{"id":8362,"date":"2018-11-15T16:20:40","date_gmt":"2018-11-15T16:20:40","guid":{"rendered":"https:\/\/www.experimentoscientificos.es\/?page_id=8362"},"modified":"2018-11-16T17:12:25","modified_gmt":"2018-11-16T17:12:25","slug":"regla-del-octeto","status":"publish","type":"page","link":"https:\/\/www.experimentoscientificos.es\/en\/regla-del-octeto\/","title":{"rendered":"Octet Rule"},"content":{"rendered":"

The\u00a0octet rule<\/strong>\u00a0o\u00a0octet rule<\/strong>\u00a0is a rule that is used in the context of the\u00a0chemistry<\/strong>. The octet rule defines the property of atoms to complete their last energy level with\u00a0eight electrons<\/strong>\u00a0in order to achieve\u00a0stability<\/strong>. Whether it is a ionic bond<\/a>, covalent<\/a> o metal<\/a>In the valence shell, the atoms will tend to give up or share in order to complete 8 electrons in the valence shell.<\/p>\n

\"regla<\/p>\n

The creator of this rule is the scientist Gilbert Newton Lewis and was established in 1917.<\/strong><\/p>\n

The basis of this rule is the noble gases, which have 8 electrons in their last shell and are the least reactive elements in all the periodic table<\/a>. Lewis noticed that by joining different ions together, they want to achieve the configuration of a noble gas, getting 8 electrons in their last shell.<\/p>\n

This rule applies to the creation of chemical bonds between atoms. The behaviour and properties of molecules will depend on the type of bond, the number of bonds per atom and the intermolecular forces.<\/p>\n

There are different types of\u00a0chemical bonding<\/a>depending on the electronegativity of the elements. In any of the bonds, the atoms tend to roadearse 8 electrons in the outermost shell.<\/p>\n