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27 August, 11:11

Below is the lewis structure of the fluoramine nh2f molecule. nfhh count the number of bonding pairs and the number of lone pairs around the left hydrogen atom.

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  1. 27 August, 11:38
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    Bonding Pair Electrons = 2

    Lone Pair of Electrons = Zero

    Explanation:

    In order to answer this question one should draw the Lewis structure of Fluoramine first following following steps.

    Step 1:

    First of all add all the valence electrons present in all elements of the given compound. i. e.

    Hydrogen * 2 = 1 * 2 = 2

    Fluorine * 1 = 7 * 1 = 7

    Nitrogen * 1 = 5 * 1 = 5

    Total Valence Electrons = 14

    Step 2:

    Draw the central atom (i. e. Nitrogen) and surround it by remaining elements. In our case Nitrogen is surrounded by two H atoms and one F atom.

    H N H

    F

    Step 3:

    Connect all atoms to central atom via a single bond and subtract 2 electrons per bond from total valence electrons. As there are three single bonds so, we will subtract 6 electrons from 14 valence electrons and are left with 8 valence electrons. Now, these remaining 8 electrons are distributed among the elements starting from most electronegative (i. e. Fluorine) and then Nitrogen. So, Fluorine will get 3 lone pair of electrons and / nitrogen will get one lone pair of electrons as shown in figure.

    Conclusion:

    As Hydrogen atoms are making only single bonds hence, they will have two bonding pair electrons per H atom and as shown in figure H atoms didn't get any lone pair of electrons.
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