Questions
Q1.
(a) Define the term first ionization energy.
(2)
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*(b) Explain why the first ionization energy of the elements down Group 1 decreases even though the atomic number increases.
(2)
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(c) The eleven successive ionization energies for sodium are given below.
(i) Explain why the successive ionization energies increase.
(1)
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*(ii) Explain how these ionization energies give evidence for the electronic structure of sodium. You may use a sketch graph if you wish.
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(d) The first ionization energy of aluminium (element 13) is lower than that of magnesium (element 12).
(i) Give the electronic structures of magnesium and of aluminium in s, p and d notation.
(1)
Magnesium
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Aluminium
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*(ii) Explain the difference in the first ionization energies of the two metals.
(1)
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(Total for question = 9 marks)
Q2.
(a)Define the term first ionization energy.
(3)
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(b)Write an equation, with state symbols, to illustrate the process occurring when the
second ionization energy of sodium is measured.
(2)
(c)The graph below shows the variation in the first ionization energies of some of the
elements in Period 3.
(i)On the graph, use crosses to show the approximate values of the first ionization
energies for the elements Na, P and S.
Join the crosses to complete your graph.
(3)
*(ii)Explain why the first ionization energies generally increase across the period
sodium to argon (Na to Ar).
(3)
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*(iii)Explain why the first ionization energy of aluminium is less than that of
magnesium.
(2)
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(d)Place the following species
in order of increasing first ionization energy, starting with the lowest.
(1)
(Total for question = 14 marks)
Q3.
This question is about the elements arsenic to rubidium which have atomic numbers 33 to 37.
The first ionization energies, Em1, of these elements are given in the table.
(a) Write the equation, with state symbols, which represents the first ionization energy of arsenic.
(2)
(b) Suggest the formulae of the hydrides of arsenic and selenium.
(2)
(c) (i) Complete the electronic configuration for an arsenic and a selenium atom using the electrons-in-boxes notation.
(2)
*(ii) Explain why the first ionization energy of selenium is lower than that of arsenic.
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*(d) Explain why the first ionization energy of krypton is higher than that of selenium.
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*(e) Explain why the first ionization energy of rubidium is lower than that of krypton.
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(f) Which of the elements, arsenic to rubidium, is likely to have atoms with the smallest atomic radius?
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(Total for Question = 13 marks)
Q4.
In which of the following series of elements is there an increase in the melting temperatures from left to right?
A Na Mg Al
B Li Na K
C B C N
D Si P S
(Total for question = 1 mark)
Q5.
Going across the Periodic Table from sodium to aluminium,
Athe melting temperature increases.
Bthe radius of the atom increases.
Cthe radius of the metal ion increases.
Dthe bonding in the element changes from metallic to covalent.
(Total for question = 1 mark)
Mark Scheme
Q1.
Q2.
Q3.
Q4.
Q5.