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# Conflicts with Rutherford Model * **Why doesn't the nucleus break when electrostatic forces of repulsion result?** * Ans: An orbiting electron is a charged accelerating particle, which then loses energy and falls into the nucleus. # Niels Bohr (1913) * Discovered the "Bohr's Model", also kn...

# Conflicts with Rutherford Model * **Why doesn't the nucleus break when electrostatic forces of repulsion result?** * Ans: An orbiting electron is a charged accelerating particle, which then loses energy and falls into the nucleus. # Niels Bohr (1913) * Discovered the "Bohr's Model", also known as the planetary atom. * **Planetary Model:** Electrons move in circular orbits within specific energy levels. * Can find an electron with high probability. * Discovered Bright line spectrum. * Tried explaining the presence of specific colors in Hydrogen's line spectrum. * Discovered Electromagnetic Spectrum. * A range of visible and invisible energy. * Only electrons on n=2 form visible light. # Bohr's Postulates * Electrons exist in circular orbits. * Electrons only exist in stationary states. * When in a stationary state, electrons do not radiate energy; they just remain in their energy level. * Each energy level for each element has its own amount of energy required. * Electrons jump between stationary states by absorbing a specific amount of energy. * Electrons move in energy levels. # Energy and Wavelength * **Lowest Energy:** Red, has longer wavelengths * **Highest Energy:** Violet, has shorter wavelengths. $E = hc/\lambda$ where E is energy h is Planck's constant c is speed of light $\lambda$ is wavelength # Problem with Bohr Model * Could only explain the spectra for single-electron systems (H, He+, Li2+, Be3+). * In multielectron systems, smaller spaces existed between colored lines, saying they had smaller energy differences within each energy level. * There are sublevels within each energy level. # Diagram Description A diagram of the Bohr model, showing electron orbits of different energies around a nucleus. A spectrum of visible light, with different colors corresponding to different wavelengths labeled, is shown alongside the diagram. Additional text and diagrams describe properties of light and energy levels, like the relationship between energy and wavelength. Another diagram shows a prism separating white light into its color components of a continuous spectrum, compared with a line spectrum for Hydrogen and other elements.