What is the electronic transition for LiCl using this equation
1/(7.01 ×〖10〗^(-7) )= R_H (1/4- 1/(n_f^2 ))
To determine the electronic transition for LiCl using the given equation, we need to use the Rydberg formula and solve for n_f, the final energy level.
The Rydberg formula is given as:
1/λ = R_H * (1/n_initial^2 - 1/n_final^2)
where λ is the wavelength of the light emitted or absorbed during the electronic transition, R_H is the Rydberg constant, and n_initial and n_final represent the initial and final energy levels.
In this case, the equation given is:
1/(7.01 × 10^(-7)) = R_H * (1/4 - 1/n_f^2)
We can rearrange this equation to solve for n_f:
R_H * (1/n_f^2) = 1/(7.01 × 10^(-7)) - 1/4
Now, let's substitute the value of R_H and solve for n_f:
R_H = 1.097 × 10^7 m^(-1)
(1.097 × 10^7 m^(-1)) * (1/n_f^2) = 1/(7.01 × 10^(-7)) - 1/4
(1/n_f^2) = (1/(7.01 × 10^(-7)) - 1/4) / (1.097 × 10^7 m^(-1))
Now, we can calculate the value of n_f by taking the square root of the reciprocal of the right-hand side:
n_f = √((1/(7.01 × 10^(-7)) - 1/4) / (1.097 × 10^7 m^(-1)))
By substituting the numerical values and evaluating the expression, you can find the electronic transition for LiCl.