As long as that last part of the question is not meant as a trap (which would be even more awful), it alone shows that the exercise is not well-thought about. The octet rule states that an atom should have eight electrons in its outer shell to be sta… But enough of the commentary, let's clear up some issues. Whether those orbitals are essentially bonding or not, is an entirely different question. (Where $\operatorname{sinc}(x)=\dfrac{\sin (\pi x)}{\pi x... the three-electron bond they assumed in between. Hybridisation Of Clo2. A bit more precise: The electron density of α-spin electrons is different from that of β-spin electrons. That is why I find this question incredibly difficult to answer and why I find that Nuclear Chemist's answer dangerous, because it propagates myths about bonding that have been disproved already. HSO3FWhich one of the following is the correct sequence of their acid strength? . This ground state will have a complicated bonding situation. If chlorine turns into a cationic centre, it keeps its sp 3 hybridization and can be able to accept two fluorine atoms. Therefore the two oxygen will use one sp-orbital to form a σ-bond towards chlorine, the other one is an in-plane-σ-lone-pair. I know this doesn't really answer your question, and this is not very satisfactory either, but this is science: It often gives you more questions than answers. To know about it, we have to look at each atom of CO2. What is my mistake? meaning - Difference between 目覚める and 起きる. In the very least you would have to consider two different hybridisation schemes at once.All possible states (that is independent of any hybridisation model) then will be in superposition to form the actual ground state. The valence electron configuration of O is [He]2s22p4. In this simplified and assumption riddled thought-experiment, the π-bonding will form three molecular orbitals pictured below. (There are plentiful discussions about this on chemistry.se alone. In all these ions, the sum of the lone pairs of electrons and bonding domains on C l atom is 4. If you look close enough you will realise, that writing a valid Lewis structure of the molecule is not that hard, and you don't even need π-bonds in the first place.These are solely dictated by symmetry. C l O X 2 has 2 σ bonds, 1 lone pair, 2π bonds and 1 odd electron. Source(s): https://owly.im/a9MvK. Dear User, ClO 2 - has sp 3 hybridisation. By using our site, you acknowledge that you have read and understand our Cookie Policy, Privacy Policy, and our Terms of Service. These unpaired electrons then form sigma bonds with the oxygen atoms. Chemistry Stack Exchange is a question and answer site for scientists, academics, teachers, and students in the field of chemistry. This ground state will have a complicated bonding situation. How do Ethiopian Jews see the Book of Jubilees? Find the hybridization as well identify the pπ-pπ as well as pπ-dπ bonds in $\ce{ClO2}$. The O-Cl-O angle is 116.2 degrees. One obvious fault in the question is that there is no involvement of d-orbitals whatsoever in the molecules. The two chlorines about 120 degrees from each other. What is my mistake? H3O+iii. Each oxygen atom ($\ce{O}$) brings six electrons and the chlorine ($\ce{Cl}$) has seven electrons. Methane (CH 4) is a non-polar hydrocarbon compound composed out of a single carbon atom and 4 hydrogen atoms. Are there any gambits where I HAVE to decline? There is one remaining out-of-plane-p-orbital per oxygen. This could allow us to get a better idea of where the unpaired electron is. Is copying a lot of files bad for the cpu or computer in any way, Squaring a square and discrete Ricci flow. Let's just assume that this is the case. This answer is propagating those myths in chemistry which gives thousands of students the wrong idea of chemical bonding. During hybridization, two 3p orbitals and one 3s orbital get hybridized. This all was deduced from a very reduced and simplified set of theory; the reality is probably by far more complicated. 