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%TCIDATA{<META NAME="Title" CONTENT="Reference/Chemistry/Cs">}
%TCIDATA{Created=Mon Aug 19 14:52:24 1996}
%TCIDATA{LastRevised=Thu Feb 13 18:59:27 1997}
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\subsubsection{Introduction}

Cesium is characterised by a spectrum containing two bright lines in the
blue (accounting for its name). Silvery white in color, it is the most
reactive and (perhaps) the softest of all metals. It is liquid in a warm
room. \ Naturally occurring cesium occurs in minute quantities in the
Earth's crust, 70 times as abundant as silver. \ Cesium reacts explosively
with water and readily combines with oxygen.

\subsubsection{Basic Data}

\begin{tabular}{ll}
Atomic number: & $55$ \\ 
Atomic mass: & $132.90543$ \\ 
Electron configuration: & [Xe]5s$^{\text{1}}$ \\ 
Atomic radius: & $r_{a}=265.5\times 10^{-12}\unit{m}$ \\ 
Melting point: & $T_{m}=301.55\unit{K}$ \\ 
Boiling point: & $T_{b}=951.6\unit{K}$ \\ 
Critical temperature: & $T_{c}=2060\unit{K}$ \\ 
Standard state: & Liquid \\ 
Color: & Silvery white \\ 
Density at 293 K: & $1873\unit{kg}/\unit{m}^{3}$ \\ 
Molar volume: & $70.96\unit{cm}^{3}$%
\end{tabular}

\subsubsection{Name}

\begin{tabular}{|l|l|l|l|l|l|}
\hline
\textbf{US} & \textbf{English} & \textbf{French} & \textbf{German} & \textbf{%
Italian} & \textbf{Spanish} \\ \hline
cesium & caesium & c\'{e}sium & Caesium & cesio & cesio \\ \hline
\end{tabular}

From the Latin word ``caesius'' meaning ``sky blue''

\subsubsection{Historical}

Cesium was discovered spectroscopically by Robert Wilhelm Bunsen and Gustav
Robert Kirchhoff in 1860 in mineral water from Durkheim. Their
identification was based upon two bright blue lines in the spectrum.

\begin{tabular}{ll}
Discoverer: & Gustav Kirchoff, \\ 
& Robert Bunsen \\ 
Date discovered: & 1860 \\ 
Where discovered: & Germany
\end{tabular}

\subsubsection{Uses}

\begin{itemize}
\item  because of its high oxygen affinity, the metal is used as a
``getter'' in electron tubes

\item  used in photoelectric cells

\item  catalyst in the hydrogenation of some organic compounds

\item  the metal can be used in ion propulsion systems. Although not usable
in the earth's atmosphere, 1 kg of caesium in outer space could propel a
vehicle 140 times as far as the burning of the same amount of any known
liquid or solid

\item  used in atomic clocks

\item  IR lamps
\end{itemize}

\subsubsection{Biological}

Cesium has no biological role but is capable of replacing potassium to some
extent if present in excess.

\subsubsection{Dangers}

Cesium compounds are encountered rarely by most people. All cesium compounds
should be regarded as highly toxic because of its chemical similarity to
potassium. Because of this similarity, the isotopes $^{\text{134}}$Cs and $^{%
\text{137}}$Cs (present in the biosphere in small amounts as a result of
radiation leaks) are very toxic. Rats fed cesium in place of potassium in
their diet die.

\subsubsection{Geological}

Cesium occurs in lepidolite and pollucite (a hydrated silicate of aluminum
and cesium), and in other sources.

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