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bbr3 bond angle

Lets consider the Lewis structure for CCl 4. An sp2 hybridization results in trigonal planar formation with B in the center and the 3 Br's on the outer corners with 120 degrees in between each of them. For trigonal pyramidal geometry the bond angle is slightly less than 109.5 degrees, around 107 degrees. Each Br forms one bond with its one valence electron. Explain why there is equal bond angle in bf3, bbr3 ,bi3,bcl3Because F,Cl,Br and I all are halogen same group and has same number of bonds involved with same no. Answer = bbr3 ( BORON TRIBROMIDE ) is Nonpolar What is polar and non-polar? Question = Is bbr3 polar or nonpolar ? Considering the valence bond theory, B would hybridize to sp2 with an extra p orbital in order to bond with 3 Br. We can draw the Lewis structure on a sheet of paper. BBr3 is trigonal planar in its electron geometry and its molecular geometry. But the bond angles are same according to most of the websites. So, in $\ce{BBr3}$ the electrons will be the closest towards boron and thus due to electron-electron repulsions $\ce{BBr3}$ will have maximum bond angle. Polar "In chemistry, polarity is a separation of electric charge leading to a molecule or its chemical groups having an electric dipole or multipole moment. Polar molecules must contain polar bonds due to a difference in electronegativity between the bonded atoms. B has 3 valence electrons able to bond with the 7 valence electrons of Br. The VSEPR designator for BBr3 is AX3 with A being the central atom and X being the ligand atoms. how can we compare the bond angles in BF3 BCl3 BBr3 BI3 Boron atoms in BX3 has six electrons in the outermost shekll and thus it can accept a pair of electrons Click hereto get an answer to your question ️ The correct order of bond angles is: Bl3

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