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Len [333]
3 years ago
12

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 Zeff=6 for a chlorine atom.
Chemistry
1 answer:
bazaltina [42]3 years ago
7 0

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.

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

where

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

n₁ = lower orbit = 3

n₂ = higher orbit = 4

R_H = Rydyberg constant = 1.09 × 10⁷ m⁻¹

λ = wave length of the light absorbed

∴

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

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

\dfrac{1}{\lambda} = 392400000\times0.0486111111

\dfrac{1}{\lambda} =19075000

\lambda = \dfrac{1}{19075000}

\lambda = \dfrac{1}{1.91\times 10^7 \ m^{-1}}

\lambda = 5.236 \times 10^{-8} m

\lambda = 52.36 \times 10^{-9} m

\lambda = 52.36\  n m

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

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