Chemical Bonding And Molecular Structure

With you'll need to form a double bond between one of the Oxygen atoms and a Nitrogen atom to fill the octets and still use only the 24 valence electrons available for the molecule.Odd-electron moleculesIn molecules with an odd number of electrons like nitric oxide, NO and nitrogen dioxide, , the octet rule is not satisfied for all the atoms

i) Dipole moment , (cancelled out)ii) iii) iv) as Fluorine is more electronegative

To determine which molecules are attracted to an external magnetic field, we need to understand their magnetic properties, specifically if they are paramagnetic or diamagnetic. Paramagnetic substances, which have unpaired electrons, are attracted to an external magnetic field. Diamagnetic substances, with all electrons paired, are not attracted to the magnetic field. (Oxygen molecule): is paramagnetic due to the presence of two unpaired electrons in its molecular orbital configuration.$ $ (Nitrogen molecule): is diamagnetic because all its electrons are paired in the molecular orbital configuration.$ $ (Fluorine molecule): is diamagnetic as it has all paired electrons in its molecular orbital configuration.$ $ (Boron molecule): is paramagnetic because it has two unpaired electrons in its molecular orbital configuration.$ \mathrm{O}_2 \mathrm{B}_2$.

Isoelectronic Series and Bond OrderIsoelectronic SeriesAnisoelectronic seriesrefers to a group of molecules or ions that share the same number of electrons. These entities generally possess identical electronic configurations, leading to similar chemical and physical properties.Bond OrderThebond orderof a molecule can be determined using Molecular Orbital Theory. It is calculated with the formula: Application to , and 1. Molecular Orbital ConfigurationsNitrogen ( ): Bonding electrons:10 (2 from , 6 from , and 2 from )Antibonding electrons:4 (2 from and 2 from )Bond order calculation: Carbon Monoxide (CO):Total electrons: 6 (from C) + 8 (from O) = 14 Bonding electrons:10 (2 from , 6 from , and 2 from )Antibonding electrons:4 (2 from and 2 from )Bond order calculation: Nitrosyl Ion ( ):Total electrons: 7 (from N) + 8 (from O) - 1 (due to positive charge) = 14 Bonding electrons:10 (2 from , 6 from , and 2 from )Antibonding electrons:4 (2 from and 2 from )Bond order calculation: ConclusionAll three species, , , and , are isoelectronic as they each contain 14 electrons. Moreover, they share an identical bond order of 3.

: With 4 bonding pairs and 2 lone pairs around xenon, the most stable shape is square planar. : With 4 bonding pairs and 1 lone pair around sulfur, the most stable shape is see-saw.

Given:Three AB₃-type molecules I, II, III have dipole momentsI =0.0 DII =0.2 DIII =1.5 DKey conceptsTrigonal planar (AX₃, no lone pair)→ perfectly symmetrical →μ = 0Examples:BF₃, BCl₃Trigonal pyramidal (AX₃E, one lone pair)→ polar →μ ≠ 0Dipole moment depends on bond polarityanddirection.NH₃ vs NF₃NH₃:Bond dipoles and lone-pair dipole act in thesame direction→large μ ≈ 1.47 DNF₃:Bond dipoles oppose lone-pair dipole →small μ ≈ 0.24 DIdentificationI (0.0 D)→ must benonpolar trigonal planar⇒BF₃II (0.2 D)→ very small dipole moment⇒NF₃III (1.5 D)→ large dipole moment⇒NH₃✅ Correct option:AI : BF₃, II : NF₃, III : NH₃