Problem 22 - A Complete Resource Book in Chemistry for JEE Main

Question

How many electrons can be accommodated in a p-orbital? (a) 6 electrons (b) 2 electrons (c) 4 electrons (d) none of these

Step-by-Step Solution

Answer

A p-orbital subshell can hold 6 electrons, thus option (a) is correct.

Step 1: Understanding the Problem

We need to determine how many electrons a p-orbital can accommodate. We will review the principles of electron configuration related to p-orbitals.

Step 2: Introduction to p-Orbital

A p-orbital is one of the three types of atomic orbitals in an atom's electron configuration. P-orbitals can hold electrons at higher energy levels starting from the second energy level (shell).

Step 3: Electron Capacity of p-Orbital

Each p-orbital can hold a maximum of two electrons, but there are three p-orbitals (px, py, pz) in a given energy level, which can collectively accommodate more electrons.

Step 4: Total Electrons in p-Subshell

The three p-orbitals together form a p-subshell. Each orbital can hold 2 electrons, so the total electron capacity is calculated as follows: \[3 ext{ orbitals} imes 2 ext{ electrons per orbital} = 6 ext{ electrons} \]

Step 5: Selection of the Correct Answer

Given the options, the correct answer is (a) 6 electrons, because a p-subshell (consisting of 3 p-orbitals) can hold a total of 6 electrons.

Key Concepts

Understanding the p-Orbital

When exploring electron configurations, the p-orbital is an essential topic. P-orbitals are part of an atom's electron cloud where the probability of finding an electron is high. These orbitals emerge from the second energy level onward and play a crucial role in the chemistry of elements.
Each p-orbital has a dumbbell shape and is oriented along one of the three axes in space: x, y, and z. These are known as the px, py, and pz orbitals. Together, they form a collection of three distinct p-orbitals in each energy level starting from the second one. The spatial orientation of p-orbitals is integral to how atoms bond with each other, influencing the geometry of molecules.

Exploring Atomic Orbitals

Atomic orbitals are regions in an atom where electrons are likely to be found. They are a fundamental concept in quantum chemistry and help explain the arrangement of electrons in an atom.
Each orbital corresponds to a specific energy state of electrons. The main types of orbitals are s, p, d, and f, each with a unique shape and capacity for electrons. The s-orbital is spherical, while the p-orbitals have a dumbbell-like shape. D and f orbitals have more complex shapes. Each type of orbital can hold a maximum number of electrons: s can hold 2, p can hold 6, d can accommodate 10, and f can hold 14 electrons.
These orbitals are arranged in increasing energy levels, and as electrons fill these orbitals, they dictate the chemical properties of an element.

The Role of the p-Subshell

Within the realm of atomic orbitals, the p-subshell is a significant component. Composed of three p-orbitals (px, py, pz), each p-subshell can hold up to 6 electrons in total.
Here's a quick breakdown:

• Each individual p-orbital can accommodate 2 electrons.
• The p-subshell, with its three orbitals, can hold 3 times the capacity of one orbital, equating to a total of 6 electrons.

This arrangement is key in electron configuration and pertains to how elements react chemically. For example, elements on the right side of the periodic table tend to fill their p-subshells, which influences their tendency to acquire additional electrons.
Understanding the p-subshell helps in comprehending various chemical reactions and bonding patterns observed in many compounds.