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Chapter 7: Problem 58

What is the difference between a \(2 p_{x}\) and a \(2 p_{y}\) orbital?

Short Answer

Expert verified
The difference between a \(2 p_{x}\) and a \(2 p_{y}\) orbital lies in their orientation in space. The \(2 p_{x}\) orbital is aligned along the x-axis while the \(2 p_{y}\) orbital is aligned along the y-axis. Except for orientation, they are equivalent in energy, size, and shape.

Step by step solution

01

Understand the quantum mechanical model

As per the quantum mechanical model of an atom, it's known that electrons reside in areas called orbitals. Orbitals are categorized into s, p, d, f based on their shape. An energy level may contain one or more types of orbitals - each energy level has one s, three p, five d, and seven f orbitals. These orbitals in any energy level are of the same size and shape but differ in their spatial orientation.
02

Comprehend the 2p energy level and its orbitals

When it comes to the 2p energy level, it contains three orbitals that are each orientated along one of the three cartesian axes - x, y, and z. Each of these is denoted as \(2 p_{x}\), \(2 p_{y}\), and \(2 p_{z}\). The number 2 signifies the second energy level or shell (principal quantum number n = 2), 'p' refers to the type of orbital, and 'x', 'y', 'z' denote the orientation. These three orbitals are equivalent in energy, size, and shape.
03

Identify the difference between \(2 p_{x}\) and \(2 p_{y}\) orbitals

The only difference between \(2 p_{x}\) and \(2 p_{y}\) orbitals is their orientation in space. The \(2 p_{x}\) orbital is aligned along the x-axis, while the \(2 p_{y}\) orbital is aligned along the y-axis. So, they differ in terms of the direction in which they are oriented.

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Most popular questions from this chapter

The \(\mathrm{He}^{+}\) ion contains only one electron and is therefore a hydrogen-like ion. Calculate the wavelengths, in increasing order, of the first four transitions in the Balmer series of the \(\mathrm{He}^{+}\) ion. Compare these wavelengths with the same transitions in a \(\mathrm{H}\) atom. Comment on the differences. (The Rydberg constant for \(\mathrm{He}^{+}\) is \(\left.8.72 \times 10^{-18} \mathrm{~J} .\right)\)

Why do the \(3 s, 3 p,\) and \(3 d\) orbitals have the same energy in a hydrogen atom but different energies in a many-electron atom?

Describe the characteristics of an \(s\) orbital, a \(p\) orbital, and a \(d\) orbital. Which of the following orbitals do not exist: \(1 p, 2 s, 2 d, 3 p, 3 d, 3 f, 4 g ?\)

Explain what is meant by a noble gas core. Write the electron configuration of a xenon core.

Indicate the number of unpaired electrons present in each of the following atoms: \(\mathrm{B}, \mathrm{Ne}, \mathrm{P}, \mathrm{Sc}, \mathrm{Mn}, \mathrm{Se},\) \(\mathrm{Kr}, \mathrm{Fe}, \mathrm{Cd}, \mathrm{I}, \mathrm{Pb}\).
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