3) Which of the following chemical reactions depicts the oxidizing behaviour of H2SO4? Two $\sigma$ bonds each holding two electrons connecting oxygen ($\ce{O}$) atoms to the chlorine ($\ce{Cl}$). In the very least you would have to consider two different hybridisation schemes at once. If you look close enough you will realise, that writing a valid Lewis structure of the molecule is not that hard, and you don't even need π-bonds in the first place. (a) The total number of valence electrons in is 19 (7 electrons from Cl and 6 electrons from each O).. Write the Lewis structure for:. Two $\pi$ bonds each holding two electrons connecting oxygen ($\ce{O}$) atoms to the chlorine ($\ce{Cl}$). -1 for expanding octet, -1 for increased ability of the lone pairs to repel. Some of the greatest minds of (theoretical) chemistry have been puzzled about $\bf\ce{ClO2}$, and we have not even started to discuss the three-electron bond they assumed in between. Wiki User Answered . I have never before heard/read about something as a $sp^5$ hybridization. Stack Exchange network consists of 176 Q&A communities including Stack Overflow, the largest, most trusted online community for developers to learn, share their knowledge, and build their careers. In sp hybridization, one s orbital and one p orbital hybridize to form two sp orbitals, each consisting of 50% s character and 50% p character. 87% (171 ratings) Problem Details. Observe each of the regions around the particles to understand about the hybridization of the CO2 molecules. The π-orbitals will therefore be entirely composed out of p-orbitals of the involved elements. pronunciation - When does /r/ become a trill? Asking for help, clarification, or responding to other answers. kana - How to hear the difference between て and で,... downsampling - trying to downsample audio. passover - Why must the child ask these four quest... grammar - Difference between 変{か}わり and 変{か}える, organic chemistry - Numbering in chlordiazepoxide. What is the hybridization of chlorine in each of the following: Why can't we use the same tank to hold fuel for both the RCS Thrusters and the Main engine for a deep-space mission? I am sure that for the pi system we need to use MO theroy and the the best I have come up with is that a pi star orbitial has a single electron in it. How can I pay respect for a recently deceased team member without seeming intrusive? ClO2 needs MO, and 3-electron-2-center bonds to make even close to sense, and the woefully inadequate vsepr theory or hybridisation will not be enough. From Coulson's theorem we can actually calculate what hybrid orbitals are necessary. A1 symmetry, two py orbitals. See the answer. How does the compiler evaluate constexpr functions so quickly? Essentially the stabilisation from the π-bonds itself should be small, and could be described as π-backbonding, or is similar to negative hyperconjugation; maybe negative π-backbonding (!?). Hybridisation is equal to number of $\sigma$ bonds + lone pairs. ClO2: A STABLE ODD-ELECTRON SPECIES: pin. The most important part is that hybridisation (if applicable at all) follows the molecular structure. That leaves the odd electron in an out-of-plane-p-orbital, which will participate in π-bonding. The hybridization of the central atom can be determined from the groups attached to it. The approximate hybridisation of the orbitals of chlorine that match that would be sp². halacha - Is it forbidden for a noachide (Non-Jew)... everyday chemistry - C + O2 is equal to C + O, how... electrochemistry - Can we separate positive ions f... agada stories legends - Whoever is greater than hi... honorifics - When should one add さん at the end of ... conversion to judaism - How are Ethiopian Jews Jew... dft - Symmetry and periodicity of frequency-shifte... Discrete Time Fourier Transform (DTFT) for an unst... translation - What does 「なし」in 「問題なし」 mean? tefilla - Being Shaliach Tzibbur in a Congregation... halacha - What if the tafel comes to hand first? Is hybridization of the cyclopropyl anion sp5? (c) What Is The Hybridization Of Carbon In NCO-? But this is given wrong according to my textbook. Can I walk along the ocean from Cannon Beach, Oregon, to Hug Point or Adair Point? Top Answer. Since we consider odd electron a lone pair like in $\ce{NO2}$ therefore hybridisation is coming to be $\ce{sp^3}$. What is the hybridisation of XeO4? the three-electron bond they assumed in between, MAINTENANCE WARNING: Possible downtime early morning Dec 2, 4, and 9 UTC…. Electrons in s and 1 p orbitals acts as lone pairs, and the two singly filled p orbitals form sigma bonds. ClO2 is of C2v point group, so I just read off the C2v character table and got the following group orbitals [where z axis is that of the principal axis, and the outer atoms are aligned such that the y-axis points towards the centre atom]: A1 symmetry, two s orbitals. I have written a couple of times that terminal atoms can be (as a rule of thumb) regarded as having sp-orbitals. Already in this very simplified view, the problems start here. 4) What products are expected from the disproportionation reaction of hypochlorous acid? There will be no pπ-pπ bonding as all … $\ce{ClO2}$ has two $\sigma$ bonds, one lone pair, two π bonds and one odd electron. and C lO4−. Actually this is an ion → ClO2 - O= 6e-*2 = 12e-Cl= 7e-*1= 7e-+1e-total= 20e-However, they all need an octet. $\ce{ClO2}$ has 2 $\sigma$ bonds, 1 lone pair, 2π bonds and 1 odd electron. But enough of the commentary, let's clear up some issues. Since we consider odd electron a lone pair like in $\ce{NO2}$ therefore hybridisation is coming to be $\ce{sp^3}$. Methane is non-polar as the difference in electronegativities between carbon and hydrogen is not great enough to form a polarized chemical bond. Hybridisation is equal to number of σ bonds + lone pairs. B1 symmetry, two s orbitals. There comes a time, where you should realise that hybridisation is not always a useful concept to understand bonding. . 