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    Name:  nn.png
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Size:  22.0 KB For this question, I am a bit confused with the dipoles in NH4+ ions. Attachment 614736614738 Is there a dipole between the dative covalent bond ? If there is, is this the reason why the dipoles cancel out because ammonium ion is symmetrical?

    Thanks.
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    (Original post by coconut64)
    Name:  nn.png
Views: 93
Size:  22.0 KB For this question, I am a bit confused with the dipoles in NH4+ ions. Attachment 614736614738 Is there a dipole between the dative covalent bond ? If there is, is this the reason why the dipoles cancel out because ammonium ion is symmetrical?

    Thanks.
    Ammonium ion is non-polar ... although the N-H bonds are polar all the individual dipoles cancel out .
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    Not in the molecular ion. It can have them In The NH3 between H-N And In the form you draw it should make H bonds with other NH4s in the negative regions of the N. Have a look at some more problems I don't So chemistry but Ammonia/Ammonium and Amine And their molecular compounds appelé everywhere So make sure You learnt all about them.
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    (Original post by charco)
    Ammonium ion is non-polar ... although the N-H bonds are polar all the individual dipoles cancel out .
    So is there a dipole between the dative covalent bond? Thanks
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    (Original post by coconut64)
    So is there a dipole between the dative covalent bond? Thanks
    All four bonds are identical and the ion is tetrahedral so that the resolved vectors all cancel out.

    Once the ion is formed there is no "dative" bond, only four shared pairs of electrons.

    To explain the formation of the ion we use the concept of dative bonding by the lone pair on the ammonia molecule.

    But, once formed, it ceases to have any meaning.
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    (Original post by charco)
    All four bonds are identical and the ion is tetrahedral so that the resolved vectors all cancel out.

    Once the ion is formed there is no "dative" bond, only four shared pairs of electrons.

    To explain the formation of the ion we use the concept of dative bonding by the lone pair on the ammonia molecule.

    But, once formed, it ceases to have any meaning.
    Thanks
 
 
 
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