List I Quantum Number |
List II Information provided |
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A. | ml | I. | Shape of orbital |
B. | ms | II. | Size of orbital |
C. | l | III. | Orientation of orbital |
D. | n | IV. | Orientation of spin of electron |
Statement I: | The energy of the \(\mathrm{He}^{+}\) ion in \(n=2\) state is same as the energy of H atom in \(n=1\) state |
Statement II: | It is possible to determine simultaneously the exact position and exact momentum of an electron in \(\mathrm{H}\) atom. |
1. | \(-\dfrac x9\) | 2. | \(-4x\) |
3. | \(-\dfrac 49x\) | 4. | \(-x\) |
Statement I: | The Balmer spectral line for H atom with lowest energy is located at \(\dfrac 5{36}\mathrm{ R_H~ cm^{-1}}\) (\(\mathrm{R_H}\) = Rydberg constant) |
Statement II: | When the temperature of blackbody increases, the maxima of the curve (intensity versus wavelength) shifts to shorter wavelength. |
I: | \(\Psi\) depends upon the coordinates of the electron in the atom. | The value of wave function,
II: | The probability of finding an electron at a point within an atom is proportional to the orbital wave function. |