Why are bond angles of h20 and nh3 104.5 and 107.5 | Molecular Shape and Bond Angles | Chemistry

Why are bond angles of h20 and nh3 104.5 and 107.5?
Queries Solved:
🔹molecular shape and bond angles
🔹why the shape of h2o and nh3 differ
🔹sp3 hybridization in h2o and nh3
🔹nh3 pyramidal shape
🔹nh3 bond angle 107
🔹h2o bent or angular shape
🔹h2o bond angle 104
🔹Why the bond angle in ammonia is 107 and that in water is 104.5 while both of them are sp3 hybridized?
The valence shell electron pair repulsion theory states that there are two types of electron pairs surrounding the centre atom.
1. Lone pair
2. Bond pair
subsequently, what are lone pair and bond pair electrons?
The lone pair is the pair of electrons that are not shared, whereas the bond pair is the pair of electrons that are shared.
Both nh3 and h2o are sp3 hybridised, but how can the type of hybridization be easily determined? To determine the type of hybridization, it is sufficient to count the total number of lone electron pairs and sigma bonds.
In the case of ammonia, there is one lone pair and three sigma bonds, resulting in a total of four hybrid orbitals indicating sp3 hybridization, but in the case of water, there are two lone pairs and two sigma bonds, resulting in a total of four hybrid orbitals showing sp3 hybridization.
The centre atom is Sp3 hybridised in both NH3 and H2O because NH3 contains 1 lone pair and 3 bond pair (sigma bond) electrons. The lone pair has a stronger repulsion, which causes the bond pairs to be compressed to an angle of 107.50, resulting in a trigonal pyramidal structure. In contrast, H2O contains two lone pairs and two bond pairs of electrons.
The lone pairings repel each other and bond pairs more strongly.
Consequently, the bond pairs are squeezed to an angle of 104.5 degrees having an angular form.
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