- #1

Noirchat

- 15

- 0

## Homework Statement

In a set of experiments on a hypothetical one-electron atm, you measure the wavelengths of photons emitted as electrons return to the ground state (n=1), as shown in the energy level diagram. You also observe that it takes 17.50 eV to ionise this atom.

Diagram shows:

n=5 --> n=1 ~ λ = 73.86nm

n=4 --> n=1 ~ λ = 75.63nm

n=3 --> n=1 ~ λ = 79.76nm

n=2 --> n=1 ~ λ = 94.54nm

(i) What is the energy of the atom in each of the levels n=1 to n=5

(ii) If an electron makes a transition from the n=4 to the n=2 level, what wavelength of light would it emit?

## Homework Equations

None provided

## The Attempt at a Solution

My attempt at A

I think i use this equation:

E = -hxR/n^2

where:

h is Planck's constant 6.626 x 10^-34

R is Rydbergs constant 1.097 x 10^7

and n is the energy level

at n=5 i get: -2.907 x 10^-28

at n=4 i get: -4.543 x 10^-28

at n=3 i get: -8.076 x 10^-28

at n=2 i get: -1.817 x 10^-27

at n=1 i get: -7.269 x 10^-27

I think i use balmers equation in part B?

1/λ = R(1/2^2 - 1/4^2) where R= 1.097 x 10^7

1/λ = 2056875

I have a feeling I'm doing this all wrong.