In the Lewis structure of the fluoramine (NH₂F) molecule, the number of bonding pairs and the number of lone pairs around the left hydrogen atom is one and zero, respectively.
In the Lewis structure of the fluoramine (given below) we can see that the two hydrogen atoms and the fluorine atom are bonded to the nitrogen central atom.
To know the number of electrons that each atom can share, we need to calculate the valence electrons for each one of them.
For H:
- Electronic configuration: 1s¹
- Number of valence electrons: 1
For F:
- Electronic configuration: 1s²2s²2p⁵
- Number of valence electrons: 7
For N:
- Electronic configuration: 1s²2s²2p³
- Number of valence electrons: 5
Now, remembering that a bonding pair is the number of electrons shared in a molecule and that a lone pair is the number of electrons that are not shared, for the fluoramine we have:
Bonding pairs
- Nitrogen: 3 pairs = 1 pair (with the right hydrogen) + 1 pair (with the left hydrogen) + 1 pair (with the fluorine)
- Right hydrogen: 1 pair (shared with the nitrogen)
- Left hydrogen: 1 pair (shared with the nitrogen)
- Fluorine: 1 pair (shared with the nitrogen)
Lone pair
- Nitrogen: 5 electrons valence - 3 electrons shared = 2 electrons (1 pair)
- Right hydrogen: 1 electron valence - 1 electron shared = 0
- Left hydrogen: 1 electron valence - 1 electron shared = 0
- Fluorine: 7 electrons valence - 1 electrons shared = 6 electrons (3 pairs)
Therefore, the number of bonding and lone pairs for the left hydrogen atom is 1 and 0, respectively.
Learn more about Lewis structure here:
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I hope it helps you!
