

1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p4

i)
State which block of the periodic table the element is in.

ii)
State how many electrons it has in its outer shell.
4b3 marks

Magnesium can be ionised to form a cation, Mg+.

i)
Write the electron configuration of an Mg+

ii)
Define the term ‘first ionisation energy'  in relation to magnesium.

4c1 mark

The periodic table can be divided into blocks.

State why are silicon, carbon, oxygen and chlorine all classified as p-block elements.

4d2 marks

This question is about the periodicity of period 3 elements.

i)
State the trend in atomic radius across period 3.

ii)

State the general trend in first ionisation energies across period 3.

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5a1 mark

Antimony, Sb, has atomic number 51.

Using section 6 of the data booklet, complete the table to show where antimony is found in the periodic table.

Period

Block

   

5b1 mark

Identify the element that is in the d-block of the periodic table which forms a 3+ ion with the following electron configuration.

[Ar] 3d3

5c1 mark

Ionisation energies can provide evidence for electron structure.

Write an equation, including state symbols, for the first ionisation energy of chlorine.

5d1 mark

An element Y has the following six first ionisation energies in kJ mol-1. These are shown in the table below.

 

1st 

2nd

3rd

4th

5th

6th

Ionisation energy (kJ mol-1)

577

1820

2740

11 600

14 800

18 400

State what group of the periodic table this element belongs to.

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1a4 marks

The periodic table displays the chemical elements, arranged in order of increasing atomic number. It is made up of groups and periods of elements.

State and explain the general trend in first ionisation energy across a period of the periodic table.

1b3 marks

The general trend in first ionisation energies stated in part (a) is seen across period 2 of the periodic table. However, boron and one other period 2 element deviate from this trend.

Identify this element and explain why it deviates from the general trend.

1c2 marks

State why nitrogen is classed as a p block element and give its full electron configuration.

1d3 marks

Identify the period 3 element that has the lowest melting point.

Explain your answer with reference to bonding and structure.

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2a3 marks

The first ionisation energy for all the elements is found in Section 8 of the IB data booklet.

i)
Define the term first ionisation energy of an element. 

ii)
Write the equation for the first ionisation energy of aluminium.
2b2 marks

The table below shows successive ionisation energies of an element A, found in period 3 of the periodic table.

Table 1

Number of electrons

1

2

3

4

5

6

7

8

Ionisation Energy
(kJ mol-1)

1012

1907

2914

4964

6274

21268

25431

29872

  

Identify element A.

Explain your answer using data from Table 1.

2c5 marks

The graph below in Figure 1 shows some information on the elements of period 3 of the periodic table.

Figure 1

3-1-ib-chemistry-sq-q2c-medium

 State and explain the trend that this graph shows, including why there are values that deviate from the trend.

2d1 mark

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

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3a3 marks

This question is about the structure of the periodic table.
Throughout the early history of the periodic table scientists have attempted to order the elements according to different properties.

State the property that is used to order the elements in the modern periodic table.

Outline how the electron configuration of elements is related to their group and period in the periodic table.

3b2 marks

This question is about the element phosphorus.

i)
State the group number, period number, and block in which you would find the element phosphorus. 

ii)
State the full electron configuration of the phosphide ion, P3-.
3c2 marks

Outline why the atomic radius is seen to decrease across period 2 (from lithium to fluorine).

3d3 marks

Gallium forms an ion smaller than its element, whereas arsenic forms an ion larger than its element.

Explain these differences in ionic radius.

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4a3 marks

Bromine and selenium are both found in period 4 of the periodic table.

State and explain which of the two has a higher electronegativity.

4b2 marks

Sketch on the axes shown below in Figure 1, a graph of the first ionisation energy against atomic number for the elements of group 1.

Figure 1

 3-1-ib-chemistry-sq-q4b-medium           

Explain the trend in ionisation energy down group 1.

4c3 marks

Discuss the similarities and differences between the trends in atomic radius and ionic radius down group 1 and group 17.

4d2 marks

State how the first ionisation energy of potassium differs from that of:

i)
Calcium 

ii)
Rubidium 

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5a2 marks

Group 17 elements are known as highly electronegative non-metal elements.

i)
Define the term electronegativity. 

ii)
State and explain the trend in electronegativity in group 17. 
5b2 marks

Define the term electron affinity and write an equation to show the first electron affinity of bromine.

5c2 marks

State, with reasons, whether the first electron affinity of iodine is more or less exothermic than bromine.

5d2 marks

Suggest why the second electron affinity of oxygen is endothermic.

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1a3 marks

This question refers to the elements in the first three periods of the Periodic Table.

Select an element from the first three periods that fits each of the following descriptions.

i)
The element with the highest first ionisation energy

[1]

ii)
The element that forms a 1 ion with the same electron configuration as helium

[1]

iii)
An element which forms a compound with hydrogen in which the element has an oxidation number of −4

[1]

1b5 marks

This question is about the elements which have atomic numbers 33 to 37.

The first ionisation energies of these elements are shown in the table below.

Element

As

Se

Br

Kr

Rb

Ionisation energy value in kJ /mol-1

947

941

1340

1351

403

i)
Suggest the formulae of the hydrides of arsenic and selenium

[2]

ii)
Explain why the first ionisation energy of rubidium is lower than that of krypton

[2]

iii)
State which of the elements, arsenic to rubidium, has atoms with the smallest atomic radius

[1]

1c3 marks

The first 3 elements of Period 3 show a general increase in melting point.

Explain this trend in melting point across these Period 3 elements.

1d3 marks

This question is about hydrogen, the element with the atomic number Z = 1.

Hydrogen can be placed in several different positions in periodic tables. One is immediately above lithium in Group 1 as shown in section 6 of the data booklet. Another is in the centre of the first row.

Evaluate the position of hydrogen when it is placed immediately above lithium and state one reason in favour and two against. 

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2a2 marks

This question is about Period 4 of the Periodic Table. 

State and explain which of K+ and Ca2+ is the smaller ion.

2b1 mark

Write the electron configuration for a Ca+ ion.

2c4 marks

The first ionisation energies of the elements H to K are shown below.

periodicity-diagram-1

State and explain the trend in first ionisation energies shown by the elements with the atomic numbers 2, 10 and 18.

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3a3 marks

Electrons in atoms occupy orbitals.

The figure below shows the first ionisation energies for six consecutive elements labelled AF

periodicity-diagram-2

Complete the graph of the first ionisation energies for the next five elements.

3b2 marks

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

3c4 marks

The sequence of the first three elements in the Periodic Table is hydrogen, helium and then lithium.

Explain why the first ionisation energy of hydrogen is less than that of helium but greater than that of lithium.

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4a3 marks

First ionisation energies decrease down groups in the Periodic Table.

Explain this trend and the effect on the reactivity of groups containing metals.

4b3 marks

The ionisation energy values show a general increase across period 4 from gallium to krypton. 
State and explain how selenium deviates from this trend. 

4c1 mark

Give one other element from period 2 or 3 which also deviates from this general trend, similar to selenium.

4d6 marks

State and explain the trends in electronegativity down group 2 and across period 3.

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