Atomic Structure (Edexcel GCSE Chemistry)

Exam Questions

4 hours31 questions
1a1 mark

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

be-electronic-structure

Particle Y is a proton.

What is particle Z?

  A an electron
  B a molecules
  C a neutron
  D a nucleus

1b1 mark

Which of these has the smallest mass?

  A an electron
  B a neutron
  C a nucleus
  D a proton

1c1 mark

What is the mass number of this atom?

  A 4
  B 5
  C 9
  D 13

1d1 mark

What is the atomic number of this atom?

  A 4
  B 5
  C 9
  D 13

1e2 marks
i)
Identify the element that contains this atom.

(1)

ii)
State what is formed when this atom loses its outer shell electrons.
(1)

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2a1 mark

Two different atoms have a different number of neutrons.

The table below shows three statements about the two atoms.

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

 The atoms are isotopes   
 The atoms must be different elements as they have a different number of neutrons  
 The atoms could be the same element if they also had the same number of protons  
 The atoms could be the same element if they also had the same number of electrons  
2b1 mark

The relative atomic mass of chlorine is 35.5.

Which is the correct reason why it is not a whole number?

  A chlorine contains half a proton
  B relative atomic mass is the average mass of all of the isotopes of that element
  C relative atomic mass is calculated from the mass of the protons divided by the mass of the neutrons
  D a chlorine molecule has a relative atomic mass of 71, so each atom has a relative atomic mass of 35.5
2c3 marks

Use words from the box to complete the sentences about chlorine.

protons atomic mass neutrons relative atomic

35-chlorine has the ................................ number of 35 and the ................................ number of 17. One atom of chlorine has 17 ................................ and electrons.

2d2 marks

The radius of a nucleus is approximately 10 000 times smaller than the radius of an atom.

Place ticks () in boxes by the two statements about the atom that are correct.

 the mass of an atom is concentrated within the nucleus  
 most of the space of an atom is filled with electrons  
 most of an atom is empty space  
 the mass of an atom is evenly distributed throughout the atoms  
 most of the charge of an atom is concentrated in the nucleus  

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3a1 mark

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

neutrons                     protons                      compound                    element                        metal

 

Isotopes are atoms of the same __________ that contain the same number of __________ and electrons but a different number of ____________.

3b2 marks

Figure 1 shows some statements about the isotopes of carbon-12 (12C) and carbon-13 (13C). 

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

 

True

False

Both carbon-12 and carbon-13 have the same number of protons

 

 

Carbon-12 has one less electron than carbon-13

 

 

Carbon-12 has one less neutron than carbon-13

 

 

Both carbon-12 and carbon-13 have the same number of neutrons

 

 

Figure 1

3c1 mark

Isotopes display the same chemical properties.

Put a tick () next to the correct statement that describes why isotopes display the same chemical properties.

Isotopes have the same number of neutrons in the nucleus

 

Isotopes have the same number of protons in the nucleus

 

Isotopes have the same number of electrons in their outer shells.

 

3d1 mark

J.J. Thomson discovered the electron and proposed a model of the atom known as the “plum pudding” model.

Which statement about the plum pudding model is true?

  A Negative electrons were located in the middle of a spherical cloud of positive charge
  B Negative electrons were spread around the edge of a spherical cloud of positive charge
  C Negative electrons were spread throughout the spherical cloud of positive charge
  D Positive charge was located in the middle of a sphere of negative charge

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4a3 marks

Use the words from the box to complete the sentences about Rutherford’s model of the atom. 

empty                     protons                  electrons                  full              concentrated                 little

 

Rutherford’s model of the atom was made up of mainly _________ space. The nucleus at the centre of the atom had ____________ mass, with ________ orbiting around the nucleus.

4b2 marks

The diagram shows the chemical symbol for lithium.

begin mathsize 36px style Li subscript 3 superscript 7 end style

Put two ticks () next to the correct statements that describe the lithium atom. 

The mass number is 3

 

The mass number is 7

 

The atomic number is 3

 

The atomic number is 7

 

4c1 mark

Hydrogen has three isotopes as shown in the diagram below.

straight H subscript 1 superscript 1 straight H subscript 1 superscript 2 straight H subscript 1 superscript 3

 Put a tick ()  in the box to show which statement best describes these isotopes. 

