"the distribution of electrons of an atom or molecule in atomic or molecular orbitals"
The arrangement of electrons in an atom's energy levels, which determines the chemical properties of the atom.
Atomic Structure: Understanding the basic structure of atoms, including the arrangement of electrons, protons, and neutrons.
Quantum Mechanics: Understanding the principles of quantum mechanics and how they relate to electron configuration.
Orbitals: Understanding the different types of orbitals (s, p, d, f) and how they are arranged within an atom.
Electron configuration notation: Understanding how to write electron configurations using chemical symbols and superscripts.
Valence electrons: Understanding the concept of valence electrons and how they relate to chemical bonding.
Periodic trends: Understanding how the periodic table can be used to predict electron configuration and chemical properties.
Pauli Exclusion Principle: Understanding the principle that no two electrons can occupy the same quantum state simultaneously.
Hund's Rule: Understanding the rule that electrons prefer to occupy separate orbitals of the same energy level, with parallel spins.
Aufbau Principle: Understanding the principle that electrons fill orbitals in order of increasing energy level.
Lewis Dot Structures: Understanding the basics of Lewis dot structures and how they are used to represent chemical bonding.
Ionic Bonds: Understanding how atoms form ions and how ionic bonds are formed between oppositely charged ions.
Covalent Bonds: Understanding how covalent bonds are formed through the sharing of electrons between atoms.
Metallic Bonds: Understanding how metallic bonds are formed in metals and how they contribute to metallic properties.
Hybridization: Understanding how hybrid orbitals are formed through the combination of atomic orbitals.
Molecular Orbital Theory: Understanding how molecular orbitals are formed through the combination of atomic orbitals in molecules.
VSEPR Theory: Understanding the principles of VSEPR theory and how they are used to predict molecular geometry.
Intermolecular Forces: Understanding the different types of intermolecular forces (Van der Waals, dipole-dipole, hydrogen bonds) and how they contribute to the properties of substances.
Single covalent bond: A bond in which one pair of electrons is shared between two atoms, typically between two nonmetals.
Double covalent bond: A bond in which two pairs of electrons are shared between two atoms, usually between two nonmetals.
Triple covalent bond: A bond in which three pairs of electrons are shared between two atoms, often between two nonmetals.
Polar covalent bond: A bond in which electrons are shared unequally between two atoms, resulting in a partial positive and partial negative charge on each end of the bond.
Nonpolar covalent bond: A bond in which electrons are shared equally between two atoms, resulting in no charge difference between the ends of the bond.
Ionic bond: A bond resulting from the transfer of electrons from one atom to another, typically between a metal and a nonmetal.
Metallic bond: A bond between metal atoms in which the outer electrons are shared by all the atoms in the metal, forming a "sea" of electrons.
Hydrogen bond: A weak bond between a hydrogen atom bonded to an electronegative atom (usually oxygen, nitrogen, or fluorine) and another electronegative atom.
Van der Waals forces: Weak attractive forces between molecules, resulting from temporary dipoles created by fluctuations in electron distribution.
"the electron configuration of the neon atom is 1s2 2s2 2p6"
"the 1s, 2s and 2p subshells"
"2 electrons"
"as moving independently in an orbital, in an average field created by all other orbitals"
"Slater determinants or configuration state functions"
"a level of energy"
"in certain conditions, electrons are able to move from one configuration to another by the emission or absorption of a quantum of energy"
"a quantum of energy, in the form of a photon"
"useful in understanding the structure of the periodic table of elements"
"useful for describing the chemical bonds that hold atoms together"
"helps explain the peculiar properties of lasers"
"helps explain the peculiar properties of semiconductors"
"atomic physics and quantum chemistry"
"each electron as moving independently in an orbital"
"laws of quantum mechanics"
"this same idea helps explain the peculiar properties of lasers and semiconductors"
"Mathematically, configurations are described by Slater determinants or configuration state functions"
"6 electrons"
"2 electrons"