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Wave-Particle Duality: The Beginnings of Quantum Mechanics.

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Presentation on theme: "Wave-Particle Duality: The Beginnings of Quantum Mechanics."— Presentation transcript:

1 Wave-Particle Duality: The Beginnings of Quantum Mechanics

2 Explain the basics of wave-particle duality. Define the relationship between quantum, photon and electron. Describe how a produced line spectra relates to the Bohr diagram for a specific element. Additional KEY Terms Absorption SpectraThreshold energy

3 PHOTOELECTRIC EFFECT Under certain conditions, shining light on a metal surface will eject electrons. Electrons given enough energy (threshold energy) can escape the attraction of the nucleus. *Light is acting like a “particle” in this experiment – collision.

4 Only high frequency light (> 1.14 x Hz) will eject electrons - acting as particle. Can only explain it if you think of it using photons in a collision.

5 Only more intense light (higher amplitude) will eject more electrons - acting as wave. Can only explain it if you think of it as changing the size of the wave.

6 Einstein (1905) - electromagnetic radiation is a stream of tiny bundles of energy called photons. Photons have no mass but carry a quantum of energy. One photon can remove one electron. Light is an electromagnetic wave, yet it contains particle-like photons of energy.

7 Compton (1922) – first experiment to show particle and wave properties of EMR simultaneously. Incoming x-rays lost energy and scattered in a way that can be explained with physics of collisions.

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9 Quantum Mechanical Model of the Atom

10 Bohr (1922) – restricting electrons to fixed orbits (n) with different quantized energy levels. Created a math equation for energy of each orbit. Equations correctly predicted the line colours of hydrogen spectra. Energy n = -(2.18 x J)/n 2

11 1.Electron absorbs radiation and jumps from ground state (its resting state) to a higher unstable energy level (excited state). 2.Electron soon loses energy and drops back down to a lower energy level – emitting the absorbed EMR. Free Atom e−e− EMR e−e− Ground State e−e− Excited State Ionization Absorption EMR nucleus > Threshold Energy < Threshold Energy

12 ΔE = E higher-energy orbit - E lower-energy orbit = E photon emitted = hf

13 Levels are discrete like quanta – no in between. Each jump/drop is associated with a specific frequency photon - same transition, same photon.

14 The size of nucleus will affect electron position around the atom – and the size of “jump” energy. Cl: 17 e - Na: 11 p + 11 e - 17 p +

15 *Each element has a unique line spectrum as each element has a unique atomic configuration.

16 Absorption spectrum – portion of visible light absorbed by an element – heating up. Emission spectrum – portion of visible light emitted by that element – cooling down.

17 CAN YOU / HAVE YOU? Explain the basics of wave-particle duality. Define the relationship between quantum, photon and electron. Describe how a produced line spectra relates to the Bohr diagram for a specific element. Additional KEY Terms Absorption SpectraThreshold energy


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