MCQ
Arrange the following in order of increasing dipole moment : $H_2O, H_2S, BF_3.$
- ✓$BF_3 < H_2S < H_2O$
- B$H_2S < BF_3 < H_2O$
- C$H_2O < H_2S < BF_3$
- D$BF_3 < H_2O < H_2S$
In $H _2 S$ and $H _2 O$ due to unsymmetrical structure net $+ve$ dipole is there. $H _2 O$ has a higher dipole due to the higher electronegativity of oxygen than sulphur.
Hence, the correct order is: $BF _3\,<\, H _2 S \,<\, H _2 O$.
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$\mathrm{Li}_{2} \mathrm{O}, \mathrm{CaO}, \mathrm{Na}_{2} \mathrm{O}_{2}, \mathrm{KO}_{2}, \mathrm{MgO}$ and $\mathrm{K}_{2} \mathrm{O}$
$O ^{2-}, F ^{-}, Al , Mg ^{2+}, Na ^{+}, O ^{+}, Mg , Al ^{3+}, F$