Why does boron not form $B^{3 +}$ ion?

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Solution

As the Boron atom is small in size a large amount of energy is needed to remove 3 electrons from the boron atom.

The atomic number of Boron is 5. Its electronic configuration is $1 s^{2} 2 s^{2} 2 p^{1}$ .
When one electron is
removed from the p orbital a He-like fulfilled s orbital is left. This is
highly stable. So the second ionization enthalpy is quite high.
Again when one electron is removed a half filled orbital is left. So the third ionization enthalpy is also quite high.
Since the total energy needed to make $B^{3 +}$ is the total of all the ionization enthalpies an enormous amount of energy is required to form it.

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Which of the following compounds of boron does not exist in the free form?

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