please help with answer and explain homo and lumo in terms of acid-bas.docx

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please help with answer and explain homo and lumo in terms of acid/base. thanks! 10) A molecule with a high HOMO and a low LUMO can act as: (A) a Lewis base only (B) a Lewis acid only (C) a Lewis base and Lewis acid (D) neither a Lewis base, nor a Lewis acid (E) an inert molecule 11) A molecule with a low HOMO and a high LUMO can act as: (A) a Lewis base only (B) a Lewis acid only (C) a Lewis base and Lewis acid (D) an inert molecule (E) none of the above Solution 10) a molecule with a high HOMO and low LUMO can act as a Lewis Base or Lewis Acid. 11) a molecule with low HOMO and high LUMO can act as an inert molecule. According to lewis acid base concept, the Homo and Lumo are the pair of orbitals that lie closest. When having a high HOMO, this is lewis base. When having a low LUMO , this is lewis acid. When the HOMO and LUMO are far they have a larger energy gap, and the HOMO-LUMO interactions do not happen. And when the HOMO and LUMO of a molecule are closer they interact with each other. .

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Amphiprotic. The preferred term is amphoteric. A compound that is amphoteric can behave as either an acid or a base. These are most commonly explained when using the Bronsted-Lowry theory of acids and bases. Sorry. NONE of these are amphoteric (or amphiprotic). In order to behave as a Bronsted-Lowry acid it must donate a proton. That narrows it down to HCl and HSO4-. In order to behave as a base it must accept a proton. A, D and E can all accept protons. HCl is a strong acid and dissociates to form H+ and Cl-. There is no tendency to gain a proton. HSO4- is a weak acid and can donate a proton, but it won\'t accept a proton to make H2SO4 because H2SO4 is a strong acid and completely dissociates. Even if one of the choices had been HSO3- we would still have a problem. It would be tempting to say that HSO3- could gain a proton to make the weak acid H2SO3. The problem is that H2SO3 does not exist in aqueous solution. It is a fictitious acid, much like H2CO3 which also cannot exist in aqueous solution. The bottom line is that NONE of these are amphoteric. ========= Follow up ========== See! HPV got suckered. Sorry, you can\'t possibly form H2SO4 and OH-. H2SO4 is a strong acid and completely dissociates to form H+ and HSO4-. The H+ will combine with OH- to make water, and you\'re right back where you started. No. HSO4- is NOT amphoteric in aqueous solution. ======= More follow up ========== \"Would it matter about the physical state?\" No. For the substance to gain a proton, it will be in aqueous solution. As soon as HCl interacts with water it will dissociate to form H+ and Cl-. =============================== You may see that HSO4- is listed as an amphoteric substance, but only because whoever wrote that didn\'t think it through. Solution Amphiprotic. The preferred term is amphoteric. A compound that is amphoteric can behave as either an acid or a base. These are most commonly explained when using the Bronsted-Lowry theory of acids and bases. Sorry. NONE of these are amphoteric (or amphiprotic). In order to behave as a Bronsted-Lowry acid it must donate a proton. That narrows it down to HCl and HSO4-. In order to behave as a base it must accept a proton. A, D and E can all accept protons. HCl is a strong acid and dissociates to form H+ and Cl-. There is no tendency to gain a proton. HSO4- is a weak acid and can donate a proton, but it won\'t accept a proton to make H2SO4 because H2SO4 is a strong acid and completely dissociates. Even if one of the choices had been HSO3- we would still have a problem. It would be tempting to say that HSO3- could gain a proton to make the weak acid H2SO3. The problem is that H2SO3 does not exist in aqueous solution. It is a fictitious acid, much like H2CO3 which also cannot exist in aqueous solution. The bottom line is that NONE of these are amphoteric. ========= Follow up ========== See! HPV got suckered. Sorry, you can\'t possibly form H2SO4 and OH-. H2SO4 is a strong acid and completely dissociates to form H+ a.

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