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[M(h2o)]3+ vs [m(h2o)]2+

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    • Thread Starter

    Just a bit of confusion that I should have sorted ages ago but haven't

    In terms of acidity of metal complexes my understanding is that;

    M3+ ions have greater charge density than their M2+ ions

    Therefore weaken O-H bond of water ligands and H+ dissociation more likely

    I recently saw in a mark scheme "M3+ results in greater polarisation (of water)"

    Can someone please expakin what this actually means in terms of IMF

    Surely if M3+ has higher charge density, it withdraws electrons from O atom and therefore O is less delta negative so O-H bond is LESS polar?

    Any help is greatly appreciated
    • Thread Starter

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