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Section 11.2 The Hydrogen Atom 1.To understand how the emission spectrum of hydrogen demonstrates the quantized nature of energy 2.To learn about Bohr’s.

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Presentation on theme: "Section 11.2 The Hydrogen Atom 1.To understand how the emission spectrum of hydrogen demonstrates the quantized nature of energy 2.To learn about Bohr’s."— Presentation transcript:

1 Section 11.2 The Hydrogen Atom 1.To understand how the emission spectrum of hydrogen demonstrates the quantized nature of energy 2.To learn about Bohr’s model of the hydrogen atom 3.To understand how the electron’s position is represented in the wave mechanical model Objectives

2 Section 11.2 The Hydrogen Atom A. The Energy Levels of Hydrogen Only certain types of photons are produced when excited Hydrogen atoms release energy. Why?

3 Section 11.2 The Hydrogen Atom A. The Energy Levels of Hydrogen Atomic states –Excited state – atom with excess energy –Ground state – atom in the lowest possible state When an H atom absorbs energy from an outside source it enters an excited state.

4 Section 11.2 The Hydrogen Atom A. The Energy Levels of Hydrogen Energy level diagram Energy in the photon corresponds to the energy used by the atom to get to the excited state.

5 Section 11.2 The Hydrogen Atom A. The Energy Levels of Hydrogen Only certain types of photons are produced when H atoms release energy. Why?

6 Section 11.2 The Hydrogen Atom A. The Energy Levels of Hydrogen Quantized Energy Levels –Since only certain energy changes occur the H atom must contain discrete energy levels.

7 Section 11.2 The Hydrogen Atom B. The Niels Bohr Model of the Atom ( ) Bohr’s model of the atom –Quantized energy levels –Electron moves in a circular orbit –Electrons jump between levels by absorbing or emitting photons of a particular wavelength Able to mathematically explain the emission spectrum of Hydrogen (compare with Rutherford)

8 Section 11.2 The Hydrogen Atom “Curiouser and curiouser” said Alice

9 Section 11.2 The Hydrogen Atom B. The Bohr Model of the Atom Bohr’s model of the atom was not totally correct. –Had difficulties with spectra of larger atoms –Electrons do not move in a circular orbit and don’t seem to behave like discrete particles all the time Maybe small particles, such as electrons, can also behave like waves having a dual nature (just like photons)……?

10 Section 11.2 The Hydrogen Atom C. The Wave Mechanical Model of the Atom (de Broglie and Schroedinger – mid-1920’s) Orbitals –Nothing like orbits –Probability of finding the electron within a certain space


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