1a) Use the table below to determine the energy in eV of the photon absorbed when an electron jumps up from the n = 1 orbit to the n = 2 orbit of a hydrogen atom. =_________ eV1b ) Use the table shown below to determine the energy in eV of the photon emitted when an electron jumps down from the n = 3 orbit to the n = 2 orbit of a hydrogen atom.=___________ eV **Allowed Values of the Hydrogen Electron's Radius and Energy for Low Values of n**This table provides the permitted values for the radius and energy of a hydrogen electron for low quantum numbers, denoted as \( n \).| \( n \) | \( r_n \) (radius in nm) | \( E_n \) (energy in eV) ||-------|-------------------------|-------------------------|| 1 | 0.053 nm | \(-13.60\) eV || 2 | 0.212 nm | \(-3.40\) eV || 3 | 0.477 nm | \(-1.51\) eV || 4 | 0.848 nm | \(-0.85\) eV |**Explanation:**- **Columns**: - **n**: Indicates the principal quantum number, which denotes the electron's energy level in a hydrogen atom. - **\( r_n \)**: Represents the radius of the electron's orbit in nanometers (nm). - **\( E_n \)**: Shows the energy of the electron in electron volts (eV), with negative values indicating bound states.As \( n \) increases, the radius \( r_n \) increases, and the energy \( E_n \) approaches zero from negative values, showing that electrons at higher energy levels are less tightly bound.

(a) When an electron jumps up from n = 1 to n =2, the energy of the emitted photon will be the difference of energies between these states. The energy of an electron when it goes up is, Now, put the values in the above relation from the given table.(b) When an electron jumps down from n = 3 to n =2, the energy of the emitted photon will be the difference of energies between these states. The energy of an electron when it goes down is, Now, put the values in the above relation from the given table.