Rule 2 should allow us to assign oxidation numbers to atoms...

Name: rule 2 should allow us to assign oxidation numbers to atoms in most compounds the strategy is to first assign the oxidation number for the most electronegative element example what are the o 73232
Uploaded: 2023-11-23T18:10:17-08:00
Duration: 6 min 2 s
Channel: Adi S
Description: rule 2 should allow us to assign oxidation numbers to atoms in most compounds the strategy is to first assign the oxidation number for the most electronegative element example what are the o 73232

Rule 2 should allow us to assign oxidation numbers to atoms in most compounds. The strategy is to first assign the oxidation number for the most electronegative element. Example: What are the oxidation numbers of Cl in the following? MgCl2, ______ CCl4, _______ Cl2, _______ ClO2- ______

Each atom in a pure metallic element has an oxidation number of zero. The oxidation number for an atom in a monatomic ion is equal to the charge on the ion. Elements of Group IA form monatomic ions with a positive charge, so their oxidation number is +1. Magnesium forms Mg2+ ions, so its oxidation number is +2. Fluorine always has an oxidation number of -1. In compounds with all other elements, the oxidation number of oxygen is -2. Chlorine has an oxidation number of -1 in compounds, except when it forms a compound with a more electronegative element, such as oxygen or fluorine. In that case, the oxidation number of chlorine can be positive. Hydrogen usually has an oxidation number of +1, except in compounds called peroxides where it has an oxidation number of -1. The algebraic sum of the oxidation numbers of all atoms in a neutral compound must be zero. In a polyatomic ion, the sum of the oxidation numbers must be equal to the charge of the ion.

Adi S.