Lothar Meyer presented his table several months after Mendeleev, but opposed his Periodic law. Nonmetals tend to gain electrons to form anions. E, Mg in the third I. Ionization energy decreases moving down a group increasing atomic radius.
Ba, Ca, Si, O, F 3.
Initially, no theoretical explanation for the Periodic Law was available and it was used only as an empirical principle, but, with the development of the quantum mechanics, it became possible to understand the theoretical basis for the Periodic Law.
The greater the number of core electrons, the greater the shielding of electrons from the core charge of the nucleus.
Periodic properties assignment
Some generalizations can be made about the electron affinities of certain groups in the periodic table. These groups contain the most naturally abundant elements, and are the most important for life. Now if we look at the various physical and chemical properties of these elements, we would find that their values tend to increase or decrease with Z in a manner that reveals a repeating pattern— that is, a periodicity. The alkali metals react vigorously with water, producing hydrogen gas and solutions of alkali metal hydroxides very exothermic. Metalloids As mentioned in the introduction, metalloids are located along the staircase separating the metals from the nonmetals on the periodic table. Which reaction do you expect to have the greater cell potential? The closer and more tightly bound an electron is to the nucleus, the more difficult it will be to remove, and the higher its ionization energy will be. However, this periodic trend is sparsely followed for heavier elements elements with atomic number greater than 20 , especially for lanthanide and actinide series. At the bottom of Group 3 in this block, notice the elements Lanthanum and Actinium, which are shaded in light green.
Electron Affinity Electron affinity reflects the ability of an atom to accept an electron.
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