4. Answer ALL parts (a) to (h). (a) Consider the values of the lattice enthalpy for the following ionic solids: Empirica

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4 Answer All Parts A To H A Consider The Values Of The Lattice Enthalpy For The Following Ionic Solids Empirica 1 (151.76 KiB) Viewed 46 times

4. Answer ALL parts (a) to (h). (a) Consider the values of the lattice enthalpy for the following ionic solids: Empirical formula AHLatt/kJ mol-¹ Zinc sulfide ZnS 3565 Caesium chloride CsCl 641 Describe the nature of the bonding present in ZnS and explain, with reasoning, why the magnitude of the lattice enthalpy is greater than for CsCl. [4%] (b) For which of the two solids above will there be a greater covalent character to the bonding? Explain the reason for your choice. [3%] (c) Magnesium, silicon, manganese, platinum and tin - which of these elements are in the d-block of the periodic table? [2%] (d) Copper(II) chloride dissolves in water to form a blue aqueous solution. Given the weakly coordinating nature of chloride anions, a new octahedral complex ion is formed. Write the formula of the complex ion formed. Identify the Lewis acid and Lewis base in this complex ion. [3%] (e) Write the sub-shell level electron configuration of the copper(II) ion [2%] (f) Consider the standard reduction potential data below: (1) 12 +2e 21- E = +0.54 V (2) Sn²+ + 2e Sn E = -0.14 V (3) Zn²+ + 2e → Zn E = -0.76 V If the two half-cells which give rise to the half-reactions (1) and (2) above are connected, forming an electrochemical cell, calculate Excell [2%] (g) Write the electrochemical cell in part (f) using standard cell notation. [2%] (h) By selecting two appropriate half-cells, write a balanced equation showing a spontaneous cell reaction that results in the formation of tin metal, Sn(s). [2%]