Use energy levels of diatomic molecules derived from molecular orbital theory to

Question

Use energy levels of diatomic molecules derived from molecular orbital theory to predict the magnetic properties of the oxygen molecule O_2 and the peroxide anion O_2 and the peroxide anion O_2^2-. a. oxygen (paramagnetic); peroxide (paramagnetic) b. oxygen (diamagnetic); peroxide (paramagnetic) c. oxygen (paramagnetic); peroxide (diamagnetic) d. Neither have magnetic properties, only metals have magnetic properties. e. oxygen (diamagnetic); peroxide (diamagnetic) Oxygen has two common molecular anions: peroxide and superoxide (O_2^2-) and superoxide (O_2^-). Use the MO energy level diagram below to identify which one of the following statements is not correct. These molecular orbitals are formed from the 2s and 2p atomic orbitals. a. The bond order of the peroxide is 1. b. The superoxide has a shorter bond than the peroxide. c. Like O_2, the peroxide is paramagnetic. d. The superoxide has a stronger bond than the peroxide. e. oxygen, O_2, has a stronger bond than either these oxides. Predict the bond order of the NO^- molecular ion. a. 2.5 b. 1.5 c. 2 d. 3 e. 1

Explanation / Answer

O2 has 12 valence electrons.

Its MO configuration is: O2 = KK(2s) 2 (2s*)2 (2p) 2 (2p) 2 (2p) 2 (2p*)1=(2p*)1 with one electron in each of the 2p* orbitals spin aligned .

O2 has two unpaired electrons in its * orbitals. Hence oxygen is paramagnetic.

O2 2– has 14 valence electrons, with four electrons in the * orbitals . hence it is diamagnetic

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