Atomic Energy Levels: Calculating Hydrogen's 5 Lowest Levels

[Jeebus]

Homework Statement

Calculate the five (5) lowest energy levels for the hydrogen atom using Bohr's model.

Homework Equations

E_{n}= -2\xime^4 Z^2/h^2 n^2[\tex]<br /> <br /> = -(2.178\times10^18 J)Z^2/n^2[\tex]&lt;br /&gt; &lt;br /&gt; &lt;h2&gt;The Attempt at a Solution&lt;/h2&gt;&lt;br /&gt; &lt;br /&gt; I get how to attempt it but how can there be 5 lowest energy levels when hydrogen has only one energy level. I&amp;#039;m puzzled.

 

[Redbelly98]

Homework Statement

Calculate the five (5) lowest energy levels for the hydrogen atom using Bohr's model.

Homework Equations

E_{n}= -2\xime^4 Z^2/h^2 n^2

= -(2.178\times10^18 J)Z^2/n^2

The Attempt at a Solution

I get how to attempt it but how can there be 5 lowest energy levels when hydrogen has only one energy level. I'm puzzled.

Hydrogen has infinitely many energy levels, corresponding to n=1,2,3,etc.

Why did you think there is only one level?

 

[gutti]

Electron arrangement of hydrogen and drawing it out basically only shows one ring.
Thinks that this is the only energy level.
Thats my guess, I got confused about that when I first started the topic.

P.S. Eventually has an ionisation level does it not? so not infinite energy levels.

 

[Redbelly98]

Typically, you will see diagrams showing an atom in it's lowest-energy state. I am guessing this is the figure you have seen. However, there are in fact more energy levels -- infinitely many -- between this lowest energy and the ionization level.

Normally an atom will be in the lowest-energy state most of the time. But it is possible to excite the atom into the higher states (without ionizing it), for example by shining light of the appropriate wavelength at the atom.

EDIT: adding links
http://hyperphysics.phy-astr.gsu.edu/hbase/hyde.html#c2
http://www.bpreid.com/applets/hel.html