Question

One of the following ions has a trigonal-planar shape: \(\mathrm{SO}_{3}^{2-} ; \mathrm{PO}_{4}^{3-} ; \mathrm{PF}_{6}^{-} ; \mathrm{CO}_{3}^{2-} .\) Which ion is it? Explain.

Short answer

The ion that has a trigonal planar shape is \(CO_{3}^{2-}\).

Step-by-step solution

Drawing Lewis Structure 1

Draw the Lewis structure of \(SO_{3}^{2-}\). It can be observed that sulphur (S) is the central atom bonded to three oxygen atoms and also carries a lone pair of electrons. This gives it a tetrahedral electronic geometry.

Drawing Lewis Structure 2

Next, draw the Lewis structure of \(PO_{4}^{3-}\). With phosphorus (P) as the central atom, it is bonded to four oxygen atoms, giving it a tetrahedral electronic geometry as well.

Drawing Lewis Structure 3

After that, draw the Lewis structure of \(PF_{6}^{-}\). Here, phosphorus (P) is the central atom and it is bonded to six fluorine atoms, resulting in an octahedral electronic geometry.

Drawing Lewis Structure 4

Finally, draw the Lewis structure of \(CO_{3}^{2-}\). In this case, carbon (C) is the central atom and is bonded to three oxygen atoms. This gives it three electron domains, meaning it has a trigonal planar electronic geometry.

Key concepts

Lewis Structure

To understand molecular geometry and determine the shape of a molecule, drawing the Lewis structure is an essential first step. It provides a visual representation of the atoms in a molecule and their bonding.

Think of Lewis structures as blueprints for molecules. Here's how they work:

• Identify the total number of valence electrons in the molecule or ion.
• Sketch the arrangement of atoms, starting by placing the least electronegative atom at the center (except for hydrogen).
• Connect the atoms with single bonds and distribute remaining electrons to satisfy the octet rule, or duet for hydrogen.
• Adjust electron pairs to manage formal charges and double check octet completion.

Lewis structures help identify areas of electron density that play a crucial role in determining the molecule's geometry.

Trigonal Planar

Trigonal planar geometry is characteristic of molecules or ions with three electron domains around the central atom, all consisting of bonding pairs. This arrangement ensures the regions of electron density are spread as far apart as possible, minimizing repulsion among them.

In a trigonal planar shape, all atoms lie in a single plane:

• The central atom forms 120° bond angles with the surrounding atoms.
• Molecules like carbonate ion \((CO_{3}^{2-})\) commonly exhibit this geometry.

This shape arises in contexts where there are no lone pairs affecting the spatial arrangement of the bonding electrons, providing the planar form.

Electron Domains

An electron domain refers to a region around a central atom where electrons are likely to be found. This includes both bonding and non-bonding (lone) pairs.

Here's how to count electron domains:

• Each bond to an atom represents one domain, regardless of whether it's a single, double, or triple bond.
• Lone pairs are also considered as one domain each.

The number and arrangement of electron domains determine the overall geometry of the molecule, as electron-pair repulsion guides them to positions of minimal interaction.

Tetrahedral Geometry

Tetrahedral geometry arises in molecules where the central atom is surrounded by four electron domains, typically all bonding pairs, arranged symmetrically around it.

Key characteristics of tetrahedral shapes:

• Identifiable by bond angles of about 109.5° between any two bonds.
• Common in molecules like methane (\(CH_4\)), where the central atom is spanned symmetrically by bonded atoms.

This geometry efficiently distributes electron domains, minimizing repulsions according to VSEPR (Valence Shell Electron Pair Repulsion) theory, providing a 3D shape that maximizes separation.