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Chapter 3: Problem 21

Why can a \(p\) sublevel hold six electrons while the \(s\) sublevel can hold no more than two electrons?

Short Answer

Expert verified
A \(p\) sublevel can hold six electrons because it comprises three sub-orbitals, each of which can hold up to two electrons. On the other hand, a \(s\) sublevel can only hold up to two electrons as it comprises a single sub-orbital that can hold two electrons.

Step by step solution

01

Understanding Orbitals and Electrons

Orbitals can be understood as energy levels of an atom where electrons reside. Each orbital can hold a certain number of electrons, and within each orbital, there are sub-orbitals. These sub-orbitals can hold up to two electrons each. The type of orbital (such as \(s\) or \(p\)) determines the number of these sub-orbitals.
02

The \(s\) Sublevel

The \(s\) orbital is the simplest type of orbital. It consists of one spherical sub-orbital that can hold up to two electrons. This is why an \(s\) sublevel is limited to a maximum of two electrons.
03

The \(p\) Sublevel

The \(p\) orbital is more complex. It consists of three dumbbell-shaped sub-orbitals, placed orthogonally to one another (one along the \(x\)-axis, one along the \(y\)-axis, and one along the \(z\)-axis). Each of these sub-orbitals can hold up to two electrons, which means a \(p\) sublevel can hold a maximum of six electrons (3 sub-orbitals times 2 electrons each equals 6 electrons).

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