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From my understanding, the difference between tetrahedral and square planar is related to their hybridization configurations. Additionally, I think that a square planar configuration is in one plane whereas tetrahedral is in multiple planes.
From my understanding, it is considered a tetrahedral when a molecule, e.g CH4, has 4 bonds but 0 lone pairs. A square planar, XeF4, has 4 bonds and 2 lone pairs. There is a difference in the amount of lone pairs reuslting in a difference in a bond angles.
Square planar and tetrahedral are both molecular geometries that are observed within the tetrahedral electron configuration subdivision. It is tetrahedral that has 109.5 degree bond angles and a molecular shape that is composed of multiple planes as well as hybridization of sp^3 while square planar has bond angles of 90 and 180 degrees and is composed of a single plane as well as a hybridization of dsp^2.
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