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प्रश्न
In solid state \[\ce{PCl5}\] is a ______.
विकल्प
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?
Compare the oxidizing action of F2 and Cl2 by considering parameters such as bond dissociation enthalpy, electron gain enthalpy and hydration enthalpy.
Write two uses of ClO2.
Write the reactions of F2 with water.
Arrange the following in the order of property indicated for the given set:
HF, HCl, HBr, HI - increasing acid strength.
Complete chemical reactions are:Cl2 + H2O →
Select the correct alternative from the choices given :
The correct order of increasing acidic strength of the oxoacids of chlorine is:
Which is the strongest acid in the following:
Bond dissociation enthalpy of E–H (E = element) bonds is given below. Which of the compounds will act as the strongest reducing agent?
| Compound | \[\ce{NH3}\] | \[\ce{PH3}\] | \[\ce{AsH3}\] | \[\ce{SbH3}\] |
| Δdiss (E – H)/kJ mol–1 | 389 | 322 | 297 | 255 |
Reduction potentials of some ions are given below. Arrange them in decreasing order of oxidising power.
| Ion | \[\ce{CIO^{-}_{4}}\] | \[\ce{IO^{-}_{4}}\] | \[\ce{BrO^{-}_{4}}\] |
| Reduction potential EΘ/V |
EΘ = 1.19 V | EΘ = 1.65V | EΘ = 1.74 V |
Which of the following is isoelectronic pair?
Which of the following statements are true?
(i) Only type of interactions between particles of noble gases are due to weak dispersion forces.
(ii) Ionisation enthalpy of molecular oxygen is very close to that of xenon.
(iii) Hydrolysis of XeF6 is a redox reaction.
(iv) Xenon fluorides are not reactive.
Give reason to explain why ClF3 exists but FCl3 does not exist.
Solubility of iodine in water may be increase by adding
The reaction \[\ce{3ClO- (aq) -> ClO3- (aq) + 2Cl- (aq) + 2Cl- (aq)}\] is an example of
