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प्रश्न
With what neutral molecule is ClO− isoelectronic? Is that molecule a Lewis base?
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उत्तर
ClO− is isoelectronic to ClF. Also, both species contain 26 electrons in all as shown.
Total electrons ClO− = 17 + 8 + 1 = 26
In ClF = 17 + 9 = 26
ClF acts like a Lewis base because the Cl atom has three lone pairs of electrons and can combine further with F to form ClF3.
संबंधित प्रश्न
Iodine exists as
- polar molecular solid
- ionic solid
- nonpolar molecular solid
- hydrogen bonded molecular solid
Fluorine is a stronger oxidising agent than chlorine. Why?
Account for the following :
Acidic character increases from HF to HI.
F2 has lower bond dissociation enthalpy than Cl2. Why?
Give two examples to show the anomalous behaviour of fluorine.
Arrange the following in the order of property indicated for the given set:
HF, HCl, HBr, HI - increasing acid strength.
Arrange the following in the decreasing order of their reducing character :
HF, HCl, HBr, HI
Cl2 acts as a bleaching agent.
Fluorine differs from the rest of the halogens in some of its properties. This is due to ____________.
The set with the correct order of acidity is:
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 |
In solid state \[\ce{PCl5}\] is a ______.
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 |
Give reason to explain why ClF3 exists but FCl3 does not exist.
Solubility of iodine in water may be increase by adding
Iodine has lowest oxidiation state in ______.
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.
Arrange the following in the increasing order of the property mentioned:
MF, MCl, MBr, MI (ionic character)
