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Chemistry 1 Chapter 5 Part I Light and Quantized Energy

Chemistry 1 Chapter 5 Part I Light and Quantized Energy. Last Updated November 6, 2015. Priority Standards. Big Idea Quantum theory provides a foundation for the atomic model and the understanding of electron behavior and arrangement. Core Concepts

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Chemistry 1 Chapter 5 Part I Light and Quantized Energy

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  1. Chemistry 1Chapter 5 Part ILight and Quantized Energy Last Updated November 6, 2015

  2. Priority Standards

  3. Big Idea • Quantum theory provides a foundation for the atomic model and the understanding of electron behavior and arrangement. Core Concepts • Electrons are arranged in main energy levels with sublevels that specify particular shapes and geometry. • Evidence for the movement of electrons between different energy levels can be observed through absorption and emission spectra. Michigan HSCE for Chemistry

  4. To physicists, Rutherford’s model did not explain how an atoms e- are arranged in the space around the nucleus and also did not account for differences in chemical behavior. Development of Atomic Model continued from previous notes

  5. Early 1900s • Observation of light were made when elements were heated. • Analysis of the light revealed that an elements chemical behavior is related to the arrangement of e- in its atoms

  6. Form of energy that exhibits wavelike behavior as it travels through space • Includes visible light which is only a small portion of EMR • (Visible Spectrum – ROY G BIV) Electromagnetic Radiation

  7. Electromagnetic Spectrum

  8. Greek Letter λLambda • Shortest distance between equivalent points (Peak to Peak) • Units = m, cm, nm • nm=nanometers 1nm = 1 x 10-9m Wavelength

  9. ν is Greek for nu • # of waves that pass a given point per second= Hz or 1/sec • 652 Hz=652 waves/sec=652/sec=652s-1 Frequency (ν)

  10. Sketch and label the parts of a wave in your notes.

  11. Amplitude=wave’s height • Speed of light =3.00x 108 m/s in a vacuum • Symbol is c • Speed of light is a product of λ and ν • c = λν • All light travels at the same speed but with different wavelength and frequency

  12. Speed of light Frequency (1/s or Hz) Wavelength (m)

  13. Electromagnetic Spectrum= classifies light based on ν and λ • ROY G BIV • Quantum= the minimum amount of energy that can be lost or gained by an atom

  14. Max Planck studied light emitted from heated objects, • Proposed emitted light is quantized • Equantum= energy • h= Planck’s constant= 6.626 x 10-34 J.s • J= Joules = Kg .m2/s2

  15. ν= frequency • Equantum = hν • Planck’s Theory= for a given frequency matter can emit or absorb energy only in whole # multiples ( 1hν, 2hν, 3hν, 4hν)

  16. Hydrogen’s Atomic Emission Spectrum

  17. Photoelectric Effect = e- called photo electrons are emitted from metals surface when light of a certain frequency shines onsurface

  18. Einstein 1905- proposed EMR has both wavelike and particle like behaviors. • Light can be thought of as a stream of tiny particles called photons. • Photons have no mass but do have quantum of energy.

  19. Einstein developed

  20. Atomic Emission Spectra:a set of ν(frequencies) of light on the electromagnetic spectrum emitted by atoms of an element.

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