Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 7: Problem 53

Give the values of the quantum numbers associated with the following orbitals: (a) \(2 p,\) (b) \(3 s,\) (c) \(5 d\).

Short Answer

Expert verified
The quantum numbers for the orbitals are: (a) 2p: [n=2, l=1, m=-1, 0, 1], (b) 3s: [n=3, l=0, m=0], (c) 5d: [n=5, l=2, m=-2, -1, 0, 1, 2]

Step by step solution

01

Orbital 2p

Identify the quantum numbers from the orbital \(2 p\). Here, 2 is the principal quantum number \(n=2\) and p corresponds to the angular momentum quantum number \(l=1\). Since p orbital can have -1, 0, 1 as the magnetic quantum number (m), the quantum numbers for 2p are [n=2, l=1, m=-1, 0, 1]
02

Orbital 3s

Identify the quantum numbers from the orbital \(3 s\). Here, 3 is the principal quantum number \(n=3\) and s corresponds to the angular momentum quantum number \(l=0\). Since s orbital can have 0 as the magnetic quantum number (m), the quantum numbers for 3s are [n=3, l=0, m=0]
03

Orbital 5d

Identify the quantum numbers from the orbital \(5 d\). Here, 5 is the principal quantum number \(n=5\) and d corresponds to the angular momentum quantum number \(l=2\). Since d orbital can have -2, -1, 0, 1, 2 as the magnetic quantum number (m), the quantum numbers for 5d are [n=5, l=2, m=-2, -1, 0, 1, 2]

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Discuss the similarities and differences between a \(1 s\) and a \(2 s\) orbital.

Give the values of the four quantum numbers of an electron in the following orbitals: (a) \(3 s,\) (b) \(4 p\), (c) \(3 d\).

In an electron microscope, electrons are accelerated by passing them through a voltage difference. The kinetic energy thus acquired by the electrons is equal to the voltage times the charge on the electron. Thus, a voltage difference of \(1 \mathrm{~V}\) imparts a kinetic energy of \(1.602 \times 10^{-19} \mathrm{C} \times \mathrm{V}\) or \(1.602 \times\) \(10^{-19} \mathrm{~J}\). Calculate the wavelength associated with electrons accelerated by \(5.00 \times 10^{3} \mathrm{~V}\).

Owls have good night vision because their eyes can detect a light intensity as low as \(5.0 \times 10^{-13} \mathrm{~W} / \mathrm{m}^{2}\). Calculate the number of photons per second that an owl's eye can detect if its pupil has a diameter of \(9.0 \mathrm{~mm}\) and the light has a wavelength of \(500 \mathrm{nm}\) \((1 \mathrm{~W}=1 \mathrm{~J} / \mathrm{s})\)

What is the de Broglie wavelength (in \(\mathrm{nm}\) ) associated with a 2.5 -g Ping-Pong ball traveling 35 mph?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Chemical Analysis

Read Explanation

Inorganic Chemistry

Read Explanation

Organic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Ionic and Molecular Compounds

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free