Statement (A): As one considers orbits with h | vedclass

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(B) In a hydrogen atom,the potential energy $(PE)$ of an electron in the $n$th orbit is given by $PE = -\frac{kZe^2}{r}$.For higher values of $n$,the

Vedclass · Accepted Answer

$A, B$ true,but $C$ false

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(B) In a hydrogen atom,the potential energy $(PE)$ of an electron in the $n$th orbit is given by $PE = -\frac{kZe^2}{r}$.For higher values of $n$,the radius $r$ increases because $r \propto n^2$.As $r$ increases,the magnitude of the negative potential energy decreases,meaning the value of the potential energy increases (becomes less negative).Thus,statement $(A)$ is correct.In Thomson's model,an atom is described as a spherical cloud of positive charge with electrons embedded within it,similar to a plum pudding. Thus,statement $(B)$ is correct.According to Bohr's model,an electron in an atom is located at a definite distance from the nucleus and revolves with a definite velocity. However,Heisenberg's uncertainty principle states that it is impossible to determine the exact position and momentum of a moving electron simultaneously.Therefore,Bohr's model contradicts the uncertainty principle,making statement $(C)$ incorrect.Hence,option $(b)$ is the correct answer.

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