3 atoms around a central atom with no lone pairs.
Three groups bound to it with no lone pairs
trigonal pyramidal
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.
three groups bound to it with no lone pairs
Three groups bound to it with no lone pairs
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
Ok let's look at the different molecules: 1. CH3COCH3 is acetone. The molecule is a trigonal planar around the central carbon with the electronegative oxygen pulling electron density towards itself. So this is a polar molecule. 2. O2 is non-polar and relies only on dispersion forces. 3. CH3OH is has hydrogen bonding, dipole-dipole forces, and dispersion forces. 4. SO3 is a trigonal planar molecule with three oxygens around the sulfur, making it non-polar. Therefore it relies only on dispersion forces. 5. H2S is another polar molecule (bent by two lone pairs on the sulfur). So SO3 and O2 are the two molecules relying mainly on dispersion (London) forces.