Question

The hydrogen bonding in oxygen compounds is more significant than that in sulphur compounds because oxygen is (1) a very small atom compared to the sulphur atom (2) more electroncgative than sulphur (3) more reactive than sulphur (4) a gas where as sulphur is a solid at room temperature

Short answer

Options (1) and (2).

Step-by-step solution

Identify the properties of oxygen

Oxygen is a very small atom and has high electronegativity. Consider these properties while evaluating the options.

Compare oxygen with sulphur regarding size

Oxygen is smaller in size compared to sulphur. Smaller atoms generally form stronger hydrogen bonds. This corresponds to option (1).

Compare oxygen with sulphur regarding electronegativity

Oxygen is more electronegative than sulphur. Higher electronegativity leads to stronger hydrogen bonding. This corresponds to option (2).

Analyze reactivity

Although oxygen is reactive, reactivity is not a primary factor in hydrogen bond formation. Option (3) is incorrect.

State of matter comparison

The physical state (gas for oxygen and solid for sulphur at room temperature) does not directly influence hydrogen bonding. Option (4) is irrelevant to hydrogen bonding strength.

Conclusion

The significant factors for stronger hydrogen bonding in oxygen compounds are the smaller size and higher electronegativity of oxygen. Hence, options (1) and (2) are correct.

Key concepts

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons.
Elements with higher electronegativity tend to pull electrons more strongly towards themselves.
This concept is important in understanding why oxygen forms stronger hydrogen bonds than sulphur.
Oxygen has a higher electronegativity than sulphur. This means that in an oxygen-hydrogen bond, the oxygen atom pulls electrons closer, creating a partial negative charge on the oxygen and a partial positive charge on the hydrogen.
This partial charge difference leads to stronger hydrogen bonding.
In contrast, sulphur's lower electronegativity results in weaker partial charges and, consequently, weaker hydrogen bonds.

• Oxygen's electronegativity leads to stronger hydrogen bonds.
• Electronegativity differences are crucial in bond formation.
• Stronger hydrogen bonds mean more significant interactions between molecules.

Atomic Size

Atomic size refers to the physical dimensions of an atom.
Smaller atoms can pack closer together, influencing how atoms bond with each other.
Oxygen is a smaller atom compared to sulphur. This smaller size allows oxygen to form stronger hydrogen bonds because the atoms are nearer to each other, and the attractive forces are stronger.
In comparison, sulphur's larger atomic size means the atoms cannot get as close together; this results in weaker hydrogen bonds.

• Oxygen's smaller size enables stronger hydrogen bonds.
• Proximity of atoms is key for bond strength.
• Smaller atoms generally lead to stronger interactions.

Oxygen vs Sulphur

Oxygen and sulphur are both in Group 16 of the periodic table, but they have distinct differences.
Understanding these differences helps explain why oxygen forms stronger hydrogen bonds.

Electronegativity: As stated earlier, oxygen is more electronegative than sulphur, leading to stronger hydrogen bonding.

Atomic Size: Oxygen is smaller in size compared to sulphur, allowing for closer proximity and stronger bonds.

Reactivity and Physical State: While reactivity and physical state also differ, these factors are less relevant to hydrogen bonding.

• Oxygen is more electronegative than sulphur.
• Oxygen's smaller size makes it bond more effectively.
• Differences in reactivity and state do not significantly impact hydrogen bonding.