Question

State the maximum number of electrons that can occupy each of the following sublevels: (a) \(1 s\) (b) \(2 p\) (c) \(3 d\) (d) \(4 f\)

Short answer

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

Step-by-step solution

Understanding Electron Capacity

Each sublevel (s, p, d, f) can hold a specific number of electrons. Electrons are filled according to the order of increasing energy levels, and each sublevel can hold a different maximum number of electrons.

Determine Electron Capacity for s Sublevel

The s sublevel consists of 1 orbital, and each orbital can hold up to 2 electrons. Therefore, the s sublevel can hold a maximum of 2 electrons.

Determine Electron Capacity for p Sublevel

The p sublevel consists of 3 orbitals, and each orbital can hold up to 2 electrons. Thus, the p sublevel can hold a maximum of \(3 \times 2 = 6\) electrons.

Determine Electron Capacity for d Sublevel

The d sublevel consists of 5 orbitals, with each orbital able to hold 2 electrons. Therefore, the d sublevel can hold up to \(5 \times 2 = 10\) electrons.

Determine Electron Capacity for f Sublevel

The f sublevel consists of 7 orbitals, and each orbital can hold 2 electrons. Therefore, the f sublevel can hold up to \(7 \times 2 = 14\) electrons.

Key concepts

Sublevel Capacity

Understanding the capacity of different sublevels is essential in mastering electron configuration. Each type of sublevel - s, p, d, and f - can hold a unique maximum number of electrons. This is due to the number of atomic orbitals each sublevel contains.

• The s sublevel, with just one orbital, can hold 2 electrons.
• The p sublevel consists of three orbitals, thus can accommodate up to 6 electrons.
• The d sublevel, with five orbitals, can house a total of 10 electrons.
• Lastly, the f sublevel, which contains seven orbitals, can contain 14 electrons.

Each of these sublevels stacks in a particular order as per the rules governing energy levels. This stacking order is critical. By knowing the electron capacity of each sublevel, students can predict how electrons fill these sublevels following the increasing order of energy.

Atomic Orbitals

Atomic orbitals are the regions within an atom where there is a high probability of finding electrons. Each orbital can hold a maximum of two electrons due to the principle of electron pairing with opposite spins. There are different types of atomic orbitals associated with each sublevel:

• The s orbitals are spherical and have only one orientation, leading to the s sublevel having a single orbital.
• The p orbitals are dumbbell-shaped and oriented in three directions, corresponding to the three orbitals in the p sublevel.
• The d orbitals are more complex with five distinct orientations, accounting for the five orbitals in the d sublevel.
• The f orbitals are even more intricate with seven distinct orientations, thus having seven orbitals in the f sublevel.

These orbitals provide the framework for understanding how electrons fill an atom and bring clarity to the organization of electron arrangements.

Energy Levels

Atoms have multiple energy layers or shells, and each shell consists of one or more sublevels. The position of sublevels across energy levels dictates the order in which electrons populate them. This order follows a specific sequence often described by the Aufbau principle. Here’s how this works: - First, electrons fill the 1s sublevel, having the lowest energy. - Next, they proceed to fill the 2s, followed by the 2p sublevels. - They continue to higher levels such as 3s, 3p, and then 3d, in accordance with increasing energy. Understanding these energy levels is crucial because the lower the energy, the more stable the atom is. Electrons will always fill the lowest available energy state as they build up within the atom, maintaining its balance and stability. This systematic filling results in the unique configuration of electrons for every element, which in turn defines the chemical behavior of that element.