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is defined as:
• The type of bond that is formed by the complete transfer of electrons.
• It is the electrostatic force that binds two ions of opposite charge.
Example: LiCl (lithium chloride) in this case the lithium transfers an electron to the chlorine atom and thus both acquire the configuration of a noble gas. 17Cl 3Li

₊ 1s2 2s1 1s2 3p2 3s2 3p2 2s2 3p1 2P6

an electron transfer

Atoms alkali metal (flu IA) can only provide an electron, which have in its valence shell. The alkaline earth metals (group IIA) can transfer two or more electrons. There are atoms such as halogens (group VIIA), which need only one electron to complete its octet, and others such as oxygen, sulfur they need more than one electron.

By losing electrons, atoms become positive ions, also called cations, and winning become negative ions or anions. There is an electrostatic attraction between the two, being the force that holds together the ions in an ionic compound. Li

₊ Li ₊ ₊ Cl Cl ⁻ ⁻
Cation Anion Salt
(Lithium) (chloride) (sodium chloride)

Run the following examples:

₊ I K potassium iodide KI O

2RB ₊

rubidium oxide Ca S ₊ calcium sulfide

₊ Mg Br Magnesium bromide
Cl
Al ₊

aluminum chloride ionic compounds are formed by reacting atoms less electronegative elements, for example: group IA, IIA, IIIA group elements, with more electronegative elements, such as the VIA and group VIIA.
Note: Due to the difficulty of representing here the formation of ionic compounds with Lewis structures, this will be presented by the teacher in the classroom. However, after studying them is from their atoms and by structure Lewis, following the formation of ionic compounds.

1. MgO

2. Na2S

3.

Al2O3 4. KL

5. CaCl2

6. BaS