Question

Each part of this question asks you about your knowledge of the hydrogen atom spectrum.

Eatom = -2.178 x10-18 J * (1/nf2 - 1/ni2)

Part 1:

Choose the electron transition that has the largest energy.

A) n = 4 → n= 1

B) n = 3 → n= 2

C) n = 4 → n= 3

D) n = 4 → n= 2

E) n = 3 → n= 1

F) n = 2 → n= 1

Part 2:

Choose the electron transition that will emit the photon with the longest wavelength.

A) n = 3 → n= 2

B) n = 4 → n= 3

C) n = 4 → n= 1

D) n = 4 → n= 2

E) n = 3 → n= 1

F) n = 2 → n= 1

Part 3:

Choose the electron transition that produces light in the visible portion of the electromagnetic spectrum.

A) n = 3 → n= 1

B) n = 4 → n= 2

C) n = 2 → n= 1

D) n = 4 → n= 1

E) n = 4 → n= 3

Answer 1

E = R*(1/nf^2 – 1/ni ^2)

R = -2.178*10^-18 J

Nf = final stage/level

Ni = initial stage/level

E = Energy per unit (i.e. J/photon)

larges energy depends therefore on

(1/nf^2 – 1/ni ^2)

then

highest level shown --> 4, therefore, we must hav ehte LOWEST level as well,

verify 4 to 1

, it exist, therefore this has the most energy

Q2

longest wavlength --> least energy

E = hc/WL

largest energy depends therefore on the leas tvalue of:

(1/nf^2 – 1/ni ^2)

choose = 4, then to n = 3

only 1 drop of level, of the highest level will be very low energy

Q3

light visible is from 400 nm to 700 nm

this corresponds to BALMER series, i.e. n = 2 at the end

from the list

4--> 2 aqua color