[funstrike123]

The transition of an electron from a higher level to a lower level results in the emission of a photon of wavelength 350.0 nm. If the energy of the higher level is -3.24 x 10^-19 J, calculate the energy of the lower level.

By using E = hv

I find E = 5.679 x 10^-28 J

How do I use this value to solve the qus?

[Corribus]

What's the relationship between the frequency and wavelength of light?

EDIT: Sorry, I should have paid more attention. I see you already figured that much out.

The transition energy is given by

ΔE = E(upper) - E(lower)

If you know what the upper energy level is, and you know what the transition energy ΔE is, then the energy of the lower energy state is easily determined by subtracting the one from the other.

[funstrike123]

What's the relationship between the frequency and wavelength of light?

speed of light = wavelength x frequency?

I used that to find E = 5.679 x 10^-28 J

Is this the answer already? omg I'm confused

[Corribus]

Sorry, I didn't read your first post well enough. Please see my edit above. But do be careful with your units.

[funstrike123]

Sorry, I didn't read your first post well enough. Please see my edit above. But do be careful with your units.

Thanks for your hint! I spent hours figuring out why my value is so small.
1nm = 10^-9 m. I see why now.