Question

Draw a filling diagram and predict the sublevel that follows \(5 s\).

Short answer

The sublevel that follows 5s is 4d.

Step-by-step solution

Understanding Electron Configuration

Electron configurations describe the distribution of electrons among the orbitals of an atom. Electrons fill these orbitals in a specific sequence known as the Aufbau principle.

Understanding the Aufbau Principle

The Aufbau principle indicates that electrons occupy the lowest energy orbitals first. The sequence of filling usually follows the order: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, and so forth.

Locating 5s in the Sequence

In the electron configuration sequence, the 5s sublevel follows the sequence: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s. We need to find the next sublevel that comes after 5s.

Identifying the Sublevel that Follows 5s

After the 5s sublevel, according to the Aufbau principle, the next sublevel to be filled is 4d. So, the sublevel that follows 5s is 4d.

Key concepts

Aufbau Principle

The Aufbau Principle is a fundamental concept in chemistry that helps explain how electrons fill the orbitals of an atom. It states that electrons will fill lower energy orbitals before they move to higher energy levels. This is because electrons naturally seek the most stable, low-energy state possible.

The word "Aufbau" comes from German, meaning "building-up," which perfectly describes how electrons build up around the nucleus, layer by layer. This principle guides us in determining the electron configurations of elements, which essentially is the arrangement of electrons in an atom's orbitals.

Understanding the Aufbau Principle is crucial because it allows scientists to predict chemical properties and behaviors of elements based on their electron arrangement. The principle also helps in visualizing how elements interact, form bonds, and create compounds.

Orbital Filling Sequence

The orbital filling sequence is the order in which electrons populate the orbitals of an atom according to their energy levels. Understanding this sequence is essential to grasp how elements and their compounds behave.

According to the Aufbau Principle, electrons follow a specific sequence, which is not strictly integer-based due to the overlap in energy levels among different shell types. The typical order starts with the low-energy filled orbitals and moves to the higher ones:

• 1s
• 2s, 2p
• 3s, 3p, 4s
• 3d, 4p, 5s
• 4d, 5p, 6s
• 4f, 5d, 6p, 7s

Understanding which orbitals fill first is crucial for chemists when predicting the behavior of atoms, particularly when determining chemical reactivity and bonding characteristics.

After 5s, for example, we move to the 4d sublevel, highlighting how the sequence does not always simply "count upwards" but depends on relative energy levels.

Sublevels in Chemistry

Sublevels in chemistry are subdivisions within electron shells of an atom, known as principal energy levels. Each shell can contain one or more sublevels, which are defined by the type of orbitals present: s, p, d, and f.

Each type of sublevel corresponds to a different shape of the region where electrons can be found. The "s" sublevel is spherical, the "p" sublevel is dumbbell-shaped, the "d" sublevel has more complex shapes, and the "f" sublevel features even more intricate geometries.

Sublevels are important because they help explain an atom's electronic configuration and chemical properties. For example, elements with a filled "s" or "p" sublevel are generally more stable and less reactive.

• The s sublevel holds a maximum of 2 electrons.
• The p sublevel can hold up to 6 electrons.
• The d sublevel accommodates up to 10 electrons.
• The f sublevel can hold up to 14 electrons.

These capacities show why understanding sublevels is vital for predicting electron configurations and chemical behaviors of elements.