The Periodic Table (AQA GCSE Chemistry)

Exam Questions

2 hours27 questions
1a1 mark

Five elements, A, B, C, D and E are shown in the periodic table in Figure 1.

The letters are not the symbols of the elements.

Figure 1

periodic-table

Use the letters A, B, C, D or E to answer the questions about the periodic table. You may use a letter more than once.

Which element has the relative atomic mass of 9?

1b1 mark

Which element has a complete outer shell of electrons?

1c1 mark

Which element is a transition element?

1d1 mark

Which element has one electron in its outer shell?

1e1 mark

Which element forms 1- ions?

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2a4 marks

Table 1 shows part of Mendeleev's periodic table of 1871.

Table 1

1 2 3 4 5 6 7
H            
Li Be B C N O F
Na Mg Al Si P S Cl



Use this and the periodic table to help you answer these questions.

Draw a ring around the correct words to complete the sentences.

  In the periodic table the rows are known as

periods.

groups.

columns.

  Mendeleev arranged most elements in order of

atomic weight.

atomic number.

number of electrons.

  He left gaps for elements which were

gases.

undiscovered.

inert.

  At regular intervals the elements have

similar properties.

the same properties.

different properties.

2b1 mark

Suggest why hydrogen should not have been put in a column with lithium and sodium.

2c1 mark

What are the columns known as in the periodic table?

2d1 mark

In the modern periodic table, how are elements arranged?

Tick (✓) one box.

In order of relative atomic mass  
In order of atomic number  
In order of reactivity  
In order of mass number  

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3a2 marks

Potassium is a Group 1 metal that reacts violently with water.

A teacher demonstrates this reaction using the apparatus shown in Figure 1. 

Figure 1

potassium-and-water

Complete the word equation of the reaction between potassium and water.

Choose the correct words from the box below.

        potassium oxide              potassium hydride                         water
oxygen            hydrogen  potassium hydroxide



potassium  +  water  →  ____________________  +  ____________________

3b2 marks

What observations would be made when potassium reacts with water.

Tick (✓) two boxes.

Potassium would sink to the bottom of the trough  
Potassium would disappear  
Bubbles would be produced  
Potassium would set fire with an orange flame  
The water would change colour  
3c1 mark

When the reaction had completed, the teacher added universal indicator solution to the trough.

The solution turned purple.

What is the pH of the solution?

Tick (✓) one box.

1  
3  
7  
13  
3d1 mark

Potassium is higher up in Group 1 of the periodic table than caesium.

Suggest how the reaction between caesium and water would be different to the reaction between potassium and water.

3e1 mark

Potassium will also undergo a reaction when heated with chlorine to form potassium chloride.

Complete the balanced symbol equation for this reaction.

___ K   +   Cl2  →  ___ KCl

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4a1 mark

Helium, neon and argon are all elements found in Group 0.

What are the elements in Group 0 also known as?

4b1 mark

Why are Group 0 elements classed as non-metals?

Tick (✓) one box.

They react to form positive ions  
They do not form positive ions  
They do not form ions  
They react to form negative ions  

4c2 marks

Tungsten filament electric light bulbs are filled with argon as shown in Figure 1.

Figure 1

tungsten-argon-lightbulb

Explain why argon does not react with tungsten.

4d2 marks

Which of the following statements are correct about the Group 0 elements?

Tick (✓) two boxes.

They all have eight electrons in their outer shell  
Their boiling points increase going down the group  
They form molecules easily  
They are all liquids at room temperature  
Their properties can be predicted from trends down the group  

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5a1 mark

This question is about Group 7 elements.

Table 1 shows the melting point and boiling point of some Group 7 elements.

Table 1

Element Melting point in oC Boiling point in oC
Chlorine -101 -25
Bromine -7 59
Iodine 114 184

What is the state of bromine at 50 oC?

5b1 mark

Which of the elements from Table 1 would be a gas at room temperature?

5c2 marks

Which two of the following statements is correct about the elements in Group 7?

Tick (✓) two boxes.

They are metals that exist as molecules of two atoms  
They have seven electrons in their outer shell  
They are non-metals that exist as molecules of two atoms  
They react with metals to form molecular compounds  
The reactivity increases down the group  

5d2 marks

Fluorine has an atomic number of 9.

Draw a diagram to show the electron arrangement of an atom of fluorine.

5e2 marks

Fluorine undergoes similar reactions to chlorine and bromine.

Explain why.

5f2 marks

Bromine can react with potassium iodide.

Complete the word equation for the reaction.

Choose the correct words from the box below.

potassium bromine potassium bromide potassium iodine
             iodine                     iodide



bromine  +  potassium iodide → ____________________  +  ____________________  

5g1 mark

Why does bromine not react with potassium chloride solution?

