At room temperature and pressure, $$$\mathrm{H}_{2} \mathrm{O}$$$ is a liquid and $$$\mathrm{H}_{2} \mathrm{~S}$$$ is a gas. What is the reason for this difference of state?

O has higher first and second ionisation energies than S .

The covalent bond between O and H is stronger than the covalent bond between S and H .

There is significant hydrogen bonding between $\mathrm{H}_{2} \mathrm{O}$ molecules but not between $\mathrm{H}_{2} \mathrm{~S}$ molecules.

The instantaneous dipole-induced dipole forces between $\mathrm{H}_{2} \mathrm{O}$ molecules are stronger than the instantaneous dipole-induced dipole forces between $\mathrm{H}_{2} \mathrm{~S}$ molecules.

Chemistry

IGCSE&ALevel

CAIE

Exam No：9701_m24_qp_12 Year：2024 Question No：8

Answer:

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3.5.1.1 more contents

3.5.1.2 more contents

3.5.1.3 more contents

3.5.1.4 more contents

3.5.1.5 more contents

3.5.1.6 more contents

3.5.1.7 more contents

3.5.2 predict the shapes of, and bond angles in, molecules and ions analogous to those specified in 3.5.1

At room temperature and pressure, $$\(\mathrm{H}_{2} \mathrm{O}\)$$ is a liquid and $$\(\mathrm{H}_{2} \mathrm{~S}\)$$ is a gas. What is the reason for this difference of state?

Answer:

Knowledge points:

Solution:

At room temperature and pressure, $$\(\mathrm{H}_{2} \mathrm{O}\)$$ is a liquid and $$\(\mathrm{H}_{2} \mathrm{~S}\)$$ is a gas. What is the reason for this difference of state?

Answer:

Knowledge points:

Solution:

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