Hot and spicy foods contain molecules that stimulate pain-detecting nerve endings. Two such molecules are piperine and capsaicin: Piperine is the active compound in white and black pepper, and capsaicin is the active compound in chili peppers. The ring structures in piperine and capsaicin are shorthand notation. Each point where lines meet represents a carbon atom. a. Complete the Lewis structure for piperine and capsaicin showing all lone pairs of electrons. b. How many carbon atoms are sp, sp2, and sp3 hybridized in each molecule? c. Which hybrid orbitals are used by the nitrogen atoms in each molecule? d. Give approximate values for the bond angles marked a through l in the above structures.
10/16 These will be the only set of notes this week! Our Midterm is on Wednesday! Since this class was just a review of the practice exam questions, I’ve taken some notes in relation to the exam that may come in handy! Double bonds: 4 shared electrons Single bonds: 2 shared electrons Triples bonds: 6 shared electrons Know the group number of period tables! They will not be included in the periodic table provided to us. Familiarize yourself with isoelectronic ions on the period table An electron added to an element will make negative ions, the element that loses that electron will be a positive ion Isoelectronic ions will be close to each other on the period table Covalent bonds will be elements on the right side of the table (except