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PCl(5) is an example of a molecule havin...

`PCl_(5)` is an example of a molecule having `sp^(3)d`-hybridisation. Three out of the orbitals in `sp_(x)p_(y)`-hybridisation while remaining two have `p_(x)d_(x^(2))`-hybridisation. If P-atom is attached to substitutuents differ in electronegativity, as in `PCl_(x)F_(5-x)`, then it is has been experimently observed that the more electronegativity substituent occupies the axial position of t.b.p geometry.
Q. The incorrect statement regarding `PCl_(2)F_(2)^-` molecule will be:

A

given compound is polar

B

both axial position occupied by F-atoms

C

both Cl atoms present in equatorial position

D

one Cl atom present at axial and other Cl atom is present at equatorial position of geometry

Text Solution

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The correct Answer is:
D
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PCl_(5) is an example of a molecule having sp^(3)d -hybridisation. Three out of the orbitals in sp_(x)p_(y) -hybridisation while remaining two have p_(x)d_(x^(2)) -hybridisation. If P-atom is attached to substitutuents differ in electronegativity, as in PCl_(x)F_(5-x) , then it is has been experimently observed that the more electronegativity substituent occupies the axial position of t.b.p geometry. Q. The highest H-C-H bond angle present in :

PCl_(5) is an example of a molecule having sp^(3)d -hybridisation. Three out of the orbitals in sp_(x)p_(y) -hybridisation while remaining two have p_(x)d_(x^(2)) -hybridisation. If P-atom is attached to substitutuents differ in electronegativity, as in PCl_(x)F_(5-x) , then it is has been experimently observed that the more electronegativity substituent occupies the axial position of t.b.p geometry. Q. The highest H-C-H bond angle present in :

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The concept of hybridisation has been introduced to explain the shapes of molecules. It involves the intermixing of two or more atomic orbitals belonging to same atom but in or more atomic orbitals beloging to sasme atom but in different sub-shells so as to intermix and redistibute energies to from equivalent orbitals called hybrid orbitals.Depending upon toh enumber and nature of the orbitals involved, the hybridisation may be divided into sp (linear), sp^(2) (trigonal), sp^(3) (tetrahedral), sp^(3)d (trigonal bipyramidal), sp^(3)d^(3) (octahedral) and sp^(3)d^(3) (pentagonal bipyramidal) types. it may be noted that the orbitals of isolated atoms never hybridise and they do so at the time of bond formation. The hybrid state of carbon in C_(2)H_(2) is same as that of carbon in:

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