Cl3CF
nope
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.
Boron trichloride does not follow the octet rule. Boron does not allow the eight required electrons in the outer shell.
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.
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.
nope
F2ccf2
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.
Boron trichloride does not follow the octet rule. Boron does not allow the eight required electrons in the outer shell.
trigonal planar
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.
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, each B-Cl bond is polar. but the molecule is having trigonal planar geometry and is a non-polar molecule.
First, it helps to draw out the Lewis structure. Boron, being the least electronegative element is in the center, with the three Bromines singly bonded around it. Each Br has an octet of electrons (3 lone pairs plus the single bond) and there are no electrons left over to go onto the Boron. This leaves Boron without an octet, but Boron is an exception to the octet rule so that's okay. So, no BBr3 does not follow the octet rule.
I don't think BCl4 is even a POSSIBLE molecule since boron has only three valence electrons; perhaps you mean BCl3 (which is nonpolar)?
there is only one answer for BCl3 and that is trigonal planer
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.