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Section 11.3 Atomic Orbitals Objectives 1. To learn about the shapes of the s, p and d orbitals 2. To review the energy levels and orbitals of the wave mechanical model of the atom 3. To learn about electron spin Section 11.3 Atomic Orbitals A. The Hydrogen Orbitals • Orbitals do not have sharp boundaries. 90% boundary Section 11.3 Atomic Orbitals A. The Hydrogen Orbitals Hydrogen Energy Levels • Hydrogen has discrete energy levels. • Called principal energy levels (electron shells) • Labeled with whole numbers • Energy is related to 1/n2 • En = E1/n2 • Energy levels are closer together the further they are from the nucleus 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 Orbital Designations Section 11.3 Atomic Orbitals Orbitals Define the Periodic Table Section 11.3 Atomic Orbitals A. The Hydrogen Orbitals Hydrogen Energy Levels • The s and p types of sublevel Section 11.3 Atomic Orbitals Representation of s, p, d atomic orbitals 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. • s, p, d, f orbitals named for sharp, principal, diffuse and fundamental lines on spectra. Further orbitals designated alphabetically Section 11.3 Atomic Orbitals s p d f f f g g g d g Section 11.3 Atomic Orbitals B. The Wave Mechanical Model: Further Development Electron Spin • Close examination of spectra revealed doublets • Need one more property to determine how electrons are arranged • Spin – electron modeled as a spinning like a top • Spin is the basis of magnetism Section 11.3 Atomic Orbitals B. The Wave Mechanical Model: Further Development Pauli Exclusion Principle • Pauli Exclusion Principle (Wolfgang Pauli 1925) - an atomic orbital can hold a maximum of 2 electrons and those 2 electrons must have opposite spins • When an orbital contains two electrons (of opposite spin) it is said to be full What are the four descriptors that define an energy level / electron’s position in an atom?
