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(a) Are the oxidation state and covalency of Al in [AICI(H2O)5] ++ same? (b) Which of the following will have the most negative electron gain enthalpy and which the least negative? P,S, Cl, F Explain your answer. (c) Using the Periodic Table, predict the formulas of compounds which might be formed by the following pairs of elements:(i) Si and Br (ii) Al and S |
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Answer» (a) No, the oxidation state of Al is +3 and the covalency is 6. (b) Electron gain enthalpy generally becomes more negative across a period as we more from left to right. Within a group, electron gain enthalpy becomes less negative down a group. However, adding an electron to the 2p-orbital leads to more repulsion than adding an electron to the larger 3p-orbital. Hence, the element with most negative electron gain enthalpy is CI and the one with the least negative electron gain enthalpy is P (c) (i) Si is a group 14 element with a valence of 4; Br belongs to the halogen family with a valence of 1. Therefore, the formula of the compound formed would be SiBr4. (ii) Al belongs to group 13 with a valence of 3, S belong to group 16 elements with valence of 2. Therefore, the formula of the compound formed would be Al2S3. |
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