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प्रश्न
Which of the following is isoelectronic pair?
पर्याय
\[\ce{ICI2, ClO2}\]
\[\ce{BrO^{-}_{2}, BrF^{+}_{2}}\]
\[\ce{ClO2, BrF}\]
\[\ce{CN^{-}, O3}\]
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उत्तर
\[\ce{BrO^{-}_{2}, BrF^{+}_{2}}\]
Explanation:
\[\ce{BrO^{-}_{2}}\] (35 + 2 × 8 + 1 = 52)
And
\[\ce{BrF^{+}_{2}}\] (35 + 2 × 9 – 1 = 52)
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संबंधित प्रश्न
Draw structure of Chlorine pentafluoride
Account for the following :
Acidic character increases from HF to HI.
F2 has lower bond dissociation enthalpy than Cl2. Why?
Write two uses of ClO2.
Arrange the following in the order of property indicated for the given set:
HF, HCl, HBr, HI - increasing acid strength.
Select the correct alternative from the choices given :
The correct order of increasing acidic strength of the oxoacids of chlorine is:
Tincture of iodine is ____________.
The set with the correct order of acidity is:
Which is the strongest acid in the following:
Which of the following pairs of ions are isoelectronic and isostructural?
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 |
Give reason to explain why ClF3 exists but FCl3 does not exist.
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.
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.
Arrange the following in the increasing order of the property mentioned:
MF, MCl, MBr, MI (ionic character)
