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Section 11.3 Atomic Orbitals • Georgia Performance Standards: – SC3 (b): Use the orbital configuration of neutral atoms to explain its effect on the atom’s chemical properties. • Essential Questions: – How do you describe the behavior of an electron? – How does the orbital configuration of atoms explain their chemical properties? Section 11.3 Atomic Orbitals Objectives 1. Compare and contrast the Bohr model and the quantum model of the atom 2. Discuss Louis de Broglie’s role in the development of the quantum model of the atom 3. Explain how the Heisenberg uncertainty principle and the Schrodinger wave equation led to the idea of atomic orbitals. 4. To learn about the shapes of the s, p, d and f orbitals 5. To review the energy levels and orbitals of the wave mechanical model of the atom 6. To learn about electron spin Section 11.3 Atomic Orbitals A. The Hydrogen Orbitals • Orbitals do not have sharp boundaries. Section 11.3 Atomic Orbitals A. The Hydrogen Orbitals Hydrogen Energy Levels • Hydrogen has discrete energy levels. – Called principal energy levels – Labeled with whole numbers Section 11.3 Atomic Orbitals A. The Hydrogen Orbitals Hydrogen Energy Levels • Each principal energy level is divided into sublevels. – Labeled with numbers and letters – Indicate the shape of the orbital Section 11.3 Atomic Orbitals A. The Hydrogen Orbitals Hydrogen Energy Levels • The s and p types of sublevel Section 11.3 Atomic Orbitals A. The Hydrogen Orbitals Hydrogen Orbitals • Why does an H atom have so many orbitals and only 1 electron? – An orbital is a potential space for an electron. – Atoms can have many potential orbitals. Section 11.3 Atomic Orbitals The Quantum “Wave” Mechanical Model of the Atom What’s wrong with the Bohr model? Section 11.3 Atomic Orbitals B. The Wave Mechanical Model: Further Development Atoms Beyond Hydrogen • The Bohr model was discarded because it does not apply to all atoms. • Atoms beyond hydrogen have an equal number of protons and electrons. – Need one more property to determine how the electrons are arranged – Spin – electron spins like a top Section 11.3 Atomic Orbitals Heisenberg, de Broglie, Schrodinger • Developed a model of the atom based on wave mechanics (quantum mechanics) – The electron bound to the nucleus seemed similar to a standing wave • De Broglie – originated the idea that the electron also shows wave properties (in addition to particulate properties) • Schrodinger – put emphasis on the wave properties of the electron Section 11.3 Atomic Orbitals Standing Waves & Musical Instruments • A string attached to a violin or guitar vibrates to produce a musical tone • The waves are “standing” because they are stationary, they don’t travel the length of the string Section 11.3 Atomic Orbitals •The dots indicate the nodes, or points of zero lateral (sideway) displacement, for a given wave. •There are limitations on the allowed wavelengths of the standing wave. •Each end of the string is fixed, so there is always anode at each end • There must be a whole number of half wavelengths in any of the allowed motions of the string Section 11.3 Atomic Orbitals Heisenberg’s Uncertainty Principle • There is a limitation to just how precisely we can know both the position and momentum of a particle at a given time. • The more accurately we know a particle’s position, the less accurately we can know its momentum, and vice versa. – Limitation is too small for large particles – Limitation is significant for small particles Section 11.3 Atomic Orbitals Heisenberg’s Uncertainty Principle • Applied to the electron: – We cannot know the exact motion of the electron as it moves around the nucleus – Therefore, it is not appropriate to assume that the electron is moving around the nucleus in a well-defined orbit, as in the Bohr model. Section 11.3 Atomic Orbitals Quantum Numbers •Principle Quantum Number (n): •Angular Momentum Quantum number (l) •Magnetic Quantum Number (ml) •Spin Quantum Number (ms) •(Pauli Exclusion Principle) Section 11.3 Atomic Orbitals Quantum Numbers for the First Four Levels of Orbitals in the Hydrogen Atom Section 11.3 Atomic Orbitals Orbital Shapes and Energies Section 11.3 Atomic Orbitals 1s Orbital Section 11.3 Atomic Orbitals 2px Orbital Section 11.3 Atomic Orbitals 2py Orbital Section 11.3 Atomic Orbitals 2pz Orbital Section 11.3 The Boundary Surface Representations of All Three 2p Orbitals Atomic Orbitals Section 11.3 Atomic Orbitals Orbital 3d x2 y 2 Section 11.3 Atomic Orbitals 3dxy Orbital Section 11.3 Atomic Orbitals 3dxz Orbital Section 11.3 Atomic Orbitals 3dyz Orbital Section 11.3 Atomic Orbitals Orbital 3d z 2 Section 11.3 The Atomic Boundary Orbitals Surfaces of All of the 3d Orbitals Section 11.3 Representation of the 4f Orbitals in Terms of Their Atomic Orbitals Boundary Surfaces Section 11.3 Atomic Orbitals B. The Wave Mechanical Model: Further Development Atoms Beyond Hydrogen • Pauli Exclusion Principle - No 2electrons in the same atom can have the same set of 4 quantum numbers. An atomic orbital can hold a maximum of 2 electrons and those 2 electrons must have opposite spins • Hund’s Rule – every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin. • Aufbau’s Principal – An electron occupies the lowest energy orbital that can receive it, then it will go back and pair up.