Question

1.. Use the energy level diagram for He+ to predict the energy required to move an electron from n=1 to n=2.

Group of answer choices

a. 3936 kJ/mol

b. 1312 kJ/mol

c. 5248 kJ/mol

2.. Use the energy diagram above the for the He⁺ ion to decide which energies can be absorbed by He⁺? (Recall what happens if the energy of a photon overcomes the binding energy!)

Group of answer choices

a. 5500 kJ/mol

b. 5500 kJ/mol and 5248 kJ/mol

c. All three

d. 5248 kJ/mol

e. 3000 kJ/mol

3.. Imagine that you shine light on a collection of hydrogen atoms (the energy diagram is in your notes!). Which statement is correct?

Group of answer choices

a. Only light with wavelengths equal to a multiple of the atomic energy levels can be absorbed.

b. All photons with energy smaller than 1312 kJ/mol can be absorbed.

c. Photons with the energy of 984 kJ/mol are the most energetic photons that can be absorbed.

d. All photons with energy greater than 1312 kJ/mol can be absorbed.

Answer 1

- AE = Eg-E, =-218x18" (watt)?? Delatomet - 2.18 x 1080 (1 1) (212 DE = - 2-18 X 1518 (244 [SE = 6.54815 in

A Elmol = 6.54 X169% 6.0227162I = 3.938 X106J De = 3938 kJ moll option A is correct. 9 To absorb energy for excitation from n=1 to naa - AEC Energy of the phon. so that Photon can supply energy to the election by which - it can reach n=d. 5948 & 5500 KJ/mol both photons will excit the election option b' is correct.

3) As atomic levels are quantized, the photons having energy equal to multiples of the atomic energy levels can be absorbed.

So option A is correct