I read that each line on a line spectra for an element represents an energy level. Hydrogen only has 1 electron which is in the first energy level so why are there so many lines on the H line spectrum?

I read that each line on a line spectra for an element represents an energy level. Hydrogen only has 1 electron which is in the first energy level so why are there so many lines on the H line spectrum?

 

The transitions involve different starting and ending states, i.e. you excite the hydrogen in various ways and let it cascade back down to the ground level. It doesn't necessarily de-excite with a single photon emission.

Why does the H line spectrum contain lines that the Na line spectrum doesn't though? Na contains an electron in the exact same energy level that hydrogens electron is located doesn't it?

Why does the H line spectrum contain lines that the Na line spectrum doesn't though? Na contains an electron in the exact same energy level that hydrogens electron is located doesn't it?

 

No. Even though the numbering system is identical and there are electrons in the n=1 state, the actual energy values depend on the amount of charge you have; Na has more protons attracting the electrons.