No,pcl3 has one lone pair and three bonded pair , shape of trigonal pyramidal with a bond angle of 107 degrees whereas bcl3 has 3 bonded pairs and no lone pairs , shape of trigonal planar with the bond angle of 120 degrees.
Yes, the bond angles are 1200, D3h symmetry
The bond in boron trichloride, BCl3, is polar covalent.
Boron is sp2 hybridised with an empty p orbital. Both chlorine and iodine have lone electron pairs of suitable symmetry to form a partial pi bond with the empty orbital of boron. This partial pi bond effect is stronger and more significant in BCl3 because there is a better energy match between the empty p of boron (LUMO) and the lone pairs of Cl (HOMO) than between boron p and the lone pairs of iodine. As a Lewis acid, boron takes an electron pair into its empty p orbital. In BCl3, the significant pi bond means that this p orbital is less electron deficient and therefore hinders the ability of the p orbital to accept an electron pair, so it is a weaker acid than BI3. Maybe consult a textbook or website for a picture to help you visualise Boron in sp2 hybridised state.
Boron trichloride is a Lewis acid forming 1:1 complexes with a wide ange of compounds such as ethers, tertiary amines, thioethethers. These involve a "coordinate bond" which simply means that an electron pairs are donated to the B atom. This readily happens as boron in BCl3 only has a half share of 6 electrons and would be more stable with 2 more.
No,pcl3 has one lone pair and three bonded pair , shape of trigonal pyramidal with a bond angle of 107 degrees whereas bcl3 has 3 bonded pairs and no lone pairs , shape of trigonal planar with the bond angle of 120 degrees.
0
its covalent bond
Yes, the bond angles are 1200, D3h symmetry
The bond in boron trichloride, BCl3, is polar covalent.
There are exactly three electron pairs attached to the Boron atom, each one of them bonded to a chlorine atom as well.
There are a infinitely growing number of bond pairs between atoms.
3 bond pairs and no lone pairs
Boron is sp2 hybridised with an empty p orbital. Both chlorine and iodine have lone electron pairs of suitable symmetry to form a partial pi bond with the empty orbital of boron. This partial pi bond effect is stronger and more significant in BCl3 because there is a better energy match between the empty p of boron (LUMO) and the lone pairs of Cl (HOMO) than between boron p and the lone pairs of iodine. As a Lewis acid, boron takes an electron pair into its empty p orbital. In BCl3, the significant pi bond means that this p orbital is less electron deficient and therefore hinders the ability of the p orbital to accept an electron pair, so it is a weaker acid than BI3. Maybe consult a textbook or website for a picture to help you visualise Boron in sp2 hybridised state.
Boron trichloride is a Lewis acid forming 1:1 complexes with a wide ange of compounds such as ethers, tertiary amines, thioethethers. These involve a "coordinate bond" which simply means that an electron pairs are donated to the B atom. This readily happens as boron in BCl3 only has a half share of 6 electrons and would be more stable with 2 more.
two
covalent