Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 2: Problem 14

What is meant by an orbital?

Short Answer

Expert verified
An orbital is a region in an atom where there is a high probability of finding an electron. There are four types of orbitals: s-orbital (spherical shape), p-orbital (dumbbell shape), d-orbital (cloverleaf shape), and f-orbital (complex shape). Orbitals are essential for understanding electron configurations of atoms and predicting their chemical properties, as they follow the Aufbau principle, where electrons occupy orbitals in increasing order of energy.

Step by step solution

01

Definition of an Orbital

An orbital is a region in an atom where there is a high probability of finding an electron. Each orbital can hold up to two electrons, and these electrons have opposite spins. Orbitals dictate the behavior of electrons around an atomic nucleus and help us understand the chemical properties and reactivity of elements.
02

Types of Orbitals

There are four types of orbitals, characterized by the different shapes of electron clouds around the atomic nucleus. These are: 1. s-orbital: Has a spherical shape and can be found in all energy levels. It can hold a total of 2 electrons. 2. p-orbital: Has a dumbbell shape and can be found in all energy levels except the first one. There are three p-orbitals (px, py, pz) in each energy level, and they can hold a total of 6 electrons. 3. d-orbital: Has a more complex, cloverleaf shape and can be found in energy levels from the third one upwards. There are five d-orbitals in each energy level, and they can hold a total of 10 electrons. 4. f-orbital: Has an even more complex shape and can be found in energy levels from the fourth one upwards. There are seven f-orbitals in each energy level, and they can hold a total of 14 electrons.
03

Understanding Orbitals in the Context of Electron Configuration

Orbitals are essential for understanding electron configurations of atoms and predicting their chemical properties. The arrangement of electrons in various orbitals follows a specific order, known as the Aufbau principle. This principle states that electrons occupy orbitals in increasing order of energy, filling lower energy levels before moving to higher ones. This helps explain the periodic table trends, such as ionization energy, electron affinity, and reactivity of elements.

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

Calculate the wavelength of light emitted when each of the following transitions occur in the hydrogen atom. What type of electromagnetic radiation is emitted in each transition? a. \(n=3 \rightarrow n=2\) b. \(n=4 \rightarrow n=2\) c. \(n=2 \rightarrow n=1\)

Valence electrons are those electrons in the outermost principal quantum level (highest \(n\) level) of an atom in its ground state. Groups \(1 \mathrm{A}\) to \(8 \mathrm{A}\) have from 1 to 8 valence electrons. For each group of the representative elements (1A-8A), give the number of valence electrons, the general valence electron configuration, a sample element in that group, and the specific valence electron configuration for that element.

In each of the following sets, which atom or ion has the smallest ionization energy? a. \(\mathrm{Ca}, \mathrm{Sr}, \mathrm{Ba}\) b. \(\mathrm{K}, \mathrm{Mn}, \mathrm{Ga}\) c. \(\mathrm{N}, \mathrm{O}, \mathrm{F}\) d. \(S^{2-}, S, S^{2+}\) e. \(\mathrm{Cs}, \mathrm{Ge}, \mathrm{Ar}\)

Predict some of the properties of element 117 (the symbol is Uus, following conventions proposed by the International Union of Pure and Applied Chemistry, or IUPAC). a. What will be its electron configuration? b. What element will it most resemble chemically?

Consider the following ionization energies for aluminum: $$ \begin{aligned} \mathrm{Al}(g) \longrightarrow \mathrm{Al}^{+}(g)+\mathrm{e}^{-} & I_{1}=580 \mathrm{kJ} / \mathrm{mol} \\ \mathrm{Al}^{+}(g) \longrightarrow \mathrm{Al}^{2+}(g)+\mathrm{e}^{-} & I_{2}=1815 \mathrm{kJ} / \mathrm{mol} \\ \mathrm{Al}^{2+}(g) \longrightarrow \mathrm{Al}^{3+}(g)+\mathrm{e}^{-} & I_{3}=2740 \mathrm{kJ} / \mathrm{mol} \\ \mathrm{Al}^{3+}(g) \longrightarrow \mathrm{Al}^{4+}(g)+\mathrm{e}^{-} & I_{4}=11,600 \mathrm{kJ} / \mathrm{mol} \end{aligned} $$ a. Account for the trend in the values of the ionization energies. b. Explain the large increase between \(I_{3}\) and \(I_{4}\).
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Organic Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Kinetics

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Making Measurements

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