* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
Download Quantum Theory
X-ray fluorescence wikipedia , lookup
Chemical bond wikipedia , lookup
Copenhagen interpretation wikipedia , lookup
Interpretations of quantum mechanics wikipedia , lookup
Quantum key distribution wikipedia , lookup
Quantum teleportation wikipedia , lookup
Elementary particle wikipedia , lookup
Orchestrated objective reduction wikipedia , lookup
X-ray photoelectron spectroscopy wikipedia , lookup
Renormalization wikipedia , lookup
Tight binding wikipedia , lookup
Bell's theorem wikipedia , lookup
Quantum state wikipedia , lookup
Relativistic quantum mechanics wikipedia , lookup
Canonical quantization wikipedia , lookup
Bohr–Einstein debates wikipedia , lookup
Symmetry in quantum mechanics wikipedia , lookup
History of quantum field theory wikipedia , lookup
EPR paradox wikipedia , lookup
Particle in a box wikipedia , lookup
Hidden variable theory wikipedia , lookup
Quantum electrodynamics wikipedia , lookup
Hydrogen atom wikipedia , lookup
Electron scattering wikipedia , lookup
Double-slit experiment wikipedia , lookup
Atomic orbital wikipedia , lookup
Matter wave wikipedia , lookup
Atomic theory wikipedia , lookup
Electron configuration wikipedia , lookup
Theoretical and experimental justification for the Schrödinger equation wikipedia , lookup
Quantum Theory Schroedinger’s Cat Place a cat in a box Also place a radioactive isotope and a vial of poison The isotope decays once per hour If the particle triggers a Geiger counter, the cat dies If the Geiger counter is not triggered, the cat lives Seal the box and wait an hour What happened to the cat? Electromagnetic Spectrum The speed of light© is 3.00 x 108 m/s Photoelectric Effect The emission of electrons from a metal when light shines on the metal Light had to be a certain minimum frequency for electrons to be emitted Wave theory of light said that any frequency of light should have worked This led to the concept of light as a particle Light as a particle Max Planck (1900) Hot objects emit light and other forms of electromagnetic radiation, but not continuously, as expected Instead, it is emitted in small, specific amounts called quanta. E=hv H=6.626 x 10 -34 J*s This number is called Planck’s constant Dual Nature of Light Albert Einstein (1905) Light behaves as a wave when it travels through space Light behaves as a particle when interacting with matter Even though it isn’t quite right to do so, you can think of light as a stream of particles that travels as a wave A photon is a massless bundle of light E photon=hv Some metals hold electrons more tightly than others and require higher frequencies to move electrons Emission Spectra Ground State Lowest energy state of an electron Excited State Higher energy state Energy is absorbed to move from ground to excited states and is released as light(photons) when returning to the ground state Specific patterns of light are emitted for any given element Continuous spectrum-continuous range of em light(rainbow) (Bright) Line emission spectrumOnly certain wavelengths of light are seen The Bohr Model Niels Bohr (1913) Allowed for electrons to have orbits Electrons have fixed energies Lower energy-closer to nucleus Higher energy-farther from nucleus Electrons can gain energy to raise to the next energy level and release the same energy when falling to the ground state This model works well for hydrogen but not for other elements Electrons as Waves Louis de Broglie (1924) Suggested that electrons could be considered as waves confined to the space around a nucleus Diffraction- bending of light around edges Wave Interference- when waves overlap Quantum Theory Werner Heisenberg (1927) The Uncertainty Principle One cannot simultaneously know the position and velocity of an electron Quantum Theory Erwin Schroedinger (1926) Wave Equation- The quantization of an electron’s energies is an outcome Quantum Theorymathematically describes wave properties of electrons and other small particles Atomic Orbitals and Quantum Numbers Quantum Numbersproperties of atomic orbitals and properties of electrons in orbitals Like the address of an electron or a seat in a stadium or theater Principal Quantum Number (n) Main energy level(shell) 1,2,3 K,L,M This would be like the section on a ticket for a stadium seat Angular Momentum Quantum Number shape of an orbital 0,1,2,3 s,p,d,f Like the row in a stadium or theater Magnetic Quantum Number m Orientation of an orbital around the nucleus +1 to -1 Like finding your seat in a stadium or theater Spin Quantum Number Ms Fundamental spin state of an electron +1/2 or -1/2 A single orbital can hold up to a maximum of 2 electrons of opposite spin This would be which direction you are facing in a theater or stadium seat Some Quantum Theory Rules Pauli Exclusion Principle- No two electrons have the same set of four quantum numbers. Or An orbital within a sublevel can contain up to 2 electrons of opposite spin Hund’s Rule- Each orbital within a sublevel receives an electron of positive spin before any can receive an electron of negative spin