All the isotopes have 1 proton

 

All the isotopes have 1 neutrons

 

One of these isotopes has 3 neutrons

 

One of these isotopes has 2 electrons

 

4d1 mark

Which statement about finding the number of neutrons in an atom is true? 

  A Number of neutrons = mass number + atomic number
  B Number of neutrons = mass number - atomic number
  C Number of neutrons = mass number x atomic number
  D Number of neutrons = mass number ÷ atomic number

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5a1 mark

Atomic models developed as scientists gained more experimental evidence.

Put a tick () next to the correct statement that describes one advancement in J.J. Thomson’s plum pudding model compared to Dalton’s model. 

 

Plum pudding model showed electrons orbiting in shells

 

Plum pudding model depicted electrons spread throughout a sphere of positive charge

 

Plum pudding model showed the atom with a nucleus in the center

 

5b1 mark

Rutherford’s gold foil experiment involved shooting a beam of positively charged particles at  gold foil.

Some positively charged particles deflected directly back.

What conclusion could be made from this observation? 

  A The atom is mainly empty space
  B There are negatively charged electrons orbiting the nucleus
  C There is a concentrated mass of positive charge at the centre of the atom
  D There is an abundance of negative charge at the centre of the atom
5c1 mark

There are two atoms with the same number of protons but a different number of neutrons.

Which statement about these atoms is true? 

  A The mass number of both atoms is the same
  B The atomic number of both atoms is different
  C The atomic and mass number of both atoms is the same
  D The atomic number is the same but the mass number is not the same
5d1 mark

The table below shows four statements about electrons.

Put a tick ()  next to the correct statement. 

Electrons have a mass of 1 and charge of -1

 

Electrons have a mass of 0 and charge of +1

 

Electrons have a mass of 0 and charge of -1

 

Electrons have a mass of 1 and charge of 0

 

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11 mark

An atom has no overall charge because there are the same number of:

 
  A Protons and neutrons
  B Protons and electrons
  C Neutrons and electrons
  D Protons, neutrons and electrons

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2a1 mark

This question is about some of the elements in groups 1 and 2 of the periodic table.

The atomic number of lithium is 3.
The mass number of a lithium atom is 7.

Which row of the table shows the number of protons, neutrons and electrons in an atom of lithium-7?

      Number of protons Number of neutrons Number of electons
  A 3 3 4
  B 3 4 3
  C 4 3 7
  D 7 4 3

2b1 mark

Lithium, sodium and potassium are in group 1 of the periodic table.

State, in terms of the electrons in their atoms, what the atoms of lithium, sodium and potassium have in common.

2c
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2 marks

Magnesium has atomic number 12.

Magnesium exists as magnesium-24, magnesium-25 and magnesium-26 atoms.

Explain, in terms of protons and neutrons, why these atoms are isotopes of magnesium.

2d2 marks

Magnesium and calcium are in group 2 of the periodic table. They are less reactive than the metals in group 1.

Calcium reacts with water to form calcium hydroxide, Ca(OH)2, and hydrogen, H2.

Ca (s) + 2H2O (l) → Ca(OH)2 (s) + H2 (g)

Describe what would be seen when a piece of calcium is dropped into a container of water.

2e2 marks

Magnesium reacts very slowly with cold water but it reacts faster with steam, H2O, to form magnesium oxide, MgO, and hydrogen.

Write the balanced equation for the reaction between magnesium and steam.

2f2 marks

The electronic configurations of magnesium and calcium are

magnesium 2.8.2
calcium 2.8.8.2

When magnesium and calcium react with water they form positive ions.

Suggest an explanation, in terms of their electronic configurations, why calcium is more reactive than magnesium.

2g
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3 marks

A sample of calcium bromide contains 0.2 g calcium and 0.8 g bromine by mass.

Calculate the empirical formula of calcium bromide.
(relative atomic masses: Ca = 40, Br = 80)

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31 mark

Which statement best describes the structure of an atom? 

  A A nucleus containing protons and neutrons, surrounded by electrons
  B A nucleus containing protons and electrons, surrounded by neutrons
  C A nucleus containing electrons and neutrons, surrounded by protons 
  D A nucleus containing protons, surrounded by neutrons and electrons

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4a2 marks

An atom of potassium has atomic number 19 and mass number 39.

i)
Give the electronic configuration of this potassium atom.
(1)
ii)
This potassium atom forms the ion K+.
Which row shows the number of protons and the number of neutrons in this potassium ion, K+?
(1)
      number of protons number of neutrons
  A 19 19
  B 19  20
  C 20  19
  D 20 20
4b2 marks

Potassium and caesium are in the same group of the periodic table.

