CHEM 110 Lecture Notes - Lecture 5: Azimuthal Quantum Number, Principal Quantum Number, Magnetic Quantum Number
Document Summary
Lecture 5: quantum numbers n(principle quantum number)- provides information about bothe size and energy of orbital the shell! Positive integer values l(angular momentum quantum number)- de nes the shape of the orbital. Ml(magnetic quantum number)- describes the spatial orientation of the orbital. Integer ranging from -l to l, including 0. Nodes- regions where there is zero probability (electron density=0) of nding an electron. number of nodes=n-1. 1s orbital has 0 node, 2s orbital has 1 node, and 3s orbital has 2 nodes. An n increases, size(and energy) of orbitals increases. P orbitals have zero electron density at (or near) the nucleus (1 node at nucleus) 2p orbital has 1 node, and 3p orbital has 2 nodes. H atom- orbital energies follow the same as bohr model orbits. Orbital energy is the energy released when an electron goes into an empty orbital (negative) Shielding- inner core electrons shield the outer valence electrons from interacting with the nucleus.
