Atomic Structure (Edexcel GCSE Chemistry)

Exam Questions

4 hours31 questions
1a1 mark

The model of the atom has changed over time due to the discovery of the different subatomic particles.

Which subatomic particles led to J.J. Thomson's plum pudding model?

  A protons
  B neutrons
  C electrons
  D nucleus
1b1 mark

The diagram shows the structure of an atom using the current model of the atom.

screen-shot-2022-10-10-at-10-27-37

How does this diagram show that this is an atom of lithium?

  A it has three electrons
  B it has three protons
  C it has three protons and two neutrons
  D it has two neutrons
1c1 mark

Complete the sentence about atoms.

The size of the nucleus is very ................................ in comparison with the overall size of an atom.

1d1 mark

Which of these statements is correct about atoms?

  A electrons are positively charged
  B the number of protons is equal to the number of neutrons
  C most of the mass of an atom is concentrated in the nucleus
  D electrons are found in the nucleus

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2a3 marks

The diagram shows the particles in an atom of an element.

2c-q1

The box gives the names of some particles. 

2c-q1-1

Use words from the box to label the diagram.

2b1 mark

The table below shows three definitions of mass number.

Put a tick () in the box to show which definition is the correct definition.

 The sum of the number of protons and electrons in the nucleus of an atom  
 The number of protons in the nucleus of an atoms  
 The sum of the number of protons and neutrons in the nucleus of an atom  
2c1 mark

Give the mass number of the atom given in part a).

2d2 marks

Complete the sentence about isotopes.

Isotopes are atoms that have the same number of ........................................ but have a different number of .......................................... .

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3a1 mark

Atoms are made up of subatomic particles.

Which statement about subatomic particles is true?

  A Neutrons and electrons are found in the nucleus. Protons are found in shells
  B Protons and neutrons are found in the nucleus. Electrons are found in shells
  C Protons and electrons are found in the nucleus. Neutrons are found in shells
  D Neutrons are found in the nucleus. Protons and electrons are found in shells
3b1 mark

The table below shows three definitions of atomic number.

Put a tick ()  next to the correct definition. 

The number of electrons in the nucleus of an atom

 

The number of protons in the nucleus of an atom

 

The sum of the number of protons and neutrons in the nucleus of an atom

 

 

3c1 mark

The table below shows four descriptions of the distribution of electrons in an atom.

Put a tick ()  in the box to show which is the correct description. 

Electrons are evenly spread throughout the nucleus

 

Electrons are found only in the outermost shell

 

Electrons are concentrated in the nucleus

 

Electrons orbit the nucleus in specific energy levels or shells

 

 

3d3 marks

Use the words from the box to complete the sentences about the description of subatomic particles. 

shell                         1                              +1                               -1                              0             

 

Protons have a relative charge of _________ and a relative mass of _________. Neutrons have a relative charge of ___________. Electrons are found in shells and have a relative charge of -1.

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4a2 marks

Figure 1 shows some statements about the nucleus of an atom.

Put ticks () in the boxes in Figure 1 to show which statements are true and which statements are false 

 

True

False

The nucleus is very small compared to the overall size of an atom

 

 

The nucleus is larger than the atom

 

 

The nucleus is about the same size as the atom

 

 

The nucleus occupies majority of the mass of an atom

 

 

Figure 1

4b2 marks

The model of an atom has changed over time due to the development in experimental techniques.

Place ticks in boxes by the two statements which best describe what the gold foil experiment revealed about the structure of the atom. 

Figure 2

The nucleus is positively charged

 

Electrons are evenly distributed throughout the atom

 

The nucleus is small and contains most of the atom’s mass

 

Protons and neutrons are evenly distributed

 

4c1 mark

The diagram shows the structure of an atom using the current model of the atom.

edx-1-1e-q4c-dot-and-cross-diagramHow does this diagram show that this is an atom of beryllium?

  A It has 9 electrons
  B It has 9 protons
  C It has 4 protons
  D It has 5 neutrons
4d2 marks

The relative mass of carbon-12 is 12 and the relative mass of carbon-13 is 13.

