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(D) The wave function for the $1s$ orbital of a hydrogen atom is given by $\Psi_{1s} = \frac{1}{\sqrt{\pi a_0^3}} e^{-r/a_0}$.$A.$ The probability den

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The total energy of the electron is maximum when it is at a distance $a_0$ from the nucleus

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(D) The wave function for the $1s$ orbital of a hydrogen atom is given by $\Psi_{1s} = \frac{1}{\sqrt{\pi a_0^3}} e^{-r/a_0}$.$A.$ The probability density $\Psi^2$ is proportional to $e^{-2r/a_0}$. At $r = 0$ (nucleus),$\Psi^2$ is maximum. This statement is correct.$B.$ The electron has a non-zero probability of being found at any distance $r$ from the nucleus,including $2a_0$. This statement is correct.$C.$ The $1s$ orbital has no angular dependence,making it spherically symmetrical. This statement is correct.$D.$ The total energy of an electron in a hydrogen atom is given by $E_n = -\frac{13.6 \ eV}{n^2}$. This energy is constant for a given orbital and does not depend on the distance $r$ from the nucleus. The energy is maximum (zero) at $r = \infty$. Therefore,this statement is incorrect.

Laws	Statements
$(1)$ Hund's Rule	$(A)$ No two electrons in an atom can have the same set of all four quantum numbers.
$(2)$ Aufbau Principle	$(B)$ Half-filled and fully-filled orbitals have greater stability.
$(3)$ Pauli Exclusion Principle	$(C)$ Electrons prefer to remain unpaired in degenerate orbitals first.
$(4)$ Heisenberg's Uncertainty Principle	$(D)$ It is impossible to determine simultaneously the exact position and exact momentum of an electron.
	$(E)$ In the ground state of atoms,orbitals are filled in the order of increasing energy.

Which one of the following about an electron occupying the $1s$ orbital in a hydrogen atom is incorrect? (Bohr's radius is represented by $a_0$)

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