it is a triple bond. Direct link to mikespar18's post Because Hydrogen has the , Posted 9 months ago. The difference, V, is (8.63) is you have each hydrogen in diatomic hydrogen would have So just based on that, I would say that this is distance between the nuclei. According to Equation 4.1.1, in the first case Q1Q2 = (+1)(1) = 1; in the second case, Q1Q2 = (+3)(1) = 3. Figure below shows two graphs of electrostatic potential energy vs. internuclear distance. And if you were to squeeze them together, you would have to put For ions of opposite charge attraction increases as the charge increases and decreases as the distance between the ions increases. at that point has already reached zero, why is . Daneil Leite said: because the two atoms attract each other that means that the product of Q*q = negative The energy of a system made up of two atoms depends on the distance between their nuclei. The observed internuclear distance in the gas phase is 156 pm. The attractive and repulsive effects are balanced at the minimum point in the curve. Which is which? So in the vertical axis, this is going to be potential energy, potential energy. Direct link to John Smith's post Is it possible for more t, Posted 9 months ago. After a round of introductions, West welcomed the members and guests to the meeting and gave a brief PowerPoint presentation on IUPAC and on the Inorganic Chemistry Division for the benefit of the first-time attendees. What I want to do in this video is do a little bit of a worked example. Kinetic energy is energy an object has due to motion. If you're seeing this message, it means we're having trouble loading external resources on our website. The observed internuclear distance in the gas phase is 244.05 pm. Figure 1. The strength of these interactions is represented by the thickness of the arrows. one right over here. So if you make the distances go apart, you're going to have Substitute the appropriate values into Equation 4.1.1 to obtain the energy released in the formation of a single ion pair and then multiply this value by Avogadros number to obtain the energy released per mole. Because as you get further Because if you let go, they're Potential energy is stored energy within an object. And we'll see in future videos, the smaller the individual atoms and the higher the order of the bonds, so from a single bond to a Careful, bond energy is dependent not only on the sizes of the involved atoms but also the type of bond connecting them. But one interesting question a very small distance. The internuclear distance at which the potential energy minimum occurs defines the bond length. That flow of electrons would be seen as an electric current (the external circuit is all the rest of the circuit apart from the molten sodium chloride.) Inserting the values for Li+F into Equation 4.1.1 (where Q1 = +1, Q2 = 1, and r = 156 pm), we find that the energy associated with the formation of a single pair of Li+F ions is, \( E = k\dfrac{Q_{1}Q_{2}}{r_{0}} = (2.31 \times {10^{ - 28}}\rm{J}\cdot \cancel{m}) \left( \dfrac{( + 1)( - 1)}{156\; \cancel{pm} \times 10^{ - 12} \cancel{m/pm}} \right) = - 1.48 \times 10^{ - 18}\; J/ion\; pair \), Then the energy released per mole of Li+F ion pairs is, \( E=\left ( -1.48 \times 10^{ - 18}\; J/ \cancel{ion pair} \right )\left ( 6.022 \times 10^{ 23}\; \cancel{ion\; pair}/mol\right )=-891\; kJ/mol \) . And that's what people And this distance right over here is going to be a function of two things. Solution of the electronic Schrodinger equation gives the energy as a func-tion of internuclear distance E elec(R). If you're seeing this message, it means we're having trouble loading external resources on our website. The graph is attached with the answer which shows the potential energy between two O atoms vs the distance between the nuclei. Direct link to Shlok Shankar's post Won't the electronegativi, Posted 2 years ago. How come smaller atoms have a shorter stable internuclear distance in a homonuclear molecule? How many grams of gaseous MgCl2 are needed to give the same electrostatic attractive energy as 0.5 mol of gaseous LiCl? a) Why is it not energetically favorable for the two atoms to be to close? energy into the system and have a higher potential energy. If Q1 and Q2 have opposite signs (as in NaCl, for example, where Q1 is +1 for Na+ and Q2 is 1 for Cl), then E is negative, which means that energy is released when oppositely charged ions are brought together from an infinite distance to form an isolated ion pair. bond, triple bond here, you would expect the Remember that the Na+ ions, shown here in purple, will be much smaller than Na atoms, and Cl- ions will be much larger than Cl atoms. Now from yet we can see that we get it as one x 2 times. Imagine what happens to the crystal if a stress is applied which shifts the ion layers slightly. How does the strength of the electrostatic interactions change as the size of the ions increases? is why is it this distance? when you think about it, it's all relative to something else. Figure 4.1.4The unit cell for an NaCl crystal lattice. Then the next highest bond energy, if you look at it carefully, it looks like this purple The vector \(r\) could be the set of the Cartesian coordinates of the atoms, or could also be a set of inter-atomic distances and angles. This creates a smooth energy landscape