1. A New Approach to the Atom Objectives: 1. Describe the atomic orbitals in terms of their shape, size, and energy. Key Terms: quantum-mechanical model, electron density, orbital principle energy level, sublevel

2. Probability & Orbitals Schrodinger stated that electron orbitals can more correctly referred to as electron clouds. An orbital is the region around the nucleus where an electron is likely to be found. Within an orbital it is more likely to find the electron nearer to the nucleus than toward its boundary There are 4 basic orbital types: s,p,d,& f orbitals. Each orbital can hold a maximum of 2 electrons each with opposite spin

3. s orbital Spherical in shape 1 st orbital in any energy level and only orbital located at n=1

4. p orbital The p orbital is dumbbell shaped The p-orbitals begins in the 2 nd energy level The are 3 orbitals in the p-orbital system The orbitals extend out on the x, y, & z axis (p x,p y,p z ) The system can hold a maximum of 6 electrons

5. d-orbital The d orbital is dumbbell and donut shaped The d-orbital begins in the 3 rd energy level The are 5 orbitals in the d-orbital system The orbitals extend out at angles to the x, y, & z axis The system can hold a maximum of 10 electrons Considered a suborbital system and is inserted after 4s

6. f-orbital The f-orbitals begins in the 4 th energy level The are 7 orbitals in the d-orbital system The orbitals extend out at angles to the x, y, & z axis The system can hold a maximum of 14 electrons Considered a suborbital system to the d-block and is inserted after 6s

7. Orbital Summary for the Principle Energy Levels The number of the energy level is equal to the number of orbital sublevels n=1 1 sublevel 1s (2 electrons) n=2 2 sublevels 2s, 2p (8 electrons) n=3 3 sublevels 3s, 3p, 3d (18 electrons) n=4 4 sublevels 4s, 4p, 4d, 4f (32 electrons) Number of electrons possible for each orbital sublevel: s = 1 (2 electrons) p = 3 (6 electrons) d = 5 (10 electrons) f = 7 (14 electrons)