H-O-H
Well, the hydrogens bring a total of two valance electrons to the mix and the oxygen contributes six, so the total valance electrons = 8
4 are used in the two bonds, so 8 - 4 = 4
Two lone pair, one above and one below the oxygen in the Lewis dot structure.
The central atom in H20 is the oxygen atom, 'O'. The oxygen atom has 2 lone pairs of electrons around it, and each lone pair has 2 electrons in it.
8 valence electrons are in the electron-dot structure of H2O. There are 2 from hydrogen and 6 from oxygen.
Oxygen has one bonding pair with each H atom, so two bonding pairs in total, and two lone pairs of electrons surrounding its central position.
its not four
angular with 109.5 degree
linear
Ammonia NH3 one lone pair on Nitrogen, Water H2O two lone pairs on Oxygen.
The central atom of ammonia is nitrogen and it has 3 bonding pairs and a lone pair around, hence it undergoes sp3 hybridization. The central atom of boron trifluoride is the boron atom, and around it has only three bonding pairs. So it hybridizes as sp2.
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angular with 109.5 degree
There are no lone pairs and it's tetrahedral.
No lone pairs
Every pair of electrons on the central atom (S) of the Lewis structure of SF6 is shared by an F atom, so therefore there are no lone pairs on the central atom.
electron-group geometry Apex!
linear
3 atoms around a central atom with no lone pairs.
Ammonia NH3 one lone pair on Nitrogen, Water H2O two lone pairs on Oxygen.
The Central atom has no lone pairs in CH4
The central atom of ammonia is nitrogen and it has 3 bonding pairs and a lone pair around, hence it undergoes sp3 hybridization. The central atom of boron trifluoride is the boron atom, and around it has only three bonding pairs. So it hybridizes as sp2.
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The lone pair electron region is the place around the central atom where electrons not bonding with another atom can be found. A lone pair of electrons are electrons that are not bonded with other atoms.