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Chemistry Unit 3 – The Atom

Chemistry Unit 3 – The Atom. Lesson 7 – Atomic Orbitals (5.1) Objective: SWBAT describe the shape, position, and number of electrons in orbitals and sublevels. Do Now: What were the contributions of de Broglie, Heisenberg, and Schrodinger? Agenda: Do Now, Notes, Questions, Work on HW.

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Chemistry Unit 3 – The Atom

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  1. ChemistryUnit 3 – The Atom Lesson 7 – Atomic Orbitals (5.1) Objective: SWBAT describe the shape, position, and number of electrons in orbitals and sublevels. Do Now: What were the contributions of de Broglie, Heisenberg, and Schrodinger? Agenda: Do Now, Notes, Questions, Work on HW

  2. Orbitals • From last time: Orbitals are 3D shapes where electrons are allowed to be. • There are four different types of orbitals, also known as sublevels. • s, p, d, f

  3. s Orbitals • They are spherical in shape. • The radius of the sphere increases with the value of n (energy level). • There is only 1 type of s orbital.

  4. p Orbitals • They are hourglass-shaped. • They have two lobes with a node between them. • There are 3 types of p orbital (x, y, z)

  5. d Orbitals • There are 5 possible d orbitals. • They resemble 4-leaf clovers, with one exception.

  6. f Orbitals • There are seven f orbitals.

  7. Orbital Rules • Every orbital is allowed to hold two electrons. • The s sublevel has one orbital, and can hold 2 electrons. • p has 3 orbitals, 6 electrons. • d has 5 orbitals, 10electrons. • f has 7 orbitals, 14 electrons

  8. Orbital Rules • The energy level number determines how many sublevels it can have. • The first energy level can only have one sublevel. • n = 1; s only • n = 2; s and p • n = 3; s, p, and d • n = 4; s, p, d, and f

  9. Comparing Bohr and Quantum • Remember the Bohr energy level rules: • n = 1: 2 electrons • n = 2: 8 electrons • n = 3: 18 electrons • n = 4: 32 electrons • Compare with the orbitals: • n = 1; s only (2 electrons) • n = 2; s and p (2 + 6 = 8 electrons) • n = 3; s, p, and d (2 + 6 + 10 = 18 electrons) • n = 4; s, p, d, and f (2 + 6 + 10 + 14 = 32 electrons)

  10. Review Questions • How many sublevels are in the n = 1, 2, 3, and 4 energy levels? • How many orbitals are in the s, p, d, and f sublevels? • How many electrons can fit in the s, p, d, and f sublevels? • How many electrons can fit in the n = 1, 2, 3, and 4 energy levels?

  11. HW 3-4 Due Monday • Friday: No Class (11th grade field trip) • Next Week: • Monday: Orbital Representations (5.2) • Tuesday: Electron Configurations (5.2), HW 3-5 Due • Wednesday: The Light Spectrum (5.3) • Thursday: Atomic Spectra – The Atomic Bar Code (5.3) • Friday: Work Day (Early Dismissal) • Approximate Unit 3 Test: Tues, Nov. 9th

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