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Chapter 8: Problem 120

Briefly describe each of the following ideas or phenomena: (a) atomic (line) spectrum; (b) photoelectric effect; (c) matter wave; (d) Heisenberg uncertainty principle; (e) electron spin; (f) Pauli exclusion principle; (g) Hund's rule; (h) orbital diagram; (i) electron charge density; (j) radial electron density.

Short Answer

Expert verified
The ten concepts are core principles and phenomena in atomic and quantum physics, covering key principles such as the atomic spectrum, photoelectric effect, matter wave, Heisenberg uncertainty principle, electron spin, Pauli exclusion principle, Hund's rule, orbital diagram, electron charge density, and radial electron density. Each has its unique definition and implication.

Step by step solution

01

Atomic (Line) Spectrum

An atomic (line) spectrum is a unique spectrum of light, emitted or absorbed by an atom, that is composed of specific wavelengths. Each wavelength corresponds to a particular transition of an electron from one energy level to another in an atom.
02

Photoelectric Effect

The photoelectric effect is the phenomenon in which electrons are emitted from a metal's surface when light of a certain frequency, or higher, is shone on it. This discovery supported the idea that light carries energy in discrete, quantized amounts, or photons.
03

Matter Wave

Matter wave, also known as de Broglie wave, can describe the wave-like behavior of particles such as electrons. The concept arose from the de Broglie hypothesis that suggests that all matter exhibits properties of both particles and waves.
04

Heisenberg Uncertainty Principle

The Heisenberg Uncertainty Principle states that it is impossible to precisely measure the exact position and momentum (or any two complementary variables) of a quantum system at the same time. The more precisely the position is measured, the less precisely the momentum can be known, and vice versa.
05

Electron Spin

Electron spin is a form of intrinsic angular momentum that is carried by electrons. It is a quantum property with two possible values: spin-up and spin-down.
06

Pauli Exclusion Principle

The Pauli Exclusion Principle states that no two electrons in an atom can have the same set of quantum numbers. That is, each electron in an atom occupies a unique quantum state, and no two electrons can be in the same state simultaneously.
07

Hund's Rule

Hund's rule specifies that when filling sublevels of an electron configuration, electrons are placed in individual orbitals before they are paired up. Essentially, each orbital in a subshell is singly occupied before any orbital is doubly occupied.
08

Orbital Diagram

An orbital diagram is a pictorial description of electrons in an atom. It shows how the orbitals of the energy levels of an atom are filled and the spin of the electrons.
09

Electron Charge Density

Electron charge density describes the distribution of an electron's charge in an atom or molecule. It usually represents the probability of finding the electron in a specific region around the nucleus.
10

Radial Electron Density

Radial electron density describes the total probability of finding an electron at different distances (radii) from the nucleus in an atom. It peaks at the most likely distance from the nucleus.

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Most popular questions from this chapter

Concerning the concept of subshells and orbitals, (a) How many subshells are found in the \(n=3\) level? (b) What are the names of the subshells in the \(n=3\) level? (c) How many orbitals have the values \(n=4\) and \(\ell=3 ?\) (d) How many orbitals have the values \(n=3, \ell=2\) and \(m_{\ell}=-2 ?\) (e) What is the total number of orbitals in the \(n=4\) level?

An electron in a one-dimensional box requires a wavelength of \(618 \mathrm{nm}\) to excite an electron from the \(n=2\) level to the \(n=4\) level. Calculate the length of the box.

What is the wavelength, in nanometers, associated with a \(1000 \mathrm{kg}\) automobile traveling at a speed of \(25 \mathrm{m} \mathrm{s}^{-1},\) that is, considering the automobile to be a matter wave? Comment on the feasibility of an experimental measurement of this wavelength.

Describe two ways in which the orbitals of multielectron atoms resemble hydrogen orbitals and two ways in which they differ from hydrogen orbitals.

What electron transition in a hydrogen atom, starting from the orbit \(n=7,\) will produce light of wavelength \(410 \mathrm{nm} ?\)
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