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- 1. Chapter 4.2<br />The Quantum Model of the Atom<br />
- 2. Objectives:<br />Discuss Louis de Broglie’s role in the development of the quantum model of the atom.<br />Compare and contrast the Bohr model and the quantum model of the atom.<br />Explain how the Heisenberg uncertainty principle and the Schrodinger wave equation led to the idea of atomic orbitals.<br />List the four quantum numbers, and describe their significance.<br />Relate the number of sublevels corresponding to each of an atom’s main energy levels, the number of orbitals per sublevel, and the number of orbitals per main energy level.<br />
- 3. Quantum Model of the Atom<br />DeBroglie<br /><ul><li> electrons confined to certain space around nucleus at specific frequencies – energy levels</li></li></ul><li>Heisenberg Uncertainty Principle<br /><ul><li> it is impossible to determine simultaneously both the position and velocity of an electron</li></ul>Schrodinger Wave Equation<br /><ul><li>Treated electrons as waves
- 4. With uncertainty principle – gave probability of finding an electron in certain regions</li></ul>These 3-D regions are called -Orbitals<br />
- 5. Quantum Theory<br />Describes mathematically the wave properties of electrons<br />Quantum Numbers – specify the properties of atomic orbitals and electrons in them<br />Principal quantum number (n) main energy level occupied by electrons<br />
- 6. 2. Angular Momentum (l) <br /><ul><li> indicates the shape of the orbital</li></ul>l = 0 1 2 3<br /> s p d f<br />
- 7. Magnetic (m) <br /><ul><li> orientation of orbital around nucleus</li></ul>m =-1,0,+1<br />m = 0<br />m =-2,-1,0,+1,+2<br />
- 8. 4. Spin Quantum Number ( +1/2, -1/2)<br />Indicates the two fundamental spin states of electron in an orbital<br />Single orbital can hold a maximum of 2 electrons<br />

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