and chemistry can be viewed from a topology perspective (of particles evolving over "valleys""and passes"). Figure 1. The relation between them is surprisingly simple: \(K = 0.5 V\). Direct link to inirah's post 4:45 I don't understand o, Posted 2 years ago. and weaker and weaker. system as a function of the three H-H distances. what is the difference between potential and kinetic energy. Typically the 12-6 Lennard-Jones parameters (n =12, m =6) are used to model the Van der Waals' forces 1 experienced between two instantaneous dipoles.However, the 12-10 form of this expression (n =12, m =10) can be used to model . Chlorine gas is produced. What is the electrostatic attractive energy (E, in kilojoules) for 130 g of gaseous HgI2? Is it possible for more than 2 atoms to share a bond? Why is that? only has one electron in that first shell, and so it's going to be the smallest. As you go from left to right along a period of the periodic table the elements increase in their effective nuclear charge meaning the valance electrons are pulled in closer to the nucleus leading to a smaller atom. Yep, bond energy & bond enthalpy are one & the same! Marked on the figure are the positions where the force exerted by the spring has the greatest and the least values. What does negative potential energy mean in this context since the repulsive energy at r=0 was positive? Potential Energy vs. Internuclear Distance (Animated) : Dr. Amal K Kumar Dr.Amal K Kumar 3.9K subscribers Subscribe 1.1K 105K views 9 years ago How & why pot. to separate these two atoms, to completely break this bond? On the same graph, carefully sketch a curve that corresponds to potential energy versus internuclear distance for two Br atoms. They're right next to each other. Direct link to Richard's post So a few points here Posted 3 years ago. As a result, the bond gets closer to each other as well." It can be used to theoretically explore properties of structures composed of atoms, for example, finding the minimum energy shape of a molecule or computing the rates of a chemical reaction. Direct link to Richard's post When considering a chemic. b) What does the zero energy line mean? The type, strength, and directionality of atomic bonding . For +3/3 ions, Q1Q2 = (+3)(3) = 9, so E will be nine times larger than for the +1/1 ions. distance between atoms, typically within a molecule. Which will result in the release of more energy: the interaction of a gaseous chloride ion with a gaseous sodium ion or a gaseous potassium ion? you say, okay, oxygen, you have one extra electron However, a reaction and hence the corresponding PESs do not depend of the absolute position of the reaction, only the relative positions (internal degrees). If you look at it, the single bond, double The energy minimum energy Table of Contents of Bonds / no. What is "equilibrium bond length"? Direct link to Taimas's post If diatomic nitrogen has , Posted 9 months ago. Direct link to Frank Wang's post "your radius for an atom , Posted 2 months ago. The distinguishing feature of these lattices is that they are space filling, there are no voids. The low point in potential energy is what you would typically observe that diatomic molecule's Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. The meeting was called to order by Division President West at ca. Below is an app from pHet which illustrates the same point for neutral atoms. Ionic substances all have high melting and boiling points. So let's call this zero right over here. energy of the spring if you want to pull the spring apart, you would also have to do it A class simple physics example of these two in action is whenever you hold an object above the ground. Why do the atoms attract when they're far apart, then start repelling when they're near? Meanwhile, chloride ions are attracted to the positive electrode (the anode). to squeeze them together? The Morse potential U (r) D e. 1 e . r R e 2 . This plays the role of a potential energy function for motion of the nuclei V(R), as sketched in Fig. - [Instructor] If you The number of neutrons in the nucleus increases b. To quantitatively describe the energetic factors involved in the formation of an ionic bond. What is the relationship between the electrostatic attractive energy between charged particles and the distance between the particles? The bond energy \(E\) has half the magnitude of the fall in potential energy. This is the energy released when 1 mol of gaseous ion pairs is formed, not when 1 mol of positive and negative ions condenses to form a crystalline lattice. One is for a pair of potassium and chloride ions, and the other is for a pair of potassium and fluoride ions. Conventionally, potential-energy curves are fit by the simple Morse functions, (ln2) although it has long been realized that this function often gives a poor fit at internuclear distances somewhat greater than the equilibrium distance. An example is. Direct link to Is Better Than 's post Why is it the case that w, Posted 3 months ago. Potential energy starts high at first because the atoms are so close to eachother they are repelling. Thinking about this in three dimensions this turns out to be a bit complex. The potential energy related to any object depends upon the weight of the object due to gravity and the height of the object from the ground. The attractive energy E a and the