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प्रश्न
In solid state \[\ce{PCl5}\] is a ______.
पर्याय
covalent solid
octahedral structure
ionic solid with \[\ce{[PCl_{6}]^{+}}\] octahedral and \[\ce{[PCl_{4}]^{-} tetrahedra}\]
ionic solid with \[\ce{[PCl_{4}]^{+}}\] octahedral and \[\ce{[PCl_{6}]^{-} tetrahedra}\]
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उत्तर
In solid state \[\ce{PCl5}\] is a ionic solid with \[\ce{[PCl_{4}]^{+}}\] octahedral and \[\ce{[PCl_{6}]^{-} tetrahedra}\].
Explanation:
APPEARS IN
संबंधित प्रश्न
Iodine exists as
- polar molecular solid
- ionic solid
- nonpolar molecular solid
- hydrogen bonded molecular solid
Account for the following: Fluorine does not exhibit positive oxidation state.
Fluorine is a stronger oxidising agent than chlorine. Why?
F2 has lower bond dissociation enthalpy than Cl2. Why?
Which halogen compound in each of the following pairs will react faster in SN2 reaction
(CH3)3 C – Cl or CH3 – Cl
Why are halogens coloured?
With what neutral molecule is ClO− isoelectronic? Is that molecule a Lewis base?
Arrange the following in the decreasing order of their reducing character :
HF, HCl, HBr, HI
Select the correct alternative from the choices given :
The correct order of increasing acidic strength of the oxoacids of chlorine is:
Cl2 acts as a bleaching agent.
Tincture of iodine is ____________.
Which one has the lowest boiling point?
Fluorine differs from the rest of the halogens in some of its properties. This is due to ____________.
Which is the strongest acid in the following:
Which of the following is isoelectronic pair?
Give reason to explain why ClF3 exists but FCl3 does not exist.
Statement I: Acid strength increases in the order given as HF << HCl << HBr << HI.
Statement II: As the size of the elements F, Cl, Br, and I increase down the group, the bond strength of HF, HCl, HBr, and HI decreases and so the acid strength increases.
In the light of the above statements, choose the correct answer from the options given below.
Give a reason for the following:
Mn+2 compounds are more stable than Fe+2 compounds.
