/*! 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 13 Explain what is meant by the ter... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 7: Problem 13

Explain what is meant by the term 鈥渆xcited state鈥� as it applies to an electron. Is an electron in an excited state higher or lower in energy than an electron in the ground state? Is an electron in an excited state more or less stable than an electron in the ground state?

Short Answer

Expert verified
The term "excited state" refers to an electron occupying a higher energy level than its ground state, which is the lowest possible energy level. An electron in an excited state has higher energy and is less stable than an electron in the ground state. The electron absorbs energy to move to a higher orbital and tends to lose this extra energy and return to the ground state through relaxation or emission of light or other electromagnetic radiation. The ground state is the most stable energy state for an electron.

Step by step solution

01

Definition of Excited State

The excited state of an electron refers to a state where the electron occupies an energy level higher than its lowest possible energy level, which is called the ground state. In this state, the electron has absorbed energy and moved to a higher orbital.
02

Energy Comparison between Excited State and Ground State

An electron in an excited state has higher energy than an electron in the ground state. This is because the electron has absorbed extra energy to move to a higher energy level or orbital.
03

Stability of Excited State and Ground State Electrons

An electron in an excited state is less stable than an electron in the ground state. In the excited state, the electron is farther from the nucleus, and it tends to move back to the ground state by losing the extra energy in the form of light or other electromagnetic radiation. This process is called relaxation or emission. The ground state is the most stable energy state for an electron, where it is attracted by the positive charge of the nucleus and is in its lowest possible energy level.

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!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Energy Levels
Think of energy levels as the steps on a ladder. Electrons have certain "rungs" or energy levels they are allowed to "stand" on.
Each rung is an energy level that corresponds to a specific amount of energy. The higher the rung, the more energy the electron has.
  • Energy levels are defined and quantized, meaning electrons cannot exist in-between these levels.
  • When an electron gains energy, it can jump to a higher energy level or orbital.
  • These higher levels are often further away from the nucleus.
This process where an electron gains energy to move up energy levels is known as excitation. Similarly, when an electron loses energy, it "jumps" down to a lower level, sometimes emitting light or radiation as a part of this energy loss.
Ground State
The ground state is like the "home" for an electron. It's the lowest energy level that an electron can occupy.
In this state, the electron is closest to the nucleus and has the least amount of energy possible within an atom.
  • The ground state is the most stable state for an electron because of its proximity to the positively charged nucleus.
  • Electrons naturally want to settle in this low-energy state, as it requires less energy overall.
  • Whenever an electron moves back to the ground state from a higher energy level, the atom may release energy, often seen as light.
This release of energy is part of why fireworks and neon lights can be so colorful and bright.
Electron Stability
Electron stability refers to how "content" an electron is within its current energy level. A stable electron is like having a peaceful electron existence close to the nucleus.
  • Electrons in their ground state are most stable because they are in their lowest possible energy level.
  • Stability decreases when an electron is in an excited state because it has moved away from the nucleus.
  • Excited electrons tend to return to the ground state quickly to regain stability, releasing energy as they do so.
This tendency toward regaining stability is a fundamental principle behind many chemical reactions and the behavior of electrons in various elements. Understanding this concept helps explain why atoms react and interact with each other to form molecules and compounds.

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

A certain oxygen atom has the electron configuration 1\(s^{2} 2 s^{2} 2 p_{x}^{2} 2 p_{y}^{2} .\) How many unpaired electrons are present? Is this an excited state of oxygen? In going from this state to the ground state, would energy be released or absorbed?

Although no currently known elements contain electrons in g orbitals in the ground state, it is possible that these elements will be found or that electrons in excited states of known elements could be in \(g\) orbitals. For \(g\) orbitals, the value of \(\ell\) is \(4 .\) What is the lowest value of \(n\) for which \(g\) orbitals could exist? What are the possible values of \(m_{\ell} ?\) How many electrons could a set of \(g\) orbitals hold?

In the ground state of mercury, Hg, a. how many electrons occupy atomic orbitals with \(n=3 ?\) b. how many electrons occupy \(d\) atomic orbitals? c. how many electrons occupy \(p_{z}\) atomic orbitals? d. how many electrons have spin "up" " \(\left(m_{s}=+\frac{1}{2}\right) ?\)

X rays have wavelengths on the order of \(1 \times 10^{-10} \mathrm{m} .\) Calcu- late the energy of \(1.0 \times 10^{-10} \mathrm{m} \mathrm{X}\) rays in units of kilojoules per mole of \(\mathrm{X}\) rays. AM radio waves have wavelengths on the order of \(1 \times 10^{4} \mathrm{m}\) . Calculate the energy of \(1.0 \times 10^{4} \mathrm{m}\) radio waves in units of kilojoules per mole of radio waves. Consider that the bond energy of a carbon-carbon single bond found in organic compounds is 347 \(\mathrm{kJ} / \mathrm{mol}\) . Would \(\mathrm{x}\) rays and/or radio waves be able to disrupt organic compounds by breaking carbon-carbon single bonds?

The wave function for the 2\(p_{z}\) orbital in the hydrogen atom is $$\psi_{2 p_{z}}=\frac{1}{4 \sqrt{2 \pi}}\left(\frac{Z}{a_{0}}\right)^{3 / 2} \sigma \mathrm{e}^{-\sigma / 2} \cos \theta$$ where \(a_{0}\) is the value for the radius of the first Bohr orbit in meters \(\left(5.29 \times 10^{-11}\right), \sigma\) is \(Z\left(r / a_{0}\right), r\) is the value for the distance from the nucleus in meters, and \(\theta\) is an angle. Calculate the value of \(\psi_{2 p_{z}}^{2}\) at \(r=a_{0}\) for \(\theta=0^{\circ}\left(z \text { axis ) and for } \theta=90^{\circ}\right.\) (xy plane).
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Chemical Analysis

Read Explanation

Physical Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Making Measurements

Read Explanation

Nuclear Chemistry

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.