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Bond angles help

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    For question Q1 (A) (ii) of this paper they ask for the shape of the dinitrogen oxide molecule. There is a triple bond between the N and N atom and a single dative bond between N and O atom therefore there are 4 areas of electron density around the central N atom one of the being a lone pair so the shape should be a trigonal pyramidal but why does the MS say accept only linear/180 degrees?? How can it be linear is the triple bond so strong or something that it makes the whole molecule linear??
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    (Original post by Hanz_a93)
    For question Q1 (A) (ii) of this paper they ask for the shape of the dinitrogen oxide molecule. There is a triple bond between the N and N atom and a single dative bond between N and O atom therefore there are 4 areas of electron density around the central N atom one of the being a lone pair so the shape should be a trigonal pyramidal but why does the MS say accept only linear/180 degrees?? How can it be linear is the triple bond so strong or something that it makes the whole molecule linear??
    Triple and double bonds act just like single bonds when working out the angles.

    The central N has a triple bond and a single bond, with no lone pairs so it is linear. The dative bond is considered a normal single covalent bond for this too.
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    (Original post by clownfish)
    Triple and double bonds act just like single bonds when working out the angles.

    The central N has a triple bond and a single bond, with no lone pairs so it is linear. The dative bond is considered a normal single covalent bond for this too.
    ahh i see! thanks !

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