Problem 69 - Chemistry Matter and Change

Question

How are the five orbitals related to an atom's d sublevel designated?

Step-by-Step Solution

Answer

The five d orbitals are designated as \(d_{xy}\), \(d_{yz}\), \(d_{zx}\), \(d_{x^2-y^2}\), and \(d_{z^2}\).

Step 1: Understand the d Sublevel

The d sublevel is a set of orbitals in an atom, specifically for energy levels where the principal quantum number is 3 or higher. Each d sublevel contains five orbitals.

Step 2: Identify Orbital Designations

The five orbitals in the d sublevel are designated based on their specific orientations in three-dimensional space. These orbitals are labeled as: \(d_{xy}\), \(d_{yz}\), \(d_{zx}\), \(d_{x^2-y^2}\), and \(d_{z^2}\).

Step 3: Relate Each Orbital Name to Orientation

Each of the d orbitals has a distinct shape and orientation: \(d_{xy}\), \(d_{yz}\), and \(d_{zx}\) orbitals are oriented between the respective axes in a coordinate system; \(d_{x^2-y^2}\) lies along the x and y axes; and \(d_{z^2}\) looks like a doughnut with a polar lobe, aligned along the z-axis.

Key Concepts

Orbitals

In atomic physics, orbitals represent regions around an atomic nucleus where electrons have a high likelihood of being located. These orbitals have unique shapes and energies that determine how they influence chemical bonding and physical properties of substances. Each orbital is characterized by a set of quantum numbers, which aid in identifying its properties and position within an atom.
For instance, orbitals come in various types such as s, p, d, and f, each with a distinct shape and capacity to hold a certain number of electrons. While s orbitals are spherical and hold up to two electrons, d orbitals have more complex shapes and can accommodate up to ten electrons, split among five unique orbitals.
Understanding orbitals is essential because they form the basis for predicting how atoms connect to form molecules. This predictive ability is a fundamental part of chemistry, providing insights into the physical and chemical behavior of elements.

Principal Quantum Number

The principal quantum number is a fundamental concept in quantum mechanics that describes the size and energy level of an electron shell within an atom. It is denoted by the letter \(n\) and takes integer values such as 1, 2, 3, and so on, correlating with the relative distance of the shell from the nucleus.

• Higher principal quantum numbers indicate shells that are further from the nucleus.
• As \(n\) increases, the energy level of the shell increases, meaning electrons in these shells require more energy to remain bound to the nucleus.
• For any atom, the number of different sublevels within a principal energy level equals \(n\). For instance, when \(n = 3\), the sublevels include s, p, and d.

The principal quantum number plays a crucial role in determining an atom's electron configuration, which in turn influences the chemical and physical properties of elements.

Orbital Orientations

Orbital orientations refer to the specific directional arrangements of d orbitals within an atom's electron cloud. The d sublevel, which consists of five orbitals, is particularly interesting because of its varied orientations in three-dimensional space:

• The orbitals \(d_{xy}\), \(d_{yz}\), and \(d_{zx}\) are oriented between two axes in a 3D coordinate system.
• The \(d_{x^2-y^2}\) orbital is oriented along the x and y axes.
• Lastly, the \(d_{z^2}\) orbital is unique, with a doughnut-shaped lobe positioned along the z-axis.

These orientations are essential for specifying how electrons reside in the d orbitals, affecting the bond angles and geometry of the molecules. The distinct spatial arrangement also influences the chemical reactivity and magnetic properties of elements, thereby playing a vital role in the material's behavior during chemical reactions and physical interactions.