Question
Out of $\mathrm{H}_2 \mathrm{O}$ and $\mathrm{H}_2 \mathrm{S}$, which is more polar?
✓
Answer
$\mathrm{H}_2 \mathrm{O}$ is more polar than $\mathrm{H}_2 \mathrm{S}$ as oxygen is more electronegative than sulphur due to smaller size.
Need a full question paper?
Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.
Explore more
Similar questions
Why do hydrides and halides of Be polymerise?
For the following equilibrium, $\text{K}_{\text{c}}=6.3\times10^{14}\text{ at }1000\text{K}$
$\text{NO(g) + O}_3\text{(g)}\rightleftharpoons\text{NO}_2\text{(g) + O}_2\text{(g)}$
Both the forward and reverse reactions in the equilibrium are elementary bimolecular reactions. What is $\text{K}_{\text{c}}$, for the reverse reaction?
→$\text{NO(g) + O}_3\text{(g)}\rightleftharpoons\text{NO}_2\text{(g) + O}_2\text{(g)}$
Both the forward and reverse reactions in the equilibrium are elementary bimolecular reactions. What is $\text{K}_{\text{c}}$, for the reverse reaction?
What are Isoelectronic species?
A sample of hard water is allowed to pass through an anion exchanger. Will it produce lather will soap easily?
What geometry $CHCl _3$ possess?
→ Why group 2 elements (Mg and Ca) are harder and denser than group 1 elements?
Which of the following reactions will get affected by increasing the pressure? Also, mention whether change will cause the reaction to go into forward or backward direction.
$\text{CH}_4\text{ (g) + 2S}_2\text{ (g)}\rightleftharpoons\text{CS}_2\text{ (g) + 2H}_2\text{S}\text{ (g)}$
→$\text{CH}_4\text{ (g) + 2S}_2\text{ (g)}\rightleftharpoons\text{CS}_2\text{ (g) + 2H}_2\text{S}\text{ (g)}$
Give the IUPAC names of the following compounds:
Represent a galvanic cell in electrode and ions containing Cu electrode dipped in molar solution of copper sulphate and silver electrode dipped in molar solution of silver nitrate.
$\Big[\text{Given E}^\circ_{\frac{\text{Cu}^{2+}}{\text{Cu(s)}}}=0.34\text{V, E}^\circ_{\frac{\text{Ag}^+}{\text{Ag(s)}}}=0.80\text{V}\Big]$
→$\Big[\text{Given E}^\circ_{\frac{\text{Cu}^{2+}}{\text{Cu(s)}}}=0.34\text{V, E}^\circ_{\frac{\text{Ag}^+}{\text{Ag(s)}}}=0.80\text{V}\Big]$
Refer to the periodic table given in your book and now answer the following questions:
Select the possible non metals that can show disproportionation reaction.
Select the possible non metals that can show disproportionation reaction.