Radiant energy is emitted when an electron of a particular atom jumps from a higher energy level to a lower energy level. If the energy released by the transition is 3.68 x 10-19 J, what atom is most likely involved?
Select one:
a. Copper – Green Light (approximately 520-565 nm)
b. Barium – Yellow Light (approximately 565-590 nm)
c. Sodium – Red-Orange Light (approximately 615-635 nm)
d. Potassium – Violet Light (approximately 380-420 nm)

Question

Radiant energy is emitted when an electron of a particular atom jumps from a higher energy level to a lower energy level. If the energy released by the transition is 3.68 x 10-19 J, what atom is most likely involved?
Select one:
a. Copper – Green Light (approximately 520-565 nm)
b. Barium – Yellow Light (approximately 565-590 nm)
c. Sodium – Red-Orange Light (approximately 615-635 nm)
d. Potassium – Violet Light (approximately 380-420 nm)

kainui · Answer

Well, if you know the relation between energy and frequency and the relation between frequency and wavelength, it's a little algebra between here and there to get the answer. Try your best and I'll help you along to figure it out, don't be afraid to guess.

anonymous · Answer

I don't know the relations...Is there a formula to them?

anonymous · Answer

Nevermind, I figured it out. The answer is a

kainui · Answer

Oh ok, I didn't calculate it out but if you're confident, I am too.