Question

Explain why Boron does not exist as B3 + ion

Answer 1

As you may know, Boron has the atomic number of 5 and hence an electronic configuration of 1s[2] 2s[2] 2p[1].

When you remove one electron from the p orbital you'll be left with a He-like fulfilled s orbital which is highly stable and hence the second ionization enthalpy will be quite high. Again when you remove one electron you'll be left with a half filled orbital and hence the third ionization enthalpy will also be pretty and since the total energy required to make B 3+ is the sum of all the ionization enthalpies, the amount of energy required makes it virtually impossible to form it.

Answer 2

$\huge\boxed{\underline{\mathcal{\red{A}\green{N}\pink{S}\orange{W}\blue{E}\purple{R}}}}$

❤⭐ :REASON:⭐❤

• ❤.. Due to $\red{\tt{Non}}$_$\purple{\tt{availability}}$ of$\orange{\tt{d}}$ orbitals,boran is unable to expand its$\green{\tt{Octet}}$.
• ❤...Therefore,the maximum cobalence of boran cannot exceed4.