Xenon difluoride, XeF2. Xenon is a noble gas, and as such has a full outer shell of eight electrons; as per the octet rule, it doesn't usually form chemical bonds. However, highly reactive nonmetals such as fluorine can induce it to do so.
F2ccf2
1 x 1024 molecules
0
trig planar
White fume is given out.
F2ccf2
nope
Cl3CF
1 x 1024 molecules
sp2
sp2
Boron trichloride does not follow the octet rule. Boron does not allow the eight required electrons in the outer shell.
0
BCl3 is the formula for Boron Chloride. As a matter of interest it does not obey the octet rule. It is also called a Lewis Acid.
Yes the sulfur needs to have two more electrons to fill the octet, and chlorine only needs one. So there are two chlorines to give sulfur one electron. The whole molecule is covalently bonded so the electrons are shared between the chlorines and the sulfur so that both the elements octets are filled.
BCl3 is non-polar. The B-Cl bonds are polar but the molecule is not. You should review shapes of molecules. Valence Shell Electron Pair Repulsion, VSEPR. Applying VSEPR on BCl3, we can find out that the shape of the molecule is trigonal planar. Due to its geometry, the bonds cancel out.
there is only one answer for BCl3 and that is trigonal planer