Stability Predictions

Chemistry Level 1

Based on bond order, which molecule or ion would you expect to have the shortest bond length and the largest bond energy?

H e X 2 X + \ce{He2+} H X 2 X + \ce{H2^+} H e X 2 \ce{He2} H X 2 \ce{H2}

Jordan Calmes by Jordan Calmes , 33, USA

This section requires Javascript.
You are seeing this because something didn't load right. We suggest you, (a) try refreshing the page, (b) enabling javascript if it is disabled on your browser and, finally, (c) loading the non-javascript version of this page . We're sorry about the hassle.

1 solution

Jordan Calmes
Feb 11, 2016

The bond orders are as follows:

H X 2 \ce{H2} = 1

H X 2 X + \ce{H2^{+}} = 0.5

H e X 2 X + \ce{He2^{+}} =0.5

H e X 2 \ce{He2} = 0

H X 2 \ce{H2} has the highest bond order. It also has the shortest bond length (74 pm) and highest bond energy (436 kJ/mol). H X 2 X + \ce{H2+} and H e X 2 X + \ce{He2^+} have the same bond order, and they both have bond lengths around 100 pm and bond energies around 250 kJ/mol. H e X 2 \ce{He2} has a bond order of 0 and is not observed in nature.

6 Helpful 2 Interesting 0 Brilliant 1 Confused

0 pending reports

×

Problem Loading...

Note Loading...

Set Loading...