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Atoms bond to achieve potential energy minimization through electron density redistribution. Think of bonding as an energetic negotiation: as two nuclei approach, attractive nuclear-electron forces compete against inter-electronic and internuclear repulsions. The optimal internuclear distance defines the equilibrium bond length at the absolute potential energy minimum. Chemical Bonding serves as the structural backbone for the entire JEE/NEET syllabus, seamlessly linking atomic periodicity to organic reaction mechanisms and inorganic coordination geometry. Aspirants frequently falter by viewing molecular geometry as arbitrary memorization rather than a spatial minimization of electrostatic repulsion (VSEPR) or constructive quantum wave interference (VB & MO theories). Mastery demands predicting central atom hybridization, lone pair distortions, bond order, and magnetic behavior systematically. Quantifying fractional charges via formal charge and dipole moments resolves ambiguities between localized covalent models and delocalized molecular orbitals.
Assuming species with identical central atom hybridization always share identical molecular shapes (e.g., classifying , , and as all having tetrahedral shapes).
Applying a single orbital energy ordering for all diatomic species in Molecular Orbital Theory regardless of atomic number.
Assuming all alkali and alkaline earth metal halides are ionic without considering Fajan's Rules, leading to wrong melting point predictions for compounds like or .
Questions Asked: 4
Topics: VSEPR Theory & Hybridization, Molecular Orbital Theory (MOT), Dipole Moment & Fajan's Rule
Questions Asked: 3
Topics: MOT & Bond Order, Hydrogen Bonding, Lewis Structures & Formal Charge
Questions Asked: 4
Topics: Hybridization of Odd-Electron Species, Dipole Moment Vectors, MOT Paramagnetism
According to Molecular Orbital Theory, which of the following ionic species has a bond order of and is paramagnetic?
Calculate total electron count for : neutral has electrons, so contains electrons.
Write the MO electronic configuration for electrons ( electron system): .
Calculate bond order using . Since there is unpaired electron in the orbital, the species is paramagnetic.
Using VSEPR theory, identify the pair of species having identical molecular geometry and identical number of lone pairs on the central atom:
Calculate steric number for : ( hybridization). It has bond pairs and lone pairs on , yielding a linear molecular geometry.
Calculate steric number for central iodine in : ( hybridization). It has bond pairs and lone pairs on the central atom.
Conclude that both and possess lone pairs on their central atoms and adopt an identical linear molecular shape with a bond angle of .
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Click HereValence Bond Theory incorrectly predicts all electrons in to be paired. According to Molecular Orbital Theory, the last two electrons fill the degenerate antibonding orbitals and . By Hund's rule of maximum multiplicity, these two electrons occupy separate orbitals with parallel spins: . The presence of these unpaired electrons makes paramagnetic.
Apply Drago's Rule. When a central atom from Period 3 or below is bonded to terminal atoms of low electronegativity (like ), hybridisation does not take place. Bonding occurs almost purely through unhybridized -orbitals, locking bond angles near (e.g., , ). In contrast, undergoes full hybridisation, yielding a significantly larger bond angle of .
Use the steric number formula . Count central valence electrons , add surrounding monovalent atoms (ignore divalent oxygen), adjust for ion charge, and divide by . Direct mapping: , , , , . Subtract bond pairs from to get lone pairs () and instantly determine shape.
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