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(B) The radius of the $n^{th}$ Bohr orbit is given by the formula: $r_n = \frac{0.529 	imes n^2}{Z} \mathring A$.For a singly ionized helium atom $(H

Vedclass · Accepted Answer

$1.06$

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(B) The radius of the $n^{th}$ Bohr orbit is given by the formula: $r_n = \frac{0.529 	imes n^2}{Z} \mathring A$.For a singly ionized helium atom $(He^+)$,the atomic number $Z = 2$.For the second Bohr orbit,$n = 2$.Substituting these values into the formula:$r_2 = \frac{0.529 	imes 2^2}{2} \mathring A$$r_2 = \frac{0.529 	imes 4}{2} \mathring A$$r_2 = 0.529 	imes 2 \mathring A$$r_2 = 1.06 \mathring A$.

Radius of the second Bohr orbit of a singly ionized helium atom is ......... $ \mathring A $

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