ChemistryAdvancedHigh School (11–12)Chemical Bonding › Molecular Orbitals and Hydrogen BondsNEETJEE Main
Created by StemPy LabMolecular orbital theory gives a bond order of and two unpaired electrons, so oxygen is paramagnetic. A student looks for a diatomic species of a second period element that has the same bond order as but is diamagnetic. Use the correct energy order of the orbitals for each species. Which species fits?
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← A student lists five statements about hybridisation. (i) In PCl₅, phosphorus is sp³d hybridised, and the two axial bonds are longer than the three equatorial bonds. (ii) In SF₆, sulphur mixes one 3s, three 3p and two 3d orbitals. (iii) In ethyne, each carbon uses two sp orbitals for σ bonds and two 2p orbitals for π bonds. (iv) In ammonia, nitrogen is sp² hybridised, with its lone pair in a p orbital. (v) Only half-filled orbitals can take part in hybridisation. How many of these statements are correct?Molecular orbital theory uses one energy order up to N₂ and another for O₂ and F₂. Read two statements about how this order shows in real molecules. Statement I: In the C₂ molecule, both bonds of the double bond are π bonds, because the four electrons after σ^* 2s go into the two π 2p orbitals. Statement II: If σ 2pz lay below the π 2p pair in B₂, as it does in O₂, then B₂ would be diamagnetic. →
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