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VALENCIA
is the combining capacity of an atom. To determine the valence of an atom, is referenced to the hydrogen atom, because when you are forming a binary compound (compound composed of two different elements) is never in combination with more than one atom of another element, which is why which gives a combined capacity of 1, ie its valence is 1.
Example:
hydrogen chloride or hydrochloric acid, HCl hydrogen atom combines with one of chlorine, so the valence of chlorine is also 1.
Cl-H1 CL17
2P6 3s2 3p2 1s2 3p2 2s2 3p1 + 1s2 1S1 3p2 3s2 3p2 2s2 3p2 2P6
H +
Therefore, the valence of hydrogen is +1 and that of chlorine is -1. D
The water molecule (H2O), oxygen combines with two hydrogen atoms, so their valence is -2. O8 O-2

3p2 2s2 3p1 1s2 3p1 1S1 + 1S1 + 3p2 1s2 3p2 2s2 3p2
H + H +
determines the valence following compounds: LiCl
,
CaCl2, AlCl3

metals (group IA) and alkaline earth (Group IIA) have a fixed valence +1, +2 respectively. There are other elements that have more than one valence or valence variable
Example:
carbon monoxide (CO) Carbon is the valence of +2 because it is combined with an oxygen atom, whose valence is -2, in the case of carbon dioxide (CO2) carbon has a valence of +4, then combined with two oxygen atoms in these cases the carbon valence of +2 and +4.
determines the valence of the following compounds:

N2O NO NO2


N2 O3 O5 N2
The nitrogen valences are 1, 2, 4, 3, 5 respectively.
the oxidation number is another concept used to describe the combining capacity of an atom. This is an integer that can be positive or negative and describes the combining capacity of an atom, as well as indicate the behavior of electrons in n compound.
In the compound lithium chloride (LiCl), lithium, losing an electron, remains ion (Li +) with an electrical charge of +1 or ion, which is equal to the number of oxidation, while chlorine, winning that electron, it becomes ion (CL-) with electric charge or oxidation number -1. As you can see by combining these two atoms, one loses an electron and the other wins, this indicates the behavior of the electron, ie, the oxidation number. LINKS BETWEEN ATOMS

Relationship between ionization energy and atomic number.
In the forming and breaking of chemical bonds, ionization energy and electrons play an important role. As we know, potential or ionization energy is the energy required to extract an electron from the atom, that energy must be able to break the force of attraction between electrons and protons in the nucleus. This force is inversely proportional to the distance between them, ie between an electron further away from the nucleus, the attraction will be less.
When an electron absorbs energy from outside the atom moves to a higher energy level (excited state) of which was (baseline), therefore, the distance from the nucleus increases and decreases the attractive force requiring less energy to remove it.
The ionization energy decreases in the periodic table upside down in a group and increases from left to right in a period analyzing the last paragraph and noting the position of the elements in the periodic table for those who are in a period closer to the noble gases, it takes more energy to remove an electron than those found at the beginning of the period, ie, the former tend to gain electrons and second to lose. Therefore
before starting the study of chemical bonds, we will explore ideas about the chemical bonds that provided the scientific Kossel and Lewis.