Question

What is the maximum number of electrons in each of the following? (a) an s sublevel (b) a \(p\) sublevel (c) a \(d\) sublevel (d) an \(f\) sublevel

Short answer

(a) 2 electrons, (b) 6 electrons, (c) 10 electrons, (d) 14 electrons.

Step-by-step solution

Understanding Orbitals and Sublevels

Electrons are arranged in orbitals within sublevels, and each orbital can hold up to 2 electrons. The types of sublevels (s, p, d, f) vary in the number of orbitals they can contain, which affects the maximum number of electrons they can hold.

Calculating Maximum Electrons in an s Sublevel

An s sublevel consists of 1 orbital. Since each orbital can hold 2 electrons, the maximum number of electrons in an s sublevel is 2.

Examining a p Sublevel

A p sublevel contains 3 orbitals. Therefore, with 2 electrons per orbital, it can hold a total of 6 electrons.

Detailing a d Sublevel

A d sublevel consists of 5 orbitals. Given that each orbital can contain 2 electrons, the maximum number of electrons a d sublevel can accommodate is 10.

Exploring an f Sublevel

An f sublevel comprises 7 orbitals. Consequently, with each orbital holding 2 electrons, it can house up to 14 electrons.

Key concepts

Atomic Orbitals

Atomic orbitals are regions around the nucleus of an atom where electrons are likely to be found. These are essentially wave functions that give the probability of finding an electron in a specific area. Understanding atomic orbitals is crucial as they form the foundation of electron configuration in atoms.

There are different shapes and sizes of atomic orbitals, which are defined by quantum numbers. The principal quantum number helps to determine the energy level, while the angular momentum quantum number defines the shape. Each type of orbital can hold a specific number of electrons, and this is what defines the sublevels of atoms which we'll explore next.

s Sublevel

The s sublevel is the simplest type of sublevel and consists of only one orbital. This single orbital has a spherical shape, symmetrically surrounding the nucleus.

Since each orbital can contain up to 2 electrons due to Pauli's Exclusion Principle, the maximum number of electrons that can occupy an s sublevel is 2. Every principal energy level begins with an s sublevel, making it the building block of more complex electron configurations.

p Sublevel

In contrast to the spherical s sublevel, the p sublevel contains three orbitals that have a dumbbell shape. These orbitals are oriented differently in space, typically along the x, y, and z axes, which gives them the ability to accommodate more electrons than an s sublevel.

Each of the three orbitals in a p sublevel can hold 2 electrons, making the p sublevel able to host a maximum of 6 electrons in total. The increase in the number of orbitals allows the p sublevel to play a significant role in the electron distribution for elements starting from the second period of the periodic table.

d Sublevel

The d sublevel is more complex and consists of five orbitals. These orbitals have more intricate shapes than the s and p sublevels, often described as cloverleaf patterns and other more elaborate configurations.

Because each orbital can hold 2 electrons, the d sublevel can contain a maximum of 10 electrons. The d orbitals begin filling at the fourth principal energy level, and they play a critical role in the chemistry of transition metals.

f Sublevel

The f sublevel is the most complex of the sublevels considered here, encompassing seven distinct orbitals. Each of these orbitals can also hold 2 electrons, allowing the f sublevel to hold a maximum of 14 electrons.

This sublevel becomes prominent in the elements referred to as lanthanides and actinides. The diverse shapes and orientations of the f orbitals are responsible for the unique properties of these elements, especially in the realm of magnetics and optics.

Maximum Electrons

Understanding the concept of maximum electrons that can be held in various sublevels is central to mastering electron configurations. Each sublevel's capacity to hold electrons is determined by the number of orbitals it houses and the fact that each orbital can accommodate up to 2 electrons.

This brings us to:

• s sublevel: 2 electrons (1 orbital x 2 electrons)
• p sublevel: 6 electrons (3 orbitals x 2 electrons)
• d sublevel: 10 electrons (5 orbitals x 2 electrons)
• f sublevel: 14 electrons (7 orbitals x 2 electrons)

These maximum capacities determine how elements are arranged in the periodic table and how they bond with others, shaping the chemical landscape of the universe.