This comes much later by the Sidgwick-Powell/Gillespie/Nyholm-VSEPR approach to molecular geometry. If we apply the Lewis formalism to the diatomic molecules of nitrogen, oxygen, and fluorine, we get N≡N, a triple bond O=O, a double bond F—F, a single bond The three molecules ...
Ans: According to the VSEPR theory, the lone pair-lone pair repulsions are stronger than the bond pair-bond pair repulsions, thereby shortening the \({\text{HOH}}\) bond angle (oxygen has two lone pairs of electrons). Therefore, since the bond angle is reduced from \({109.5^ \circ ...
In water, oxygen has sp^(3) - hydridisation and the bond angle of HOH should have been 109^(@)28. In H(2)O the oxygen atom is surrounded by two shared pairs and two lone pairs of electrons. From VSEPR theory , lone pair - lone pair repulsions
In the general molecular geometry for water and dihydrogen sulfide, this shape is a tetrahedron with the central atom (O or S) in the center of this... Learn more about this topic: VSEPR Theory | Chart & Model from Chapter 5/ Lesson 11 ...