Single Choice

The ice floats on water because:

Asolids have lesser density than liquids
Bit has open-cage like structure in which lesser molecules are packed per mL than water
Correct Answer
Cice is lighter than water
Dwhen ice is formed water molecules come closer and start floating.

Solution

in the solid state (ice), intermolecular interactions lead to a highly ordered but loose structure in which each oxygen atom is surrounded by $$4$$ hydrogen atoms; two of these hydrogen atoms are covalently bonded to the oxygen atom, and the two others (at longer distances) are hydrogen bonded to the oxygen atom’s unshared electron pairs.
this open structure of ice causes its density to be less than that of the liquid state, in which the ordered structure is partially broken down and the water molecules are (on average) closer together. When water freezes, a variety of structures are possible depending on the conditions. $$9$$ different forms of ice are known and can be interchanged by varying external pressure and temperature.

SIMILAR QUESTIONS

Chemical Bonding

The low density of ice compared to water is due to:

Chemical Bonding

Statement 1 : Conc $$\mathrm{H}_{2}\mathrm{S}\mathrm{O}_{4}$$ is a low volatility and viscos nature acid. Statement2: lt is due to Hydrogen bonding.

Chemical Bonding

Identify the correct statement(s) given below. (a) $$O_2$$ is paramagnetic. (b) $$H_2O$$ is liquid while $$H_2S$$ is gas under given conditions. (c) Boiling point of $$H_2O$$ is abnormally high.

Chemical Bonding

The correct order of boiling point is:

Chemical Bonding

The electronegativities of nitrogen and chlorine are almost same. However, $$NH_3$$ exists as liquid whereas $$HCl$$ as gas due to __________ between the molecules of $$NH_3$$.

Chemical Bonding

Hydrogen bonding plays a central role in the following phenomena :

Chemical Bonding

In solid ice, oxygen atom is surrounded

Chemical Bonding

Hydrogen halide with the highest boiling point is:

Chemical Bonding

Which of the following observations can be explained on the basis of hydrogen bonding? (i) $$H-F$$ has higher boiling point than other halogen acids. (ii) $$H_2O$$ has highest boiling point among hydrides of group 16 elements. (iii) $$NH_3$$ has lower boiling point than $$PH_3$$.

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