Q1. The diagram below shows the values of the first ionisation energies of some of the elements in Period 3.
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1 Q1. The diagram below shows the values of the first ionisation energies of some of the elements in Period 3. (a) (b) On the above diagram, use crosses to mark the approximate positions of the values of the first ionisation energies for the elements Na, P and S. Complete the diagram by joining the crosses. Explain the general increase in the values of the first ionisation energies of the elements Na Ar. In terms of the electron sub-levels involved, explain the position of aluminium and the position of sulphur in the diagram. Explanation for aluminium... Explanation for sulphur... (4) (Total 10 marks) Page 1 of 12
2 Q2. Which one of the following lists the first ionisation energies (in kj mol 1 ) of the elements Mg, Al, Si, P and S in this order? A B C D (Total 1 mark) Q3. In which one of the following pairs is the first ionisation energy of element Y greater than that of element X? electronic configuration of element X electronic configuration of element Y A 1s 1 ls 2 B 1s 2 2s 2 ls 2 2s 2 2p 1 C 1s 2 2s 2 2p 3 ls 2 2s 2 2p 4 D 1s 2 2s 2 2p 6 ls 2 2s 2 2p 6 3s 1 (Total 1 mark) Q4. Which one of the following ionisations requires less energy than the first ionisation energy of oxygen? A B C S(g) S + (g) + e O + (g) O 2+ (g) + e N(g) N + (g) + e D F(g) F + (g) + e (Total 1 mark) Q5. Which one of the following explains why boron has a lower first ionisation energy than beryllium? A B C D A boron atom is smaller than a beryllium atom. In beryllium all the electrons are paired in full sub-shells. A beryllium atom has fewer protons than a boron atom. In boron the 2p electron occupies a higher energy level than a 2s electron. (Total 1 mark) Page 2 of 12
3 Q6. There is a general trend in the values of the first ionisation energies of the elements Na to Ar. The first ionisation energies of the elements Al and S deviate from this trend. (a) Write an equation, including state symbols, to represent the process for which the energy change is the first ionisation energy of Na. (b) State and explain the general trend in the values of the first ionisation energies of the elements Na to Ar. Trend... Explanation... State how, and explain why, the values of the first ionisation energies of the elements Al and S deviate from the general trend. How the values deviate from the trend... Explanation for Al... Explanation for S... (5) (Total 10 marks) Q7. This question is about Period 3 of the Periodic Table. (a) Deduce which of Na + and Mg 2+ is the smaller ion. Explain your answer. Smaller ion... Explanation (b) Write an equation to represent the process that occurs when the first ionisation energy for sodium is measured.... Page 3 of 12
4 The first ionisation energies of some Period 3 elements are shown in the following graph. Complete the graph by plotting the approximate first ionisation energy values for magnesium and sulfur. Explain why the first ionisation energy of sulfur is different from that of phosphorus (4) (Total 7 marks) Q8. (a) When aluminium is added to an aqueous solution of copper(ii) chloride, CuCl 2, copper metal and aluminium chloride, AlCl 3, are formed. Write an equation to represent this reaction. Page 4 of 12
5 (b) (i) State the general trend in the first ionisation energy of the Period 3 elements from Na to Ar. (ii) State how, and explain why, the first ionisation energy of aluminium does not follow this general trend. (4) Give the equation, including state symbols, for the process which represents the second ionisation energy of aluminium. (d) State and explain the trend in the melting points of the Period 3 metals Na, Mg and Al. Trend... Explanation... (Total 9 marks) Q9. (a) State the meaning of the term first ionisation energy of an atom. (b) Complete the electron arrangement for the Mg 2+ ion. 1s 2... Identify the block in the Periodic Table to which magnesium belongs. Page 5 of 12
6 (d) Write an equation to illustrate the process occurring when the second ionisation energy of magnesium is measured. (e) The Ne atom and the Mg 2+ ion have the same number of electrons. Give two reasons why the first ionisation energy of neon is lower than the third ionisation energy of magnesium. Reason 1... Reason 2... (f) There is a general trend in the first ionisation energies of the Period 3 elements, Na Ar (i) State and explain this general trend. Trend... Explanation... (ii) Explain why the first ionisation energy of sulphur is lower than would be predicted from the general trend. (5) (Total 12 marks) Q10. The following diagram shows the first ionisation energies of some Period 3 elements. (a) Draw a cross on the diagram to show the first ionisation energy of aluminium. Page 6 of 12
7 (b) Write an equation to show the process that occurs when the first ionisation energy of aluminium is measured. State which of the first, second or third ionisations of aluminium would produce an ion with the electron configuration 1s 2 2s 2 2p 6 3s 1 (d) Explain why the value of the first ionisation energy of sulfur is less than the value of the first ionisation energy of phosphorus. (e) Identify the element in Period 2 that has the highest first ionisation energy and give its electron configuration. Element... Electron configuration... (f) 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. Trend... Explanation... (Total 11 marks) Page 7 of 12
8 Q11. The successive ionisation energies for element X are shown in the following graph. Which element is X? A B C D Nitrogen Phosphorus Aluminium Boron (Total 1 mark) Q12. Which change requires the largest amount of energy? A He + (g) He 2+ (g) + e B Li(g) Li + (g) + e C Mg + (g) Mg 2+ (g) + e D N(g) N + (g) + e (Total 1 mark) Q13. This question is about the first ionisation energies of some elements in the Periodic Table. (a) Write an equation, including state symbols, to show the reaction that occurs when the first ionisation energy of lithium is measured. Page 8 of 12
9 (b) State and explain the general trend in first ionisation energies for the Period 3 elements aluminium to argon. Trend... Explanation... (Extra space)... There is a similar general trend in first ionisation energies for the Period 4 elements gallium to krypton. State how selenium deviates from this general trend and explain your answer. How selenium deviates from this trend... Explanation... (Extra space)... (d) Suggest why the first ionisation energy of krypton is lower than the first ionisation energy of argon. (e) The table below gives the successive ionisation energies of an element. First Second Third Fourth Fifth Ionisation energy / kj mol Deduce the group in the Periodic Table that contains this element. Page 9 of 12
10 (f) Identify the element that has a 5+ ion with an electron configuration of 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 (Total 10 marks) Q14. The element rubidium exists as the isotopes 85 Rb and 87 Rb (a) State the number of protons and the number of neutrons in an atom of the isotope 85 Rb Number of protons... Number of neutrons... (b) (i) Explain how the gaseous atoms of rubidium are ionised in a mass spectrometer (ii) Write an equation, including state symbols, to show the process that occurs when the first ionisation energy of rubidium is measured... The table shows the first ionisation energies of rubidium and some other elements in the same group. Element sodium potassium rubidium First ionisation energy / kj mol State one reason why the first ionisation energy of rubidium is lower than the first ionisation energy of sodium Page 10 of 12
11 (d) (i) State the block of elements in the Periodic Table that contains rubidium... (ii) Deduce the full electron configuration of a rubidium atom... (e) A sample of rubidium contains the isotopes 85 Rb and 87 Rb only. The isotope 85 Rb has an abundance 2.5 times greater than that of 87 Rb Calculate the relative atomic mass of rubidium in this sample. Give your answer to one decimal place (f) By reference to the relevant part of the mass spectrometer, explain how the abundance of an isotope in a sample of rubidium is determined. Name of relevant part... Explanation (g) Predict whether an atom of 88 Sr will have an atomic radius that is larger than, smaller than or the same as the atomic radius of 87 Rb. Explain your answer. Atomic radius of 88 Sr compared to 87 Rb... Explanation (Total 16 marks) Page 11 of 12
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