/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 14 What is meant by an orbital?... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 7: Problem 14

What is meant by an orbital?

Short Answer

Expert verified
An orbital is a mathematical function that describes the wave-like behavior of an electron or a pair of electrons in an atom, representing the most probable regions where they can be found. Orbitals have various shapes depending on the energy level and angular momentum quantum numbers (l), such as s, p, d, and f orbitals. The energy level of an orbital is determined by the principal quantum number (n) and the angular momentum quantum number (l), with higher values indicating higher energy levels.

Step by step solution

01

Understanding the Wave-like Properties of Electrons

Electrons possess both particle-like and wave-like properties. The wave-like nature of electrons helps us understand how they behave around the nucleus of an atom. Usage of quantum mechanics allows the determination of probability distributions describing the regions where the electron is most likely to be found.
02

Orbital Shapes

Orbitals come in various shapes that reflect the probability distribution of finding an electron around the nucleus. The shape of an orbital is determined by the energy level and angular momentum quantum numbers (l). 1. s orbitals: Spherical shape and have no directional preference. They have an angular momentum quantum number, l = 0. 2. p orbitals: Dumbbell-shaped and have directional preference. They have an angular momentum quantum number, l = 1. 3. d orbitals: Have more complex shapes with four of them having a cloverleaf shape, whereas one of them is shaped like a dumbbell with a torus around it. They have an angular momentum quantum number, l = 2. 4. f orbitals: Have more complex shapes and have an angular momentum quantum number, l = 3. As we go on to higher orbitals (g, h, etc.), the shapes become more complicated, and their description becomes less intuitive.
03

Orbital Energy Levels

The energy level of an orbital is determined by two quantum numbers: the principal quantum number (n) and the angular momentum quantum number (l). The higher the value of n, the higher is the energy of the orbital; the higher the value of l, the higher is the energy within a given n. For a hydrogen atom, the relationship between the energy level and these quantum numbers is: E = -13.6 eV / n^2 Where E is the energy of the orbital, eV stands for electron volts (a unit of energy), and n is the principal quantum number (positive integer values like 1, 2, 3, etc.). In summary, an orbital is a region where an electron is most likely to be found in an atom, depending on its energy and angular momentum. The shapes of orbitals give insights into the probability distribution of the electron in an atom, which aids in understanding its behavior and chemical properties.

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.

Over 30 million students worldwide already upgrade their learning with 91影视!

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

An ion having a \(4+\) charge and a mass of \(49.9\) amu has 2 electrons with principal quantum number \(n=1,8\) electrons with \(n=2\), and 10 electrons with \(n=3 .\) Supply as many of the properties for the ion as possible from the information given. (Hint: In forming ions for this species, the \(4 s\) electrons are lost before the \(3 d\) electrons.) a. the atomic number b. total number of \(s\) electrons c. total number of \(p\) electrons d. total number of \(d\) electrons e. the number of neutrons in the nucleus f. the ground-state electron configuration of the neutral atom

In defining the sizes of orbitals, why must we use an arbitrary value, such as \(90 \%\) of the probability of finding an electron in that region?

Which of the following electron configurations correspond to an excited state? Identify the atoms and write the ground-state electron configuration where appropriate. a. \(1 s^{2} 2 s^{2} 3 p^{1}\) b. \(1 s^{2} 2 s^{2} 2 p^{6}\) c. \(1 s^{2} 2 s^{2} 2 p^{4} 3 s^{1}\) d. \([\mathrm{Ar}] 4 s^{2} 3 d^{5} 4 p^{1}\) How many unpaired electrons are present in each of these species?

For each of the following pairs of elements \((\mathrm{Mg}\) and \(\mathrm{K}) \quad(\mathrm{F}\) and \(\mathrm{Cl})\) pick the atom with a. more favorable (exothermic) electron affinity. b. higher ionization energy. c. larger size.

Complete and balance the equations for the following reactions. a. \(\mathrm{Li}(s)+\mathrm{N}_{2}(g) \rightarrow\) b. \(\mathrm{Rb}(s)+\mathrm{S}(s) \rightarrow\)
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Kinetics

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Analysis

Read Explanation

Chemistry Branches

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.