Explain, in terms of electrons, why potassium and caesium are in the same group.

4c2 marks

Fluorine boils at –188 °C.
There are forces between fluorine molecules.

Explain, in terms of these forces, why the boiling point of fluorine is low.

4d3 marks

Potassium reacts with fluorine to form potassium fluoride.
Potassium fluoride is a solid.

Complete the balanced equation for this reaction and add the state symbols.

.................K (...........) + F2 (g) → .................KF (...........)

4e1 mark

What are the elements in group 1 of the periodic table called?

  A alkali metals
  B fullerenes 
  C halogens 
  D noble gases
4f2 marks

Figure 14 shows the melting points and boiling points of elements in group 7 of the periodic table.

fig-14-q8f-1cho-2f-paper-1-nov-2020
Figure 14

i)
Give, using Figure 14, the boiling point of bromine.
(1)
boiling point of bromine = ..................................... °C

ii)
State which two elements from Figure 14 are solids at room temperature.
(1)

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51 mark

Higher Only 

Element Cu has two isotopes. Their mass numbers are 63 and 65. 

  • Cu- 63 has a percentage abundance of 69.2%
  • Cu- 65 has a percentage abundance of 30.8% 

Estimate the relative atomic mass of element Cu. 

  A Below 63
  B Between 63.5 and 64
  C Between 64 and 64.5
  D Above 64.5

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1a3 marks

Explain how Chadwick’s work on the atomic model led to a better understanding of the existence of isotopes. 

1b3 marks

The diagram below shows two atoms.

edx-1-1-hard-paper-2-q1b

Compare the structures of both atoms. 

1c2 marks

Explain why the atoms in part b) react in the same way. 

1d2 marks

Compare the mass number and atomic number of the atoms mentioned in question 1b. 

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2a4 marks

The Bohr model of the atom introduced significant advancements in atomic theory.

Discuss the limitations of the earlier atomic models in explaining the behaviour of electrons within an atom. 

2b4 marks

The diagram below shows the chemical symbols of two isotopes of uranium.

begin mathsize 36px style U subscript 92 superscript 235 end style                     begin mathsize 36px style U subscript 92 superscript 238 end style

Explain why uranium-235 and uranium-238 are categorised as isotopes of the same element. 

2c4 marks

Explain the difference in charge between a magnesium atom and magnesium ion. 

2d2 marks

Higher Tier Only:

The table in figure 1 shows three isotopes of magnesium with varying abundances.

Explain why the relative atomic mass of magnesium is 24.3 and not a number closer to 24 or 26.

 

Percentage abundance (%)

Magnesium-24

78.7

Magnesium-25

10.1

Magnesium-26

11.2

Figure 1

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3a3 marks

Describe the limitations of Dalton’s atomic model and Thomson’s plum pudding model in describing the structure of the atom.

3b3 marks

Explain why the nucleus is described as a concentrated mass at the centre of an atom.

3c2 marks

Explain the structure of an atom according to the plum pudding model. 

3d3 marks

Explain what the discovery by J.J. Thomson was and what it proved. 

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4a6 marks

Explain the difference in charge of the nucleus of an atom and an atom as a whole. 

4b3 marks

Explain the structure of an atom according to the nuclear model. 

4c3 marks

Explain the contributions of different scientists to the understanding of the atomic structure.

4d3 marks

Explain the presence of forces within an atom and its impact. 

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5a3 marks

Higher Tier Only

Explain why the masses and charges of subatomic particles are described as ‘relative atomic masses’ and ‘relative atomic charges’.

5b4 marks

Compare the relative sizes of the following things: atom, nucleus and electrons. 

5c3 marks

The diagram shows the chemical symbol of magnesium and lithium.

Mg subscript 12 superscript 24                             begin mathsize 36px style Li subscript 3 superscript 7 end style

Explain the difference in nucleon number of an atom of magnesium and the nucleon number of an atom of lithium. 

5d2 marks

Higher Tier Only

Explain why percentage abundance of isotopes is taken into consideration when calculating the relative atomic mass. 

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