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    1) Explain in terms of electronic configurations why Fe2+ ions are readily oxidised to Fe3+ ions, but Mn2+ ions are not readily oxidised to Mn2+.

    2) Cobalt forms a complex compund of formula [Co(NH3)4Cl2]+Cl-
    i) What is the oxidation state of cobalt in this compund?
    ii) Give the name of the complex ion in this compund ( [Co(NH3)4Cl2]+ )
    iii) How many moles of silver chloride would be immediately precipitated from one mole of this compound in aqeous solution by the addition of excess silver nitrate?

    Thankz in advance :tsr:
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    1. Fe2+ ion had 6 3d electrons, Fe3+ has 5, 5 is very stable because it is completely half filled. I think you typed out the second sentence, but it also has to do with the stability of the ions formed.

    2. (i) 3+, as the NH3s are neutral and each Cl- is a -1, and the overall is +1.
    (ii) tetraamminedichlorocobalt(III)
    (iii) immediately, onle one mole, the Cl- ionically bonded to the ion. one more of Cl- precipitates one mole of AgCl with excess silver ions.
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    (Original post by mik1w)
    1. Fe2+ ion had 6 3d electrons, Fe3+ has 5, 5 is very stable because it is completely half filled. I think you typed out the second sentence, but it also has to do with the stability of the ions formed.
    I presume you mean the d shell. The reason why it is the more stable is you have no pairs of electrons in the 3d shell, hence the energy is lowered because there is no electron repulsion.
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    thankz i gets it!!
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    [QUOTE=mik1w]1.
    (ii) tetraamminedichlorocobalt(III)
    QUOTE]

    aint that a mouthfulll.lol
 
 
 
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