Quantum Mechanical Model Of Atom

Each quantum number must follow these rules:
- Principal quantum number : any positive integer (here , valid)
- Azimuthal quantum number :
- Magnetic quantum number : ranges from to in integers
- Spin quantum number : or

For Option (2):
Given , then must be only 0, not .
So having with is not valid.
Hence, this set of quantum numbers is incorrect.

The correct option is (B):

The energy of electromagnetic radiation is directly proportional to its frequency and inversely proportional to its wavelength. The electromagnetic spectrum, in decreasing order of energy, is as follows:

Gamma rays > X-rays > UV rays > Visible light > IR rays > Microwaves > Radio waves

Hence, among the given options:

X-rays have the highest energy
Followed by UV rays
Then IR rays
And finally radio waves with the lowest energy

Thus, the correct order of decreasing energy is: X-rays > UV rays > IR rays > Radio waves

The correct option is (C):

The quantum mechanical model of the atom was developed by Erwin Schrodinger.
He formulated a wave equation, known as Schrodinger’s wave equation, which describes the behavior of electrons in an atom as wave-like entities.
This model is based on the principles of quantum mechanics and replaced Bohr’s model by removing its limitations.
It successfully explains the shapes of orbitals, the probability of finding electrons, and other atomic behaviors not addressed by earlier models.

The correct option is (C): Schrodinger

The correct answer is Principal quantum number.

Explanation:

Principal quantum number (n): This quantum number defines the main energy level or shell of an electron in an atom. It can never be zero. It starts from 1 (n = 1) and increases (n = 2, 3, etc.).

Azimuthal quantum number (l): This quantum number defines the shape of the orbital (subshells). The value of lll can be zero, for s-orbitals (which have spherical shapes). For p-orbitals, l=1l = 1l=1, d-orbitals have l=2l = 2l=2, and f-orbitals have l=3l = 3l=3.

Magnetic quantum number (m): This quantum number defines the orientation of the orbital in space. The value of mmm depends on lll and can range from −l-l−l to +l+l+l, including zero.

Thus, the principal quantum number (n) cannot have a value of zero, making it the correct answer.

Correct answer: Line spectra of H atom

Explanation:
Bohr's atomic model successfully explained the line spectra of the hydrogen atom. According to Bohr, electrons revolve in discrete energy levels, and the emission or absorption of light occurs when electrons jump between these levels.

Each jump corresponds to a specific amount of energy, resulting in a spectral line. This explained the presence of distinct lines in the hydrogen emission spectrum.

However, Bohr's model could not explain the fine structure (very closely spaced lines) observed in more detailed spectra.

Hence, the correct answer is: Line spectra of H atom.

Correct answer: K, L, M,...

Explanation:
The principal quantum number ( ) determines the main energy level or shell of an electron in an atom. These shells are designated by the letters:

- K shell
- L shell
- M shell
- N shell
and so on.

Hence, the correct answer is: K, L, M,...

The quantum number that gives information about the orientation of an orbital is the magnetic quantum number. This quantum number defines the orientation of the orbital in space with respect to the other orbitals.

The correct option is (C): Magnetic quantum number

Hund’s Rule states that electrons will fill degenerate orbitals (orbitals of the same energy) singly before pairing up. This explains why nitrogen has 3 unpaired electrons in its 2p-orbitals, as the 2p orbitals are degenerate and Hund’s rule applies.
Thus, the correct answer is Hund.