3 atoms around a central atom with no lone pairs.
Three groups bound to it with no lone pairs
The molecular structure is trigonal pyramidal.
Ammonia (NH3) has a trigonal pyramidal shape due to its three bonding pairs and one lone pair of electrons around the central nitrogen atom.
The molecule geometry of HNO2 is bent or angular. This is due to the presence of two bonding pairs and one lone pair of electrons around the central nitrogen atom, resulting in a trigonal planar arrangement with a bond angle of approximately 120 degrees.
The molecular shape of BFI2 is linear. This is because the molecule has two bonding pairs and no lone pairs around the central Boron atom, resulting in a linear geometry.
three groups bound to it with no lone pairs
Three groups bound to it with no lone pairs
The molecular structure is trigonal pyramidal.
Three groups bound to it with no lone pairs
the electronic geometry is the arrangement of REDs around the central atom. these REDs consist of both bonding pairs and lone pairs where the bonding pairs can either be single, double or tripple bonds. . REDs ELECTRONIC GEOMETRY 2 LINEAR 3 TRIGONAL PLANAR 4 TETRAHEDRAL 5 TRIGONAL BYPYRAMIDAL 6 OCTAHEDRAL
Trigonal Pyramidal. It is not trigonal planar because there is one lone pair around the central atom, just like the shape of ammonia.
The lone unbonded pair of electrons around nitrogen dictates that the NBr3 molecule will have a 3-D trigonal pyramidal shape.
How do lone pairs around the central atom affect the polarity of the molecule?
No. First of all, NH2- is an ion, not a molecule. Second, it has a bent geometry, similar to that of a water molecule.
Trigonal pyramidal
Trigonal Pyramidal
The intermolecular forces for O2 and H2S would be mainly due to London dispersion forces since they have only nonpolar covalent bonds. CH3OH and SO3 would have additional intermolecular forces due to hydrogen bonding and dipole-dipole interactions. CH3COCH3 would have dipole-dipole interactions as well as London dispersion forces.