# Orbital Quantum Numbers And Total Electron Energy

**1. The problem statement, all variables and given/known data**

The orbital quantum number for the electron in the hydrogen atom is l = 4. What

is the smallest possible value (in eV) for the total energy of this electron? (Use the

quantum mechanical model of the hydrogen atom.)

**2. Relevant equations**

**3. The attempt at a solution**

I know that the angular momentum of the electron is given by;

[itex]L = \sqrt{l(l + 1)}\frac{h}{2 \pi}[/itex]

[itex]L = \sqrt{20} \frac{h}{2 \pi}[/itex]

L = 4.64×10^{-33} Kgm^{2}s^{-1}

My text book doesn’t really discuss the QM picture of the atom, so I don’t know how to relate this to the energy of the electron.

I know how to do it for the Bohr model, but clearly that’s no good.

I appreciate any help you can give,

thanks!

http://ift.tt/1faxeBK

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