CHEM 150 1nd Edition Lecture 22Outline of Last Lecture • The H atom is one proton and one electron.• The energy of an orbital is determined solely by n.• All orbitals in a shell have the same energy.Outline of Current Lecture • The uncertainty principle (pp 328-329) quantifies our inability to know everythingabout something as small as an electron. The act of observing them changes them.• Our perception of an electron as a wave may be due to this limit.• The electron wave occupies all of space but the electron particle must be somewhere. • The square of the wave function in an area is the probability of finding the electron in that area. We often think of the area in space where the electron spends90% of its time as the ‘shape’ of the atomic orbital.• This is how we get the orbital “pictures” in section 7.7• Main group elements form monatomic ions that have a pseudo-noble gas configuration (sn2np2).Current LectureQ: What is the ground state electron configuration of the monatomic ions formed byOxgyen Calcium Chlorine -Transition metal ions do not generally achieve a psuedo-noble gas configuration -Upon ionization, the energy of the (n-1)d orbitals drops below the energy of the ns orbitals. As aresult, transition metals lose the electrons from the highest numbered s orbital first.Q: What is the electron configuration of the Fe2+ ion? A: Q: Draw the orbital box diagram for the Cr3+ ionA d10 configuration is very stable. Ions will rarely destroy this configurationZn2+Sn4+-These ions have a psuedo-noble gas configuration (d10 only beyond the noble gas)• If a atom, ion or molecule has unpaired electrons it is paramagnetic.• If all the electrons are paired, the substance is diamagneticQ: Draw orbital diagrams for the following. Are they paramagnetic or
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