The Question is from NEET guide , and it was created by the author Mr. S M HUSSAIN

Question

Which factor does NOT contribute significantly to the difference in bond lengths between single, double, and triple bonds?

Mr. S M HUSSAIN · Accepted Answer

## CORE INFORMATION
✓ **Answer**: D
## CONCEPT FRAMEWORK
	**Primary Concept**: Bond Length and Bond Order
	**Related Topics**: Covalent Bonds, Bond Strength, Atomic Radius
	**Prerequisites**: Understanding of chemical bonding, bond order, and electronegativity.
## SOLUTION PATHWAY
**Given Information**:
	The question asks about factors affecting bond length differences between single, double, and triple bonds.
**Method & Steps**:
	1.	Analyze how bond order affects bond length.
		Reasoning: Higher bond order (triple > double > single) implies more shared electrons and a stronger attraction between atoms, resulting in shorter bond lengths.
		Formula/Rule: Bond Order is inversely proportional to bond length.
	2.	Assess the impact of atomic size.
		Reasoning: Larger atoms generally have longer bond lengths due to increased atomic radii.
		Key Point: Atomic size is a significant factor in determining bond length.
	3.	Evaluate the relationship between bond strength and bond length.
		Reasoning: Stronger bonds (triple > double > single) typically have shorter bond lengths due to increased electron density between the bonded atoms.
		Result: A stronger bond usually has a shorter bond length.
	4.	Determine the influence of electronegativity differences on bond length.
		Reasoning: Electronegativity differences primarily affect bond polarity and ionic character, with a minimal direct impact on bond length between the same types of atoms, which is the situation when comparing single, double, and triple bonds.
		Key Point: Electronegativity differences affect bond polarity more than the bond length.
 ## OPTION ANALYSIS
[A] :x: Bond order directly influences bond length; higher bond order results in shorter bond lengths. This is a major factor.
[B] :x: Atomic size plays a role; larger atoms form longer bonds. This is also a key factor in bond length.
[C] :x: Bond strength correlates with bond length; stronger bonds are shorter. This is a significant factor.
[D] ✓: Electronegativity differences primarily affect bond polarity, not bond length between similar atoms in single, double, or triple bonds. While electronegativity differences do play a role in bond length in ionic compounds, when we're comparing the same atoms bonded with different orders, it is not a significant factor.
 ## LEARNING AIDS
	**Common Mistakes**:
		1.[Error 1]: Confusing bond polarity with bond length. Polarity is related to electronegativity differences, whereas bond length is more directly tied to bond order and atomic size.
		2.[Error 2]: Assuming that any property that affects bonding will automatically affect bond length. Electronegativity differences affect bond polarity significantly, but not bond length in the case of comparing single, double, and triple bonds.
	**Quick Tips**:
		1.[Helpful shortcut]: Remember the acronym 'BAS' - Bond Order, Atomic Size, and Strength are major factors for bond length, with electronegativity differences being a minor factor when comparing single, double, and triple bonds.
		2.[Memory aid]: Visualize the bonds: more electron density (triple bond) pulls the atoms closer, leading to shorter bonds.

Mr. S M HUSSAIN · Answer

Bond Order

Mr. S M HUSSAIN · Answer

Atomic Size

Mr. S M HUSSAIN · Answer

Bond Strength

Mr. S M HUSSAIN · Answer

The correct Option is "Electronegativity differences"

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