1. Atomic structure
A section of Chemistry, 9701
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The Periodic Table we currently use is derived directly from that proposed in 1869 by Mendeleev who had noticed patterns in the physical and chemical properties of the elements he had studied. The diagram below shows the first ionisation energies of the first 18 elements of the Periodic Table. first ionisation energy / kJ mol–1 0 1 2 3 4 5 6 7 8 9 proton number 10 11 12 13 14 15 16 17 18 H He Ne Na Ar Li Give the equation, including state symbols, for the first ionisation energy of carbon. Explain why sodium has a lower first ionisation energy than magnesium. Explain why magnesium has a higher first ionisation energy than aluminium. Explain why helium, He, and neon, Ne, occupy the two highest positions on the diagram. Explain why the first ionisation energy of argon, Ar, is lower than that of neon, which is lower than that of helium. The first ionisation energies of the elements Na to Ar show a variation. Some physical properties show similar variations. The atomic radius of the elements decreases from Na to Cl. Give a brief explanation of this variation. The cations formed by the elements Na to Al are smaller than the corresponding atoms. Give a brief explanation of this change. The oxides of the elements of the third Period behave differently with NaOHand HCl . In some cases, no reaction occurs. Complete the table below by writing a balanced equation for any reaction that occurs, with heating if necessary. If you think no reaction takes place write ‘no reaction’. You do not need to include state symbols in your answers. MgO+ NaOH MgO+ HCl Al2O3+ NaOH + H2O Al2O3+ HCl SO2+ NaOH SO2+ HCl
9701_w11_qp_23
THEORY
2011
Paper 2, Variant 3
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