Alright, so here's the problem.
"If a helium atom absorbs a photon with a wavelength of 58.44 nm, one electron will be promoted from the 1s orbital to the 2p orbital.
A) Find the energy, in J, gained by a helium atom undergoing this transition."
First part's easy. E = hc/wavelength. The answer in the answer key is 3.399 x 10^-19, but I'm only getting 3.4 x 10^-18. Could it be a typo or am I doing something wrong:
E = [(6.626*10^-34 Js)(3*10^8 m)]/(58.44*10^-9 m).
However, B) is confusing me.
"The ionization energy of helium is 2372 kJ/mol. Suppose that a helium atom has already undergone the transition above, so that it has one electron in a 2p level. What is the longest wavelength of light that would be capable of supplying enough energy to eject an electron from this excited helium atom, producing a He+ ion?"
I'm assuming I'm going to have to use my result from part A, as well as the ionization energy that they gave me, but I have no idea what to do with them. Any advice?
"If a helium atom absorbs a photon with a wavelength of 58.44 nm, one electron will be promoted from the 1s orbital to the 2p orbital.
A) Find the energy, in J, gained by a helium atom undergoing this transition."
First part's easy. E = hc/wavelength. The answer in the answer key is 3.399 x 10^-19, but I'm only getting 3.4 x 10^-18. Could it be a typo or am I doing something wrong:
E = [(6.626*10^-34 Js)(3*10^8 m)]/(58.44*10^-9 m).
However, B) is confusing me.
"The ionization energy of helium is 2372 kJ/mol. Suppose that a helium atom has already undergone the transition above, so that it has one electron in a 2p level. What is the longest wavelength of light that would be capable of supplying enough energy to eject an electron from this excited helium atom, producing a He+ ion?"
I'm assuming I'm going to have to use my result from part A, as well as the ionization energy that they gave me, but I have no idea what to do with them. Any advice?