Atomic Theory Lecture 3 PDF

PL1001 Pharmaceutical Chemistry ATOMIC THEORY Lecture 3 Dr Alberto Di Salvo  The fourth quantum number: Electron Spin ms = +1/2 (spin up) or -1/2 (spin down) Spin is a fundamental property of electrons, like its charge and mass....

PL1001 Pharmaceutical Chemistry ATOMIC THEORY Lecture 3 Dr Alberto Di Salvo  The fourth quantum number: Electron Spin ms = +1/2 (spin up) or -1/2 (spin down) Spin is a fundamental property of electrons, like its charge and mass. (spin up) (spin down) Sizes, Shapes, and orientations of orbitals n determines size l determines shape ml determines orientation size shape orientation The energy of an orbital of a hydrogen atom or any one electron atom only depends on the value of n shell = all orbitals with the same value of n subshell = all orbitals with the same value of n and l an orbital is fully defined by three quantum numbers, n, l, and ml Each shell of QN = n contains n subshells n = 1, one subshell n= 2, two subshells, etc Each subshell of QN = l, contains 2l + 1 orbitals l = 0, 2(0) + 1 = 1 l = 1, 2(1) + 1 = 3 Shapes of s, p and d orbitals E Shapes of f orbitals s orbitals Shape of s orbitals Nodes in s orbitals: 1s no nodes, 2s one node, 3s two nodes p orbitals Shape of p orbitals Nodes in 2p orbitals: angular node that passes through the nucleus Orbital is “dumb bell” shaped Important: the + and - that is shown for a p orbital refers to the mathematical sign of the wavefunction, not electric charge! d orbitals Shape of d orbitals Nodes in 3d orbitals: two nodes that passes through the nucleus Orbital is “four leaf clover” shaped d orbitals are important for metals f orbitals Shell Subshell Orbital n=4 l=3 f +3 +2 +1 0 -1 -2 -3 4f Shape of f orbitals One of 7 possible f orbitals. All have 3 nodes that pass through the nucleus Atomic orbitals and the periodic table