Pearson Edexcel International GCSE (9–1) · CHEMISTRY · Chapter
The Periodic Table
103 practice questions
Topics covered
- The arrangement of the electrons in an atom19 practice questions
- Drawing diagrams of electronic configurations19 practice questions
- Electronic configurations and the periodic table19 practice questions
- Metals and non-metals in the periodic table18 practice questions
- Differences between the properties of metals and non-metals19 practice questions
Practice questions
31–40 of 103
Question 31
3 marks · Normal
Answer and see the solution →Explain why the electronic configuration of neon is considered stable. Refer to its atomic number and how electrons are arranged in its shells.
Question 32
4 marks · Normal
Answer and see the solution →The table below shows the electronic configurations of four elements, labelled A, B, C and D.
Element Number of electrons in each shell A 2, 8, 1 B 2, 6 C 2, 8 D 2, 5 (a)[1 mark]Which element has the largest number of shells?
(b)[1 mark]Which element has a full outer shell?
(c)[1 mark]Which element is likely to be chemically unreactive? Give a reason for your answer.
(d)[1 mark]How many electrons are in the outer shell of element D?
Question 33
1 mark · Normal
Answer and check →Which statement correctly describes the rule for filling electron shells up to the third shell?
- A.First shell can hold up to 2 electrons, second and third shells can each hold up to 8 electrons.
- B.Each shell can hold up to 8 electrons.
- C.First and second shells can each hold up to 2 electrons, third shell holds up to 8.
- D.First shell can hold up to 8 electrons, second and third up to 2.
Question 34
2 marks · Normal
Answer and see the solution →State the electronic configuration (number of electrons in each shell) for the element nitrogen (atomic number 7).
Question 35
4 marks · Normal
Answer and see the solution →Below is the electronic configuration diagram for an atom of carbon.
Diagram: Carbon atom – two shells; 2 electrons in first shell, 4 electrons in second shell (dots shown). (a)[1 mark]How many electrons are there in total in this atom?
(b)[1 mark]How many shells are in this atom?
(c)[1 mark]How many electrons are in the outer shell?
(d)[1 mark]Write the electronic configuration (number of electrons in each shell) for this atom.
Question 36
2 marks · Hard
Answer and see the solution →The diagram below represents the electronic configuration of an atom using shells and electrons:
Electronic configuration of an atom X Shell 1 contains 2 electrons, shown as crosses or dots. Shell 2 contains 4 electrons, shown as crosses or dots.
Interpret this diagram to answer the following:
(a)[1 mark]How many electrons are present in atom X?
(b)[1 mark]State the electronic configuration of atom X using numbers to show the electrons in each shell.
Question 37
5 marks · Hard
Answer and see the solution →Answer the following about the rules for filling electron shells up to the third shell.
(a)State the maximum number of electrons that can occupy:
(i)[1 mark]the first shell
(ii)[1 mark]the second shell
(iii)[1 mark]the third shell, up to atomic number 10
(b)[1 mark]Describe the order in which electrons fill these shells in an atom.
(c)[1 mark]Explain why the first shell is always filled before electrons occupy the second shell.
Question 38
2 marks · Hard
Answer and see the solution →Draw a diagram to show the electronic configuration of an atom of fluorine (atomic number 9). Represent the shells as circles and the electrons as dots or crosses.
Question 39
1 mark · Easy
Answer and see the solution →State which period in the Periodic Table an element with electronic configuration 2,8,6 is found in.
Question 40
3 marks · Easy
Answer and see the solution →Magnesium has the atomic number 12.
(a)[1 mark]Write the electronic configuration of magnesium.
(b)[1 mark]State the number of electrons in its outer shell.
(c)[1 mark]Identify the group in the Periodic Table where magnesium is found.