Question

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Answer 1

Explanation:

1.

(1) pcl5= phosphorous penta chloride

(2) sF6= sulphur hexa flouride

(3) Iodine hepta flouride

2. axial bonds are vertical bonds and equitorial bonds are horizontal bonds.

horizontal bonds are shorter than vertical bonds.

so, so, axial bonds are longer when compared to equitorial bonds.

Answer 2

1) i) Phosphorus atom is sp3d hybridized in the excited state. The geometry of PCl5 is trigonal bipyramidal . ... The remaining two P-Cl bonds (axial bonds) lie above & below the plane of the triangle at bond angle 90°.

ii) These six orbitals get hybridised to form six sp3d2hybrid orbitals. Each of these sp3d2 hybrid orbitals overlaps with 2p orbital of fluorine to form S-F bond. Thus, SF6 molecule has octahedral structure as shown in fig.1.28. The dotted electrons represent electrons from F-atoms.

iii) When it is bonded to seven Fluorine atoms through sigma bonds, the total number of electron pairs around Iodine becomes 7 with no lone pair of electrons left. Thus the hybridisation of IF7 is sp3d3 with no lone pair of electrons and this corresponds to pentagonal bipyramidal geometry.

2) The axial bonds are longer than equatorial bonds because the axial Cl atoms suffer from more repulsion then the equatorial Cl atoms,as a result the axial Cl atoms tries to reside far away from the equatorial Cl atoms, & hence axial bond are longer than equatorial bonds.

3) [Ni(CN)4]2- is a square planar geometry formed by dsp2 hybridisation and not tetrahedral by sp3. [Ni(CN)4]2- is diamagnetic, so Ni2+ ion has 3d8 outer configuration with two unpaired electrons.

4) Didn't understood the question .sorry

Hope it helps you !!!