Advertisements
Advertisements
Question
Explain why:
(1) Interhalogen compounds are more reactive than the related elemental halogens.
(2) Sulphur exhibits the tendency for catenation but oxygen does not.
(3) On being slowly passed through water, PH3 forms bubbles but NH3 dissolves.
Solution
(1)
This is because these are polar and have lower bond energies.
(2)
This is because of higher S - S bond energy `((213"kJ")/"mol")` as compared to O-O bond energy `((138"kJ")/"mol")`
(3)
This is because PH3 is insoluble in water (HOH-bonds) but NH3 is highly soluble in water due to H-bonds.
APPEARS IN
RELATED QUESTIONS
Draw structure of Chlorine trifluoride
Find the INCORRECT match.
Which among the following pairs of halogen forms the interhalogen compound of the type \[\ce{XX^{'}_7}\]?
What is the oxidation state of bromine in the product?
\[\ce{Br2 + \underset{(excess)}{3F2} ->?}\]
The CORRECT statement about bromine trifluoride is:
The bent T-shaped interhalogen is ____________.
Which of the following interhalogen is a colourless liquid at room temperature?
BrF undergoes disproportionation to form Br2 and another interhalogen compound. What is the oxidation state of Br in this interhalogen compound?
What type of hybridization is observed in interhalogen compounds of the type \[\ce{XX^'_3}\]?
Which of the following is not the characteristic of interhalogen compounds?
