The molecular shape of BF3 is planar (see Table 10.1 ). If a fluoride ion is attached to the B a

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The molecular shape of BF3 is planar (see Table 10.1 ). If a...

The molecular shape of $\mathrm{BF}_{3}$ is planar (see Table 10.1 ). If a fluoride ion is attached to the $B$ atom of $B F_{3}$ through a coordinate covalent bond, the ion $\mathrm{BF}_{4}^{-}$ results. What is the shape of this ion?

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Key Concepts

VSEPR Theory

The Valence Shell Electron Pair Repulsion (VSEPR) theory is a fundamental concept in chemistry used to predict the geometry of molecules and ions. It states that electron pairs around a central atom will arrange themselves as far apart as possible in order to minimize repulsion. This theory is essential in determining that a molecule or ion with four regions of electron density, such as BF4–, adopts a tetrahedral geometry.

Tetrahedral Geometry

Tetrahedral geometry is a molecular shape where a central atom is surrounded symmetrically by four atoms, with bond angles of roughly 109.5°. This arrangement minimizes electron-pair repulsions and is commonly observed in molecules or ions with four bonding pairs and no lone pairs on the central atom.

Coordinate Covalent Bonding

Coordinate covalent bonding involves the sharing of an electron pair where both electrons come from the same atom. This type of bond is significant in cases such as the formation of BF4–, where a fluoride ion donates an electron pair to the boron atom in BF3, resulting in a stable tetrahedral ion.

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