Home
Class 12
CHEMISTRY
Which one of PCl(4)^(+) & PCl(4)^(-) is ...

Which one of `PCl_(4)^(+)` & `PCl_(4)^(-)` is not likely to exist, why?

Text Solution

Verified by Experts

`PCl_(4)^(-)` has no existence because 10 electrons cannot be accommodated in four `sp^(3)` -hybrid orbitals of P-atom.
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • P-BLOCK ELEMENTS

    CHHAYA PUBLICATION|Exercise SOLVED NCERT TEXTBOOK PROBLEMS|58 Videos

  • P-BLOCK ELEMENTS

    CHHAYA PUBLICATION|Exercise NCERT EXERCISE QUESTIONS|49 Videos

  • P-BLOCK ELEMENTS

    CHHAYA PUBLICATION|Exercise SLOVED WBCHSE SCANNER|31 Videos

  • ORGANIC CHEMISTRY : BASIC PRINCIPLES AND TECHNIQUES

    CHHAYA PUBLICATION|Exercise WARM UP EXERICSE|132 Videos

  • POLYMERS

    CHHAYA PUBLICATION|Exercise SOVLED CBSE SCANNER|18 Videos

Similar Questions

Explore conceptually related problems

In the soild state , PCl_(5) exists in the lonic form as [PCl_(4)]^(+) [PCl_(6)]^(-) . What are the shapes of these two ions ? Why ?

Why does the PCl_(5) exist but NCl_(5) does not ?

The shape of PCl_5 is

PCl_(3) fumes is moist air - explain.

(i) why does the PCl_(5) exist but NCl_(5) does not? (ii) why does BaSO_(4) not soluble in water?

How does PCl_(5) exist in the solid state ?

In a certain polar solvent, PCl_(5) undergoes ioonisation as follows: 2PC l_(5) hArr PCl_(4)^(+)+PCl_(6)^(-) , predict geometrical shapes of all the species involved.

In a certain polar solvent, PCl_(5) undergoes ioonisation as follows: 2PC l_(5) hArr PCl_(4)^(+)+PCl_(6)^(-) , predict geometrical shapes of all the species involved.

All the P - Cl bonds in PCl_(5) are not equivalent - why ?

Why PbI_(4) has no existence ?

Home
Profile