Abstract
When writing equations of chemical dissociation, students and scholars are taught two fundamental rules to balance the equation. On both sides of the equation, the types of elements and their quantity are conserved, as well as the global electrical charge. This paper introduces additional methods during dissociation of gaseous compounds, to precisely describe how electrical charges locally move and how bonding structures are modified. Specific rules revolving around electrons pairs displacements are developed and applied to about 150 dissociations of small gaseous molecules using atoms from the three first rows of the periodic table. Results obtained tend to demonstrate the relevance of these tools for chemists.
Highlights
In gaseous phase, chemical dissociations start with compounds in the form of molecules [1]
This paper introduces additional methods during dissociation of gaseous compounds, to precisely describe how electrical charges locally move and how bonding structures are modified
Specific rules revolving around electrons pairs displacements are developed and applied to about 150 dissociations of small gaseous molecules using atoms from the three first rows of the periodic table
Summary
Chemical dissociations start with compounds in the form of molecules [1]. Atoms and charges positions are frequently displaced Such dissociations are usually described through an equation, with compounds on the left and products on the right [2]. Auvert and after the dissociation, no information is given when very simple chemical steps occur These steps may give local charges, electrons’ positions and bonds’ repartitions in every compound before, during and after each chemical step. This paper will start by briefly recalling the even-odd rule, the covalent rule and the specific periodic table for gaseous molecules. It will describe the three types of electron displacements that can occur in a chemical reaction, resulting in bond modifications and charges’ re-localizations.
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