Question

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.

Answer 1

Answer:

            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.