There are many so called trends that the periodic table follows. One of the many trends is that electronegativity, the tendency needed to attract electrons; ionizations energy, the amount of energy that is needed to rid an electron from the ground state of an atom; electron affinity, the capability of an atom to obtain an electron, decreases along with the group. The melting point, the energy needed to melt solid into a liquid; boiling point, the energy need to change liquid into a gas; metallic character; and the atomic radii size all increase increase as the group increases. These are all common characteristics on the periodic table that associate themselves to the law of periodicity because they deal with elements in particular groups having patterned relationships and similarities.
Group IA on the periodic table also has the name of Alkali Earth metals. Group IA includes Hydrogen, Lithium, Sodium, Potassium, Rubidium, Cesium, and Francium. Although Hydrogen is in Group 1A, it is not an Alkali Earth metal because it is very different from the rest of the elements and does not fit in any gr...
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... person to discover that fluorine 's electronegativity was 4,0, and because of this, he could estimate many other elements 's electronegativity.
Ionization energy is the amount of energy that an atom in gaseous form must absorb to create a cation by releasing an electron. The more electrons the atom loses, the more energy will be required for the discard, which means that the closer an electron is the more difficult it will be to extract. Ionization energy can be measured in kJ/mol, which is how much energy is necessary for every atom to oust a single electron each. Since the ionization energy is majorly impacted by the distance the electrons are away from the nucleus, the atomic radius, the energy will decrease from right to left in the periods. The ionization will have the opposite trend as the atomic radius because the atomic radius increases from right to left.
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