Calculation Of Number Of pπ-pπ And dπ-dπ Bonds|Participation Of Orbitals In Hybridisation|XeF5- Pentagonal Planar|XeF6, IF6- Capped Octahedral / Distorted Octahedral |TeCl62-, SbCl63-, ICI6- Perfect Octahedral|Drago's Rule|Summary

Drago's Rule|Bonding In SO3|Bonding In SO2|Calculation Of Number of Pπ-Pπ Bonds and Dπ-Dπ Bonds|Comparison Of Bond Angle|Summary

Drago's Rule|Bonding In SO3|Bonding In SO2|Calculation Of Number of Pπ-Pπ Bonds and Dπ-Dπ Bonds|Comparison Of Bond Angle|Summary

Read the passage given below and answer the following questions : According to Valence Bond Theory, the metal atom or ion under the influence of ligands can use its (n-1)d, ns, np or ns, np, nd orbitals for hybridisation to yield a set of equivalent orbitals of definite geometry such as octahedral, tetrahedral, square planar and so on. These hybridised orbitals ar allowed to overlap with ligand rbitals that can donate electron pairs for bonding. Assertion (A) : In the diamagnetic octahedral complex, [Co(NH_(3))_(6)]^(3+) , the cobalt ion is in +3 oxidation state. Reason (R) : Six pairs of electrons, one from each NH_(3) molecule, occupy the six hybrid orbitals.

Hybridisation Of Elements Involving d Orbitals|Formation Of PCl5 (sp3d Hybridisation)|Formation Of SF6 (sp3d2 Hybridisation)|IF7|Bonding In SO3|Bonding In SO2|Calculation Of Number Of pπ-pπ And pπ-dπ Bonds|Summary

Find the number of species where d_(x^(2)-y^(2)) orbital participate in hybridisation . {:(XeF_(6),SF_(6),IF_(7),XeO_(3)),(PCl_(5),PF_(5),,):}

Hybridisation helps us to understand the geometry of the molecules. This is because hybridised orbitals are directed in space in some preferred directions to have stable arrangement, which determine the geometry. The common hybridisation are sp (linear), sp^(2) (trigonal planar), sp^(3) (tetrahedral), sp^(3)d (trigona bipyramidal), sp^(3)d^(2) (octahedral) and sp^(3)d^(3) (pentagonal bipyramidal). The presence of lone pairs in addition to bond pairs distort the geometry because "lone pair "-" lone pair repulsion"gt" lone pair "-" bond repulsion" gt" bond pair" -"bond pair repulsion" . What is the hybridisation and shape of XeF_(4) molecule?

Hybridisation helps us to understand the geometry of the molecules. This is because hybridised orbitals are directed in space in some preferred directions to have stable arrangement, which determine the geometry. The common hybridisation are sp (linear), sp^(2) (trigonal planar), sp^(3) (tetrahedral), sp^(3)d (trigona bipyramidal), sp^(3)d^(2) (octahedral) and sp^(3)d^(3) (pentagonal bipyramidal). The presence of lone pairs in addition to bond pairs distort the geometry because "lone pair "-" lone pair repulsion"gt" lone pair "-" bond repulsion" gt" bond pair" -"bond pair repulsion" . Give an example of molecule involving sp^(3) hybridisation.

Hybridisation helps us to understand the geometry of the molecules. This is because hybridised orbitals are directed in space in some preferred directions to have stable arrangement, which determine the geometry. The common hybridisation are sp (linear), sp^(2) (trigonal planar), sp^(3) (tetrahedral), sp^(3)d (trigona bipyramidal), sp^(3)d^(2) (octahedral) and sp^(3)d^(3) (pentagonal bipyramidal). The presence of lone pairs in addition to bond pairs distort the geometry because "lone pair "-" lone pair repulsion"gt" lone pair "-" bond repulsion" gt" bond pair" -"bond pair repulsion" . Which d - orbitals are involved in sp^(3)d^(2) hybridisation in SF_(6) molecule?