typos fixed thnaks to Zach

1 files changed, 8 insertions, 6 deletions

diff --git a/spectr.tex b/spectr.tex
index 78e6d64..14f4f77 100644
--- a/spectr.tex
+++ b/spectr.tex
@@ -83,15 +83,16 @@ Fig.~\ref{Hspec.fig} shows the energy levels of hydrogen, and indicates a large
 transitions, grouped into series with the common electron final state.  Emitted photon frequencies
 span the spectrum from the UV (UltraViolet) to the IR (InfraRed). Among all the series only the
 Balmer series, corresponding to $n_2$ = 2, has its transitions in the visible part of the spectrum.
-Moreover, from all the possible transitions, we will be able to to observe and measure only the
+Moreover, from all the possible transitions, we will be able to observe and measure only the
 following four lines: $n_1=6 \rightarrow  2$, $5 \rightarrow  2$, $4 \rightarrow 2$,
  and $3 \rightarrow 2$.
 
 \begin{figure}
 \includegraphics[width=0.7\linewidth]{./pdf_figs/spec}
 \caption{\label{Hspec.fig}Spectrum of Hydrogen. The numbers on the left show the energies of the
-hydrogen levels with different principle quantum numbers $n$ in $eV$. The wavelength of emitted
-photon in {\AA}  are shown next to each electron transition. }
+hydrogen levels with different principle quantum numbers $n$ in $eV$. The
+wavelength of the emitted
+photon in {\AA}  is shown next to each electron transition. }
 \end{figure}
 
 %In this lab, the light from the hydrogen gas is broken up into its spectral
@@ -117,7 +118,8 @@ potassium (K), rubidium (Rb), cesium (Cs) and Francium (Fr)]. All these elements
 electron shell with one extra unbound electron. Not surprisingly, the energy level structure for this
 free electron is very similar to that of hydrogen. For example, a Na atom has 11 electrons, and its
 electronic configuration is $1s^22s^22p^63s$.  Ten closed-shell electrons effectively screen the
-nuclear charge number ($Z=11$) to an effective charge $Z^*\approx 1$, so that the $3s$ valent
+nuclear charge number ($Z=11$) to an effective charge $Z^*\approx 1$, so
+that the $3s$ valence
 electron experiences the electric field potential similar to that of a hydrogen atom, given by the
 Eq.~\ref{Hlevels_inf}.
 
@@ -413,7 +415,7 @@ $P_{3/2}$. These two transition frequencies  are very close to each other, and t
 the spectrometer the width of the slit should be very narrow. However, you may not be able to see
 some weaker lines then. In this case you should open the slit wider to let more light in when
 searching for a line. If you can see a spectral line but cannot resolve the doublet, record the
-reading for the center of the spectrometer line, and use the average of two wavelengthes given above.
+reading for the center of the spectrometer line, and use the average of two wavelengths given above.
 
 \textbf{Measurements of the fine structure splitting}. Once you measured all visible spectral lines,
 go back to some bright line (yellow should work well), and close the collimator slit such that you
@@ -571,7 +573,7 @@ with respect to the normal to the plane containing the slits.
 %D}{\lambda}\sin\theta} \right]^2.
 %\end{equation}
 
-An interference on $N$ equidistant slits illuminated by a plane wave
+Interference on $N$ equidistant slits illuminated by a plane wave
 (Fig.~\ref{grating}b) produces much sharper maxima. To find light intensity on
 a screen, the contributions from all N slits must be summarized taking into
 account their acquired phase difference, so that the optical field intensity