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Cl3CF
Wiki User
∙ 12y ago
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.
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Does BCl3 follow the octet rule?
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.
Does BCl3 violate the octet rule?
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.
Why BCL3 is Lewis acid?
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.
What is the formula for the compound boron chloride?
The formula for boron chloride is BCl3. It consists of one boron atom and three chlorine atoms.
Which one doesn't follow the octet rule nh3 cf4 bcl3 ash3 hcl?
HCl doesn't follow the octet rule because hydrogen can only have 2 valence electrons and doesn't need a full octet to achieve a stable configuration.
Does BCl3 follow the octet rule?
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.
What molecules does not violate the octet rule no bcl3 bef2 sef6 f2ccf2?
F2ccf2
Does BCl3 violate the octet rule?
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.
Which one doesn't follow the octet rule nh3 cf4 bcl3 ash3 hcl?
HCl doesn't follow the octet rule because hydrogen can only have 2 valence electrons and doesn't need a full octet to achieve a stable configuration.
What is the electronic geometry of BCl3 Enter the electronic geometry of the molecule.?
trigonal planar
BCl3 H2O NH3 and PCl3 which is non-polar?
BCl3 and PCl3 are non-polar molecules because they have a symmetrical trigonal planar geometry, causing the bond dipoles to cancel each other out. H2O and NH3 are polar molecules due to their bent and trigonal pyramidal geometries, respectively, which result in an uneven distribution of electron density.
What is the formula for the compound boron chloride?
The formula for boron chloride is BCl3. It consists of one boron atom and three chlorine atoms.
Does BCl3 have polar bonds?
Yes, BCl3 has polar covalent bonds because of the electronegativity difference between boron and chlorine. However, the molecule as a whole is nonpolar due to its symmetrical trigonal planar geometry which results in a net dipole moment of zero.
Does BBr3 obey octet rule?
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.
Is BCl4 a polar or nonpolar molecule?
BCl4 is a nonpolar molecule because the pull of the chlorine atoms cancel each other out, resulting in a symmetric distribution of charge.
What are the shapes of BCl3?
there is only one answer for BCl3 and that is trigonal planer
BCl3 PCl3 CS2 NO3 SO3 NH3 IF5 XeF2 SO2 Which of these molecules has a central atom that violates the octet rule?
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.
