10 posts • Page 1 of 1
When do we know to use the expanded octet rule. For example in SO4 (2-) both the four single bonded and 2 single 2 double bonded lewis structures are correct just one is more stable. Is there a way of knowing when we should use an expanded octet?
You would use it when there is a more stable Lewis structure available, as in SO4 (2-). More stable = less energy, which is what we want. While the four single bonded Lewis structure is possible, it's only possible in that single form. However, the 2 single 2 double bonded Lewis structure has resonance. Lewis structures that have resonance are also more stable, which is another clue that the expanded octet (2 single bond, 2 double bond) is the better choice.
Why can P, S, and Cl accommodate more than 8 valence electrons? I know the course reader says they have d-orbitals in the valence shell that accommodate additional electrons, but I'm not sure I understand what that means because their electrons do not occupy a d-orbital. Can somebody please clarify?
Is there a limit to how many electrons an atom can accommodate? Say, the sulfur atom has an electron configuration of and 2 empty spaces in its d-orbital. Does this mean sulfur can thus accommodate 2 more electrons/one extra loan pair? Can it accommodate more? If so, why is that?
104422816 wrote:Also, is it only Hydrogen and Helium that can have less than an octet?
I don't know how to answer Joanna's question, but I believe lithium, beryllium, and boron also have less than an octet even when bonded with other atoms.
Who is online
Users browsing this forum: No registered users and 1 guest