The amount of energy absorbed in the process in which an electron is added to a neutral isolated gaseous atom to form a gaseous ion with a 1- charge, has a negative value if energy is released.
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Short-lived species formed by the collision of dissolved ions of opposite charges.
Molecular orbital resulting from head-on overlap of two atomic orbitals.
Equilibrium constant that applies to the dissociation of a comples ion into a simple ion and coordinating species (ligands).
The dispersing medium of a solution.
One of the two mirror-image forms of an optically active molecule.
Complex species that contain ammonia molecules bonded to metal ions.
Solution that resists change in pH, contains either a weak acid and a soluble ionic salt of the acid or a weak base and a soluble ionic salt of the base.
For acid-base titrations, organic compounds that exhibit different colors in solutions of different acidities, used to determine the point at which reaction between two solutes is complete.
A molecular orbital higher in energy than any of the atomic orbitals from which it is derived, lends instability to a molecule or ion when populated with electrons, denoted with a star (*) superscript or symbol.
Isomers in which a particular ligand bonds to a metal ion through different donor atoms.
Nuclide that is produced in a nuclear decay.
A ligand atom whose electrons are shared with a Lewis acid.
A liquid as defined by NFPD and DOT as having a flash point below 37.8°C (100°F).
Any species that can accept a share in an electron pair.
Lead Storage Battery
Secondary voltaic cell used in most automobiles.
High energy particles or rays emitted during the nuclear decay processes.
A solid characterized by a regular, ordered arrangement of particles.
Refers to crystals having the same atomic arrangement.
Different forms of the same element in the same physical state.
Aufbau ('building up') Principle
Describes the order in which electrons fill orbitals in atoms.