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Why molecules of the type AX4 take a tetrahedral form often than the square planar form?
Wiki User
∙ 12y ago
I guess I would first make 2 types of clarifications for this questions.
First- We have to make the distinction between molecule geometry which is usually sort of what you see in a Lewis dot structure (2D), to molecule shape which is where VSEPR comes in (3D)
Second- AX?, AX-(what), AX3, AX5, AX4...
Either way usually in VSEPR, each X is trying to get as much space as possible in a 3D form, thus a tetrahedral form will be preferred over a square planar. Each X will be approximately 109.5 degrees apart from each other, instead of 90 degrees.
Wiki User
∙ 11y ago
Molecules of type AX4 often take a tetrahedral form due to the presence of four electron pairs around the central atom, leading to a geometry with minimal repulsion between the electron pairs. In a tetrahedral arrangement, the bond angles are around 109.5 degrees, which allows for maximum separation between the bonding pairs.
Wiki User
∙ 12y agothe only repulsion happening is between the substituents,
so it is in its optimal (lowest) energy state as the tetrahedral form.
Square planar molecules (like AX4E2) contain 2 lone pairs that produce electron to bond repulsion that result in the lowest energy form to be square planar.
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A tetrahedral shape is defined by having four equally spaced vertices connected by edges that form four triangular faces. This shape is characterized by having bond angles of approximately 109.5 degrees between adjacent bonds. In chemistry, molecules with a tetrahedral geometry often have four electron pairs around a central atom, resulting in a symmetrical and three-dimensional structure.
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