therefore, oxygen molecule is a paramagnetic in nature. Those with positive bonding order are considered stable molecule while those with negative bond order or zero bond order are unstable molecule. (ii) Calculate the pH value of 0.01M CH3 COOH if it is 5% dissociated. Hence, the electronic configuration of the molecular orbitals accounts admirably for the paramagnetic properties of oxygen. Molecular orbitals are formed by combination of atomic orbitals. They have higher energy than atomic orbitals. We can calculate the bond order in the O 2 molecule by noting that there are eight valence electrons in bonding molecular orbitals and four valence electrons in antibonding molecular orbitals in the electron configuration of this molecule. A molecular orbital diagram, or MO diagram, is a qualitative descriptive tool explaining chemical bonding in molecules in terms of molecular orbital theory in general and the linear combination of atomic orbitals (LCAO) method in particular. Q1: Arrange the species O2, O2-, O2+ the decreasing order of bond order and stability and also indicate their magnetic properties. The first photo is straight from a 2006 edition Pearson general chemistry textbook, and it shows you what the molecular orbital (MO) diagram for O2 is. no. Ans: The stabilities of these can be best explained using Molecular orbital theory. But experimental evidence for some diatomic molecules have shown that the above sequence of energy levels of MOs is not correct for all the molecules. According to Molecular Orbital Theory individual atoms combine to form molecular orbitals, as the electrons of an atom are present in various atomic orbitals and are associated with several nuclei. This kind of mixing of orbitals or symmetry interaction is not applicable for O2 and F2 molecule formation because of larger energy gap between 2s and 2p orbitals for these atoms. Electrons in a molecule are said to occupy molecular orbitals. Greater the bond order, greater is the. soo, you can verify the below link for any further clarifiaction and also for ur answer of the molecular orbit configuration for peroxide ion Molecular Orbital Theory O2– – = σ1s2,σ*1s2,σ2s2,σ*2s2,σ2px2, π2py2= π2pz2,π*2py2=π*2pz2,σ*2px0. Therefore, a molecular orbital is polycentric and atomic orbital is monocentric. The stability of a molecule is measured by its bond dissociation energy. The bond order in O2+ and O2 is, respectively, 1.5 and 2. No. For eac… O 2 + is more stable than O 2-.Because According to molecular orbital theory O 2 + has 15 electrons &it has one electron in antibonding orbital. This is because _____. Sol. Fig. No. Complete List of Packages for Medical Preparation, Linear Combination of Atomic Orbital(LCAO), Difference between Atomic Orbitals and Molecular Orbitals, Order of Energies of Various Molecular Orbitals. Each horizontal line represents one orbital that can hold two electrons. The molecular orbital configuration ofO2, O2-, O22-, O2+ are as follows:O2 = σ1s2, σ*1s2, σ2s2, σ*2s2, σ2pz2, π2px2 = π2py2,  π*2px1 = π*2py1Bond order = (10-6)/2 = 2, Number of unpaired electrons = 2, Therefore paramagnetic, O2- = σ 1s2, σ *1s2, σ 2s2, σ *2s2, σ 2pz2, π2px2 = π2py2, π*2px2 = π*2py1Bond order = (10-7)/2 = 1.5, Number of unπaired electrons = 1, Therefore paramagnetic, O22- = σ1s2, σ*1s2, σ2s2, σ*2s2, σ2pz2, π2px2 = π2py2, π*2px2 = π*2py2, Bond order = (10-8)/2 = 1, Number of unpaired electrons = 0, Therefore diamagnetic, O2+ = σ1s2, σ*1s2, σ2s2, σ*2s2, σ2pz2, π2px2 = π2py2, π*2px1= π*2py0, Bond order = (10-5)/2 = 2.5, Number of unpaired electrons = 1, Therefore paramagnetic. B) there are more electrons in the bonding orbitals than in the antibonding orbitals. A linear combination of properly oriented atomic orbitals for the formation of sigma s … The number of unpaired electrons in O2+ and O22- is, respectively, 1 and 0. Linear Combination of Atomic Orbitals (LCAO). The molecular orbital configuration of O 2 , O 2 - , O 2 2- , O 2 + are as follows: O 2 = σ1s 2 , σ*1s 2 , σ2s 2 , σ*2s 2 , σ2p z 2 , π2p x 2 = π2p y 2 , π*2p x 1 = π*2p y 1 Bond energy and bond order both increase with decreasing bond length. (ii) The extent of overlapping between the atomic orbitals. No. of electrons in BMO - No. 2. This is among the greatest successes of the molecular orbital theory. Triplet oxygen, 3 O 2, refers to the S = 1 electronic ground state of molecular oxygen (dioxygen). It is represented by s. When molecular orbital is formed by subtraction of wave function, the type of molecular orbitals formed are called Antibonding Molecular Orbitals and is represented byΨMO = ΨA - ΨB. Molecular Orbital Theory ( with molecualr orbitals) ... electron configuration of this molecule. Therefore in 1932 F. Hood and RS. On the basis of molecular orbital theory, select the most appropriate option. 