The Odd Shape of Life ( carbon)

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SUMMARY

The discussion centers on the molecular geometry of carbon (CH3) and its unique triangular planar shape, contrasting it with the trigonal pyramidal shapes of other Group 14 elements (Si, Ge, Sn, Pb). The speaker asserts that carbon's shape results from the distribution of its unpaired electron across three orbitals, forming a "Y" configuration. This phenomenon is attributed to the concept of hybridization, specifically sp2 hybridization in CH2, which leaves one electron in an unhybridized p orbital. The role of electronegativity in influencing these shapes is also suggested as a key factor.

PREREQUISITES
  • Understanding of VSEPR (Valence Shell Electron Pair Repulsion) theory
  • Knowledge of hybridization concepts, particularly sp2 hybridization
  • Familiarity with molecular geometry and orbital shapes
  • Basic principles of electronegativity and its effects on molecular structure
NEXT STEPS
  • Research VSEPR theory and its applications in predicting molecular shapes
  • Study hybridization types and their implications in molecular bonding
  • Explore the effects of electronegativity on molecular geometry
  • Examine the molecular structures of other Group 14 elements for comparative analysis
USEFUL FOR

Chemistry students, molecular geometry enthusiasts, and anyone interested in the structural properties of carbon and its group counterparts.

bjon-07
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Hi, I have a question

CH3, doublet (one unpaired electron) has a triangular planor shape.
According to vspr theory it should have a tiangular pryimidal shape. The rest of the elements in row 14 ( Si, Ge, Sn, Pb) all have a tringular pryimidal shape.

From what i understand, in carbon which is shaped like a "Y" the unpaired electron is spread out equal above and below the the 'plane' which makes up the "2D" three orbitals that take the shape of the Y.

Why don't the other elements in column 14 have this same feature. i have feeling that is has something to do with electron negativey.

thank you
 
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The CH2 CH2 has a double bond in between then which will make an sp2 hybridized bond, which leave one electron in the unhybridized P orbital, which will be perpendicular to the plane, which the carbons and hydrogens lie in.

Nautica
 

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