Is BCI3 polar or non polar ,identify the negative ends
I'd say that like CCl4, the molecule is basically pyramidal in shape, so it has no "ends" for polarity.
To determine if a molecule is polar or nonpolar, we need to consider its molecular geometry and the polarity of its individual bonds.
BCI3, also known as boron trichloride, consists of one boron atom (B) and three chlorine atoms (Cl). Boron is in Group 13 of the periodic table, and chlorine is in Group 17.
To determine the molecular geometry of BCI3, we can use the VSEPR theory (Valence Shell Electron Pair Repulsion). According to VSEPR, the three chlorine atoms will arrange themselves as far apart as possible to minimize electron repulsion, resulting in a trigonal planar shape.
Now, each chlorine atom forms a covalent bond with the boron atom, and since chlorine is more electronegative than boron, these bonds are polar, with the chlorine atoms being partially negative (δ-) and the boron atom being partially positive (δ+).
However, even though the bonds are polar, the symmetric arrangement of the three chlorine atoms around the central boron atom cancels out the individual bond polarities, making the molecule as a whole nonpolar.
So, in the case of BCI3, it is a nonpolar molecule. There are no negative ends to identify since the molecule as a whole has no distinct positive or negative regions.