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CAUSES OF REACTIVITY

In general, any time a Chemical Reaction occurs it is due to the chemical being able to enter a more stable {Link without Title} state. Quantum Chemistry provides the most in depth and exact understanding of the reason this occurs. Electrons exist in Orbital s that are the result of solving the Schrödinger Equation for specific situations.

All things (values of the ''n'' and ''m''l Quantum Numbers ) being equal, the order of stability of electrons in a system from least to greatest is unpaired with no other electrons in similar orbitals, unpaired with all degenerate orbitals half filled and the most stable is a filled set of orbitals. In order to achieve one of these orders of stability, an atom will react with another atom, thereby stabilizing both atoms. For example, a lone Hydrogen atom has a single electron in its 1s orbital. It becomes significantly more stable (as much as 100 Kilocalories per Mole , or 420 Kilojoules per mole) when reacting to form H2.

It is for this same reason that Carbon will almost always form four Bonds . Its ground state Valence configuration is 2s2 2p2, half filled. However, the Activation Energy to go from half filled to fully filled p orbitals is so small, it is negligible and as such carbon will form them almost instantaneously, meanwhile the process releases a significant amount of energy ( Exothermic ). This four equal bond configuration is called sp3 Hybridization ..


CHEMICAL KINETICS AND REACTIVITY

The rate of any given reaction A → products (important point is that the Order is first) is governed by the equation:

Rate=k {Link without Title}

where the Rate is the number of moles per second consumed in the rate-determining step of the reaction, {Link without Title} is the Concentration of the substance in moles per liter and ''k'' is the reaction constant which is constant for that temperature and pressure, though it is independent of concentration. The greater the reactivity of a compound the higher the value of ''k'' and the higher the rate.


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