MCQ
The high density of water compared to ice is due to
- ✓Hydrogen bonding interactions
- BDipole-dipole interactions
- CDipole-induced dipole interactions
- DInduced dipole-induced dipole interactions
✓
Answer
Correct option: A.
Hydrogen bonding interactions
(a) Water is dense than ice because of hydrogen bonding interaction and structure of ice.
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
Following eclipsed form of propane is repeated after rotation by an angle of......$^o$
→During change of $O_2$ to $O_2^-$ ion, the electron adds on which one of the following orbitals?
→Given
→$XNa_2HAsO_3 + YNaBrO_3 + ZHCl \longrightarrow$
$NaBr + H_3AsO_4 + NaCl$
The values of $X, Y$ and $Z$ in the above redox reaction are respectively
$C{H_3} - C{H_2} - C \equiv CH\mathop {\xrightarrow{R}}\limits_{{H_2}O} $ Butanone, $R$ is
→In a one-litre flask, 6 moles of $A$ undergoes the reaction $A(\mathrm{~g}) \rightleftharpoons \mathrm{P}(\mathrm{g})$. The progress of product formation at two temperatures (in Kelvin), $\mathrm{T}_1$ and $\mathrm{T}_2$, is shown in the figure:
→If $T_1=2 T_2$ and $\left(\Delta G_2^{\Theta}-\Delta G_1^{\varphi}\right)=R T_2 \ln x$, then the value of $x$ is. . . . .
$\left[\Delta G_1^\theta\right.$ and $\Delta G_2^\theta$ are standard Gibb's free energy change for the reaction at temperatures $T_1$ and $T_2$, respectively.]
The most stable carbocation is
If $5.85\,gms$ of $NaCl$ are dissolved in $90\,gms$ of water, the mole fraction of $NaCl$ is
→$B.P.$ of branched chain alkanes as compared to straight chain alkanes are
→Stability order of following carbocation's
→$(i)\,\begin{array}{*{20}{c}}
{C{H_3} - \mathop C\limits^ \oplus - C{H_3}} \\
| \\
{\,\,\,\,\,\,OC{H_3}}
\end{array}$
$(ii)\,\begin{array}{*{20}{c}}
{C{H_3} - \mathop C\limits^ \oplus - C{H_3}} \\
| \\
{\,\,\,\,\,\,C{H_3}}
\end{array}$
$(iii)\begin{array}{*{20}{c}}
{C{H_3} - \mathop C\limits^ \oplus {H_2} - NH} \\
{\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,|} \\
{\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,C{H_3}}
\end{array}$
$(iv)\,C{H_3} - \mathop C\limits^ \oplus {H_2}$
The oxidation states of phosphorus vary from