1.4. Ionisation energy
A subsection of Chemistry, 9701, through 1. Atomic structure
Listing 10 of 131 questions
Explain what is meant by the term ionisation energy. The fi rst seven ionisation energies of an element, A, in kJ mol–1, are 1012 1903 2912 4957 6274 21 269 25 398. State the group of the Periodic Table to which A is most likely to belong. Explain your answer. Complete the electronic confi guration of the element in Period 2 that is in the same group as A. 1s2 Another element, Z, in the same period of the Periodic Table as A, reacts with chlorine to form a compound with empirical formula ZCl 2. The percentage composition by mass of ZCl 2 is Z, 31.13; Cl , 68.87. Defi ne the term relative atomic mass. Calculate the relative atomic mass, Ar, of Z. Give your answer to three signifi cant fi gures. Ar of Z = The chlorides of elements in Period 3 of the Periodic Table show different behaviours on addition to water, depending on their structure and bonding. Write equations to show the behaviour of sodium chloride, NaCl , and silicon chloride, SiCl 4 , when separately added to an excess of water. NaCl SiCl 4 State and explain the differences in behaviour of these two chlorides when added to water, in terms of their structure and the bonding found in the compounds. Sulfur reacts with fl uorine to form SF6. State the shape and bond angle of SF6. shape of SF6 bond angle of SF6
9701_s14_qp_21
THEORY
2014
Paper 2, Variant 1
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Complete the table to show the composition and identity of some atoms and ions. name of element nucleon number atomic number number of protons number of neutrons number of electrons overall charge lithium +1 oxygen Beams of protons, neutrons and electrons behave differently in an electric field due to their differing properties. The diagram shows the path of a beam of electrons in an electric field. Add and label lines to represent the paths of beams of protons and neutrons in the same field. electron beam The fifth to eighth ionisation energies of three elements in the third period of the Periodic Table are given. The symbols used for reference are not the actual symbols of the elements. ionisation energies, kJ mol–1 fifth sixth seventh eighth X 21 269 25 398 29 855 Y 27 107 31 671 Z 11 018 33 606 State and explain the group number of element Y. group number explanation State and explain the general trend in first ionisation energies across the third period. Explain why the first ionisation energy of element Y is less than that of element X. Complete the electronic configuration of element Z. 1s2 A sample of strontium exists as a mixture of four isotopes. Information about three of these isotopes is given in the table. mass number abundance 9.86% 7.00% 82.58% Calculate the abundance of the fourth isotope. abundance = % The relative atomic mass of this sample of strontium is 87.71. Calculate the mass number of the fourth isotope. mass number =
9701_s16_qp_21
THEORY
2016
Paper 2, Variant 1
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Define first ionisation energy. Successive ionisation energies for elementA are shown in Table1.1. Table 1.1 ionisation 1st 2nd 3rd 4th 5th 6th 7th 8th ionisation energy / kJ mol–1 11 000 13 300 71 000 84 100 Use Table1.1 to deduce the group of the Periodic Table that A belongs to. Explain your answer. Group  Across Period3 there is a general trend for first ionisation energies to increase due to the increase in attraction between the nucleus and the outer electron. Explain why the first ionisation energy of sulfur is less than the first ionisation energy of phosphorus. In an Al 2+ ion the nuclear attraction for the outer electron is stronger than in an atom of Na. Compare the electronic structures of Al 2+ and an atom of Na and explain why the third ionisation energy of aluminium is greater than the first ionisation energy of sodium. An isotope of copper has a relative isotopic mass of 65. Complete Table1.2 for an atom of copper-65. Table 1.2 atomic number nucleon number number of neutrons electronic arrangement copper-65  The element copper has a relative atomic mass of 63.5. Calculate how many atoms are present in 1.05 g of copper.  atoms of copper present = Copper has a melting point of 1085 °C and a high electrical conductivity. Explain these properties of copper by referring to its structure and bonding. 
9701_s22_qp_23
THEORY
2022
Paper 2, Variant 3
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Questions Discovered
131