repulsive energy energy E r of an Na + Cl - pair depends on the inter-atomic distance, r according to the following equations: E a = 1.436 r E r = 7.32 10 6 r 8 The total bond energy, E n is the sum of the attractive energy term E a and the repulsive energy term E r: E n = E a + E r However, the large negative value indicates that bringing positive and negative ions together is energetically very favorable, whether an ion pair or a crystalline lattice is formed. On the Fluorine Molecule. Which will result in the release of more energy: the interaction of a gaseous sodium ion with a gaseous oxide ion or the interaction of a gaseous sodium ion with a gaseous bromide ion? At distances of several atomic diameters attractive forces dominate, whereas at very close approaches the force is repulsive, causing the energy to rise. The figure below is the plot of potential energy versus internuclear distance (d) of H 2 molecule in the electronic ground state. Attractive forces operate between all atoms, but unless the potential energy minimum is at least of the order of RT, the two atoms will not be able to withstand the disruptive influence of thermal energy long enough to result in an identifiable molecule. Won't the electronegativity of oxygen (which is greater than nitrogen )play any role in this graph? of Bonds, Posted 9 months ago. Well, we looked at Calculate the amount of energy released when 1 mol of gaseous Li+F ion pairs is formed from the separated ions. And just as a refresher of The internuclear distance at which the potential energy minimum occurs defines the bond length. completely pulling them apart. with each other. So that's one hydrogen atom, and that is another hydrogen atom. February 27, 2023 By scottish gaelic translator By scottish gaelic translator Thus, E will be three times larger for the +3/1 ions. energy is released during covalent bond formation? point in potential energy. becomes zero for a certain inter-molecular distance? Lets consider the energy released when a gaseous Na+ ion and a gaseous Cl ion are brought together from r = to r = r0. \n \n The PES concept finds application in fields such as chemistry and physics, especially in the theoretical sub-branches of these subjects. The points of maximum and minimum attraction in the curve between potential energy ( U) and distance ( r) of a diatomic molecules are respectively Medium View solution > The given figure shows a plot of potential energy function U(x) =kx 2 where x= displacement and k = constant. So this is at the point negative - 27895391. sarahussainalzarooni sarahussainalzarooni 06.11.2020 . So, no, the molecules will not get closer and closer as it reaches equilibrium. However, in General Relativity, energy, of any kind, produces gravitational field. So this one right over here, this looks like diatomic nitrogen to me. Now, what we're going to do in this video is think about the By chance we might just as well have centered the diagram around a chloride ion - that, of course, would be touched by 6 sodium ions. molecular hydrogen, or H2, which is just two hydrogens { "Chapter_4.0:_What_is_a_Chemical_Bond" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Chapter_4.1:_Ionic_Bonding" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Chapter_4.2:_Lattice_Energies_in_Ionic_Solids" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Chapter_4.3:_Chemical_Formulas" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Chapter_4.4:_Naming_Ionic_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Chapter_4.5:_End_of_Chapter_Material" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "Chapter_4:_Ionic_Bonding" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Chapter_5:_Covalent_Bonding" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Chapter_6:_Molecular_Geometry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "hypothesis:yes", "showtoc:yes", "license:ccbyncsa", "authorname:anonymous", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FCourses%2FHoward_University%2FGeneral_Chemistry%253A_An_Atoms_First_Approach%2FUnit_2%253A__Molecular_Structure%2FChapter_4%253A_Ionic_Bonding%2FChapter_4.1%253A_Ionic_Bonding, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), Chapter 4.2: Lattice Energies in Ionic Solids, Sodium chloride has a high melting and boiling point, The electrical behavior of sodium chloride, status page at https://status.libretexts.org. Direct link to kristofferlf's post How come smaller atoms ha, Posted 2 years ago. And so if you just look at that trend, as you go from nitrogen to oxygen, you would actually See Calculate Number of Vibrational Modes to get a more details picture of how this applies to calculating the number of vibrations in a molecule. diatomic molecule or N2. about is the bond order between these atoms, and I'll give you a little bit of a hint. about, pause this video, is which graph is the potential energy as a function of internuclear distance for each of these diatomic molecules. Direct link to Tzviofen 's post So what is the distance b, Posted 2 years ago. The potential energy function for the force between two atoms in a diatomic molecule which is approximately given as, U (x)= a x12 b x6. A comparison is made between the QMRC and the corresponding bond-order reaction coordinates (BORC) derived by applying the Pauling bond-order concept . From the graph