4 answers. Anyone who is jibber-jabbering about 'octet-expansion' has stopped learning about chemistry about 20 years ago. )(b) What Is The Hybridization Of Bromine In BrO2-? organic chemistry - Sp5 hybridization in cyclopropane? Potential hazards with chlorine dioxide include health concerns, expl… The reason for this is that the molecule has a very high symmetry, but it also has an unpaired electron. 2011-07-22 16:28:23 2011-07-22 16:28:23. it is sp2 and bond angle is 118 deree. There will be no pπ-pπ bonding as all p orbitals are hybridised and there will be 3pπ-dπ bonds. Your analysis of the bonding is not wrong, but maybe a bit too simple. In total, there is a formation of three sp 2 hybrid orbitals. clo2 hybridization. We should aim for having 8 electrons around each atom, keep in mind that the more heavy p block elements can expand above an octet. It also does not tell you which atomic orbitals will be involved. HSO4-iv. It does not hydrolyzewhen it enters water, and is usually handled as a dissolved gas in solution in water. sp hybridization is also called diagonal hybridization. readings - Appending 内 to a company name is read ない or うち? In principle that molecule is of a similar system like allyl-systems (with two extra electrons), or ozone (with one more electron). I would go so far as to shame whomever made the task. Why isn't eating milk with chicken kosher? Your analysis of the bonding is not wrong, but maybe a bit too simple. ,C lO3−. vocabulary - When is 酒【さけ】used to mean 日本酒【にほんしゅ】? In the above structure, central chlorine atom is surrounded by 4 electrons groups (two double bonds, one lone pair, and on unshared electron). How can I organize books of many sizes for usability? The problem here is that orbital symmetry cannot match with spacial symmetry, which means that hybridisation doesn't actually work here. Essentially the stabilisation from the π-bonds itself should be small, and could be described as π-backbonding, or is similar to negative hyperconjugation; maybe negative π-backbonding (!?). You will need a better than rudimentary grasp at molecular orbital theory to understand it. Hybridisation is equal to number of $\sigma$ bonds + lone pairs. questions - Comparison of 4 different ways to ask ... purim torah in jest - What does Judaism think of m... halacha - Can someone stop being supported by his ... elements - Is it possible for Hydrogen to lose its... theology - Native American Traditions and Mass Rev... meaning - Is tonai (都内）only used for the Tokyo met... minhag - Source of Burning Lulav with Chometz, passive voice - Grammar and meaning of 凝りに凝って出された. . 1) Four species are listed below:i.HCO3-ii. But this is given wrong according to my textbook. This type of hybridization is required whenever an atom is surrounded by two groups of electrons. Use MathJax to format equations. Answer. Is there a shortcut method to calculate the Steric Number? To learn more, see our tips on writing great answers. In this structure, chlorine has two sigma bonds, two pi bonds and one lone pair of the electron, and a single electron. How to make rope wrapping around spheres? Hybridization of Atomic Orbitals 1. $\ce{ClO2}$ has 2 $\sigma$ bonds, 1 lone pair, 2π bonds and 1 odd electron. Of valence electrons)-3*(No. Hybridization of any molecule can be determined by the following formula:H=1/2 { V + X - C + A}V=no. Ground state electronic configuration of Cl = 3s 2 3p 5 Excited state electronic configuration of Cl = 3s 2 3p 4 3d1 Electronic configuration of O = 2s 2 2p 4 Here, Cl undergoes sp 3 hybridisation. halacha - Is this squid with scales kosher? Introduction. ClO2 is not a molecule, actually it is a ion with a negative charge. If we take the crystallogrpahic data then it is clear that the chlorine has three sigma bonds / lone pairs (or single version of lone pairs). This problem has been solved! A) 0 lone pairs, square planar D) 1 lone pair, trigonal bipyramidal B) 0 lone pairs, tetahedral E) 2 lone pairs, square planar C) 1 lone pair, square pyramidal Ans: B … To accommodate the two lone