Advertisements
Advertisements
Question
Give reasons Fluoride ion has higher hydration enthalpy than chloride ion.
Advertisements
Solution
Fluoride ion is smaller in size than the chloride ion. Hence, when the two are dissolved in water, the energy of hydration released in the case of fluoride ion will be more than chloride ion due to stronger interactions (ion-dipole) between the ion and the water molecules in the former. Fluorine being more electronegative than chlorine will form stronger H-bonds with hydrogen present in the water molecule.
`triangleH_("hyd")F^(-) > triangle H_("hyd") Cl^(-)`
RELATED QUESTIONS
Write the IUPAC name of the given compound:
Name the following compound according to the IUPAC system.
Write the IUPAC name of the following compound:
C6H5 – O – C2H5
3-Methylbutane-2-ol on heating with HI gives ______
Write IUPAC name of the following compound (CH3)2 N − CH2CH3
Write structural formulae for 1-Ethylcyclohexanol.
Write structural formulae for Cyclohex-2-en-1-ol.
Glycerol is ____________.
Give IUPAC names of the following compound:
\[\begin{array}{cc}
\phantom{..}\ce{H}\phantom{...}\ce{CH3}\phantom{.}\ce{H}\phantom{..}\\
\phantom{}|\phantom{....}|\phantom{....}|\phantom{}\\
\ce{H - C - C - C - H}\\
\phantom{}|\phantom{....}|\phantom{....}|\phantom{}\\
\phantom{.}\ce{H}\phantom{...}\ce{OH}\phantom{.}\ce{H}\phantom{.}\\
\end{array}\]
Explain why Lewis acid is not required in bromination of phenol?
