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| author | Eugeniy Mikhailov <evgmik@gmail.com> | 2014-10-14 09:00:56 -0400 |
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| committer | Eugeniy Mikhailov <evgmik@gmail.com> | 2014-10-14 09:00:56 -0400 |
| commit | 11a83108836f1888304be1c7ec9e76c1e900cefd (patch) | |
| tree | 274ea78780859a1ef046ff6a141662c46e59c169 | |
| parent | 0b6c775c00628073786f29fb9c93d8ada9a901cf (diff) | |
| download | manual_for_Experimental_Atomic_Physics-11a83108836f1888304be1c7ec9e76c1e900cefd.tar.gz manual_for_Experimental_Atomic_Physics-11a83108836f1888304be1c7ec9e76c1e900cefd.zip | |
typos fixed thanks to Caroline and me
| -rw-r--r-- | spectr.tex | 6 |
1 files changed, 3 insertions, 3 deletions
@@ -40,7 +40,7 @@ is a fundamental physical constant called the {\bf Rydberg constant} (here $m_e$ mass). Numerically, ${R_y} = 1.0974 \times 10^5 cm^{-1}$ and $hc{R_y} = 13.605 eV$. Because the allowed energies of an electron in a hydrogen atom, the electron can change its state -only by making a transition (``jump'') from an one state of energy $E_1$ to another state of lower +only by making a transition (``jump'') from one state of energy $E_1$ to another state of lower energy $E_2$ by emitting a photon of energy $h\nu = E_1 - E_2$ that carries away the excess energy. Thus, by exciting atoms into high-energy states using a discharge and then measuring the frequencies of emission one can figure out the energy separation between various energy levels. Since it is @@ -133,7 +133,7 @@ same principle number $n$ but different angular momenta $l$ are split (\emph{i.e energies). -To take onto account the modification of the atomic spectra while still using the same basic +To take into account the modification of the atomic spectra while still using the same basic equations as for the hydrogen, it is convenient to introduce a small correction $\Delta_l$ to the principle quantum number $n$ to take into account the level shifts. This correction is often called a {\it quantum defect}, and its value % an effective nuclei charge $Z^*$ keeping the For each particular value @@ -148,7 +148,7 @@ depends on the angular momentum $l$, and does not vary much between states with quantum numbers $n$ but same $l$\footnote{The accepted notation for different electron angular momentum states is historical, and originates from the days when the proper quantum mechanical description for atomic spectra has not been developed yet. Back then spectroscopists had categorized -atomic spectral lines corresponding to their appearend: for example any spectral lines from electron +atomic spectral lines corresponding to their appearance: for example any spectral lines from electron transitions from $s$-orbital ($l=0$) appeared always \textbf{S}harp on a photographic film, while those with initial electron states of $d$-orbital ( $l=2$) appeared always \textbf{D}iffuse. Also spectral lines of \textbf{P}rinciple series (initial state is $p$-orbital, $l=1$) reproduced the |