5 Order of Energy Levels for Boron, Carbon, Nitrogen etc. Therefore, an electron in an atom may be described as occupying an atomic orbital, or by a wave function Ψ, which are solution to the Schrodinger wave equation. Consider two atoms A and B which have atomic orbitals described by the wave functions ΨA and ΨB .If electron cloud of these two atoms overlap, then the wave function for the molecule can be obtained by a linear combination of the atomic orbitals ΨA and ΨB i.e. Molecular Orbital theory correctly predicts paramagnetism of oxygen gas, O2. 6 Order of Energy for O2 and Higher molecules, σ 1s, σ *1s, σ 2s, σ *2s, [π 2px = π 2py], σ 2px [π *2px= π *2py], σ*2pz, Fig. The molecular orbital theory (MO) has been introduced for the diatomic hydrogen molecules. Electrons may be considered either of particle or of wave nature. Similarly, the energy of σ *2s lowered while that of σ *2px becomes higher. a) The bond order of O2 is 2.5 and it is paramagnetic b) The bond order of O2 is 1.5 and it is paramagnetic c) The bond order of O2 is 2 and it is diamagnetic d) The bond order of O2 … All the elements in the second period before oxygen have the difference in energy between the 2s and 2p orbital small enough, so that s-p mixing (combination) can occur lowering the energy of the σ (2s) and σ* (2s) and increasing the energy of the σ (2p) and σ* (2p) molecular orbitals. Thus, the bond order is two. E.i) State and explain Le Chatelier’s principle. The bond length in the oxygen species can be explained by the positions of the electrons in molecular orbital theory. Anti-Bonding Molecular Orbitals (ABMO) - Energy of Anti Bonding Molecular Orbitals is higher than Bonding Molecular Orbitals because the electron try to move away from the nuclei and are in repulsive state. d) discuss the magnetic character of each molecule Thus, the bond order is two. For the second period elements, the 2s and 2p orbitals are important for MO considerations. Molecular orbital formed by addition of overlapping of two s orbitals shown in figure no. The relative energy levels of atomic and molecular orbitals are typically shown in a molecular orbital diagram (Figure 8). The molecular orbital diagram representing this order of energy levels is shown in fig. Using molecular orbital theory; a) draw the MO diagrams for O2, O2+, and O2-. No. by subtraction or addition of wave functions of atomic orbitals, The above equation forms two molecular orbitals. According to the symmetry interactions, the two orbitals of the same symmetry repel each other and the lower energy orbital lowers down more while the higher energy orbital is energized more. The C 2 molecule is diamagnetic because all electrons are paired there are no unpaired electrons. The bond order decreases in the order isO2+ >O2>O2->O22-so, we conclude stability is directly proportional to bond order. Notice: JavaScript is required for this content. Answer. b. there are two unpaired electrons in the MO electron configuration of O2 c. the energy … Therefore, Combination of two atomic orbitals results in formation of two molecular orbitals, bonding molecular orbital (BMO) whereas other is anti-bonding molecular orbital (ABMO). Valence Bond Theory fails to answer certain questions like Why He2 molecule does not exist and why O2 is paramagnetic? The Energies of Bonding Molecular Orbitals and Anti-Bonding Molecular Orbitals are shown in figure below: The factors upon which relative energies of molecular orbitals depend are: (i) Energies of the Atomic orbitals combining to form Molecular Orbitals. 