# 8.S: Atomic Structure (Summary)

- Page ID
- 10321

## Key Terms

angular momentum orbital quantum number (l) | quantum number associated with the orbital angular momentum of an electron in a hydrogen atom |

angular momentum projection quantum number (m) | quantum number associated with the z-component of the orbital angular momentum of an electron in a hydrogen atom |

atomic orbital | region in space that encloses a certain percentage (usually 90%) of the electron probability |

Bohr magneton | magnetic moment of an electron, equal to \(\displaystyle 9.3×10^{−24}J/T\) or \(\displaystyle 5.8×10^{−5}eV/T\) |

braking radiation | radiation produced by targeting metal with a high-energy electron beam (or radiation produced by the acceleration of any charged particle in a material) |

chemical group | group of elements in the same column of the periodic table that possess similar chemical properties |

coherent light | light that consists of photons of the same frequency and phase |

covalent bond | chemical bond formed by the sharing of electrons between two atoms |

electron configuration | representation of the state of electrons in an atom, such as \(\displaystyle 1s^22s^1\) for lithium |

fine structure | detailed structure of atomic spectra produced by spin-orbit coupling |

fluorescence | radiation produced by the excitation and subsequent, gradual de-excitation of an electron in an atom |

hyperfine structure | detailed structure of atomic spectra produced by spin-orbit coupling |

ionic bond | chemical bond formed by the electric attraction between two oppositely charged ions |

laser | coherent light produced by a cascade of electron de-excitations |

magnetic orbital quantum number | another term for the angular momentum projection quantum number |

magnetogram | pictoral representation, or map, of the magnetic activity at the Sun’s surface |

metastable state | state in which an electron “lingers” in an excited state |

monochromatic | light that consists of photons with the same frequency |

Moseley plot | plot of the atomic number versus the square root of X-ray frequency |

Moseley’s law | relationship between the atomic number and X-ray photon frequency for X-ray production |

| measure of the strength of the magnetic field produced by the orbital angular momentum of the electron |

Pauli’s exclusion principle | no two electrons in an atom can have the same values for all four quantum numbers \(\displaystyle (n,l,m,ms)\) |

population inversion | condition in which a majority of atoms contain electrons in a metastable state |

principal quantum number (n) | quantum number associated with the total energy of an electron in a hydrogen atom |

radial probability density function | function use to determine the probability of a electron to be found in a spatial interval in r |

selection rules | rules that determine whether atomic transitions are allowed or forbidden (rare) |

spin projection quantum number (\(\displaystyle m_s\)) | quantum number associated with the z-component of the spin angular momentum of an electron |

spin quantum number (s) | quantum number associated with the spin angular momentum of an electron |

spin-flip transitions | atomic transitions between states of an electron-proton system in which the magnetic moments are aligned and not aligned |

spin-orbit coupling | interaction between the electron magnetic moment and the magnetic field produced by the orbital angular momentum of the electron |

stimulated emission | when a photon of energy triggers an electron in a metastable state to drop in energy emitting an additional photon |

transition metal | element that is located in the gap between the first two columns and the last six columns of the table of elements that contains electrons that fill the d subshell |

valence electron | electron in the outer shell of an atom that participates in chemical bonding |

Zeeman effect | splitting of energy levels by an external magnetic field |

## Key Equation

Orbital angular momentum | \(\displaystyle L=\sqrt{l(l+1)}ℏ\) |

z-component of orbital angular momentum | \(\displaystyle L_z=mℏ\) |

Radial probability density function | \(\displaystyle P(r)dr=∣ψ_{n00}∣^24πr^2dr\) |

Spin angular momentum | \(\displaystyle S=\sqrt{s(s+1)}ℏ\) |

z-component of spin angular momentum | \(\displaystyle S_z=m_sℏ\) |

Electron spin magnetic moment | \(\displaystyle \vec{μ_s}=(\frac{e}{m_e})\vec{S}\) |

Electron orbital magnetic dipole moment | \(\displaystyle \vec{μ}=−(\frac{e}{2m_e})\vec{L}\) |

Potential energy associated with the magnetic interaction between the orbital magnetic dipole moment and an external magnetic field \(\displaystyle vec{B}\) | \(\displaystyle U(θ)=−μ_zB=mμ_BB\) |

Maximum number of electrons in a subshell of a hydrogen atom | \(\displaystyle N=4l+2\) |

Selection rule for atomic transitions in a hydrogen-like atom | \(\displaystyle Δl=±1\) |

Moseley’s law for X-ray production | \(\displaystyle (Z−1)=constant\sqrt{f}\) |

## Summary

#### 8.1 The Hydrogen Atom

A hydrogen atom can be described in terms of its wave function, probability density, total energy, and orbital angular momentum.

The state of an electron in a hydrogen atom is specified by its quantum numbers (

*n*,*l*,*m*).In contrast to the Bohr model of the atom, the Schrödinger model makes predictions based on probability statements.

The quantum numbers of a hydrogen atom can be used to calculate important information about the atom.

#### 8.2 Orbital Magnetic Dipole Moment of the Electron

A hydrogen atom has magnetic properties because the motion of the electron acts as a current loop.

The energy levels of a hydrogen atom associated with orbital angular momentum are split by an external magnetic field because the orbital angular magnetic moment interacts with the field.

The quantum numbers of an electron in a hydrogen atom can be used to calculate the magnitude and direction of the orbital magnetic dipole moment of the atom.

#### 8.3 Electron Spin

The state of an electron in a hydrogen atom can be expressed in terms of five quantum numbers.

The spin angular momentum quantum of an electron is

*=*\(\displaystyle +½\). The spin angular momentum projection quantum number is \(\displaystyle*m*=+½\) or \(\displaystyle −½\) (spin up or spin down)._{s}The fine and hyperfine structures of the hydrogen spectrum are explained by magnetic interactions within the atom.

#### 8.4 The Exclusion Principle and the Periodic Table

Pauli’s exclusion principle states that no two electrons in an atom can have all the same quantum numbers.

The structure of the periodic table of elements can be explained in terms of the total energy, orbital angular momentum, and spin of electrons in an atom.

The state of an atom can be expressed by its electron configuration, which describes the shells and subshells that are filled in the atom.

#### 8.5 Atomic Spectra and X-rays

Radiation is absorbed and emitted by atomic energy-level transitions.

Quantum numbers can be used to estimate the energy, frequency, and wavelength of photons produced by atomic transitions.

Atomic fluorescence occurs when an electron in an atom is excited several steps above the ground state by the absorption of a high-energy ultraviolet (UV) photon.

X-ray photons are produced when a vacancy in an inner shell of an atom is filled by an electron from the outer shell of the atom.

The frequency of X-ray radiation is related to the atomic number

*Z*of an atom.

#### 8.6 Lasers

Laser light is coherent (monochromatic and “phase linked”) light.

Laser light is produced by population inversion and subsequent de-excitation of electrons in a material (solid, liquid, or gas).

CD and Blu-Ray players uses lasers to read digital information stored on discs.

## Contributors and Attributions

Samuel J. Ling (Truman State University), Jeff Sanny (Loyola Marymount University), and Bill Moebs with many contributing authors. This work is licensed by OpenStax University Physics under a Creative Commons Attribution License (by 4.0).