Excited States of Hydrogen
Suppose a hydrogen atom’s energy is -1.51 eV. How many separate states are available to it? Take into account the possible values of \ell, m, and m_s.
Interpret and Anticipate
This example is much like Example 42.3, where we used the energy-level diagram in Figure 42.7 to find that the principal quantum number in this case is n = 3. Now we must find the possible values for \ell, m, and m_s..
SOLVE
From Table 42.4, use \ell=0,1,2, \ldots(n-1) to find the values for the orbital quantum number when n = 3.
\ell=0,1,2Consulting Table 42.4 again, use m=0, \pm 1, \pm 2, \ldots \pm \ell to find the values for the orbital magnetic quantum number for each possible value of \ell. Count the number of states for each unique value of \ell and m.
\begin{array}{llc}\hline \ell & m & \text { Number of states } \\\hline 0 & 0 & 1 \\1 & -1,0,1 & 3 \\2 & -2,-1,0,1,2 & 5 \\\hline\end{array}For each state, the electron can be either spin up (m_s = 1/2) or spin down (m_s = -1/2). Add up the number of unique states specified by \ell and m, and then multiply by 2.
Number of states = 2(1 + 3 + 5) = 18
CHECK AND THINK
In all 18 of these states, hydrogen has the same energy E (-1.51 eV). So the 18 states form a single shell. This shell is broken into three subshells for the three values of l. Each subshell has the same energy and the same orbital angular momentum L, but within the subshells for \ell=1 \text { and } \ell=2 there is variation in the orbital magnetic moment (\mu_{orbit})_z. In addition, in each state the spin magnetic moment (\mu_{spin})_z is either up or down.
Table 42.4 Allowed values for quantum numbers. | ||
Name | Symbol | Allowed Values |
Principal | n | 1, 2, 3,… |
Orbital | \ell | 0, 1, 2, … (n – 1) |
Orbital magnetic | m | 0, \pm 1, \pm 2, \ldots \pm \ell |
Spin | s | 1 / 2 |
Spin magnetic | m_s | \pm 1 / 2 |