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Light and Atoms

5.1. Light and Atoms. 5.1. The Development of Atomic Models. The Development of Atomic Models What was inadequate about Rutherford’s atomic model?. 5.1. The Development of Atomic Models. Rutherford’s atomic model could not explain the chemical properties of elements.

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Light and Atoms

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  1. 5.1 Light and Atoms • .

  2. 5.1 The Development of Atomic Models • The Development of Atomic Models • What was inadequate about Rutherford’s atomic model?

  3. 5.1 The Development of Atomic Models • Rutherford’s atomic model could not explain the chemical properties of elements. • Rutherford’s atomic model could not explain why objects change color when heated.

  4. 5.1 The Development of Atomic Models • The timeline shows the development of atomic models from 1913 to 1932.

  5. Bohr’s model Bohr Model • Electrons orbit the nucleus in “shells” Electrons can be bumped up to a higher shell if hit by an electron or a photon of light.

  6. 5.3 Light • According to the wave model, light consists of electromagnetic waves. • Electromagnetic radiation includes radio waves, microwaves, infrared waves, visible light, ultraviolet waves, X-rays, and gamma rays. • All electromagnetic waves travel in a vacuum at a speed of 2.998  108 m/s.

  7. 5.3 Light • According to the wave model, light consists of electromagnetic waves. • Electromagnetic radiation includes radio waves, microwaves, infrared waves, visible light, ultraviolet waves, X-rays, and gamma rays. • All electromagnetic waves travel in a vacuum at a speed of 2.998  108 m/s.

  8. 5.3 Light • The electromagnetic spectrum consists of radiation over a broad band of wavelengths.

  9. 5.3 Atomic Spectra • Atomic Spectra • What causes atomic emission spectra?

  10. 5.3 Atomic Spectra • When atoms absorb energy, electrons move into higher energy levels. These electrons then lose energy by emitting light when they return to lower energy levels.

  11. 5.3 Atomic Spectra • A prism separates light into the colors it contains. When white light passes through a prism, it produces a rainbow of colors.

  12. 5.3 Atomic Spectra • When light from a helium lamp passes through a prism, discrete lines are produced.

  13. 5.1 The Bohr Model • The Bohr Model • What was the new proposal in the Bohr model of the atom?

  14. 5.1 The Bohr Model • Bohr proposed that an electron is found only in specific circular paths, or orbits, around the nucleus.

  15. 5.1 The Bohr Model • Each possible electron orbit in Bohr’s model has a fixed energy. • The fixed energies an electron can have are called energy levels. • A quantum of energy is the amount of energy required to move an electron from one energy level to another energy level.

  16. 5.1 The Bohr Model • Like the rungs of the strange ladder, the energy levels in an atom are not equally spaced. • The higher the energy level occupied by an electron, the less energy it takes to move from that energy level to the next higher energy level.

  17. 5.1 The Quantum Mechanical Model • Austrian physicist Erwin Schrödinger (1887–1961) used new theoretical calculations and results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom. • The modern description of the electrons in atoms, the quantum mechanical model, comes from the mathematical solutions to the Schrödinger equation.

  18. 5.1 The Quantum Mechanical Model • The propeller blade has the same probability of being anywhere in the blurry region, but you cannot tell its location at any instant. The electron cloud of an atom can be compared to a spinning airplane propeller.

  19. 5.1 The Quantum Mechanical Model • In the quantum mechanical model, the probability of finding an electron within a certain volume of space surrounding the nucleus can be represented as a fuzzy cloud. The cloud is more dense where the probability of finding the electron is high.

  20. 5.1 Atomic Orbitals • Atomic Orbitals • How do sublevels of principal energy levels differ?

  21. 5.1 Atomic Orbitals • An atomic orbital is often thought of as a region of space in which there is a high probability of finding an electron. • Each energy sublevel corresponds to an orbital of a different shape, which describes where the electron is likely to be found.

  22. 5.1 Atomic Orbitals • Different atomic orbitals are denoted by letters. The s orbitals are spherical, and p orbitals are dumbbell-shaped.

  23. 5.1 Atomic Orbitals • Four of the five d orbitals have the same shape but different orientations in space.

  24. 5.1 Atomic Orbitals • The numbers and kinds of atomic orbitals depend on the energy sublevel.

  25. 5.1 Atomic Orbitals • The number of electrons allowed in each of the first four energy levels are shown here.

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