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61 mark

What is the modern name for atomic weight?

  • Mass number

  • Relative formula mass

  • Atomic number 

  • Relative atomic mass 

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1a3 marks

John Newlands first began developing the idea of a periodic table of elements around 140 years ago.

He jotted down the elements known at that time in order, starting with the lightest atoms.

From here he arranged them into seven groups as shown in Figure 1 below. 

Figure 1

aqa-gcse-sq-m-1-3-q1a

There are differences between the groups in Newlands’ periodic table and those in the modern day table. 

Write down three of these differences, basing your comparisons up to the element calcium.

1b1 mark

Suggest a reason why this part of Newlands' table differed from the modern version.

1c1 mark

Some time later Dimitri Mendeleev developed the periodic table of the elements. 

In his version he arranged the elements according to their relative atomic masses and properties.

Where Mendeleev put tellurium (Te) and iodine (I) in his table is indicated in Figure 2 below. 

He placed them in these positions because of their properties.

Figure 2

1-2-q1c-ver1

Identify the error in this arrangement of tellurium and iodine.

1d1 mark

In the modern periodic table this arrangement is not a problem.

Explain why not.

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2a3 marks

The electronic structures of atoms from three different elements are shown.

    2,8,1                         2,8,8                        2,8,8,1
element W               element Y                  element Z

Name the elements W, Y and Z.

2b2 marks

Explain why element Z is more reactive than element W.

2c2 marks

Explain why element Y is unreactive.

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31 mark

Iodine is found above astatine in Group 7 of the periodic table.

What is its formula and state at room temperature?

  Formula State at room temperature 
 A I liquid
 B I solid
 C I2 liquid
 D I2 solid

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    41 mark

    The diagram shows the electron structures of some elements. 5-RNJfAE_1-1

    Which two elements have similar chemical properties?

    • A and B

    • A and C

    • B and C 

    • B and D 

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    5a1 mark

    Sodium and potassium are both alkali metals.

    Explain in terms of their electronic structures, why both elements are placed in Group 1 in the periodic table.

    5b1 mark

    Use the Data Sheet to answer this question.

    The electronic structures of some atoms and ions are shown in Figure 1 below.

    Figure 1

    electronic-structures-of-atoms-and-ions

    Which structure represents an atom of sodium?

    5c1 mark

    Which structure represents a potassium ion?

    5d2 marks

    All of the alkali metals react with cold water.

    Lithium reacts as follows:

    lithium + water → lithium hydroxide + hydrogen

    Complete and balance the symbol equation for this reaction.

    __________  +  __________  →  2LiOH  +  __________

    5e1 mark

    Potassium and sodium also react with water but the observed reactions are not the same. 

    How does the reactivity of potassium differ from sodium?

    5f1 mark

    State one difference in their electronic structures which explains the difference in reactivity between potassium and sodium.

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    6a2 marks

    The Group 1 metals have similar chemical properties.

    Describe one chemical reaction that could be used to show that lithium, sodium and potassium have similar chemical properties. 

    State the reactant you would use and the substances produced.

    6b2 marks

    All of the halogens react with hydrogen but there are differences in their reactivity.

    Fluorine reacts explosively at very low temperatures and in the absence of light.

    Chlorine reacts explosively at room temperatures but requires light.

    Bromine requires light and a temperature of around 200 oC to react.

    Given the above information, suggest and explain the conditions required for hydrogen and iodine to react.

    6c3 marks

    Explain the trend in reactivity in the Group 7 elements with reference to their electronic structures.

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    7a1 mark

    Table 1 below gives the melting points of some of the elements of Group 7.

    Table 1

    Element Atomic number Melting point in oC
    Fluorine 9 -220
    Chlorine 17 -101
    Bromine 35 -7
    Iodine 53 114
    Astatine 85 ?

    Using the information in Table 1, predict a value for the melting point of astatine.

    7b1 mark

    State which halogens are solids at 40 °C.

    7c1 mark

    Draw a diagram to show how the electrons are arranged in an atom of fluorine.

    7d1 mark

    As for the alkali metals, the Group 7 elements all have similar chemical properties.

    Using their electron arrangements, give a reason for their similarity.

    7e2 marks

    Xenon is an unreactive element. 

    Explain why xenon is so unreactive.

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    81 mark

    When sodium reacts with water an alkaline solution is formed.

    Which statement explains why this happens?

    • It contains an ionic compound

    • It contains hydroxide ions

    • It contains water

    • Hydrogen gas is made 

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    9a1 mark

    Fluorine reacts with most elements but does not react with argon.

    The atomic number of fluorine is 9, chlorine is 17 and argon is 18.

    In which group of the periodic table are fluorine and chlorine placed?

