Identify which molecule in each of the following pairs has stronger $H$-bonding:
$(i)$ $H_2O$ and $H_2S$
$(ii)$ $NH_3$ and $PH_3$
$(iii)$ $HF$ and $HCl$
$(i)$ $H_2O$ and $H_2S$
$(ii)$ $NH_3$ and $PH_3$
$(iii)$ $HF$ and $HCl$
(A) $(i)$ $H_2O$ has stronger $H$-bonding than $H_2S$ because oxygen is more electronegative than sulfur.
$(ii)$ $NH_3$ has stronger $H$-bonding than $PH_3$ because nitrogen is more electronegative than phosphorus.
$(iii)$ $HF$ has stronger $H$-bonding than $HCl$ because fluorine is more electronegative than chlorine.
In all cases,the strength of $H$-bonding depends on the electronegativity of the atom bonded to the hydrogen atom.
$(ii)$ $NH_3$ has stronger $H$-bonding than $PH_3$ because nitrogen is more electronegative than phosphorus.
$(iii)$ $HF$ has stronger $H$-bonding than $HCl$ because fluorine is more electronegative than chlorine.
In all cases,the strength of $H$-bonding depends on the electronegativity of the atom bonded to the hydrogen atom.
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Similar Questions
The correct statement/s about Hydrogen bonding is/are:
$A$. Hydrogen bonding exists when $H$ is covalently bonded to a highly electronegative atom.
$B$. Intermolecular $H$ bonding is present in $o$-nitrophenol.
$C$. Intramolecular $H$ bonding is present in $HF$.
$D$. The magnitude of $H$ bonding depends on the physical state of the compound.
$E$. $H$-bonding has a powerful effect on the structure and properties of compounds.
Choose the correct answer from the options given below:
$A$. Hydrogen bonding exists when $H$ is covalently bonded to a highly electronegative atom.
$B$. Intermolecular $H$ bonding is present in $o$-nitrophenol.
$C$. Intramolecular $H$ bonding is present in $HF$.
$D$. The magnitude of $H$ bonding depends on the physical state of the compound.
$E$. $H$-bonding has a powerful effect on the structure and properties of compounds.
Choose the correct answer from the options given below:
Intramolecular $H$-bond is present in
Medium
View SolutionWater,Ethanol,and Ether are all liquids at room temperature; why do their boiling points differ?
Medium
View SolutionThe hydrides of the first elements in groups $15-17$, namely $NH_3$, $H_2O$ and $HF$ respectively show abnormally high values for melting and boiling points. This is due to
$HF$ has the highest boiling point among hydrogen halides because it has:
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