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Explain the ionic bond formation in (MgO) . |
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Answer» Solution :MAGNESIUMOXIDE `(MgO)` : Electronic configuration of Mg ` - 1s^(2) 2s^(2) 2p^(5) 3s^(2)` Electronic configuration of `O - 1s^(2) 2s^(2) 2p^(6) 3s^(2) 3p^(4)` (i) Magnesium has two electrons in its valence shell and oxygen has six electrons in its valence shell (ii) By losing two electrons Mg acquires the inert gas configurationof Neon and become a dipositive cation `Mg^(2+) : Mg to Mg^(2) + 2e^(-)` (iii) Oxygen ACCEPTS the two electrons to become a dinegative oxide anion `O^(2-)` there by attaining the inert gas configuration of Neon. `O + 2^(-) to O^(2-)` (iv) These two inons `Mg^(2+) " and " O^(2-)` combine to form an ionic crystal in which they are held together by electrostatic attractionforces. (v) During the FORMATION of magnesium oxide crystal `601.6` KJ `MOL^(-1)` energy is reduced , Thisfavours the formation of magnesium oxide `(MgO)` and its stabilisation . |
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