KEY HW 4.1 Electron Configurations

Page 1: Electron Configurations Overview

• Recall: Bohr Models

  • Rings represent different energy levels that electrons can occupy.

  • Within each ring, there are additional sub-levels that classify electron locations more specifically.

• Revised Atomic Model

  • Atomic Orbitals: Founded on Schrödinger's Equation, describing the probability of finding an electron at various locations around the nucleus.

  • The shaded areas in orbital shapes indicate a region of high probability of locating the electron.

  • Electrons and the nucleus interact to create the most stable arrangement of electrons possible.

• Three Principles for Electron Arrangement:

  1. Aufbau Principle:

     • Electrons fill the lowest energy levels first.

     • Sequence of filling: 1s, 2s, 2p, 3s, 3p, 3d, etc.

Page 2: Atomic Models and Electron Configuration

• Pauli Exclusion Principle

  • No two electrons can have the same set of four quantum numbers (i.e., an orbital can hold a maximum of two electrons).

• Hund's Rule

  • Electrons occupy degenerate orbitals singly before pairing up.

• Practice Level 1

  • Draw the Bohr Model, Aufbau Diagram, and electron configurations for:

    1. Hydrogen

    2. Carbon

    3. Oxygen

    4. Chlorine

Page 3: Continued Practice with Atomic Models

• Practice Level 2

  • Draw the Bohr Model, Aufbau Diagram, and electron configurations for:

    1. Calcium (20)

    2. Scandium (21)

    3. Manganese (25)

    4. Selenium (34)

Page 4: Homework - Atomic Models Reflection

• Homework Part I: Reflection Questions

  1. Which representation is more accurate: Bohr model or quantum model?

  2. What does the quantum model illustrate?

  3. Arrange the sublevels in decreasing energy: 2p, 4s, 3s, 3d, 3p.

• Homework Part II

  • Draw the Bohr model, Aufbau diagram, and electron configurations for:

    1. Na

    2. Nb

    3. Y

    4. Cs

    5. Sb

    6. O2-

    7. Na+

    8. Fe3+

Page 5: Additional Electron Configurations

• Electron Configurations Practice

  • Understand configurations up to Kr (Krypton) and the occupancy of s, p, d orbitals.

  • Note any variations due to ionization or electron loss.

Page 6: Review Concepts

• Review Important Concepts

  • Revisit the rules regarding electron configurations and orbital shapes.

  • Analyze the shapes and probabilities associated with electron placement in atomic orbitals.