Question

Weekend Challenge Question (General Chemistry)

Answer 1

In an experiment, potassiul fluoride was shown to have an ionic bond. The bond length of of the KF is \(0.217~ nm\). Find the \(\Delta E\), in \(\frac{kJ}{mol}\), for the formation of this potassium fluoride bond from the neutral \(K\) and \(F\) atoms. [NOTE: assume that the potassium and fluorine ions are \(\underline{point~charges}\).

The ionization energies and \(e^-\) affinity ares:
\begin{array}{|l|l|lc|}
\hline
&Ionization~Energy~\frac{kJ}{mol}&Electron ~Affinity~\frac{kJ}{mol}\\
\hline
potassium&418&48\\
\hline
Fluorine &1680&328&\\
\hline
\end{array}

Answer 2

I'd start by deciding which element undergoes oxidation, and which reduction...

Answer 3

When an electrons joins flourine, energy is released as it becomes a bound system.

My guess is.... (418-328)kJ/mol

Though i am not sure what the assumption is for...