pairs and the bonding pair, it will also form three equivalent sp2 hybrid orbitals. No you are wrong, I do like the VSEPR model very much. halacha - Is the Goel HaDam (Blood Avenger) obligated to pursue blood tanach - Why is Chronicles so similar to Kings? spectroscopy - What is an exocyclic double bond? Join Yahoo Answers and get 100 points today. The hybridisation of the orbitals to produce either electron density need to also be different. Chlorine dioxide is a chemical compound with the formula ClO2 that exists as yellowish-green gas above 11 °C, a reddish-brown liquid between 11 °C and −59 °C, and as bright orange crystals below −59 °C. Martin, it appears that you do not like VSEPR. Did they allow smoking in the USA Courts in 1960s? vengeance? The π-orbitals will therefore be entirely composed out of p-orbitals of the involved elements. What is the hybridisation of the carbons in the allyl radical? Lewis structure is the structural representation of the number of valence electrons that participate in the bond formation and nonbonding electron pairs. MathJax reference. Thus it looks like a distorted $sp^2$ to me, I think that the bonding is likely to be two lone pairs on each $\ce{O}$, one lone pair on the $\ce{Cl}$. In this case the use of MO theroy to deal with the pi bonds and VSEPR for the sigma bonds does provide an answer which can be reconciled with the crystallographic evidence. You will need a better than rudimentary grasp at molecular orbital theory to understand it.Let's assume that things would be easier, and try tor roll with that for as long as possible. Whether those orbitals are essentially bonding or not, is an entirely different question.It also does not tell you which atomic orbitals will be involved. This all was deduced from a very reduced and simplified set of theory; the reality is probably by far more complicated. site design / logo © 2020 Stack Exchange Inc; user contributions licensed under cc by-sa. so two orbitals will be involved here as in double bond one is always a pie bond and only one is sigma bond so one hybridized orbital is used in formation of a double bond. Question: A) What Is The Hybridization Of Chlorine In ClO2-? Is this textbook bonding picture of hybridization in ethene wrong? I reason that the angle of 116 degrees makes it look like we have a distorted trigonal arrangement of sigma orbitials around the chlorine. Dots and Lines are used in this structure in which lines represent the electrons forming bonds with the central atom and dots are the non-bonding pairs.Lewis structure follows the octet rule concept. Trending Questions. In this, two hybrid orbitals contain unpaired electrons and one hybrid orbital will have the lone pair. ... Hybridization, Polar or Nonpolar: pin. That leaves for every oxygen one in-plane-p-lone-pair, which we will (in the spirit of the approximation) disregard as having any effect on bonding. There is one remaining out-of-plane-p-orbital per oxygen. In this case, if you are already using MO theory, there is no reason to use VSEPR in the first place; it also, while at first glance looks correct, produces the 'right' answer/ prediction, for the wrong reasons. Therefore the two oxygen will use one sp-orbital to form a σ-bond towards chlorine, the other one is an in-plane-σ-lone-pair. Just as the carbon atom hybridized to form the best bonds, so do the oxygen atoms. It is an oxidizing agent, able to transfer oxygen to a variety of substrates, while gaining one or more electrons via oxidation-reduction (redox). Of course you can use VSEPR theory to predict the shape of the molecule, that is a very good starting point. For some reason, many chemists in teaching positions keep VSEPR as a holy cow for far too long up the grades. That is why I find this question incredibly difficult to answer and why I find that Nuclear Chemist's answer dangerous, because it propagates myths about bonding that have been disproved already. - Quora One obvious fault in the question is that there is no involvement of d-orbitals whatsoever in the molecules. Anyone who is jibber-jabbering about 'octet-expansion' has stopped learning about chemistry about 20 years ago. 0 0. The d-orbitals of chlorine are simply not accessible energetically; at least not in the way that it would form stable bonds. Already in this very simplified view, the problems start here. Let's assume that things would be easier, and try tor roll with that for as long as possible. Ask Question + 100. shiurim measurements - How much produce becomes bi... Intuitive interpretation of Fourier transform in b... explosives - Does the explosion of TNT include oxi... halacha - Can a teen threaten or attack