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Chapter 10: Problem 27

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

Short Answer

Expert verified
In the potential energy curve for F2, the energy lowers as the two fluorine atoms approach each other to form a bond, reaching its lowest (most negative) value at the equilibrium bond length. Once the bond becomes too short, the atoms will repel each other, leading to an increase in potential energy, causing the curve to rise.

Step by step solution

01

Understand the concept of a Potential Energy Curve

A potential energy curve graphs the change in potential energy of a molecule as a function of bond length. At infinite separation, the molecule's components (in this case, two fluorine atoms) are at their baseline energy level. As they begin to combine, the potential energy decreases as they stabilize into a molecule. Once the bond becomes too short, the atoms repel each other, leading to an increase in potential energy.
02

Create the Axes of the Graph

Plot the potential energy on the Y-axis and the bond length (or interatomic distance) on the X-axis. Potential energy is usually measured in units of energy like Joules but we can just use a scale since we won't have exact values. Bond length can be measured in nanometres (nm), picometres (pm), Angstroms (Å), etc.
03

Plot the Curve

Start by plotting a point at infinite bond length with zero relative energy. Then, curve down towards a minimum point, which represents the most stable bond length or equilibrium bond length. Once you reach this minimum energy point, curve upwards again to denote how energy increases as bond length decreases further due to repulsion.
04

Annotate the Graph

Mark the lowest point on the curve 'equilibrium bond length', denoting the most energetically stable conformation of the molecule. The minimum energy value is the bond dissociation energy, represented as D0. It's the energy necessary to break one mole of bonds from the equilibrium position to infinity without causing an electronic excitation.

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Most popular questions from this chapter

The allene molecule \(\mathrm{H}_{2} \mathrm{C}=\mathrm{C}=\mathrm{CH}_{2}\) is linear (the three \(\mathrm{C}\) atoms lie on a straight line \() .\) What are the hybridization states of the carbon atoms? Draw diagrams to show the formation of sigma bonds and pi bonds in allene.

Acetylene \(\left(\mathrm{C}_{2} \mathrm{H}_{2}\right)\) has a tendency to lose two protons \(\left(\mathrm{H}^{+}\right)\) and form the carbide ion \(\left(\mathrm{C}_{2}^{2-}\right),\) which is present in a number of ionic compounds, such as \(\mathrm{CaC}_{2}\) and \(\mathrm{MgC}_{2}\). Describe the bonding scheme in the \(\mathrm{C}_{2}^{2-}\) ion in terms of molecular orbital theory. Compare the bond order in \(\mathrm{C}_{2}^{2-}\) with that in \(\mathrm{C}_{2}\).

What are the hybrid orbitals of the carbon atoms in the following molecules? (a) \(\mathrm{H}_{3} \mathrm{C}-\mathrm{CH}_{3}\) (b) \(\mathrm{H}_{3} \mathrm{C}-\mathrm{CH}=\mathrm{CH}_{2}\) (c) \(\mathrm{CH}_{3}-\mathrm{C} \equiv \mathrm{C}-\mathrm{CH}_{2} \mathrm{OH}\) (d) \(\mathrm{CH}_{3} \mathrm{CH}=\mathrm{O}\) (e) \(\mathrm{CH}_{3} \mathrm{COOH}\)

Predict the geometry of the following molecules and ion using the VSEPR model: (a) \(\mathrm{CH}_{3} \mathrm{I},\) (b) \(\mathrm{ClF}_{3}\), (c) \(\mathrm{H}_{2} \mathrm{~S}\) (d) \(\mathrm{SO}_{3},\) (e) \(\mathrm{SO}_{4}^{2-}\)

Which of the following species is not likely to have a tetrahedral shape? (a) \(\operatorname{SiBr}_{4},\) (b) \(\mathrm{NF}_{4}^{+}\) (c) \(\mathrm{SF}_{4}\) (d) \(\mathrm{BeCl}_{4}^{2-},\) (e) \(\mathrm{BF}_{4}^{-},\) (f) \(\mathrm{AlCl}_{4}^{-}\)
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