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Chapter 10: Problem 25

Draw a potential energy curve for the bond formation in \(\mathrm{F}_{2}\).

Short Answer

Expert verified
The potential energy curve for \(\mathrm{F}_{2}\) bond formation starts at a higher energy when the atoms are separated, decreases to a minimum point indicating the most stable bond length, and then rises sharply as the atoms get too close and repulsions dominate.

Step by step solution

01

Understanding potential energy curve

A potential energy curve is a graph that shows the change in the potential energy of a system as a function of some variable, typically interatomic distance. The valley or trough of the curve represents the most stable point of the system, where the potential energy is at its minimum.
02

Understanding \(\mathrm{F}_{2}\) bond formation

Bond formation in \(\mathrm{F}_{2}\) involves the pairing of two unpaired electrons, one from each Fluorine atom. As two Fluorine atoms approach each other, the electron-proton attractions lower the potential energy of the system. Repulsions (electron-electron and proton-proton) also occur, but the attractions are stronger so the potential energy still decreases overall. Once the atoms are in contact, repulsions begin to take over, and the potential energy starts to rise if the atoms get any closer.
03

Creating potential energy curve

On the x-axis, indicate the separation distance of the two atoms, with higher values to the right. On the y-axis, mark the potential energy. Start from a high point on the y-axis (representing separated atoms). With decreasing separation distance (moving to the left), the energy should initially decrease, reaching a minimum point (the bond length) and then rise sharply as the atoms get too close and the repulsion takes over.

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Most popular questions from this chapter

Draw the Lewis structure of ketene \(\left(\mathrm{C}_{2} \mathrm{H}_{2} \mathrm{O}\right)\) and describe the hybridization states of the \(\mathrm{C}\) atoms. The molecule does not contain \(\mathrm{O}-\mathrm{H}\) bonds. On separate diagrams, sketch the formation of sigma and pi bonds.

Describe the hybridization of phosphorus in \(\mathrm{PF}_{5}\).

Write the ground-state electron configuration for \(\mathrm{B}_{2}\). Is the molecule diamagnetic or paramagnetic?

Describe the bonding scheme of the \(\mathrm{AsH}_{3}\) molecule in terms of hybridization.

What is the relationship between the dipole moment and bond moment? How is it possible for a molecule to have bond moments and yet be nonpolar?
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