Magnesium second ionization energy

Since the process removes the second electron from a magnesium atom, the ionization energy of Mg+ is called the second ionization energy of magnesium. 

The second ionization energy for magnesium is 1451 kj/ mol. How much energy, in kilojoules, must be absorbed by 1.50 g of gaseous magnesium atoms to convert them to gaseous Mg + ions ... 

The second ionization energy of magnesium is only about twice as great as the first, but the third ionization energy is 10 times as great. Why does it take so much more energy to remove the third electron ... 

For magnesium, the first significant jump occurs between the second ionization energy (1451 kj/mol) and the third (7733 kj/mol). We would expect two electrons to be removed, and the most commonly found ion should be Mg ". For aluminum, the third ionization energy is 2745 kJ/mol, whereas the fourth is 11,578 kj/mol. We would expect three ionizations to occur, so aluminum should form Al +. 

In general, ionization energy increases from left to right across a given period. Aluminum, however, has a lower ionization energy than magnesium. Explain. The first and second ionization energies of K are 419 kJ/mol and 3052 kJ/mol, and those of Ca are 590 kJ/mol and 1145 kJ/mol, respectively. Compare their values and comment on the differences. 

For sodium, there is a huge jump between the first and second ionization energies. For magnesium, the ionization energy roughly doubles from the first to the second, but then a huge jump occurs between the second and third ionization energies. What is the reason for these jumps ... 

The third ionization energy of magnesium is more than ten times the first ionization energy. This large increase occurs because the third ionization removes a core electron (2 p) rather than a valence electron (3. ). Removing core electrons from any atom requires much more energy than removing valence electrons. The second ionization... 

In other words, each successive ionization requires more energy. As an example, the first, the second and the third ionization energies of magnesium, Mg, are given below. 

Calculate the difference between the sum of the first two ionization energies of magnesium and the sum of the first two electron affinities of oxygen. Deduce whether the transfer of two electrons from one to the other in the gas phase is spontaneous. (The second electron affinity of oxygen is —816kJ/mol.)... 

The L shell can accommodate a total of 8 electrons, and as further electrons are added to form the sequence of elements beryllium, boron, carbon, etc., these electrons take their place in the second shell until finally, at the end of the second period, neon (Z = 10) is reached, with both the first and second shells fully occupied and with an electronic structure which can be symbolized as (2, 8). The addition of further electrons to form the sequence of elements sodium, magnesium, etc., of the third period requires the formation of a new shell, and in sodium (Z = 11) a single electron occupies the M shell of principal quantum number 3 again the ionization energies reflect the difference in energy between this electron and those more tightly bound in the L and K shells. 

When atoms lose more than one electron, the ionization energy to remove the second electron is always more than the ionization energy to remove the first. Similarly, the ionization energy to remove the third electron is more than the second and so on. However, the increase in ionization energy upon the removal of subsequent electrons is not necessarily uniform. For example, consider the first three ionization energies of magnesium ... 

Notice the trends in the first, second, and third ionization energies of sodium (group 1 A) and magnesium (group 2 A), as shown at left. 

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