Hydride of boron occurs as B2H6 but B2Cl6 does not exist. This is because

Question

Hydride of boron occurs as B2H6 but B2Cl6 does not exist. This is because (A) pπ-dπ back bonding is possible in B2H6 but not in B2Cl6 (B) boron and hydrogen have almost equal values of electronegativity (C) boron and chlorine have almost equal atomic sizes (D) small hydrogen atoms can easily fit in between boron atoms but large chlorine atoms do not.

Tardigrade Admin · Accepted Answer

Hydride of boron occurs as B 2 H 6 but B 2 Cl 6 does not exist. This is because small hydrogen atoms can easily fit in between boron atoms but large chlorine atoms do not. Note: Instead of B 2 Cl 6, the stable compound is BCl 3 which acts as a Lewis acid and accepts a lone pair of electrons from ammonia to form BCl 3 arrow NH 3.

Q. Hydride of boron occurs as $B_{2} H_{6}$ but $B_{2} C l_{6}$ does not exist. This is because

p $π$ -d $π$ back bonding is possible in $B_{2} H_{6}$ but not in $B_{2} C l_{6}$

boron and hydrogen have almost equal values of electronegativity

boron and chlorine have almost equal atomic sizes

small hydrogen atoms can easily fit in between boron atoms but large chlorine atoms do not.

Q. Hydride of boron occurs as B2​H6​ but B2​Cl6​ does not exist. This is because

pπ-dπ back bonding is possible in B2​H6​ but not in B2​Cl6​

boron and hydrogen have almost equal values of electronegativity

boron and chlorine have almost equal atomic sizes

small hydrogen atoms can easily fit in between boron atoms but large chlorine atoms do not.

Q. Hydride of boron occurs as $B_{2} H_{6}$ but $B_{2} C l_{6}$ does not exist. This is because

p $π$ -d $π$ back bonding is possible in $B_{2} H_{6}$ but not in $B_{2} C l_{6}$