Question

Consider the \(\mathrm{A}_{2} \mathrm{X}_{4}\) molecule depicted here, where \(\mathrm{A}\) and \(\mathrm{X}\) are elements. The A-A bond length in this molecule is \(d_{1}\), and the four \(\mathrm{A}-\mathrm{X}\) bond lengths are each \(d_{2}\). (a) In terms of \(d_{1}\) and \(d_{2}\), how could you define the bonding atomic radii of atoms \(\mathrm{A}\) and \(\mathrm{X}\) ? (b) In terms of \(d_{1}\) and \(d_{2}\), what would you predict for the \(\mathrm{X}-\mathrm{X}\) bond length of an \(\mathrm{X}_{2}\) molecule? [Section 7.3]

Short answer

The bonding atomic radii for atoms A and X can be defined as \(r(A) = \frac{d_{1}}{2}\) and \(r(X) = d_{2} - \frac{d_{1}}{2}\), respectively. In terms of d1 and d2, the X-X bond length of an X2 molecule would be \(d_{X-X} = 2d_{2} - d_{1}\).

Step-by-step solution

It is given that the molecule is AX4, where A and X are elements. AX4 denotes that there is one A atom, surrounded by four X atoms. A-A bond length is d1, and each A-X bond length is d2. 2. Define atomic radii for Atoms A and X.

It is important to remember that the bond length is a measure of the distance between two atomic nuclei. If we denote the radius of atom A as r(A) and the radius of atom X as r(X), then the sum of the atomic radii of two interacting atoms would be equal to their bond length. We can represent this in two equations: Separation between A atoms in a molecule (d1): \( d_{1} = r(A) + r(A) \) Separation between A and X atoms in a molecule (d2): \( d_{2} = r(A) + r(X) \) 3. Solve for atomic radii r(A) and r(X) in terms of bond lengths d1 and d2.

From the above equations, we can write each atomic radii in terms of d1 and d2. For r(A): \( r(A) = \frac{d_{1}}{2} \) For r(X): \( r(X) = d_{2} - \frac{d_{1}}{2} \) 4. Predict the X-X bond length of an X2 molecule.

We can use the relationship between atomic radii and bond length to predict the X-X bond length in an X2 molecule. Since the X2 molecule has two X atoms, we would have a bond length of: \( d_{X-X} = r(X) + r(X) \) 5. Substitute r(X) in terms of d1 and d2 into the equation for d(X-X).

Using the expression for r(X) from step 3, substitute it into the equation for d(X-X) from step 4. \( d_{X-X} = [d_{2} - \frac{d_{1}}{2}] + [d_{2} - \frac{d_{1}}{2}] \) 6. Simplify the expression for the X-X bond length.

Combine the terms to find the simplified expression for the X-X bond length. \( d_{X-X} = 2d_{2} - d_{1} \) The bond length of an X2 molecule, in terms of d1 and d2, would be \( 2d_{2} - d_{1} \).

Key concepts

Understanding Atomic Radii

The concept of atomic radii is central to understanding molecular structures. It refers to the size of an atom, essentially the distance from the nucleus to the outer boundary of the electron cloud. As atoms bond together to form molecules, their atomic radii have a direct impact on the bond lengths we observe.

When two atoms combine to form a bond, the distance between their nuclei is essentially the bond length. Atomic radii can be measured in a bonded state, where each atom's radius contributes to the overall bond length. For instance, if we denote the atomic radius of atom A as r(A) and atom X as r(X), then the bond length between them, which is the sum of their radii, is critical for molecular modeling.

To deduce atomic radii from bond lengths, we can use simple algebraic manipulation. Given the bond length between identical atoms A (d1), we infer r(A) to be half of d1. Similarly, for dissimilar atoms A and X with a bond length of d2, subtracting r(A) from d2 gives us r(X). These insights are not only fundamental in predicting molecular structures, but they also enable chemists to understand interactions within a molecule at a granular level.

Molecular Geometry's Influence on Bond Lengths

Molecular geometry describes the three-dimensional arrangement of atoms within a molecule. It is a crucial factor influencing bond lengths. Atoms are not static; they inhabit specific orientations that minimize electron repulsion and maximize bond formation, described by VSEPR (Valence Shell Electron Pair Repulsion) theory.

Different molecular shapes come from various bonding and non-bonding electron pair interactions. Take a tetrahedral geometry, such as in an AX4 molecule, where one atom A is at the center, and four atoms X are positioned at the corners of a tetrahedron. In this shape, the bond lengths can be uniform if all the surrounding atoms are the same, or vary if there are different atoms bonded to the central atom.

As part of molecular geometry, bond angles also contribute to bond lengths. In a tetrahedral molecule, the bond angles are approximately 109.5 degrees, providing a spherical shape that often leads to equivalent bond lengths. In different geometries, like linear or trigonal planar, bond lengths can differ due to the varied spatial arrangements and bond angles involved. Understanding molecular geometry is, therefore, essential for accurate bond length prediction.

Predicting Bond Lengths

Predicting bond lengths is a complex but essential skill in chemistry. Knowing the atomic radii and molecular geometry, we can make educated guesses about the distances between bonded atoms. The bond length is influenced by the types of atoms bonded together, their sizes, and the number of shared electrons that constitute the bond.

For instance, in a diatomic X2 molecule, the bond length can be estimated by doubling the atomic radius of X, derived from another molecule containing X. The method used in our exercise involves parsing out atomic radii from known bond lengths in a compound molecule, then applying them to predict bond lengths in a simpler molecule.

It's important to remember that multiple bonds (double or triple bonds) will be shorter than single bonds due to the increased attraction between the bonded atoms. Moreover, the more electronegative an atom, the more it will pull shared bonding electrons towards itself, often resulting in a shorter bond length. Predictions can be refined by considering these additional factors, which enhance the accuracy of our molecular models.