College

We appreciate your visit to Determine the wavelength of the energy that needs to be absorbed for a 3p electron in chlorine to be promoted to the 4s subshell Assume. This page offers clear insights and highlights the essential aspects of the topic. Our goal is to provide a helpful and engaging learning experience. Explore the content and find the answers you need!

Determine the wavelength of the energy that needs to be absorbed for a 3p electron in chlorine to be promoted to the 4s subshell. Assume that [tex]$Z_{\text{eff}} = 6$[/tex] for a chlorine atom.

Answer :

Answer:

The wavelength of the energy that needs to be absorbed = 52.36 nm

Explanation:

For this study;

Let consider the Rydgberg equation from Bohr's theory of atomic model:

i.e.

[tex]\dfrac{1}{\lambda} = R_H (Z^*)^2( \dfrac{1}{n_1^2}-\dfrac{1}{n_2^2})[/tex]

where

Z* = effective nuclear charge of atom = Z - σ = 6

n₁ = lower orbit = 3

n₂ = higher orbit = 4

[tex]R_H[/tex] = Rydyberg constant = 1.09 × 10⁷ m⁻¹

λ = wave length of the light absorbed

∴

[tex]\dfrac{1}{\lambda} = 1.09 \times 10^7}(6)^2( \dfrac{1}{3^2}-\dfrac{1}{4^2})[/tex]

[tex]\dfrac{1}{\lambda} = 1.09 \times 10^7}(36)( \dfrac{1}{9}-\dfrac{1}{16})[/tex]

[tex]\dfrac{1}{\lambda} = 392400000\times0.0486111111[/tex]

[tex]\dfrac{1}{\lambda} =19075000[/tex]

[tex]\lambda = \dfrac{1}{19075000}[/tex]

[tex]\lambda = \dfrac{1}{1.91\times 10^7 \ m^{-1}}[/tex]

[tex]\lambda = 5.236 \times 10^{-8} m[/tex]

[tex]\lambda = 52.36 \times 10^{-9} m[/tex]

[tex]\lambda = 52.36\ n m[/tex]

Therefore, the wavelength of the energy that needs to be absorbed = 52.36 nm

Thanks for taking the time to read Determine the wavelength of the energy that needs to be absorbed for a 3p electron in chlorine to be promoted to the 4s subshell Assume. We hope the insights shared have been valuable and enhanced your understanding of the topic. Don�t hesitate to browse our website for more informative and engaging content!

Rewritten by : Barada

To find the wavelength of the photon absorbed when an electron is promoted from the 3p to the 4s subshell in a chlorine atom, first calculate the energy difference between these levels. Then, use Planck’s equation (E=hc/λ) to find the corresponding wavelength.

The problem is asking us to figure out the wavelength of the photon, which is necessary for promoting an electron in chlorine from the 3p to the 4s subshell. To solve this, we first need to find the energy difference (ΔE) between these shells and then use Planck’s equation E=hc/λ to determine the wavelength of the absorbed photon.

The energy levels of the atomic orbitals can be calculated with the formula E=-hcR(Zeff/n)², where h is Planck’s constant, R is the Rydberg constant, Zeff is the effective nuclear charge, and n is the principal quantum number. After calculating the energy for the 3p (n=3) and 4s (n=4) energy levels, we find the difference between these two levels, which should be the energy of the photon (ΔE) absorbed.

Next, we substitute ΔE into the Planck’s equation (E=hc/λ). After solving for λ, we have the wavelength of the absorbed photon.

Caution should be taken in this process not to switch wavelengths or energy scales in-between the calculations.

For more such question on wavelength visit:

https://brainly.com/question/28995449

#SPJ3