NH2- is sp3 hybridized and there is 2 bonding and 2 lone pair of electron,that's why shape of NH2 is angular.
Trigonal planar because it has three bonding pairs and one lone pair
Trigonal pyramidal. As has 5 valence electrons. It forms single bonds with each of the F atoms, donating one electron to each bond. This leaves 2 unbonded electrons, or a single lone pair. Thus the molecule has 4 different groups attached to As, and the electron configuration is tetrahedral. A tetrahedral configuration with one lone pair results in a trigonal pyramidal molecular geometry.
its a trigonal pyramid but it can also be tetrahedral because it has a lone pair of electron bonded to the centrel atom (P)
In XeO2Cl2 :– Hybridization of Xe = sp³d Molecular geometry = Trigonal Bypyramidal Molecular shape = See-Saw shape Two oxygen atoms and one lone pair of Xe are at equatorial positions whereas two Cl atoms are at axial positions.Two oxygen atoms and one lone pair of Xe are at equatorial positions whereas two Cl atoms are at axial positions. **(**General confusion:– According to Bent's rule; in Trigonal Bypyramidal geometry, more electronegative atom prefers to stay at axial position. Now, Electronegativity of O > Electronegativity of Cl So, you might think that why Oxygen atoms are present at equatorial positions. This is so because bent's rule also states that double bonds and lone pairs prefer to stay at equatorial positions and this factor dominates the electronegativity factor**)**
It takes up space like an "invisible" atom.
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.
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.
The lone pair pushes bonding electron pairs away.
The molecular shape of ammonia (NH3) is trigonal pyramidal. It has a lone pair of electrons on the nitrogen atom, causing the molecule to have a distorted tetrahedral shape.
The lone pair pushes bonding electron pairs away.
The lone pair repels the electrons of the adjacent bonds more so than does a bonding pair of electrons, so thus alters the molecular geometry of the molecule.
The lone pair pushes bonding electron pairs away.
The lone pair pushes bonding electron pairs away.
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.