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Characteristic of the post-transition minerals, tendency of the outermost s electrons to remain nonionized or un shared in compounds.

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Chemical Kinetics

The study of rates and mechanisms of chemical reactions and of the factors on which they depend.

Pairing

A favourable interaction of two electrons with opposite m , values in the same orbital.

Nuclide Symbol

Symbol for an atom A/Z E, in which E is the symbol of an element, Z is its atomic number, and A is its mass number.

Haber Process

A process for the catalyzed industrial production of ammonia from N2 and H2 at high temperature and pressure.

Dynamic Equilibrium

An equilibrium in which processes occur continuously, with no net change. When two (or more) processes occur at the same rate so that no net change occurs.

Nodal Plane

A region in which the probability of finding an electron is zero.

 

Voltaic Cells

Electrochemical cells in which spontaneous chemical reactions produce electricity, also called galvanic cells.

 

Oil

Liquid triester of glycerol and unsaturated fatty acids.

Dimer

Molecule formed by combination of two smaller (identical) molecules.

Cathode

Electrode at which reduction occurs in a cathode ray tube, the negative electrode.

Dilution

Process of reducing the concentration of a solute in solution, usually simply by mixing with more solvent.

Electrophile

Positively charged or electron-deficient.

Photon

A packet of light or electromagnetic radiation, also called quantum of light.

 

Hess' Law of Heat Summation

The enthalpy change for a reaction is the same whether it occurs in one step or a series of steps.

Organic Chemistry

The chemistry of substances that contain carbon-hydrogen bonds.

Square Planar Complex

Complex in which the metal is in the center of a square plane, with ligand donor atoms at each of the four corners.

Ionization Isomers

Isomers that result from the interchange of ions inside and outside the coordination sphere.

Thermodynamics

The study of the energy transfers accompanying physical and chemical processes.

Valence Shell Electron Pair Repulsion Theory

Assumes that electron pairs are arranged around the central element of a molecule or polyatomic ion so that there is maximum separation (and minimum repulsion) among regions of high electron density.

 

Formal Charge

A method of counting electrons in a covalently bonded molecule or ion, counts bonding electrons as though they were equally shared between the two atoms.