Complete the following table about the subatomic particles found in two isotopes of carbon.

 

 

Number of protons

Number of neutrons

Number of electrons

 carbon-12

 6

 …………….

 6

 carbon-13

 6

 …………….

 6

 

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5a1 mark

Atoms have no charge overall.

Put a tick () next to the correct statement that describes why atoms have no overall charge. 

Atoms have the same number of protons and neutrons

 

Atoms have the same number of protons and electrons

 

Atoms have the same number of neutrons and electrons

 

5b4 marks

Use the words from the box to complete the sentences about the description of the structure of an atom. 

positively           negatively               neutrons              protons          magnetic       electrostatic 

 

The nucleus is ___________ charged due the presence of __________. There is _____________   attraction between the nucleus and ___________ charged electrons orbiting around the nucleus. This is what keeps an atom together.

5c1 mark

Atoms are made up of subatomic particles.

Which statement about the nucleus is true?

  A The nucleus has negligible mass
  B The nucleus contains protons and electrons
  C The mass of an atom is concentrated in the nucleus because it contains protons and electrons
  D The mass of an atom is concentrated in the nucleus because it contains protons and neutrons
5d1 mark

The diagram shows the structure of a beryllium atom using the current model of the atom.

edx-1-1-easy-paper-1-q5d

What is the nucleon number of this atom of beryllium? 

  A 14
  B 9
  C 8
  D 5

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1
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1 mark

The atomic structure of an unknown element is shown below. 

1-1_q1-edexcel-gcse-mcq

What is the atomic number and mass number for the unknown element?

 
      Atomic Number Mass Number
  A 6 11
  B 5 11
  C 5 6
  D 6 10

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2a3 marks

Atoms contain electrons, neutrons and protons.


i)
Draw one line to link each particle to its correct relative charge.
(2)
fig-q3ai-1cho-1f-paper-1-june-2018
ii)
Which of the following is the relative mass of a proton?
(1)
  A 0
  B 1 over 1837
  C
  D -1
2b1 mark

Argon is in group 0 of the periodic table.

Identify, using the periodic table, which of these elements is in the same period as argon.

  A bromine
  B iron 
  C magnesium 
  D xenon 
2c3 marks

Figure 4 shows the atomic number and mass number of two isotopes of argon.

isotope atomic number mass number
argon-38 18 38
argon-40 18 40

Figure 4

Describe the structure of an atom of argon-38 and of an atom of argon-40.

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31 mark

As the atomic model developed, protons, neutrons and electrons were discovered. 

What was the correct order of discovery?

 
      First Second Third
  A Proton Neutron Electron
  B Proton Electron Neutron
  C Electron Proton Neutron
  D Electron Neutron Proton

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4a3 marks

Chlorine has an atomic number of 17.

Figure 3 shows the arrangement of electrons in an atom of chlorine.

fig-3-q2a-1cho-1f-paper-1-nov-2020

Figure 3

i)
What is the electronic configuration of this atom?
(1)
  A 10.7
  B 17 
  C 2.8.7 
  D 7.8.2 

ii)
Explain, using Figure 3, why chlorine belongs to group 7 of the periodic table.
(2)
4b
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5 marks

The nucleus of an atom is made up of protons and neutrons.
Atoms of chlorine contain 17 protons.


Figure 4 shows some information about a proton, a neutron and an electron.

  relative mass relative charge
proton 1 +1
neutron 1 0
electron very small  -1

Figure 4

i)
Explain, using the information in Figure 3 and Figure 4, why atoms of chlorine have no overall charge.

(2)

ii)
Atoms of chlorine-37 have a mass number of 37.
Calculate the number of neutrons in atoms of chlorine-37.

(1)

number of neutrons = .................................................

iii)
There are two isotopes of chlorine, chlorine-35 and chlorine-37.
Explain the meaning of the term isotopes.

(2)

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51 mark

Chlorine–35 and chlorine–37 are isotopes. 

Which statement describes an isotope?

