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The lone pair forces bonding atoms away from itself
The lone pair pushes bonding electron pairs away.
The lone pair pushes bonding electron pairs away.
It takes up space like an "invisible" atom.
107.5 approximately, as the molecule is based on a tetrahedral shape, which should have 109.5 degree bonds, but the lone pair on the N causes the bond angles to be slightly decreased, by about 2 degrees
The lone pair forces bonding atoms away from itself
The lone pair creates repulsion between the molecules attached to it and distorts the shape.
The lone pair pushes bonding electron pairs away.
The lone pair pushes bonding electron pairs away.
The lone pair pushes bonding electron pairs away.
Lone pairs do not affect the shape of diatomic molecules, and Lone pairs are electrons that are not in bonds. Lone pairs do not affect the shape if they are not on the central atom.
The lone pair pushes bonding electron pairs away.
The lone pair pushes bonding electron pairs away.
The shape would be pyramidal because of the lone pair nitrogen has
The lone pair pushes bonding electron pairs away.
Tetrahedral bond angle of a molecule which have a lone pair electron is 107, smaller than regular 109.5, due to the repulsion of electrons of lone pair.
A lone pair of electrons takes up space despite being very small. Lone pairs have a greater repulsive effect than bonding pairs. This is because there are already other forces needing to be taken into consideration with bond pairs. So to summarize: Lone pair-lone pair repulsion > lone pair-bond pair repulsion > bond pair-bond pair repulsion. This makes the molecular geometry different.