Studied by 0 people
Electron Structure
Describes the arrangement of electrons around an atom's nucleus, including energy levels and orbitals.
Shells
Groups of atomic orbitals that have the same principal quantum number, n, representing different energy levels.
Sub-shells
Divisions of shells designated as s, p, d, or f, each with specific maximum electron capacity.
Atomic Orbitals
Regions around the nucleus where pairs of electrons are likely to be found.
Electron Configuration
The distribution of electrons in an atom's orbitals, determined by the atomic number.
Ionic Bonding
The electrostatic attraction between positively and negatively charged ions formed when electrons are transferred.
Covalent Bonding
The strong attraction formed when two nonmetals share electron pairs.
Dative Bonding
A type of covalent bond where both electrons in a shared pair are supplied by one atom.
Electronegativity
The ability of an atom to attract bonding electrons in a covalent bond.
Permanent Dipole
A dipole that occurs when there is a difference in electronegativity across a bond, creating partial positive and negative regions.
Induced Dipole
A temporary dipole that occurs when the electron distribution around a molecule is influenced by nearby charges.
Van der Waals Forces
Weak intermolecular forces arising from induced dipole interactions between molecules.
Hydrogen Bonding
The strongest type of intermolecular force, occurring between hydrogen and highly electronegative atoms like N, O, or F.
Macromolecular Structure
A structure composed of covalently bonded atoms in a giant lattice, resulting in high melting points and rigidity.
Diamond
A macromolecular structure made of carbon atoms, each bonded to four others, known for its hardness.
Graphite
A macromolecular structure of carbon arranged in layers, with free electrons allowing electrical conductivity.
Simple Molecular Substances
Substances composed of covalently bonded molecules held together by weak van der Waals forces, resulting in low melting points.
