{"id":7945,"date":"2018-06-03T12:01:03","date_gmt":"2018-06-03T12:01:03","guid":{"rendered":"https:\/\/www.experimentoscientificos.es\/?page_id=7945"},"modified":"2018-11-16T14:27:28","modified_gmt":"2018-11-16T14:27:28","slug":"enlaces-quimicos","status":"publish","type":"page","link":"https:\/\/www.experimentoscientificos.es\/en\/enlaces-quimicos\/","title":{"rendered":"Chemical bonds"},"content":{"rendered":"

The\u00a0chemical bonds <\/b>are the processes responsible for the interactions between the atoms<\/a> and molecules.\u00a0<\/b>\u00a0The interactions between atoms and molecules is such a complex process that quantum physics comes into play. In simple terms, a\u00a0chemical bonding<\/b>\u00a0is the force that exists between atoms once a stable system has been formed. We can classify chemical bonds into 3: ionic bond<\/a>, covalent bond<\/a> y metallic bond<\/a>.<\/p>\n

All the bodies we know, from molecules, crystals, metals and gases are linked by chemical bonds. It is the chemical bonds that will determine the both physical and chemical properties of the objects<\/strong>. The type of bonding between atoms and molecules will depend mainly on the atomic structure, number of electrons and electronegativity<\/a> of the atom.<\/p>\n

WHY CHEMICAL BONDS OCCUR<\/h2>\n

Single atoms are usually not chemically stable elements (with the exception of the noble gases). This is due to the number of electrons in the atoms. The electrons in the atom are distributed in different orbitals (energy levels) around the atom, from the first level to the last one they can complete. Each level must have a certain number of electrons to be considered stable. If the last level is not completed, the atom tends to lose electrons or pick up electrons to create a stable structure.<\/p>\n

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The number of electrons an atom must lose or gain to complete the last level is known as the oxidation number<\/a>\u00a0or valence electrons. The oxidation number corresponds to the number with which the atom is charged. It will be positively charged if it loses electrons and negatively charged if it has to gain electrons to complete the last shell.<\/p>\n

Although the bonds are complex and must be explained by quantum theory, through some simplification rules we will look at 3 types of bonds: ionic bond<\/strong>, covalent bond<\/strong> y metallic bond<\/strong>.<\/p>\n

CLASSIFICATION OF CHEMICAL BONDS<\/h2>\n

ION BONDING<\/a><\/h3>\n

The basis of a\u00a0ionic bond<\/a>\u00a0is a bond where an atom with extra electrons to complete the last shell is joined with an atom that lacks electrons, so that both atoms are complete.<\/p>\n

An ionic bond can also occur between a negatively charged molecule and a metal (positively charged). This is the case with sulphates, which are formed by ionic sulphate bonds of different metals, hence their solubility.<\/p>\n

PROPERTIES OF IONIC BONDS<\/strong><\/p>\n

The elements with ionic bonds have common properties, which are detailed below:<\/p>\n