sigma bonds are stronger than pi bonds

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The question presents a simple true/false statement about bond types. 
Option 1: True. In general chemistry, sigma bonds arise from end-to-end (head-on) overlap between orbitals, which leads to a strong, cylindrically symmetric bond that is typically higher in bond dissociation energy. This stronger overlap also accounts for the fact that sigma bonds can rotate around the bond axis (free rotation) without breaking the bond, whereas pi bonds result from side-to-side overlap of p orbitals and are weaker because this overlap is less effective and more angularly delicate. Consequently, when a single bond is formed, it is a sigma bond and tends to be stronger than a pi bond; in multiple bonds, the additional pi bond is weaker than the sigma component and is more reactive and easier to break. 
Option 2: False. One might encounter counterpoints in specific, unusual cases or interpret “stronger” in a context that isn’t about bond strength (for example, saying certain pi interactions can be unusually strong in conjugated systems or during resonance stabilization). However, the standard teaching is that sigma bonds are stronger than pi bonds due to greater orbital overlap and bond energy considerations. It is also important to recall that in a double bond, the sigma component is typically the stronger of the two bonds, while the pi component is comparatively weaker and more reactive. 
In summary, the conventional view attributes greater intrinsic strength to sigma bonds compared to pi bonds, with the caveat that chemical context and bond type (single vs. multiple) can influence how we describe stability, reactivity, or overall bond energy in nuanced ways.

sigma bonds are stronger than pi bonds

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sigma bonds are stronger than pi bonds

View Explanation

Log in for full answers

Similar Questions

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