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The strength of the M-O bond tends to increase with the charge and decrease as the size of the metal ion increases. In fact there is a very good linear correlation between hydration enthalpy and the ratio of charge squared to ionic radius, z 2 /r. [4] For ions in solution Shannon's "effective ionic radius" is the measure most often used. [5]
The important interaction between phosphate and magnesium ions makes magnesium essential to the basic nucleic acid chemistry of all cells of all known living organisms. More than 300 enzymes require magnesium ions for their catalytic action, including all enzymes using or synthesizing ATP and those that use other nucleotides to synthesize DNA ...
The molar ionic strength, I, of a solution is a function of the concentration of all ions present in that solution. [3]= = where one half is because we are including both cations and anions, c i is the molar concentration of ion i (M, mol/L), z i is the charge number of that ion, and the sum is taken over all ions in the solution.
For multivalent ions, it is usual to consider the conductivity divided by the equivalent ion concentration in terms of equivalents per litre, where 1 equivalent is the quantity of ions that have the same amount of electric charge as 1 mol of a monovalent ion: 1 / 2 mol Ca 2+, 1 / 2 mol SO 2−
Normally an ion would bond an inert gas atom more strongly, as attraction varies as 1/R 4, compared to 1/R 6 for a van der Waals molecule, and in an ion, the electron cloud shrinks due to the more positive charge attracting it. However in the doubly excited state both of the magnesium atoms are in p suborbitals, which can be arranged so that ...
For ions, the charge on a particular atom may be denoted with a right-hand superscript. For example, Na +, or Cu 2+. The total charge on a charged molecule or a polyatomic ion may also be shown in this way, such as for hydronium, H 3 O +, or sulfate, SO 2− 4. Here + and − are used in place of +1 and −1, respectively.
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This is the energy per mole necessary to remove electrons from gaseous atoms or atomic ions. The first molar ionization energy applies to the neutral atoms. The second, third, etc., molar ionization energy applies to the further removal of an electron from a singly, doubly, etc., charged ion.