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The Quantum Model of the Atom 25 Lancer Boulevard Wanaque, NJ 07465 45 Lakeland Lane Lancerville, NJ 08732 18 Lancer Boulevard Wanaque, NJ 07465 Only works for Hydrogen Why couldn’t electrons jump to any level – not just specific energy levels? Why didn’t atom collapse? What about the chemical behavior of atoms? Postulated electrons also have a dual wave-particle nature Electrons act like waves confined around the nucleus (standing waves) and therefore could only have certain frequencies Video – Tacoma Narrows Bridge These correspond to the energy of Bohr’s orbits. Investigation showed that electrons can be diffracted and can interfere with each other These are wave properties Electrons have a dual wave-particle nature. Locate electrons using photons Photons change position and/or velocity of an electron Interference: Example waves in water https://www.youtube.com/watch?v=3LLOoW15Z nY It is impossible to know both the position and the velocity of an electron or any other particle. Developed very complicated equations Equations treated electrons as waves Solution of the equation allowed for only specific energies and frequencies of waves Their ideas led to a new theory of the atom Call Quantum Theory/Quantum Mechanics Describes mathematically the wave properties of electrons and other small particles Waves in macroscopic vs. microscopic particles Give us only an area of probability of finding an electron Use the concept of orbital (area where it is likely you will find the electron) rather than orbit (path of the electron) Orbital – three dimensional region around the nucleus that indicates the probable location of the electron Orbitals described by 4 Quantum Numbers which indicated the properties of the orbitals and the electrons in those orbitals. First three result from the solution of Schrödinger’s Wave Equations Fourth is the spin of the electron Quantum numbers are n, l, m, s Called the Principal Quantum Number Gives energy level and period As n increases electron energy increases As n increases the distance from the nucleus to the electron increases Always a positive integer (n = 1, 2, 3, 4, …) Number of orbitals in an energy level = n2 ◦ 1st Energy Level – 1 orbital ◦ 2nd Energy Level – 4 orbitals ◦ 3rd Energy Level – 9 orbitals Number of electrons in an energy level = 2n2 ◦ 1st Energy Level – 2 electrons ◦ 2nd Energy Level – 8 electrons ◦ 3rd Energy Level – 18 electrons Called the angular momentum Quantum Number Gives the shape of the orbital l = 0, 1, 2, …., (n-1) Shapes associated with letters Stand for names given to groups of lines in the spectra of alkali metals ◦ ◦ ◦ ◦ s – sharp (Spherical shape) p – principal (Dumb-bell shape) d – diffuse (More complex) f – fundamental After f – orbitals are alphabetical, i.e. g, h, i, etc. 1st Energy Level – 1 Orbital – s 2nd Energy Level – 2 Orbitals – s and p 3rd Energy Level – 3 Orbitals – s, p and d Etc. Shorthand ◦ ◦ ◦ ◦ ◦ 1s 2s, 2p 3s, 3p, 3d 4s, 4p, 4d, 4f Etc. Gives the Orientation of the Orbital in 3 dimensions s – spherical – only 1 orientation p – dumb bell – 3 orientations: px, py, pz d – double dumb bell – 5 orientations f – “CRAZY!!!” – 7 orientations m = -l, …..0…….+l So for p orbitals m = -1, 0, 1 Accounts for magnetic properties of the electron Magnetic properties are due to the spin of the charged electrons Magnet demo Each orbital can hold 2 electrons ( Remember # of electrons = 2n2) Values for s = + ½ and – ½ Demo – butterfly orbital The atom is like an onion – in layers Between each layer is an area where there are no electrons – nodes