Answer:
n .= 1 to 4
Explanation:
From the Planck 5
E = hc/lambda
Where lambda is wavelength
E= hf
We will explain the answer here with respect to wavelength. It should be understood that the higher the wavelength of transition, the lower the frequency.
This means that longer transitions will occur at lesser frequencies. From the options the biggest transition is from 2 to 94, while the smallest is from 1 to 4
The transition from 1 to 4 is expected to have the highest energy as it has the shortest wavelength,
Transition from 2 to 94 has the longest wavelength, lowest energy and least frequency
Transition that would absorb the highest energy is n = 2 to n = 9
According to the Bohr model of the atom, an electron in an atom can absorb energy and move from a lower to higher energy level. This energy is emitted when the electron returns to ground state.
The magnitude of energy absorbed or emitted depends on the difference in energy between the two energy levels. The larger the energy difference between the energy levels, the larger the energy absorbed or emitted and vice versa.
The greatest frequency photon is absorbed when the greatest energy transition occurs. This is the transition n = 2 to n = 9.
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