For the given electronic transitions,which of the following statements is correct?

Among the following,the correct statement$(s)$ for electrons in an atom is(are):
$A$. Uncertainty principle rules out the existence of definite paths for electrons.
$B$. The energy of an electron in $2s$ orbital of an atom is lower than the energy of an electron that is infinitely far away from the nucleus.
$C$. According to Bohr's model,the most negative energy value for an electron is given by $n=1$,which corresponds to the most stable orbit.
$D$. According to Bohr's model,the magnitude of velocity of electrons increases with increase in values of $n$.

Given below are two statements:
Statement $I$: Rutherford's gold foil experiment cannot explain the line spectrum of hydrogen atom.
Statement $II$: Bohr's model of hydrogen atom contradicts Heisenberg's uncertainty principle.
In the light of the above statements,choose the most appropriate answer from the options given below:

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

Which one is the wrong statement?

Match the equations given in List-$I$ with their names in List-$II$.

List-$I$	List-$II$
$(1)$ $\Delta x \cdot \Delta p \ge \frac{h}{4\pi}$	$(A)$ De Broglie equation
$(2)$ $mvr \ge \frac{nh}{2\pi}$	$(B)$ Uncertainty principle
$(3)$ $\lambda = \frac{h}{\sqrt{2m(KE)}}$	$(C)$ Frequency equation of $H$-spectrum
$(4)$ $\nu = 3.29 \times 10^{15} \left( \frac{1}{n_i^2} - \frac{1}{n_f^2} \right)$	$(D)$ Angular momentum is quantized