Advertisements
Advertisements
Question
Which of the following is isoelectronic pair?
Options
\[\ce{ICI2, ClO2}\]
\[\ce{BrO^{-}_{2}, BrF^{+}_{2}}\]
\[\ce{ClO2, BrF}\]
\[\ce{CN^{-}, O3}\]
Advertisements
Solution
\[\ce{BrO^{-}_{2}, BrF^{+}_{2}}\]
Explanation:
\[\ce{BrO^{-}_{2}}\] (35 + 2 × 8 + 1 = 52)
And
\[\ce{BrF^{+}_{2}}\] (35 + 2 × 9 – 1 = 52)
APPEARS IN
RELATED QUESTIONS
Iodine exists as
- polar molecular solid
- ionic solid
- nonpolar molecular solid
- hydrogen bonded molecular solid
Draw structure of Chlorine pentafluoride
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.
Account for the following :
Acidic character increases from HF to HI.
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
Give two examples to show the anomalous behaviour of fluorine.
Write the reactions of F2 with water.
With what neutral molecule is ClO− isoelectronic? Is that molecule a Lewis base?
Select the correct alternative from the choices given :
The correct order of increasing acidic strength of the oxoacids of chlorine is:
Which one has the lowest boiling point?
The set with the correct order of acidity is:
In solid state \[\ce{PCl5}\] is a ______.
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.
Write the name and formula of oxoacid of fluorine.
