I have no clue what this is asking and how to even do it...when i say no clue I mean...really...blank! Please help. Thank you in advanced.

Four wavelengths of light are each quantized to excite electrons of a given atom to a particular higher energy shell. Assign wavelengths of 496nm, 356nm, 701nm, and 591nm to the shift with which they are most likely associated.

a. n=1 to n=2

b. n=1 to n=4

c. n=1 to n=3

d. n=3 to n=4

Question

I have no clue what this is asking and how to even do it...when i say no clue I mean...really...blank! Please help. Thank you in advanced.

Four wavelengths of light are each quantized to excite electrons of a given atom to a particular higher energy shell. Assign wavelengths of 496nm, 356nm, 701nm, and 591nm to the shift with which they are most likely associated.

a. n=1 to n=2

b. n=1 to n=4

c. n=1 to n=3

d. n=3 to n=4

azureilai · Answer

Well first, keep this in mind. When an electron jumps to a higher level, they require energy. Similarily, when they jump to a lower level, they release energy. This might help with calculations http://physics.bu.edu/~duffy/semester2/c37_energylevels.html