Quantum Atom

Problem Bohr model of the atom only successfully predicted the behavior of hydrogen Good start, but needed refinement

Heisenberg Uncertainty Principle It is not possible to know both the position and momentum (mv) of an electron Cannot assume that the electron is moving around the nucleus in a well- defined orbit as in the Bohr model

Louis de Broglie Suggested matter that is assumed to be of a particle nature, does have wavelike properties Developed an equation for actually calculating this wavelength of matter For very small particles, wavelength is significant

Wave Function Erwin Schrodinger developed a series of equations that describe the areas of probability of finding an electron There are different values of these wave functions that occur at different energy levels Wave function are called Orbitals

Quantum Mechanics Describes mathematically the properties of an electron Shows regions of probability of finding an electron

Quantum Numbers Principal Quantum Number (n) – same as the Bohr energy level Also called shells Range from n=1 to n=7

Subshell or Sublevel Angular Momentum Number Come in four types s subshell (spherical) p subshell (dumbbell) d subshell (four lobes) f subshell

Orbital Magnetic Quantum Number These are the orbitals (hold 2 e - each) Each sublevel may have more that one orbital with a different orientation in space s ( 1 orbital) p ( 3 orbitals) d (5 orbitals) f (7 orbitals)

Main LevelSublevelsNumber of orbitals Electrons in sublevels Total Electrons in Main Level 1s122 2spsp spdspd spdfspdf

Degenerate Orbitals Orbitals that have the same energies

Electron Spin Number Electron behaves as if it is spinning on its axis Fourth Quantum number is the spin number

Spinning electrons produce magnetic fields

Pauli Exclusion Principle No two electrons can have the same set of four quantum numbers If an orbital has two electrons in it, they must have different spins Electrons in the same orbital with different spins are called paired electrons