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Explain redox reactions on the basic of electron transfer. Give suitable examples. |
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Answer» Solution :`2Na_((s))+Cl_(2(g))to2NaCl_((s))` `4Na_((s))+O_(2)to2Na_(2)O` `2Na+StoNa_(2)S` Given reactions are redox reactions all the reactions Na is converting into`NaCl,Na_(2)OandNa_(2)S`. At this TIME Na is attached to elements having more electronegative so Na form OXIDATION and chlorine, OXYGEN and sulphur attached to electropositive element so it form reduction. NaCl, `Na_(2)OandNa_(2)S` ionic compounds so it will the INDICATED as `Na^(+)Cl^(-),(Na^(+))_(2)O^(-2)and(Na^(+))_(2)S^(-2)`. Above three reaction can be indicated as reduction by `2e^(-)`.   This reactions are redox reaction so electron transfer are element to another element. During oxidation reaction `e^(-)` LOSES then positive ion is obtained and during reduction `e^(-)` receive so if reactant is positive then its positive. Charge decreases if reactant is neutral then it will give negative ion. The reagent loses `e^(-)` is known as reducing agent, the reagent accept `e^(-)` is known as oxidising agent. |
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