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WorksheetsL6th Periodicity end of topic test [Total 39 marks]
Total questions: 20
Worksheet time: 1hrs 2mins
The elements phosphorus, sulfur, chlorine and argon are in the p block of the Periodic Table.
(a) State why these elements are classified as p block elements. [1 mark]
(b) State the trend in atomic radius from phosphorus to chlorine and explain the trend. [2 marks]
In terms of atomic structure, explain why the van der Waals’ forces in liquid argon are very weak. [2 marks]
Q2.The elements in Period 2 show periodic trends.
(a) State the general trend in first ionisation energies from carbon to neon. Deduce the element that deviates from this trend and explain why this element deviates from the trend.
[4 marks]
(b) Select the correct equation, including state symbols, for the reaction that occurs when the first ionisation energy of carbon is measured. [1 mark]
C(g) + e− → C+(g)
C(g) + e− → C-(g)
C(g) → C+(g) + e−
(c) Explain why the second ionisation energy of carbon is higher than the first ionisation energy of carbon. [1 mark]
(d) Deduce the element in Period 2, from lithium to neon, that has the highest second ionisation energy. [1 mark]
Lithium
Beryllium
Boron
Fluorine
Neon
Q3.There are many uses for compounds of barium.
(a) (i) Select the correct equation for the reaction of barium with water. [1 mark]
Ba + H2O → BaO + H2
Ba + 2H2O → Ba(OH)2 + H2
2Ba + 2H2O → 2BaOH + H2
2Ba + 2H2O → 2BaH2 + O2
(ii) State the trend in reactivity with water of the Group 2 metals from Mg to Ba. [1 mark]
Increases
Decreases
Stays the same
(b) Give the formula of the least soluble hydroxide of the Group 2 metals from Mg to Ba. Do not worry about formatting the formula. [1 mark]
(c) State how barium sulfate is used in medicine.
Explain why this use is possible, given that solutions containing barium ions are poisonous. [2 marks]
Q4. Define the term electronegativity and explain why the electronegativity values of the Group II elements Be–Ba decrease down the group. [4 marks]
(a) State the type of structure shown by a crystal of silicon.
Explain why the melting point of silicon is very high. [3 marks]
(b) State the type of structure shown by crystals of sulfur and phosphorus.
Explain why the melting point of sulfur is higher than the melting point of phosphorus. [3 marks]
(c) Explain why aluminium is malleable.
[2 marks]
(d) Explain why the melting point of aluminium is higher than the melting point of sodium. [3 marks]
The diagram shows the first ionisation energies of some Period 3 elements.
(a) Where would the cross for the first ionisation energy of Al be in comparison to the other crosses on the graph? [1 mark]
Lower than the crosses for Mg and Si.
Higher than the crosses for Mg and Si.
Higher than the cross for Mg but lower than the cross for Si.
(b) State which of the first, second or third ionisations of aluminium would produce an ion with the
electron configuration 1s2 2s2 2p6 3s1. [1 mark]
First
Second
Third
(c) Explain why the value of the first ionisation energy of sulfur is less than the value of the first ionisation energy of phosphorus. [2 marks]
(d) State the trend in first ionisation energies in Group 2 from beryllium to barium.
Explain your answer in terms of a suitable model of atomic structure. [3 marks]