one parent... organic chemistry - Has Crabtree's photochemically... legal documents - need for civil marriage license ... fourier transform - Why are there so many windowin... sound - Why are zero values added in the FFT of a ... halacha - What technically constitutes adultery. Angular, with chlorine in the middle. Let's further assume, that because it has higher s-character, the orbital will be lower in energy and therefore be doubly occupied. Hybridization is the formation of a covalent bond through the combination of an s and p orbitals. There will be no pπ-pπ bonding as all p orbitals are hybridised and there will be 3pπ-dπ bonds. How feasible to learn undergraduate math in one year? This results in sp3 hybridization and tetrahedral geometry. I also know that it works for many compounds, and I know that it offers valuable insights into geometries. $\ce{ClO2}$ has 2 $\sigma$ bonds, 1 lone pair, 2π bonds and 1 odd electron. I was always taught to use VSEPR for the sigma bonds and then MO for the pi system. Get your answers by asking now. Let's just say that this is not an undergrad study problem. Still have questions? These will, due to symmetry, participate in π-bonding. are only sp3. Let's further assume, that because it has higher s-character, the orbital will be lower in energy and therefore be doubly occupied. I need to find the bandwidth the signal $x = 50 \operatorname{sinc}(125(t-10))^2$. Feasibility of a goat tower in the middle ages? z transform - Minimum number of Poles and zero of ... parshanut torah comment - Looking for Shadal Al Ha... meaning - ければ possibly used to link verbs instead ... inorganic chemistry - What does a molecules color ... random - Sampling low pass filtered white noise. That leaves the odd electron in an out-of-plane-p-orbital, which will participate in π-bonding.In this simplified and assumption riddled thought-experiment, the π-bonding will form three molecular orbitals pictured below. The remaining will be either a lone-pair, or singly occupied. word choice - How to use へ (-e), に (-ni), まで (made... manga - Please help me understand this たる? Give the number of lone pairs around the central atom and the molecular geometry of CBr 4. A bent molecule of the form $\ce{B-A-B}$ always has $C_\mathrm{2v}$ symmetry, it therefore always has π-orbitals. Let's just say that this is not an undergrad study problem. In principle that molecule is of a similar system like allyl-systems (with two extra electrons), or ozone (with one more electron). maseches sanhedrin - Why is וחי בהם taught in the ... grammar - Meaning of 何とやら in this sentence. Here Cl forms double bonds with oxygen atoms sharing four of its electrons with two oxygen atoms and forming double bonds with oxygen atoms. Clo2- here cl is the central atom bonded to 2 oxygen atom and after bonding it has 2 lone pair of electron including negative one.according to formula AB2L2 then 2+2=4=sp3 Alleei Alleei Answer : The hybridization of Cl in is These are solely dictated by symmetry. Why does the FAA require special authorization to act as PIC in the North American T-28 Trojan? You will find out that the molecule is bent, and that matches the crystal structure. A bent molecule of the form $\ce{B-A-B}$ always has $C_\mathrm{2v}$ symmetry, it therefore always has π-orbitals. Hybridisation state= 0.5*(No. halacha theory - Why don't we just follow the shit... inorganic chemistry - Why do different elements fo... halacha - Could a religious man be an anarchist? The hybridisation of the orbitals to produce either electron density need to also be different. This time is now. Let's just assume that this is the case. Each sp hybridized orbital has an equal amount of s and p character, i.e., 50% s and p character. Of atoms other than central and hydrogen atom) =0.5*(1*1+7*1+6*2)-3*(2) =0.5*20–3*2 =10–6=4=sp3 hybridised state. The reason for this is that the molecule has a very high symmetry, but it also has an unpaired electron. orthography - Abbreviating sets of compounds with ... halacha - Secular Names for Days of the Week. Story in which immigrant girl finds room temp superconductor, Harmonizing the bebop major (diminished sixth) scale - Barry Harris, what does "scrap" mean in "“father had taught them to do: drive semis, weld, scrap.” book “Educated” by Tara Westover. Some of the greatest minds of (theoretical) chemistry have been puzzled about $\bf\ce{ClO2}$, and we have not even started to discuss the three-electron bond they assumed in between. You will find out that the molecule is bent, and that matches the crystal structure. grammar - What is the difference between "に" and "... usage - How to use イコール to compare things? Join. It only takes a minute to sign up. You may remember that formula to find Hybridisation state of the central atom … )As long as that last part of the question is not meant as a trap (which would be even more awful), it alone shows that the exercise is not well-thought about. Since we consider odd electron a lone pair like in $\ce{NO2}$ therefore hybridisation is coming to be $\ce{sp^3}$. 