9 Molecular Orbital Diagram for CO. Let’s take a question to understand it more clearly. They have lower energy than atomic orbitals involved. Electronic configuration of oxygen = 1s 2 2s 2 2p 4. For a diatomic molecule, the atomic orbitals of one atom are shown on the left, and those of the other atom are shown on the right. of electrons in ABMO)/ 2. The two electrons in the hydrogen molecule may both be accommodated in the 1s g orbital if their spins are paired and the molecular orbital configuration for H 2 is 1s g 2. The order of increasing energy of molecular orbitals obtained by combination of 1s, 2s and 2p orbitals of two atoms is →, σ1s, σ *1s, σ 2s, σ *2s, σ 2pz, π 2px = π 2py, π *2px= π *2py, σ *2pz. Number of molecular orbitals formed is equal to the number of atomic orbitals. First BMO are filled then ABMO starts filling because BMO has lower energy than that of ABMO. 2. = (No. 2SO2(g)+ O2(g)⇌2SO3(g); ∆= - 42k.cal. The greater the overlap, the more the bonding orbital is lowered and the anti-bonding orbital is raised in energy relative to AOs. Molecular orbital theory explanation Dashed lines show which of the atomic orbitals combine to form the molecular orbitals. molecular orbital diagram of O 2 + Electronic configuration of O 2 + In the case of O 2-17 electrons are present &3 electrons are present in antibonding orbitals. Register & Get Sample Papers solutions instantly. Magnetic property: There are two unpaired electrons . An electron Molecular orbital is under the influence of two or more nuclei depending upon the number of atoms present in the molecule. A) the bond order in O2 can be shown to be equal to 2. A molecular orbital can hold two electrons, so both electrons in the H 2 molecule are in the σ 1s bonding orbital; the electron configuration is (σ 1 s) 2. 2. BMO has lower energy and hence greater stability than ABMO. Formation of molecular orbitals occurs by the combination of atomic orbitals of proportional symmetry and comparable energy. United Atom Method. Although the Lewis structure and molecular orbital models of oxygen yield the same bond order, there is an important difference between these models. On the basis of this principle discuss the conditions for obtaining the maximum yield of SO3 in the following reaction. It is similar to constructive interference occurring in phase because of which electron probability density increases resulting in formation of bonding orbital. Molecular orbital energy level diagram of N 2 molecule • Bond order = (8 2)/2 = 3 (N ≡ N) • Absence of unpaired electrons showed that N 2 molecule is diamagnetic. The filling of molecular orbitals leaves 2 unpaired electrons in each of the π * (2p y) and π * (2p z) orbitals. It is similar to destructive interference occurring out of phase resulting in formation of antibonding orbitals. On the other hand, if there are unpaired electrons in the molecule, the substance is paramagnetic (attracted by the magnetic field). For Example, if we look at CO Molecule, it is diamagnetic as all the electron in CO are paired as in the figure below: Fig. 8 Order of Energy for N2 and lower molecules. Just as with atoms, we can write a molecular electron configuration for O2 σ2σ*2σ2π4π*2 We can also calculate the O–O bond order: BO 1 2 # bonding e# anti-bonding e  1 2 The unusual electron configuration prevents molecular oxygen from reacting directly with many other molecules, which are often in the singlet state. Mulliken came up with theory known as Molecular Orbital Theory to explain questions like above. The same method can be applied to other diatomic molecules, but involving more than the 1s atomic orbitals. But the bond dissociation energy is directly proportional to the bond order. This kind of energy reversal is due to mixing of 2s and 2p orbitals where the energy difference is very close, that is, for B, C, and N atoms. The molecular orbital diagram for C 2 molecule is :. Magnetic character - If all the electrons in the molecule of a substance are paired, the substance is diamagnetic (repelled by the magnetic field). If number of electrons more in antibonding orbital the molecule become unstable. Certain rules are to be followed while filling up molecular orbitals with electrons in order to write correct molecular configurations: Order of energy of various molecular orbitals is as follows: σ1s, σ *1s, σ 2s, σ *2s, σ 2pz, [π2px = π2py], [π*2px= π*2py], σ *2pz, Fig. Fig. The higher the bond order value, smaller is the bond length. From the diagram, the molecular electronic configuration of oxygen is. c) determine which molecule has the strongest bond. The electronic configuration of C 2 is K K (σ2s) 2 (σ * 2s) 2 n(2px) 2 n(2py) 2. 