# Why isn't bond dissociation energy/bond enthaply measured in Newtons?

TL;DR Summary
Why isn't average bond dissociation energy/bond enthalpy measured in units of force/Newtons (kg*m/s^2)?
I understand every bond chemically has a length and energy to break, and energy is Newton*meters.
Is the Bond enthaply/Bond disassociation energy equivalent to the force needed to break the bond * the bond length?

Why don't we say, to break the bond from O to H we need to put magnets on left of the O and right of the H and apply some pulling force of XYZ?

Is the Bond enthaply/Bond disassociation energy equivalent to the force needed to break the bond * the bond length?
No, it’s the energy required to move the atoms infinitely far apart. Think of it this way: force is the gradient of energy (derivative of energy with respect to distance)
$$F = \nabla E \left(=\frac{dE}{dx}\right)$$
At the equilibrium bond length, energy is at a minimum, meaning that the gradient (and therefore the force) is zero—this makes sense because a system at equilibrium has no net force acting on it.

TeethWhitener said:
No, it’s the energy required to move the atoms infinitely far apart. Think of it this way: force is the gradient of energy (derivative of energy with respect to distance)
$$F = \nabla E \left(=\frac{dE}{dx}\right)$$
At the equilibrium bond length, energy is at a minimum, meaning that the gradient (and therefore the force) is zero—this makes sense because a system at equilibrium has no net force acting on it.
It's an accepted model to represent atoms diatomic as ball attached to spring attached to ball so equilibrium is false. They can't be infinitely far apart because I can disassociate hydroxide in a small vial of very small size.

It's an accepted model to represent atoms diatomic as ball attached to spring attached to ball so equilibrium is false. They can't be infinitely far apart because I can disassociate hydroxide in a small vial of very small size.
I have no idea where you’re getting this from. I think you’re trying to say that bonds can be modeled as harmonic oscillators. And of course harmonic oscillators have an equilibrium point. It’s at the bottom of the potential well.

Also, the bond dissociation energy is a limit as the distance between atoms goes to infinity. Practically, with most bonds, once atoms are separated by more than a few angstroms they’re essentially dissociated.

Astronuc and berkeman
It's an accepted model to represent atoms diatomic as ball attached to spring attached to ball so equilibrium is false. They can't be infinitely far apart because I can disassociate hydroxide in a small vial of very small size.
The harmonic oscillator is an approximation. And you can in principle model a molecule as a balls on sticks that oscillate like a spring, but it's usually not sufficient for quantum mechanical calculations. Molecular dynamics force fields often model bonds with Hooke's law.

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