) Define the term first ionization energy. | Exercises Chemistry

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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(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. (2)

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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)

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Questions

Q1.

(a) Define the term first ionization energy. (2) ............................................................................................................................................. ............................................................................................................................................. ............................................................................................................................................. *(b) Explain why the first ionization energy of the elements down Group 1 decreases even though the atomic number increases. (2) ............................................................................................................................................. ............................................................................................................................................. ............................................................................................................................................. ............................................................................................................................................. ............................................................................................................................................. ............................................................................................................................................. (c) The eleven successive ionization energies for sodium are given below.

(i) Explain why the successive ionization energies increase. (1) ............................................................................................................................................. ............................................................................................................................................. ............................................................................................................................................. *(ii) Explain how these ionization energies give evidence for the electronic structure of sodium. You may use a sketch graph if you wish. (2)

(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 ............................................................................................................................................. Aluminium ............................................................................................................................................. *(ii) Explain the difference in the first ionization energies of the two metals. (1) ............................................................................................................................................. ............................................................................................................................................. ............................................................................................................................................. ............................................................................................................................................. (Total for question = 9 marks)

(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) ............................................................................................................................................. ............................................................................................................................................. ............................................................................................................................................. .............................................................................................................................................

*(iii) Explain why the first ionization energy of aluminium is less than that of magnesium. (2) ............................................................................................................................................. ............................................................................................................................................. ............................................................................................................................................. ............................................................................................................................................. ............................................................................................................................................. ............................................................................................................................................. (d) Place the following species in order of increasing first ionization energy, starting with the lowest. (1)

(Total for question = 14 marks)

*(e) Explain why the first ionization energy of rubidium is lower than that of krypton. (2) ............................................................................................................................................. ............................................................................................................................................. ............................................................................................................................................. ............................................................................................................................................. ............................................................................................................................................. .............................................................................................................................................

(f) Which of the elements, arsenic to rubidium, is likely to have atoms with the smallest atomic radius? (1) .............................................................................................................................................

(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, A the melting temperature increases. B the radius of the atom increases. C the radius of the metal ion increases. D the bonding in the element changes from metallic to covalent. (Total for question = 1 mark)

) Define the term first ionization energy., Exercises of Chemistry

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