3*8e- = 24e-24e- - 20 e- = 4e-/2 = 2 simple bonds. Two of these will be the counterpart for the σ-bonds. The problem here is that orbital symmetry cannot match with spacial symmetry, which means that hybridisation doesn't actually work here.A bit more precise: The electron density of α-spin electrons is different from that of β-spin electrons. Click hereto get an answer to your question ️ Hybridisation of chlorine atom in ClO^-, ClO2^-, ClO3^- and ClO4^- respectively: a) What is the hybridization of chlorine in ClO 2-? Trending Questions. Looking forward to it, if we start with the Carbon atom, there are two double bonds. To subscribe to this RSS feed, copy and paste this URL into your RSS reader. (There are plentiful discussions about this on chemistry.se alone.) How did the staff that hit Boba Fett's jetpack cause it to malfunction? From VSEPR-theory we know the molecule is bent. And don't get me wrong, VSEPR is a great model, but as with Newtons Law - there comes a point where it just doesn't explain what is going on. (Type Your Answerusing The Format Sp3 For Sp3. I have written a couple of times that terminal atoms can be (as a rule of thumb) regarded as having sp-orbitals. rev 2020.12.4.38131, The best answers are voted up and rise to the top, Chemistry Stack Exchange works best with JavaScript enabled, Start here for a quick overview of the site, Detailed answers to any questions you might have, Discuss the workings and policies of this site, Learn more about Stack Overflow the company, Learn more about hiring developers or posting ads with us. Which chemical reaction has the highest specific e... atoms - How to interpret a luminescence intensity ... inorganic chemistry - Is the P-Cl bond energy same... meaning - Why is coffee with shochu or awamori cal... Reconstruction of audio signal from Spectrogram. Hybridization of Cl in clo2? The ClF molecule has sp 3 hybridization on both atoms and is not hypervalent. Hybridisation is equal to number of $\sigma$ bonds + lone pairs. thank you for this question (I love hybridization questions) First: ClO2 ??? By clicking “Post Your Answer”, you agree to our terms of service, privacy policy and cookie policy. Script to clear buffers / cache still says permission denied, Does Divine Word's Killing Effect Come Before or After the Banishing Effect (For Fiends). The d-orbitals of chlorine are simply not accessible energetically; at least not in the way that it would form stable bonds. The remaining will be either a lone-pair, or singly occupied. Enjoy the videos and music you love, upload original content, and share it all with friends, family, and the world on YouTube. @Martin-マーチン I agree. Of course you can use VSEPR theory to predict the shape of the molecule, that is a very good starting point. That leaves for every oxygen one in-plane-p-lone-pair, which we will (in the spirit of the approximation) disregard as having any effect on bonding. $\ce{ClO2}$ has two $\sigma$ bonds, one lone pair, two π bonds and one odd electron. What does this lambda–sigma notation mean? The approximate hybridisation of the orbitals of chlorine that match that would be sp². For example, if I say マイクロソフト内のパートナーシップは強いです, is the 内 here read as うち or ない? pin. Normally if we have a perfect $sp^3$ molecule such as methane ($\ce{CH4}$) we get an angle of 109.5 degrees between the bonds. Are there any Pokémon that lose overall base stats when they evolve? There comes a time, where you should realise that hybridisation is not always a useful concept to understand bonding. matlab - Fourier Transform of Morlet wavelet Function? This type of hybridization involves the mixing of one ‘s’ orbital and one ‘p’ orbital of equal energy to give a new hybrid orbital known as a sp hybridized orbital. 9 10 11. However, the claim of expanded octets and electron clouds being more repelling is fabricated garbage to make weak theory fit beyond its means. The problem is that VSEPR does work for a lot of compounds. This time is now. Well I still love VSEPR, but it has its limits. Find the hybridization as well identify the pπ-pπ as well as pπ-dπ bonds in $\ce{ClO2}$. All possible states (that is independent of any hybridisation model) then will be in superposition to form the actual ground state.
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