Wiki User
∙ 12y agoXenon 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.
Wiki User
∙ 12y agoIF5 and XeF2 violate the octet rule since they have more than 8 valence electrons around the central atom (Iodine and Xenon, respectively). In IF5, iodine has 10 valence electrons, and in XeF2, xenon has 12 valence electrons.
F2ccf2
1 x 1024 molecules
There are no lone pairs on the central atom in BCl3 because boron (B) is in group 13 (or 3A) and can have only 3 bonds around it.
BCl3 has a trigonal planar shape, with the boron atom at the center and three chlorine atoms symmetrically arranged around it, each separated by 120 degrees. It only has three electron pairs around the central boron atom, resulting in a flat, triangular molecular geometry.
BCl3 is the molecule that has polar bonds but is non-polar overall. Despite having polar B-Cl bonds, the molecule is symmetrical, with the chlorine atoms arranged in a trigonal planar geometry around the central boron atom resulting in a cancelation of dipole moments, making the molecule non-polar.
F2ccf2
No, BCl3 does not follow the octet rule as boron only has 6 valence electrons in this molecule. Boron can form stable compounds with less than an octet due to its electron deficiency.
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 a Lewis acid because it can accept an electron pair from a Lewis base. Boron in BCl3 has an incomplete octet, making it electron deficient and capable of accepting an electron pair to complete its octet, giving it a positive charge.
BCl3 and BEH2 obey the octet rule because Boron and Beryllium are exceptions to the octet rule and can have stable electron configurations with less than 8 electrons. Cl3CF, NO, and SbF5 do not obey the octet rule because they have incomplete or expanded valence shells.
1 x 1024 molecules
sp2
The central atom in BCl3 is boron, which has only three valence electrons. Since it forms three bonds with the chlorine atoms, the hybridization of the central boron atom is sp2.
There are no lone pairs on the central atom in BCl3 because boron (B) is in group 13 (or 3A) and can have only 3 bonds around it.
Molecules that do not violate the octet rule include hydrogen (H2), beryllium (BeCl2), and boron (BCl3). These molecules satisfy the octet rule by having less than eight electrons around the central atom.
BCl3 has 3 bond pairs. Each chlorine atom forms a single covalent bond with the central boron atom.
The formula for boron chloride is BCl3. It consists of one boron atom and three chlorine atoms.