To identify the shapes of the s, p , d, and f orbitals

1. Objectives • To identify the shapes of the s, p, d, and f orbitals • To describe the energy levels and orbitals of the wave mechanical model of the atom • To characterize electron spin

2. Wave Mechanical Model of the Atom • Describes the probability of finding an electron in certain locations around the nucleus • Energy of electrons is quantized • Electrons have wave-like character • Electrons move randomly throughout atomic orbitals • Heisenberg Uncertainty Principle applies – the exact location of an electron cannot be determined at any point in time

3. A. The Hydrogen Orbitals • Energy Levels • Electrons are associated with energy levels • Called principal energy levels • Labeled with a quantum # (n) • n = 1, 2, 3 … • Each energy level can have one or more sublevels

4. A. The Hydrogen Orbitals

5. A. The Hydrogen Orbitals • Orbitals do not have sharp boundaries.

6. Shapes of Orbitals p orbitals – 3 types (dumbbell-shaped

7. Shapes of Orbitals d orbital – 5 types

8. Shapes of Orbitals f orbitals – 7 types

9. A. The Hydrogen Orbitals # sublevels = quantum # “n” n = 1  1 sublevel  s n = 2  2 sublevels  s, p n = 3  3 sublevels  s, p, d n = 4  4 sublevels  s, p, d, f

10. A. The Hydrogen Orbitals • Hydrogen Energy Levels • The s and p types of sublevel

11. 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.

12. An electron’s location is determined by … …principle quantum #  sublevel  orbital  spin • As “n” increases… …electron energy increases …the size of the orbital increases (electrons are farther away from the nucleus)

13. Pauli Exclusion Principle • an atomic orbital can hold a maximum of 2 electrons. • If an orbital contains 2 electrons, they must have opposite spins

14. Orbital energy diagram