2. b) determine the bond order for all three molecules. a. there are more electrons in the bonding orbitals than in the antibonding orbitals. Copyright © 2010-2019 www.emedicalprep.com. MOED of 'O 2 ' : Electronic configuration of Oxygen (Z = 8) is 1s 2 2s 2 2p 4. The electron configuration of O2+ is (σ2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*)1. To obtain the molecular orbital energy-level diagram for O 2, we need to place 12 valence electrons (6 from each O atom) in the energy-level diagram shown in Figure 9.10. The electronic configuration of O2– is KK (σ (2s))2 (σ∗(2s))2 (π (2px))2 (π (2py))2 (σ (2pz))2 (π∗(2px))2 (π∗(2py))2 Nb= 8, Na= 6 Bond order=1 The presence of no unpaired electron makes the molecule diamagnetic. The electrons in the Molecular Orbital formed by subtraction of overlapping of two s orbitals are shown in figure no. All rights reserved. But if one or more molecular orbitals are singly occupied it is paramagnetic. 27) Molecular Orbital theory correctly predicts paramagnetism of oxygen gas, O2. C) the energy of the π2p MOs is higher than that of the σ2p MO D) there are two unpaired electrons in the MO electron configuration of O2 … The electron configurations are shown below where we have 16 electrons to … The wave function of a molecular orbital may be obtained by one of two method:1. 2 Formation of Bonding and Anti-Bonding Orbital. Finally, the energy of the σ *2px becomes higher than π2py and π2pz which remain unchanged in the symmetry interaction. From that diagram, you can then easily fill out what the O2- and O2+ MO diagrams should be—and that is in the second photo I included. Bonding Molecular Orbitals (BMO) - Energy of Bonding Molecular Orbitals is less than that of Anti Bonding Molecular Orbitals because the attraction of both the nuclei for both the electron (of the combining atom) is increased. For example, homonuclear diatomic molecules of second row elements like Li2, Be2, B2 , C2, N2 , the σ 2pz  MOs is higher in energy than π 2px and π 2py MOs, σ1s, σ *1s, σ 2s, σ *2s, [π 2px = π 2py], σ 2pz [π *2px= π *2py], σ*2pz. The molecular orbitals formed by the combination of the atomic orbitals are shown in the center. When addition of wave function takes place, the type of molecular orbitals formed are called Bonding Molecular orbitals and is represented by ΨMO = ΨA + ΨB. The Lewis structure O=O does not accurately represent the diradical nature of molecular oxygen; molecular orbital theory must be used to adequately account for the unpaired electrons. As per this method the formation of orbitals is because of Linear Combination (addition or subtraction) of atomic orbitals which combine to form molecule. 1s Atomic Orbitals (AOs) of two atoms form two Molecular Orbitals (MOs) designated as s1s and s *1s.The 2s and 2p orbitals (eight AOs of two atoms) form four bonding MOs and four anti-bonding MOs as: Anti – Bonding MOσ: σ *2s, σ *2pz, π *2px, π *2py, Using Spectroscopy, the energy levels of these molecular orbitals are determined experimentally. (i) Formation Oxygen molecule: Electronic configuration of oxygen atom-1s² 2s² 2p⁴ Atomic orbitals of oxygen combine to form molecular orbitals. Accordingly, σ 2s and σ 2px have same symmetry and similarly for   σ *2s and σ *2px the energy of σ 2s is lowered and that of the σ 2px becomes higher. It is represented by s* (*) is used to represent antibonding molecular orbital) called Sigma Antibonding. If value of bond order is positive, it indicates a stable molecule and if the value is negative or zero, it means that the molecule is unstable. The bond energies increase in the order: O22- < O2- < O2 < O2+. Magnetic Behavior: If all the molecular orbitals in species are spin paired, the substance is diamagneti. An electron in atomic orbital is under the influence of only one positive nucleus of the atom. ( σ 1 s ) 2 . BO = bonding orbitals ABO = Anti-bonding orbitals O 2: Atomic orbitals are inherent property of an atom. π2p and π*2p molecular orbitals originate from the 2py and 2pz atomic orbitals of the two oxygen atoms. It may be defined as the half of difference between the number of electrons present in the bonding orbitals and the antibonding orbitals that is, Bond order (B.O.) When two oxygen atoms combines, the molecular orbital energy level diagram is as shown in the figure. 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