Ionization Energies of the Elements

Of more fundamental importance is the plot of first-stage ionization energies of the elements, i.e. the energy /m required to remove the least tightly bound electron from the neutral atom in the gas phase ... 

Figure 2.3 First-stage ionization energies of the elements.

As we move down a given group, the valence electrons are further and further away from the nucleus. The first ionization energies of the elements, which is the energy required to remove an electron from an isolated gaseous atom, decrease while the atomic radii increase. 

How does the effective nuclear charge affect the ionization energies of the elements in a period on the periodic table ... 

Figure 4.3. Ionization energies of the elements. The values of the energies (in kJ/mol of atoms) of 1 st and 2nd ionization are shown. Notice the periodic character of these values as a function of the atomic number. Notice the similar trends of the two graphs when the same number of electrons are considered the maxima, for instance, are observed for the 1 st ionization of He and the 2nd ionization of Li, for 1st and 2nd ionization ofNe andNa+, respectively (having both 10 electrons), etc.

The first ionization energies of the elements are plotted in Figure 1.4. There is a characteristic pattern of the values for the elements Li to Ne which is repeated for the elements Na to Ar, and which is repeated yet again for the elements K, Ca and A1 to Kr (the s- and p-block elements of the fourth period). In the latter case, the pattern is interrupted by the values for the 10 transition elements of the d-block. The fourth period pattern is repeated by the fifth period elements, and there is an additional... 

The effects are observable by a comparison of the metallic radii, the first three ionization energies and the first electron attachment energy of the Group 11 elements as shown in Table 7.3, and the metallic radii and the first two ionization energies of the elements of Group 12 (Zn, Cd and Hg) as given in Table 7.4. 

The / terms are the successive ionization energies of the element M, and the E term is the electron attachment energy of the element X. 

Values of the first and second ionization energies of the elements, as determined spectroscopically, are given in Table 2-5. 

Table 2-5.—First and Second Ionization Energies of the Elements ...

Step 2 Form the gaseous cation of the metal. This step requires the ionization energy of the element and possibly the sum of the first and higher ionization energies. The corresponding arrow points upward. 

Figure 3.4 shows the measured ionization energies of the elements plotted against their atomic numbers. Note that these ionization energies are reported in kj per mole of atoms following the discussion of Section 3.2, 1 eV per atom equals 96.48 kJ per mole. 

TABLE 3.1 Successive Ionization Energies of the Elements Hydrogen through Argon... 

The ionization energy of an atom is defined as the minimum energy necessary to detach an electron from the neutral gaseous atom (see Section 3.3). It can be obtained directly from the photoelectron spectrum of an atomic gas. Appendix F lists measured ionization energies of the elements, and Figure 5.24 shows the periodic trends in first and second ionization energies with increasing atomic number. 

Provided that sufficient energy is transferred to a plasma, atoms can also be ionized. This depends on the temperature of the plasma and also on the ionization energy of the elements. As these ions have discrete energy levels between which... 

The second ionization energies of the elements calcium through manganese increase from left to right in the periodic table with the exception that 72(Cr) > /2(Mn). The electron configurations of the elements are ... 

Of more fundamental importance is the plot of first-stage ionization energies of the elements,... 

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