Why The Bond Angle Of Methane Is 109 Instead Of 90?

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Why the bond angle of methane is 109 instead of 90?

• Thread starter Thread starter scientist91
• Start date Start date Apr 30, 2007
• Tags Tags Angle Bond Methane

Click For Summary The discussion centers on the geometry of sp3 hybrid orbitals, specifically addressing why the bond angle is approximately 109.5 degrees instead of 90 degrees. It highlights that in three-dimensional space, four points arranged around a central atom form a tetrahedron, which minimizes electron pair repulsion. This tetrahedral arrangement is crucial for the stability of molecules like methane, which has four C-H bonds. A bond angle of 90 degrees would lead to increased repulsion and instability, making the tetrahedral shape and corresponding bond angle of 109.5 degrees essential for molecular stability. The conversation also critiques the limitations of valence shell theory in explaining these concepts effectively. scientist91 Messages 133 Reaction score 0 I know that the sp3 hybrid orbitals form 109 angle, but why the angle is not 90. If the angle is 109 the repulsion is minimized or what? Show some comparations. Thank u. Chemistry news on Phys.org

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sicjeff Messages 46 Reaction score 0 I believe your problem lies in the fact that you are only looking in two dimensions. What orbital theory are you using? Valence shell theory is useless for all practical applications anyway. Andronicus1717 Messages 32 Reaction score 1 3 Dimensions Indeed, in 3d space four points equally spaced around a center point form a tetrahedron, not a square, hence your bond angle of 109.5 degrees. Kushal Messages 438 Reaction score 1 methane consists of four bonded pairs, i.e 4 C-H bonds. So as to minimize repulsion, the molecule adopts a tetrahedral shape, hence bond angle becomes 109.5. with bond angle of 90, the molecule would not be very stable.

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