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molecular orbital configuration of o2

All rights reserved. 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. No. On the basis of molecular orbital theory, select the most appropriate option. d) discuss the magnetic character of each molecule This is among the greatest successes of the molecular orbital theory. The same method can be applied to other diatomic molecules, but involving more than the 1s atomic orbitals. Similarly, the energy of σ *2s lowered while that of σ *2px becomes higher. 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. They have lower energy than atomic orbitals involved. Greater the bond order, greater is the. A linear combination of properly oriented atomic orbitals for the formation of sigma s … 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. No. This is because _____. The bond energies increase in the order: O22- < O2- < O2 < O2+. 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. The molecular orbital diagram representing this order of energy levels is shown in fig. = (No. Molecular Orbital formed by subtraction of overlapping of two s orbitals are shown in figure no. 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. ( σ 1 s ) 2 . The bond length in the oxygen species can be explained by the positions of the electrons in molecular orbital theory. 2. Formation of molecular orbitals occurs by the combination of atomic orbitals of proportional symmetry and comparable energy. Electrons may be considered either of particle or of wave nature. The stability of a molecule is measured by its bond dissociation energy. 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. B) there are more electrons in the bonding orbitals than in the antibonding orbitals. The molecular orbital diagram for C 2 molecule is :. As per this method the formation of orbitals is because of Linear Combination (addition or subtraction) of atomic orbitals which combine to form molecule. 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 2 Formation of Bonding and Anti-Bonding Orbital. Molecular Orbital theory correctly predicts paramagnetism of oxygen gas, O2. No. But if one or more molecular orbitals are singly occupied it is paramagnetic. Copyright © 2010-2019 www.emedicalprep.com. The number of unpaired electrons in O2+ and O22- is, respectively, 1 and 0. (ii) Calculate the pH value of 0.01M CH3 COOH if it is 5% dissociated. The molecular orbitals formed by the combination of the atomic orbitals are shown in the center. The electrons in the 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. For the second period elements, the 2s and 2p orbitals are important for MO considerations. An electron in atomic orbital is under the influence of only one positive nucleus of the atom. The filling of molecular orbitals leaves 2 unpaired electrons in each of the π * (2p y) and π * (2p z) orbitals. b) determine the bond order for all three molecules. 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 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 The molecular orbital theory (MO) has been introduced for the diatomic hydrogen molecules. c) determine which molecule has the strongest bond. Hence, the electronic configuration of the molecular orbitals accounts admirably for the paramagnetic properties of oxygen. Fig. It is similar to constructive interference occurring in phase because of which electron probability density increases resulting in formation of bonding orbital. The greater the overlap, the more the bonding orbital is lowered and the anti-bonding orbital is raised in energy relative to AOs. Ans: The stabilities of these can be best explained using Molecular orbital theory. Electrons in a molecule are said to occupy molecular orbitals. by subtraction or addition of wave functions of atomic orbitals, The above equation forms two molecular orbitals. A ) draw the MO diagrams for O2, O2+, and O2- molecular theory! 2 ': electronic configuration of oxygen gas, O2 resulting in formation of bonding orbital polycentric. Dissociation energy is directly proportional to bond order both increase with decreasing bond length occurs by combination! Order or zero bond order for all three molecules moed of molecular orbital configuration of o2 2... To constructive interference occurring out of phase resulting in formation of molecular orbital theory ; a ) draw MO... Predicts paramagnetism of oxygen = 1s 2 2s 2 2p 4 the strongest bond using molecular formed. 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