Quote: "Energy levels are certain discrete values of energy that a bound quantum mechanical system or particle can take on."
The different energy levels that electrons can occupy around the nucleus of an atom, and how these levels can change due to absorption or emission of energy.
Bohr Model: Describes how electrons occupy quantized energy levels in an atom.
Energy Levels: Correspond to specific energies of an electron in an atom.
Spectroscopy: Study of how atoms interact with light.
Emission Spectra: Patterns of light emitted by excited atoms when they return to lower energy levels.
Absorption Spectra: Patterns of light absorbed by atoms to promote electrons to higher energy levels.
Quantum Mechanics: Study of the behavior of particles at the atomic and subatomic level.
Schrödinger Equation: Describes the behavior of electrons in atoms.
Quantum Numbers: Set of numbers that determine the state and energy of an electron in an atom.
Pauli Exclusion Principle: No two electrons can occupy the same energy level or state simultaneously.
Hund's Rule: Electrons tend to fill orbitals in a way that maximizes their spin.
Ground State: The lowest energy state of an atom.
Excited State: Higher energy state of an atom when an electron absorbs energy.
Ionization: Process of removing or adding electrons to an atom.
Quantum Tunneling: Phenomenon in which particles move through potential barriers even if they don't have enough energy to overcome it.
Fine Structure: Small energy differences between energy levels, which are due to the spin or angular momentum of electrons.
Zeeman Effect: Splitting of spectral lines in the presence of a magnetic field.
Stark Effect: Splitting of spectral lines in the presence of an electric field.
Isotopes: Atoms with the same number of protons but different number of neutrons in the nucleus.
Nuclear Spin: Property of protons and neutrons with a magnetic moment due to their angular momentum.
Hyperfine Structure: Small energy differences between energy levels due to the interaction between nuclear spin and orbital angular momentum of electrons.
Atomic Orbital: The region in which an electron has a high probability of being found in an atom.
Atomic Electron Configuration: The arrangement of electrons in the atom's energy levels.
Photoelectric Effect: Phenomenon in which electrons are ejected from the surface of a metal when exposed to light of a certain frequency.
Compton Scattering: Interaction between photons and electrons that results in the scattering of radiation.
Radiation Dose: The amount of energy absorbed by a material due to radiation.
Ground state level: This is the lowest energy level of an atom, which is the stable and most common state for an atom.
Excited state level: This is a higher energy level than the ground state level, and it occurs when an atom absorbs energy.
Principal quantum level: This describes the main energy level of an atom, denoted by the quantum number 'n'. It determines the size and energy of the atomic orbitals.
Azimuthal quantum level: This is also known as the subsidiary quantum level or angular momentum quantum number 'l'. It determines the shape of the atomic orbitals.
Magnetic quantum level: This is also known as the magnetic quantum number 'm'. It describes the orientation of the atomic orbitals in space around the nucleus.
Spin quantum level: This is also known as the spin quantum number 's'. It describes the intrinsic angular momentum or spin of the electrons in an atom.
Total angular momentum level: This is also known as the total angular momentum quantum number 'j', which is the sum of the orbital and spin angular momentum of an electron.
Fine structure level: This is the splitting of energy levels due to the interaction of the electron's spin and orbital motion.
Hyperfine structure level: This is the further splitting of the fine structure levels due to the interaction between the electron's spin and the nuclear spin.
Zeeman effect level: This is the splitting of energy levels in an external magnetic field, which results in the appearance of spectral lines.
Quote: "Classical particles can have any amount of energy."
Quote: "An electron shell or principal energy level may be thought of as the orbit of one or more electrons around an atom's nucleus."
Quote: "The shells correspond with the principal quantum numbers (n = 1, 2, 3, 4 ...) or are labeled alphabetically with letters used in the X-ray notation (K, L, M, N...)."
Quote: "The first shell can hold up to two electrons."
Quote: "The second shell can hold up to eight (2 + 6) electrons."
Quote: "The nth shell can in principle hold up to 2n^2 electrons."
Quote: "Atoms' electrons will generally occupy outer shells only if the more inner shells have already been completely filled by other electrons."
Quote: "Atoms may have two or even three incomplete outer shells."
Quote: "If an atom is at the lowest possible energy level, it and its electrons are said to be in the ground state."
Quote: "If an atom is at a higher energy level, it is said to be excited, or any electrons that have higher energy than the ground state are excited."
Quote: "An energy level is regarded as degenerate if there is more than one measurable quantum mechanical state associated with it."
Quote: "The energy levels of the electrons in atoms, ions, or molecules are bound by the electric field of the nucleus."
Quote: "Energy levels can also refer to vibrational or rotational energy levels in molecules."
Quote: "The energy spectrum of a system with such discrete energy levels is said to be quantized."
Quote: "The shells correspond with the principal quantum numbers (n = 1, 2, 3, 4 ...)."
Quote: "The third shell can hold up to 18 (2 + 6 + 10) electrons."
Quote: "However, this is not a strict requirement: atoms may have two or even three incomplete outer shells."
Quote: "If the potential energy is set to zero at infinite distance from the atomic nucleus or molecule, the usual convention, then bound electron states have negative potential energy."
Quote: "This contrasts with classical particles, which can have any amount of energy."