What do we mean by electrons emit energy as light when they move to lower energy orbits?

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Solution

When electrons are at higher energy levels, they are unstable because of the high energy they possess in that higher energy levels

After some time, they come back to the original states( ground state ) in which they are stable, emitting the higher energy they had in the higher energy level

This energy emitted is equal to the difference in energies of the two states, that is, the higher energy state and the ground state

This energy is emitted in a frequency that lies in the light region of the Electromagnetic spectrum which can be seen by Electroscopy

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43.56

k c a l / m o l

I

I I

n = n_{1}

3

n = n_{2}

6

E_{2}

E_{1}

E_{2} - E_{1} = Δ E

λ = \frac{h c}{Δ E}

- ν = R Z^{2} (\frac{1}{n_{1}^{2}} - \frac{1}{n_{2}^{2}})

R = 1.097 \times 10^{5} c m^{- 1}

\begin{matrix} List - I & List - II (I) If the ionisation potential for hydrogen-like atom & (P) 5.48 \times 10^{- 32} c R J in a sample is 122.0 e V, then the energy of the last line of Paschen series for this atom is: (II) In a single isolated atom, an electron makes & (Q) 6.6 \times 10^{- 32} c R J transition from fifth excited state such that no spectral lines are observed in the visible range then maximum number of different types of photons observed is: (III) The difference in energy of the second line & (R) 6 of Lyman series and last line of Brackett series in a hydrogen sample is: (IV) The energy of the electromagnetic radiation & (S) 4 emitted during the transition of electron in between the two levels of L i^{2 +} ion whose principal quantum number sum is 4 and difference is 2 is: (T) 6.6 \times 10^{- 34} c R J (U) 0.53 \times 10^{- 30} c R J \end{matrix}

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