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Problem: Formation of the H2 molecule as atomic orbitals overlap.From the graph, what is the bond length in the H2 molecule?

🤓 Based on our data, we think this question is relevant for Professor Howell's class at OSU.

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We’re being asked to determine the bond length in the H2 molecule based on the given diagram:


• as the H–H distance decreases

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Problem Details

A line graph has H-H distance on the X-axis (increasing), and energy (kilojoules per mole) on Y-axis (increasing).  At very short distances, the nucleus-nucleus repulsion is increasingly important.  As the distance increases, the energy rapidly drops; the potential energy decreases with increasing orbital overlap.  The energy decreases far below zero, reaching a minimum of negative 435 kilojoules per mole at an H-H distance of 0.74 angstroms. This point is the balance between attractive and repulsive forces. As the distance then increases further, the potential energy slowly increases, toward an asymptote with 0 kilojoules per mole.

Formation of the H2 molecule as atomic orbitals overlap.

From the graph, what is the bond length in the H2 molecule?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Bond Energy concept. If you need more Bond Energy practice, you can also practice Bond Energy practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Howell's class at OSU.