    9b2 marks

    Draw a diagram to show the electron arrangement of an atom of chlorine.

    9c3 marks

    Explain why fluorine is more reactive than chlorine.

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    10a1 mark

    An electric light bulb is shown in Figure 1 below. 

    The tungsten filament conducts electricity when the light is switched on and heats up to a high temperature, giving off light.

    Figure 1

    tungsten-argon-lightbulb

    The bulb has a closed atmosphere containing argon only. 

    What reaction would occur if air was used instead of argon?

    10b3 marks

    With reference to the electronic structure of the argon atom, explain why it is used in light bulbs.

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    1a2 marks

    Mendeleev classified the known elements into a table by ordering them by their atomic weights.

    His periodic table was published in 1869 and it showed the elements that had been discovered at that time.

    Part of his periodic table is shown in Table 1.

    Use the information in Table 1 and your periodic table to answer the questions.

    Table 1

    Group 1 Group 2 Group 3 Group 4 Group 5 Group 6 Group 7
    H            
    Li Be B C N O F
    Na Mg Al Si P S Cl

    Hydrogen is an element from Mendeleev's table that is not in the same group of the modern periodic table.

    Give two reasons why it should not be in Group 1.

    1b2 marks

    Give two reasons why hydrogen could be placed in Group 1.

    1c2 marks

    Give two reasons why hydrogen could be placed in Group 7.

    1d4 marks

    The modern periodic table arranges the elements in order of atomic number.

    What scientific discoveries allowed elements to be placed in their correct period and group?

    How did this knowledge allow elements to be correctly placed?

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    2a2 marks

    The halogens are found in Group 7 of the periodic table.

    Table 1 shows the melting point and boiling point of some of the halogens.

    Table 1

    Element Melting Point in oC Boiling Point in oC
    Fluorine -220 -188
    Chlorine -101 -25
    Bromine -7 59
    Iodine 114 184

    What is the state of chlorine at -100 oC and at 0 oC? 

    State at -100 oC: ____________________

    State at 0 oC: ____________________

    2b3 marks

    Explain why the boiling point of the Group 7 elements increases as you go down the group as shown in Table 1.

    2c2 marks

    The halogens all react with hydrogen to form the corresponding hydrogen halide.

    Explain why the halogens all react in a similar way.

    2d3 marks

    Predict and explain the difference in the rate of the reaction between hydrogen with chlorine and between hydrogen and iodine.

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    3a2 marks

    This question is about Group 1 metals.

    The reaction between three Group 1 metals, lithium, sodium and potassium, with water was demonstrated by a teacher.

    The teacher added a few drops of universal indicator to water in a trough. They then dropped a small piece of the Group 1 metal into the water.

    Write the balanced symbol equation for the reaction between lithium and water.

    3b4 marks

    In terms of electronic structure, state and explain the difference in reactivity between potassium and water compared with lithium and water.

    3c3 marks

    State what colour the universal indicator turned when potassium was added to water and explain why it changes to this colour.

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    4a4 marks

    Element Z has the following properties:

    • It is a solid at room temperature
    • Does not conduct heat or electricity
    • Forms simple molecules with non-metals
    • Forms giant ionic lattices with metals in which it has a 1- ion

    Select the formula of the compound formed when element Z reacts with calcium from the list below.

    CaO CaCl2 CaI2 CaS CaBr



    Explain your answer using the information provided.

    4b5 marks

    Calcium is a Group 2 metal. Group 2 metals show similar trends in reactivity to Group 1 metals as you go down the group. 

    Magnesium is another Group 2 metal.

    Explain why, in terms of atomic structure, magnesium reacts in a similar way to calcium with element Z but it is less reactive than calcium.

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    5a2 marks

    Table 1 shows the electronic structures of five elements.

    The letters are not the chemical symbols of the element.

    Table 1

    Element Electronic structure
    J 2,8,8
    K 2,8,1
    L 2,8,8,1
    M 2,7
    N 2,8,4

    Give the letters of two elements that belong to the same group in the periodic table.

    State the group that they belong to.

    Use Table 1 and the periodic table.

    5b2 marks

    Give a letter of the element that can form a giant covalent structure when reacted with oxygen.

    State the name of the giant covalent structure formed.

    Use Table 1 and the periodic table.

    5c3 marks

    Give the letter of the element that is monatomic.

    Explain your answer.

    5d1 mark

    Give the letters of two elements that are gases at room temperature.

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    61 mark

    A student carried out a displacement reaction using an unknown halogen and a salt containing a halide ion.

    As the reaction progressed they observed the formation of a dark brown solution.

    Which halogen and salt did the students react together?  

    • Potassium iodide + bromine

    • Potassium bromide + chlorine

    • Potassium chloride + bromine

    • Potassium chloride + iodine

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