Crystal field designation for an outer orbital complex, all t2g and eg orbitals are singly occupied before any pairing occurs.
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An organic ion carrying a negative charge on a carbon atom.
Structures of a compound that differ by the extent of rotation about a single bond.
Valence Bond Theory
Assumes that covalent bonds are formed when atomic orbitals on different atoms overlap and the electrons are shared.
Solution in which no more solute will dissolve.
Weak repulsion by a magnetic field.
At the same temperature and pressure, equal volumes of all gases contain the same number of molecules.
Unit of electrical charge.
Nuclide that is produced in a nuclear decay.
A technique for separation of ions by rate and direction of migration in an electric field.
Discovered: known in India and China before 1500 and to the Greeks and Romans before 20 BC as the copper-zinc alloy brass
Origin: The name is derived from the German ‘Zink’.
Atomic no: 30
Mass No: 65
Description: A grey metal with a blue tinge. World production exceeds 7 million tons a year, and it is used to galvanise iron to prevent it rusting. It is also employed in alloys and batteries, and as zinc oxide to stabilise rubber and plastics. Zinc is essential for all living things, and is important for growth and development. The average human body contains about 2.5 grams and takes in about 15 milligrams per day. Some foods have above average levels of zinc, including herring, beef, lamb, sunflower seeds and cheese.
Hydrocarbons that contain double or triple carbon-carbon bonds.
A state of dynamic balance in which the rates of forward and reverse reactions are equal, there is no net change in concentrations of reactants or products while a system is at equilibrium.
A substance such as hydrogen, deuterium, oxygen or paraffin capable of slowing fast nuetrons upon collision.
A compound formed by interaction of sucrose with a metallic oxide, usually lime, and useful in the purification of sugar.
A group of atoms derived from an alkane by the removal of one hydrogen atom.
The solid and liquid states.
Refers to crystals having the same atomic arrangement.
The scattering of light by colloidal particles.
Amount of energy that must be absorbed by reactants in their ground states to reach the transition state so that a reaction can occur. In other words, activation energy is the minimum energy required for a chemical reaction to occur.
The interaction of orbitals on different atoms in the same region of space.