Which molecule `AX_(3),AX_(4),AX_(5),AX_(6)` is most likely to have a trigonal bipyramidal structure if A has no lone pair?

Compare the shapes of p-orbital and sp-hybrid orbital Which on has a greater directional orientation ? (b) What are the hybridisation state of each C-atom in the following molecules ? (i) Benzene (ii) CH_(3) CH_(2) CH_(2) CH_(3) (iii) HC -= CH (iv) CH_(2) =CH- CH= CH_(2) (v) CH_(3) - CH =CH - CH_(3) (c ) What hybidisation is expected on the central atom of each of the following molecules ? (d) (i) Which molecule AX_(3),AX_(4),AX_(5),AX_(6) is likely to have to a trigonal bipyramid structure (ii) If the central atom A has no lone pairs, what type of hybridisation will it have .

Which of the following has trigonal bipyramidal structure?

The PCl_(5) molecule has trigonal bipyramidal structure. Therefore, the hybridization of p orbitals should be

Which of the molecules has trigonal bipyramidal geometry with bond angles 120^(@) and 90^(@) ?

What are the possible geometrical shapes of covalent molecules of the general formula AX_(2) and AX_(3) (X=a monovalent atom) when the central atom A has (i) no lone pair of electrons, (ii) one lone pair of electrons and (iii) two lone pairs of electrons.

Predict the dipole moment of : (i) a molecule of the type AX_(4) having square planar geometry (ii) a molecule of type AX_(5) having trigonal bipyramidal geometry (iii) a molecule of the type AX_(6) having octahedral geometry.

Why is that in the SF_(4) molecule, the lone pair of electrons occupies an equatorial position in the overall trigonal bipyramidal arrangement in preferencr to an axial position ?

Statement : SF_4 has lone pair of electron at equatorial position in preference to axial position in the overall trigonal bipyramidal geometry . Explanation : If lone pair is at equatorial position , then only repulsion is minimum .