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Bohr ing Model of the Atom

Bohr ing Model of the Atom. Check HWK Theory of Atomic Spectra Practice Problem Work on next assignment. An explanation of Atomic Spectra. Consider where the electron starts When we write electron configurations we are writing the lowest energy.

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Bohr ing Model of the Atom

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  1. Bohring Model of the Atom • Check HWK • Theory of Atomic Spectra • Practice Problem • Work on next assignment

  2. An explanation of Atomic Spectra • Consider where the electron starts • When we write electron configurations we are writing the lowest energy. • The energy level and electron starts from is called its ground state.

  3. Where the electron starts • When we write electron configurations we are writing the lowest energy. • The energy level and electron starts from is called its ground state.

  4. Changing the energy • Let’s look at a hydrogen atom

  5. Changing the energy • Heat or electricity or light can move the electron up energy levels

  6. Changing the energy • As the electron falls back to ground state it gives the energy back as light

  7. Changing the energy • May fall down in steps • Each with a different energy

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  9. Ultraviolet Visible Infrared • Further they fall, more energy, higher frequency. • This is simplified • the orbitals also have different energies inside energy levels • All the electrons can move around.

  10. Ultraviolet Visible Infrared • Bohr Model of Hydrogen Atom (1914) • Explain line spectra – e- orbiting nucleus • En = (-Rh) (1/n2) Rh=Rydberg constant = 2.18 x10-18 J n = Principle Quantum Number

  11. E= (-Rh) (1/ 2) = 0 • E = Ef – Ei = h •  = E h  = (Rh)( 1/ni2 - 1/nf2 ) h ni>nf  (-) emitted nf>ni  (+) absorbed

  12. Rh = 2.18 x10-18 J  = (Rh)( 1/ni2 - 1/nf2 ) h Sample Problem h=6.626 x10-34J•s • Calculate the wavelength of light involved in the transition from n=4 to n=2. • Is this light absorbed or transmitted?  = -6.17 x1014 1/s  = 486 nm (violet) The light is given off or emitted.

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