shown, Y2 = N2, X2 = O2, Z2 = H2. Molten sodium chloride conducts electricity because of the movement of the ions in the melt, and the discharge of the ions at the electrodes. This molecule's only made up of hydrogen, but it's two atoms of hydrogen. The best example of this I can think of is something called hapticity in organometallic chemistry. expect your atomic radius to get a little bit smaller. Thus, in the process called electrolysis, sodium and chlorine are produced. Figure 4.1.5 Cleaving an ionic crystal. Yeah you're correct, Sal misspoke when he said it would take 432 kJ of energy to break apart one molecule when he probably meant that it does that amount of energy to break apart one mol of those molecules. This diagram is easy enough to draw with a computer, but extremely difficult to draw convincingly by hand. Answer: 3180 kJ/mol = 3.18 103 kJ/mol. Now we would like to verify that it is in fact a probability mass function. used to construct a molecular potential energy curve, a graph that shows how the energy of the molecule varies as bond lengths and bond angles are changed. The negative value indicates that energy is released. An example is the PES for water molecule (Figure \(\PageIndex{1}\)) that show the energy minimum corresponding to optimized molecular structure for water- O-H bond length of 0.0958 nm and H-O-H bond angle of 104.5. And if they could share A sodium ion has a +1 charge; an oxide ion, a 2 charge; and a bromide ion, a 1 charge. In the example given, Q1 = +1(1.6022 1019 C) and Q2 = 1(1.6022 1019 C). If we get a periodic The following graph shows the potential energy of two nitrogen atoms versus the distance between their nuclei. If the atoms were any closer to each other, the net force would be repulsive. very close together (at a distance that is. internuclear distance graphs. The quantum-mechanically derived reaction coordinates (QMRC) for the proton transfer in (NHN)+ hydrogen bonds have been derived from ab initio calculations of potential-energy surfaces. Coulomb forces are increasing between that outermost Graphed below is the potential energy of a spring-mass system vs. deformation amount of the spring. What are the predominant interactions when oppositely charged ions are. If you're behind a web filter, please make sure that the domains *.kastatic.org and *.kasandbox.org are unblocked. temperature, pressure, the distance between around the internuclear line the orbital still looks the same. Potential, Kinetic, and Total Energy for a System. a row, your radius decreases. The mechanical energy of the object is conserved, E= K+ U, E = K + U, and the potential energy, with respect to zero at ground level, is U (y) = mgy, U ( y) = m g y, which is a straight line through the origin with slope mg m g. In the graph shown in Figure, the x -axis is the height above the ground y and the y -axis is the object's energy. But as you go to the right on If one mole (6.022 E23 molecules) requires 432 kJ, then wouldn't a single molecule require much less (like 432 kJ/6.022 E23)? just a little bit more, even though they might In the minimum of a potential energy curve, the gradient is zero and thus the net force is zero - the particles are stable. And to think about why that makes sense, imagine a spring right over here. We can thus write the Schrodinger equation for vibration h2 2 d2 dR2 +V(R) (R) = E(R) (15) Graph Between Potential Energy and Internuclear Distance Graphs of potential energy as a function of position are useful in understanding the properties of a chemical bond between two atoms. In NaCl, of course, an electron is transferred from each sodium atom to a chlorine atom leaving Na+ and Cl-. It might be helpful to review previous videos, like this one covering bond length and bond energy. Transcribed Image Text: (c) A graph of potential energy versus internuclear distance for two Cl atoms is given below. A potential energy surface (PES) describes the potential energy of a system, especially a collection of atoms, in terms of certain parameters, normally the positions of the atoms. The bond energy is energy that must be added from the minimum of the 'potential energy well' to the point of zero energy, which represents the two atoms being infinitely . 7. A PES is a conceptual tool for aiding the analysis of molecular geometry and chemical reaction dynamics. This page titled Chapter 4.1: Ionic Bonding is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by Anonymous. In the above graph, I was confused at the point where the internuclear distance increases and potential energy become zero. The power source (the battery or whatever) moves electrons along the wire in the external circuit so that the number of electrons is the same. it in the previous video. Hard Calculate the amount of energy released when 1 mol of gaseous MgO ion pairs is formed from the separated ions. And why, why are you having The nuclear force (or nucleon-nucleon interaction, residual strong force, or, historically, strong nuclear force) is a force that acts between the protons and neutrons of atoms.Neutrons and protons, both nucleons, are affected by the nuclear force almost identically. The potential-energy-force relationship tells us that the force should then be negative, which means to the left. Over here, I have three potential energies as a function of Between any two minima (valley bottoms) the lowest energy path will pass through a maximum at a. The major difference between the curves for the ionic attraction and the neutral atoms is that the force between the ions is much stronger and thus the depth of the well much deeper, We will revisit this app when we talk about bonds that are not ionic. And so it would be this energy. The energy as a function of internuclear distance can be animated by clicking on the forward arrow at the bottom left corner of the screen. It is a low point in this Legal. But the other thing to think The positive sodium ions move towards the negatively charged electrode (the cathode). This is more correctly known as the equilibrium bond length, because thermal motion causes the two atoms to vibrate about this distance. There is a position with lowest potential energy that corresponds to the most stable position. Methods of calculating the energy of a particular atomic arrangement of atoms are well described in the computational chemistry article, and the emphasis here will be on finding approximations of \((V(r)\) to yield fine-grained energy-position information. Direct link to Richard's post Potential energy is store, Posted a year ago. Direct link to allie's post can two atoms share a bon, Posted 5 months ago. where m and n are integers, and C n and C m are constants whose values depend on the depth of the energy well and the equilibrium separation of the two atoms' nuclei. As shown by the green curve in the lower half of Figure 4.1.2 predicts that the maximum energy is released when the ions are infinitely close to each other, at r = 0. And to think about that, I'm gonna make a little bit of a graph that deals with potential be a little bit bigger. Consequently, in accordance with Equation 4.1.1, much more energy is released when 1 mol of gaseous Li+F ion pairs is formed (891 kJ/mol) than when 1 mol of gaseous Na+Cl ion pairs is formed (589 kJ/mol). The bond energy is energy that must be added from the minimum of the 'potential energy well' to the point of zero energy, which represents the two atoms being infinitely far apart, or, practically speaking, not bonded to each other. lowest potential energy, is shortest for the diatomic molecule that's made up of the smallest atoms. Bond Order = No. The resulting curve from this equation looks very similar to the potential energy curve of a bond. A diatomic molecule can be represented using a potential energy curve, which graphs potential energy versus the distance between the two atoms (called the internuclear distance). found that from reddit but its a good explanation lol. The minimum potential energy occurs at an internuclear distance of 75pm, which corresponds to the length of the stable bond that forms between the two atoms. candidate for diatomic hydrogen. Now, what if we think about shell and your nucleus. What happens at the point when P.E. In this question we can see that the last to find the integration of exodus to de power two points one. They're close in atomic radius, but this is what makes Part 3. 6. Is it the energy I have to put in the NaCl molecule to separate the, It is the energy required to separate the. And let's give this in picometers. -Internuclear Distance Potential Energy. Because of long-range interactions in the lattice structure, this energy does not correspond directly to the lattice energy of the crystalline solid. good with this labeling. Here Sal is using kilojoules (specifically kilojoules per mole) as his unit of energy. Potential energy is stored energy within an object. This right over here is the bond energy. for diatomic hydrogen, this difference between zero The relative energies of the molecular orbitals commonly are given at the equilibrium internuclear separation. Potential energy and kinetic energy Quantum theory tells us that an electron in an atom possesses kinetic energy \(K\) as well as potential energy \(V\), so the total energy \(E\) is always the sum of the two: \(E = V + K\). their valence electrons, they can both feel like they Chlorine forms shorter, stronger, more stable bonds with hydrogen than bromine does. Molecular and ionic compound structure and properties, https://www.khanacademy.org/science/ap-chemistry-beta/x2eef969c74e0d802:molecular-and-ionic-compound-structure-and-properties/x2eef969c74e0d802:intramolecular-force-and-potential-energy/v/bond-length-and-bond-energy, Creative Commons Attribution/Non-Commercial/Share-Alike. were to find a pure sample of hydrogen, odds are that the individual The closer the atoms come to each other, the lower the potential energy. And for diatomic oxygen, towards some value, and that value's Direct link to asumesh03's post What is bond order and ho, Posted 2 years ago. It would be this energy right over here, or 432 kilojoules. Direct link to Iron Programming's post Yep, bond energy & bond e, Posted 3 years ago. This distance is the same as the experimentally measured bond distance. If I understand your question then you asking if it's possible for something like three atoms to be connected to each other by the same bond. And so that's why they like to think about that as you see this high bond energy, that's the biggest And actually, let me now give units. The figure below is the plot of potential energy versus internuclear distance of H2 molecule in the electronic ground state.