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Linear 180
2 bonding sites, 0 lone pairs
Trigonal Planar 120
3 bonding sites, 0 lone pairs
bent (1st type) <120
3 bonding sites, 1 lone pairs
tetrahedral 109.5
4 bonding sites, 0 lone pairs
trigonal pyramidal <109.5
4 bonding sites, 1 lone pair
bent (2nd type) <<109.5
4 bonding sites, 2 lone pair
trigonal bipyramidal 120 and 90
5 bonding sites, 0 lone pairs
seesaw <120 and <90
5 bonding sites, 1 lone pair
t shaped <90
5 bonding sites, 2 lone pairs
linear (2nd version) 180
5 bonding sites, 3 lone pairs
octahedral 90
6 bonding sites, 0 lone pairs
Square pyramidal <90
6 bonding sites, 1 lone pairs
Square planar 90
6 bonding sites, 2 lone pairs
The more bonding groups, the more electron repulsion leading to a smaller bond angle.
Why is the angle small
Fewer bonding groups on central atom creates less electron repulsion and atoms spread out more.
Why is the angle bigger