<p>Hi can somebody please help me with the following AP chem questions? I'm stuck on these...</p>
<ol>
<li><p>What common characteristics do the lines in the Balmer series have?</p></li>
<li><p>Fundamentally, why must all the lines in the hydrogen spectrum between 250 and 700nm belong to the Balmer series?</p></li>
<li><p>In the normal, hydrogen atom the electron is in the lowest energy state, which is the ground state. The maximum electronic energy that a hydrogen atom can have is 0 kJ/mole at which point the electron would essentially be removed from the atom and it would become a H+ ion. How much energy in kJ/moles does it take to ionize a H atom?
The ionization energy of hydrogen is often expressed in units other than kJ/mole. What would it be in J/atom? </p></li>
</ol>
<p>My class didn’t go very in-depth into the Balmer series, but the lines the different series and in the atomic emission spectrum of an H atom are meant to relate to the energy differences between the different energy levels. </p>
<p>When you’re talking about “ionization energy,” I’m going to assume that mean the energy that will be absorbed or emitted in order to excite an electron or allow it to fall back to its ground state. In that case you use the Rydberg equation: E = Rh (1/n^2), where Rh is the constant -2.18 x 10^18 and n is the energy level. Note that as n increases, the total energy becomes less negative and approaches 0.</p>