\(O - O\) bond length in \(H _2 O _2\) is X than the \(O - O\) bond length in \(F _2 O _2\)The \(O - H\) bond length in \(H _2 O _2\)is Y than that of the\(O - F\) bond in \(F _2 O _2\)Choose the correct option for \(\underline{X} and \underline{Y}\) from those given below :
\(O - O\) bond length in \(H _2 O _2\) is X than the \(O - O\) bond length in \(F _2 O _2\)The \(O - H\) bond length in \(H _2 O _2\)is Y than that of the\(O - F\) bond in \(F _2 O _2\)Choose the correct option for \(\underline{X} and \underline{Y}\) from those given below :
Show Hint
Electronegativity and atomic size influence bond lengths. Higher electronegativity differences lead to shorter bonds, and smaller atomic radii also contribute to shorter bond lengths.
X-shorter, Y-shorter
X - shorter, Y - longer
X - longer, Y - shorter
X-longer, Y-longer
The Correct Option is C
Solution and Explanation
Step 1: Analyze the O–O bond length
In \(\text{H}_2\text{O}_2\), the oxygen atoms are bonded to hydrogen atoms. In \(\text{F}_2\text{O}_2\), the oxygen atoms are bonded to fluorine atoms. Fluorine is more electronegative than hydrogen. The higher electronegativity of fluorine in \(\text{F}_2\text{O}_2\) leads to a greater pull of electron density towards the fluorine atoms, which weakens the O–O bond and increases its bond length. Therefore, the O–O bond length in \(\text{H}_2\text{O}_2\) is longer than in \(\text{F}_2\text{O}_2\). So, \(X\) is longer.
Step 2: Analyze the O–H and O–F bond lengths
The O–H bond is formed between oxygen and hydrogen, while the O–F bond is formed between oxygen and fluorine. Fluorine has a smaller atomic radius than hydrogen. Also, oxygen and fluorine have much closer electronegativities, leading to a shorter O–F bond compared to the O–H bond where there’s a larger electronegativity difference. Therefore, the O–H bond length in \(\text{H}_2\text{O}_2\) is shorter than the O–F bond length in \(\text{F}_2\text{O}_2\). So, \(Y\) is shorter.
Conclusion
The O–O bond length in \(\text{H}_2\text{O}_2\) is longer than in \(\text{F}_2\text{O}_2\), and the O–H bond length is shorter than the O–F bond length. This corresponds to option (4).
Top Questions on Bond Parameters
The bond angles \( b_1, b_2, b_3 \) in the above structure are respectively in \( ^\circ \):
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C. Intramolecular H bonding is present in HF.
D. The magnitude of H bonding depends on the physical state of the compound.
E. H-bonding has powerful effect on the structure and properties of compounds.
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The correct order of bond enthalpy \(\left( kJ mol ^{-1}\right)\) is :
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Questions Asked in JEE Main exam
Let $\left\lfloor t \right\rfloor$ be the greatest integer less than or equal to $t$. Then the least value of $p \in \mathbb{N}$ for which
\[ \lim_{x \to 0^+} \left( x \left\lfloor \frac{1}{x} \right\rfloor + \left\lfloor \frac{2}{x} \right\rfloor + \dots + \left\lfloor \frac{p}{x} \right\rfloor \right) - x^2 \left( \left\lfloor \frac{1}{x^2} \right\rfloor + \left\lfloor \frac{2}{x^2} \right\rfloor + \dots + \left\lfloor \frac{9^2}{x^2} \right\rfloor \right) \geq 1 \]
is equal to __________.
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Concepts Used:
Chemical Bonding and Molecular Structure
Such a group of atoms is called a molecule. Obviously, there must be some force that holds these constituent atoms together in the molecules. The attractive force which holds various constituents (atoms, ions, etc.) together in different chemical species is called a chemical bond.
Types of Chemical Bonds:
There are 4 types of chemical bonds which are formed by atoms or molecules to yield compounds.
- Ionic Bonds - Ionic bonding is a type of chemical bonding which involves a transfer of electrons from one atom or molecule to another.
- Covalent Bonds - Compounds that contain carbon commonly exhibit this type of chemical bonding.
- Hydrogen Bonds - It is a type of polar covalent bonding between oxygen and hydrogen wherein the hydrogen develops a partial positive charge
- Polar Bonds - In Polar Covalent chemical bonding, electrons are shared unequally since the more electronegative atom pulls the electron pair closer to itself and away from the less electronegative atom.
Factors Affecting Bond Enthalpy in Chemical Bonding:
- Size of the Atom
- Multiplicity of Bonds
- Number of Lone Pair of Electrons Present
- Bond Angle