 
  A Atoms with the same number of protons and different numbers of electrons
  B Atoms with the same number of neutrons and different numbers of electrons
  C Atoms with the same number of protons and different numbers of neutrons
  D Atoms with the same number of neutrons and different numbers of protons

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6a
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3 marks

Higher Tier Only 

Titanium and iron are examples of transition metals.

Figure 6 shows the percentage abundance of each isotope in a sample of titanium.

fig-6-q6a-1cho-1h-paper-1-nov-2020

Figure 6

Calculate the relative atomic mass of titanium in this sample.

relative atomic mass = ......................................

6b4 marks

Iron, when heated in air, reacts with oxygen to form iron oxide.

i)
This reaction is an example of
(1)
  A crystallisation
  B distillation 
  C neutralisation 
  D oxidation 

ii)
The equipment shown in Figure 7 can be used to find the mass of oxygen that combines with iron.
fig-7-q6bii-1cho-1h-paper-1-nov-2020
Figure 7

Describe how the equipment shown in Figure 7 could be used to find the mass of oxygen that combines with 0.500 g of iron wool in a crucible and lid of known mass.

(3)

6c
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4 marks

2.24 g of iron combines with 0.96 g of oxygen to form an oxide of iron.

Determine the formula of this oxide of iron and use it to complete the balanced equation.

(relative atomic masses: Fe = 56.0, O = 16.0)

You must show your working.

balanced equation for the reaction is

................ Fe + ................O2 → ................................................

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1a3 marks

Rutherford’s gold foil experiment led to the development of a different model of the atom.

Describe Rutherford’s model of the atom.

1b2 marks

Atoms contain protons, neutrons and electrons. Their masses and charges are compared to each other and are known as relative atomic masses and relative atomic charges.

Complete the table to show the correct relative atomic masses and charges.  

 

Relative atomic mass

Relative atomic charge

proton

1

……………..

neutron

……………..

0

electron

……………..

……………..

1c4 marks

Explain why atoms have a neutral charge. 

1d3 marks

In terms of subatomic particles, compare the isotopes of carbon shown in the diagram below.

straight C subscript 6 superscript 12          straight C subscript 6 superscript 13          straight C subscript 6 superscript 14

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2a2 marks

The atomic model developed by scientists has changed over time as experimental evidence improved understanding.

Explain how Niels Bohr contributed to the atomic model. 

2b3 marks

Compare the relative atomic masses and relative atomic charges of the subatomic particles within an atom. 

2c2 marks

Higher Tier Only

Figure 1 shows the percentage abundance of two isotopes of chlorine.

 

Percentage abundance (%)

Chlorine-35

75

chlorine-37

25

Figure 1

Calculate the relative atomic mass of chlorine. 

2d3 marks

Explain why carbon-12 and carbon-13 are isotopes of the same element.

Give your answer in terms of subatomic particles. 

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3a5 marks

Compare J.J. Thomson’s plum pudding model with Rutherford’s nuclear model of the atom. 

3b2 marks

Explain what isotopes are. 

3c4 marks

Explain how the gold foil experiment led to a better understanding of the nucleus. 

3d5 marks

Explain how the characteristics of subatomic particles within an atom contribute to the overall charge and mass of an atom. 

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4a3 marks

Explain the impact of the discoveries of the electrons, nucleus and neutron on the evolution of the atomic model. 

4b3 marks

Higher Tier Only

Explain how the relative atomic mass of an element is calculated and use the example in figure 1 to illustrate your explanation. 

 

Percentage abundance (%)

Magnesium-24

78.7

Magnesium-25

10.1

Magnesium-26

11.2

Figure 1

4c4 marks

Explain the relationship between mass number and atomic number in determining the identity and properties of an element. Use carbon-12 and carbon-13 as an example. 

4d3 marks

Explain the structure of an atom according to the current atomic model. 

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5a2 marks

Bohr further developed the atomic model proposed by Rutherford.

Compare the main features of Bohr’s improvement to the atomic model.

5b3 marks

Rutherford’s model of the atom improved the understanding of the atom. Explain how older models were limited in their understanding of the atom. 

5c3 marks

Explain why isotopes of an element will have similar chemical properties.

5d2 marks

Explain why an atom does not collapse inwards. 

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