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    (Original post by iHeartCookies)
    Just wondering if someone could help me with this question please:

    Explain why high oxidation states are common at the beginning of the period whereas lower oxidation states are preferred at the end of the series? (It's for the 3d elements btw & it needs to be related to ionisation energy) (2 marks)

    I found this in my notes but I'm not sure if it's the answer or not :confused: :

    This is due to the increase in ionisation energies as the period is transversed. Formation of a compound requires that the energy required to form the gaseous ions is less than the energy gained through bond formation and lattice energy. Since more and more energy is required to oxidise the metal and the bond energy (lattice energy) only increases slowly the highest oxidation state attained decreases.

    The question/notes make no sense to me.. so if someone could kindly try and explain it to me a bit ?

    Thanks!
    yes, what you have in your notes is correct.

    Basically, as you go along a period, the nuclear charge increases, so ionisation energy increases. Since oxidation of metals requires them to be ionised, it follows that they will show a tendency to become less easily oxidised as you go along a period.

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