2 posts • Page 1 of 1
So when a chemical bond forms the resulting arrangement of the two nuclei and their electrons had a lower energy than the total energy of the separate atoms. I could totally mesmerize this fact, but I want to know why and what happens that makes this so
Well, reactivity is typically from atoms without a full valence shell. Therefore in the case of both covalent and ionic bonding, if an octet or another desired number of E is satisfied, the atom will be less likely to react in order to achieve this completeness. For ionic bonds, I know a large amount of energy is given off when the ionic solid is formed as opposed to when the separate ions exist. Anions give off E when they are formed and cations take up E when they are formed. More E is taken than given off. However, when the ions combine to form a crystalline for example, the amount of energy that is given off is much more than the E that was required/taken up/absorbed to make that cation. Therefore in the end, a lower E is achieved by the solid than the separate ions. Hope this helps.
Who is online
Users browsing this forum: No registered users and 2 guests