See link 1 for an energy level diagram of the bonding and antibonding orbitals in the molecule and molecular ions of oxygen. O2 : KK. It is stable. Use the molecular orbital model to fully describe the bonding in O2+, O2, O2-, and O22-. Here i make a table according to the Molecular orbital theory. Relative stabilities of O2, O2-, O22-, O2+ and N2, N2+, N2-, N22-(viii) Molecular orbital theory, Qualitative treatment of homonuclear diatomic molecules of first two periods (Hydrogen to Neon). 1 The electron configuration of O2+ is (σ 2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*)2. Bond order is the number of bonds. Paramagnetic We can work this out by looking at the molecular orbital diagram of O_2 O_2^+ has 1 fewer electron than O_2 which is what gives it the positive charge. For a diatomic molecule e.g O2 has bond order two because O=O is a double bond. 2 The bond order in O2+ and O2 is, respectively, 2.5 and 2. Compare the bonding in O2^2-, O2-, O2, and O2^2+. 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. The... See full answer below. The bond length in the oxygen species, O2+, O2, O2-, O2^(2-), can be explained by the positions of the electrons in molecular orbital theory. a. Decreasing order of stability of O2, O-2, O2+ and O22- is: (A) O2 > O2+ > O22- > O2- (B) O-2 > O22- > O2+ > O2 (C) O2+ > O2 > O2- > O22- (D) O22- In fact, it's the perioxide ion. Bond order in O 2 + = 10-5/2= 2.5 Bond order in O 2 - = 10-7/2 = 1.5 Bond order in O 2 2- = 10-8/2 = 1 . Bond order of O 2. Electronic configuration of O. Bond order of O 2 + Electronic configuration of can be written as: Bond order of O 2 + =1/2 (8-3)= 2.5. Removing one electron from the pi orbital still leaves one unpaired electron in the other pi* orbital. Check me out: http://www.chemistnate.com Oct 17,2020 - In which of the following processes, the bond order has increased and paramagnetic character has changed to diamagnetic?a)N2→N2+b)O2→O2+c)O2→O22-d)NO → NO+Correct answer is option 'D'. Electronic configuration of O 2-ion will be: Bond order of = 1/2(8-5) = 1.5 = paramagnetic . Bond energy and bond order both increase with decreasing bond length. Which is expected to have the longest O-O bond? Hence, the bond order of oxygen molecule is 2. Similarly, the electronic configuration of O 2 + can be written as: Bond order of O 2 + = 1/2(8-3) = 2.5 = paramagnetic . b.The number of unpaired electrons in O2- and O2 is, respectively, 1 and 2. c.The bond order in O2- and O22- is, respectively, 1.5 and 1. d.Bond length and bond energy both increase with increasing bond order. Bond order =1/2(N b-N a) = 1/2(8-4) = 2 = Paramagnetic . The bond order in O2+ and O2 is, respectively, 1.5 and 2. Which of the following has fractional bond order : (A) O2^2+ (B) O2^2- (C) F2^2- (D) H2^- asked Oct 10, 2019 in Chemical bonding and molecular structure by KumarManish ( 57.6k points) chemical bonding Bond order = 1/2 (8-4) =2. ans. Bond order O 2 + will form by removal of 1 electron from O2.The electron will be removed from π * 2p x or π * 2p y orbital. Bond order is the number of bonds. Compare the bonding in -peroxide - O2-2, -superoxide - O2-, -dioxygen - O2, and the -dioxygenyl ion - O2+. e.The electron configuration of O2- is (σ2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*)4. The bond energies increase in the order: O22- < O2- < O2 < O2+. Arrange in order of increasing stability O2 , O2+, O2-, O2^2- - Chemistry - NCERT Solutions; Board Paper Solutions; Ask & Answer; School Talk; Login; GET APP; Login Create Account. Determine which of the following statements are true and which are false. O2^+2 means it loses 2 e-,there are 4 e- in p_orbitals.According to MOT(molecular orbital theory) 6 e- are in bonding molecular orbitals BMO and 2 e- are in antibonding molecular orbitals ABMO Formula to find bond order is No.of e in BMO — NO. The bond order for the O 2 2-is 1 (one). For a diatomic molecule e.g O2 has bond order two because O=O is a double bond. Number of anti-bonding electrons = 4 . Include Lewis structures, molecular orbital structures, bond order and number of unpaired electrons, bond lengths, and bond strengths in discussion. The bond energies increase in the order: O2+ < O2 < O2- < O22-. True of False - a. Bonbd order of O 2 2- is = B.O = (10-8)/2 = 2/2 = 1 The higher the value of bond order, higher is the stability of the bond, so on the basis of above information, we can say that, O 2 + ion is more stable than O 2 , O 2 - and O 2 2- ions. Energy level diagrams, bonding, antibonding molecular orbitals, bond order, paramagnetism of O2 molecule. Specie No. Number of bonding electrons = 8. Thus, the bond order of O 2 + is 2.5. O 2 + is more stable than O 2-. Arrange the species O2, O2^+, O2^-, and O2^2- in order of increasing O-O bond length. of electrons (Nb-Na)/2 = bond order Magnetism O22- 18 (10-8)/2 = 1 Diamagnetic O2- 17 (10-view the full answer Nov 25,2020 - Among the species O2, O2-, O22-, O2+ their respective bond order values are w, x, y and z respectively. Find an answer to your question Among o2,o2-,o2-2,o2+,o2+2 which posses highest bond order Asked by an Inorganic Chemistry (College Level) student, November 6, 2016 If number of electrons more in antibonding orbital the molecule become unstable. The electron would be removed from the pi orbital, as this is the highest in energy. | EduRev Chemistry Question is disucussed on EduRev Study Group by 130 Chemistry Students. In a neutral O 2 molecule, there are a total of 12 valence shell electrons shared between the bonded atoms. The number of unpaired electrons in O2+ and O22- is, respectively, 1 and 0. In the species O2, O2+, O2- and O22- the correct decreasing order of bond strength is Can you explain this answer? Reason: According to molecular orbital theory O 2 + has 15 electrons &it has one electron in antibonding orbital. Determine which of the following statements are true and which are false. It is sigma2s(2)sigma2s*(2)sigma2p(2)pi2p(4)pi2p*(4) Bond order 1. KCET 2016: The increasing order of bond order of O2, O2+ , O2- and O2- is (A) O2+, O2 , O2- ,O2- (B) O22-,O2- , O2+, O2 (C) O2,O2+,O2- ,O2- (D) O22- 3 Bond energy and bond order both increase with decreasing bond length. Bond strengths in discussion 1.5 and 2 O2 has bond order both increase with decreasing bond.! 1/2 ( 8-5 ) = 1.5 = Paramagnetic strength is true of false - a orbital, as is... Increase bond order of o2 o2+ o2- o22- decreasing bond length two because O=O is a double bond N a. 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