Name: Methods of Representing Electronic Configuration
Uploaded: 2019-07-19
Duration: 11 min 48 s
Description: The electron configuration of an atom is the representation of the arrangement of electrons distributed among the orbital shells and subshells. Learn more.

Question

The Balmer series of spectral lines for hydrogen appear in the visible region. What is the lower energy level that these electronic transitions start from, and what transitions correspond to the spectral lines at

379.0 nm

and

430.0 nm

, respectively?

Accepted Answer

In Balmer series, electrons finally jump from high energy level to lower energy level of $n_{f} = 2$

General equation for wave number and wave length:

$ν = \frac{1}{λ} = R_{H} [\frac{1}{n_{f}^{2}} - \frac{1}{n_{i}^{2}}]$

$R_{H} =$ Rydberg constant $(1.097 \times 10^{7} m^{- 1})$

The energy level (first transition) from which this electronic transition start from is $n_{i} = 3$ .

$\frac{1}{λ} = R_{H} [\frac{1}{n_{f}^{2}} - \frac{1}{n_{i}^{2}}]$

In Balmer series, $n_{f} = 2,$ for $λ = 379 nm$

$\frac{1}{379 \times 10^{- 9} m} = 1.097 \times 10^{7} m^{- 1} [\frac{1}{2^{2}} - \frac{1}{{n_{i}}^{2}}] \frac{1}{4.16} = \frac{1}{4} - \frac{1}{n_{i}^{2}} n_{i} = 10.1 \approx 10$

Spectral line at $379 nm$ correspond to the transition $n = 10 \to n = 2$

$For λ = 430 nm \frac{1}{430 \times 10^{- 9} m} = 1.097 \times 10^{7} m^{- 1} [\frac{1}{2^{2}} - \frac{1}{{n_{i}}^{2}}] \frac{1}{4.71} = \frac{1}{4} - \frac{1}{n_{i}^{2}} n_{i} = 5.1 \approx 5$

Spectral line at $430 nm$ correspond to the transition $n = 5 \to n = 2$

The Balmer series of spectral lines for hydrogen appear in the visible region. What is the lower energy level that these electronic transitions start from, and what transitions correspond to the spectral lines at $379.0 nm$ and $430.0 nm$ , respectively?

Important Questions on Atomic Structure and the Periodic Table

Learn and Prepare for any exam you want !

The Balmer series of spectral lines for hydrogen appear in the visible region. What is the lower energy level that these electronic transitions start from, and what transitions correspond to the spectral lines at 379.0 nm and 430.0 nm, respectively?

Important Questions on Atomic Structure and the Periodic Table

Learn and Prepare for any exam you want !

The Balmer series of spectral lines for hydrogen appear in the visible region. What is the lower energy level that these electronic transitions start from, and what transitions correspond to the spectral lines at $379.0 nm$ and $430.0 nm$ , respectively?