The lone pair pushes bonding electron pairs away.
The lone pair pushes bonding electron pairs away.
The lone pair pushes bonding electron pairs away.
The lone pair pushes bonding electron pairs away.
The lone pair pushes bonding electron pairs away.
The lone pair forces bonding atoms away from itself
Electron pair geometry considers both bonding and lone pairs of electrons around a central atom, while molecular geometry focuses solely on the arrangement of bonded atoms. This can lead to different geometries when there are lone pairs present; for example, in ammonia (NH₃), the electron pair geometry is tetrahedral due to one lone pair, but the molecular geometry is trigonal pyramidal. The presence of lone pairs affects bond angles and the overall shape of the molecule, resulting in distinct geometries.
The lone pair pushes bonding electron pairs away.
It is a bent molecule because of Oxygen's lone pairs
NH2- is sp3 hybridized and there is 2 bonding and 2 lone pair of electron,that's why shape of NH2 is angular.
A lone pair of electrons can affect the molecular shape by repelling bonded pairs of electrons, causing distortions in the molecule's geometry. This can lead to changes in bond angles and overall molecular shape.
It takes up space like an "invisible" atom.
The shape would be pyramidal because of the lone pair nitrogen has