What do you mean by de-electronation? What is oxidation number? Explain
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When a metal rod is emerged into its own ion solution, a potential difference is developed between metal rod its solution. This occurs due to processes known as electronation and de-electronation
De-electronation: The metal atoms have a tendency to pass into the solution as cations and leave behind electrons on the metal rod. This produces an electrode potential and the electrode undergoing de-electronation is anode (oxidation/ electrode).
Electronation: Cations of the solution accept electrons from the metal to form neutral metal atoms. This produces an electrode potential, and the electrode undergoing electronation(i.e addition of electrons) is the cathode (reduction/ electrode).Oxidation number is a measure of the charge of an atom if the electrons shared in bonding were held only by the more electronegative atom. For example, in water (H2O), oxygen is more electronegative than hydrogen. This would give oxygen all the electrons and an oxidation number of -2 and each hydrogen an oxidation number of +1. Keeping track of the oxidation states in a reaction is important to know if an oxidation or reduction (change in oxidation state) has occurred. For a neutral element (He), the oxidation number is 0; for a charged ion (Fe3+), the oxidation number is equal to the charge (+3). For a polyatomic ion, the sum of the oxidation numbers of the atoms is equal to the net charge.
De-electronation: The metal atoms have a tendency to pass into the solution as cations and leave behind electrons on the metal rod. This produces an electrode potential and the electrode undergoing de-electronation is anode (oxidation/ electrode).
Electronation: Cations of the solution accept electrons from the metal to form neutral metal atoms. This produces an electrode potential, and the electrode undergoing electronation(i.e addition of electrons) is the cathode (reduction/ electrode).Oxidation number is a measure of the charge of an atom if the electrons shared in bonding were held only by the more electronegative atom. For example, in water (H2O), oxygen is more electronegative than hydrogen. This would give oxygen all the electrons and an oxidation number of -2 and each hydrogen an oxidation number of +1. Keeping track of the oxidation states in a reaction is important to know if an oxidation or reduction (change in oxidation state) has occurred. For a neutral element (He), the oxidation number is 0; for a charged ion (Fe3+), the oxidation number is equal to the charge (+3). For a polyatomic ion, the sum of the oxidation numbers of the atoms is equal to the net charge.
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when heat is released
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