Unit Plan #6 - Arrangement of Electrons in Atoms

Unit Plan 6:  Arrangement of Electrons in Atoms
Chemistry Level 2/Mrs. Wissler

Learning Objectives:  The student will be able to
  1. Explain the mathematical relationship among the speed, wavelength, and frequency of electromagnetic radiation.
  2. Discuss the dual wave-particle nature of light.
  3. Describe the Bohr model of the hydrogen atom.
  4. Compare and contrast the Bohr model and the quantum model of the atom.
  5. Explain how the Heisenberg uncertainty principle and the Schrodinger wave equation led to the idea of atomic orbitals.
  6. List the four quantum numbers and describe their significance.
  7. Relate the number of sublevels corresponding to each of an atom’s main energy levels, the number of orbitals per sublevel, and the number of orbitals per main energy level.
  8. List the total number of electrons needed to fully occupy each main energy level.
  9. State and apply Aufbau principle, the Pauli Exclusion Principle, and Hund’s rule.
  10. Describe the electron configurations for the atoms of any element using orbital notation and electron-configuration notation.
Essential Questions:    How can atomic models be used to explain atoms and help us understand the interaction of elements and compounds? 

Central Concepts: Atomic models are used to explain atoms and help us understand the interaction of elements and compounds observed on a macroscopic scale.  The periodic table displays the repeating patterns, which are related to the atoms’ outermost electrons.

Text: Ch. 4 - all section objectives and bolded vocabulary


Day 1              A,B – 12/21    D-12/22
Notes:  Wave and Particle Properties of Light, Electromagnetic Spectrum
Flame Test Set Up and Lighting Practice
HW: Guided Reading Sec 4.1 The Development of a New Atomic Model #1-13

Day 2              A,B – 12/23    D-1/4
Lab:  Flame Test
HW: Guided Reading questions #14-22 (D block)

Day 3              A,B – 1/5        D- 1/6
Demonstration:  Spectroscopes Natural and Artificial Light
Notes:  Line-Emission Spectra and the Bohr Model
Lab:  Complete Unknowns for Flame Test
HW:  Flame Test Lab Report

Day 4              A,B – 1/7        D-1/8
Warm Up:  Bohr Model Quiz Review
Group Study Questions
Powerpoint:  Wave and Particle Properties of Electrons, Heisenberg and Schrodinger
HW:  Study for Bohr Model Quiz

Day 5               A,B – 1/11     D-1/12
Bohr Model Quiz
Finish Wave and Particle Properties of Electrons
Graphic Organizer/Models:  Quantum Model of the Atom and Orbital Shapes
Midterm Review Materials
HW:  Sec 4.2 Guided Reading, Review for Midterm

Day 6              A,B – 1/13      D-1/14
Graphic Organizer:  spdf block Periodic Table
Notes:  electron configuration and atomic sublevels/energy graph
Practice:  Electron Configuration Notation and Orbital Notation
Notes:  Aufbau Principle, Pauli Exclusion Principle and Hund’s Rule
HW: Electron Configuration Practice, Review for Midterm

Day 7              A,B – 1/15      D-1/19
Unit 1-5 Review
Practice Midterm
HW:  study for Midterm, prepare notecard


MCAS Chemistry Frameworks:
ü  MCAS 2.3 Recognize discoveries from Dalton (atomic theory), Thomson (the electron), Rutherford (the nucleus), and Bohr (planetary model of atom), and understand how each discovery leads to modern theory.
ü  MCAS 2.4 Write the electron configurations for the first twenty elements of the periodic table.
ü  MCAS 3.3 Relate the position of an element on the periodic table to its electron configuration and compare its reactivity to the reactivity of other elements in the table.
ü  MCAS 3.4 Identify trends on the periodic table (ionization energy, electronegativity, and relative sizes of ions).