Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

10. Periodic Properties of the Elements

The Electron Configuration

General Chemistry

10. Periodic Properties of the Elements

The Electron Configuration

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Multiple Choice

Which electron configuration represents a violation of the Auf Bau Principle?

Illustration showing electron configurations with red boxes highlighting a violation of the Auf Bau Principle.

Illustration showing electron configurations with one highlighted as violating the Auf Bau Principle.

Illustration showing electron configurations, highlighting one that violates the Auf Bau Principle with a red box.

Illustration showing electron configurations with highlighted boxes indicating a violation of the Auf Bau Principle.

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Verified step by step guidance

Step 1: Understand the Aufbau Principle, which states that electrons fill orbitals starting from the lowest energy level to the highest. This means orbitals are filled in the order of increasing energy (e.g., 1s, 2s, 2p, 3s, etc.).

Step 2: Examine the provided electron configurations in the images. Look for any violations where electrons are placed in higher energy orbitals before lower energy orbitals are completely filled.

Step 3: Identify configurations where the 1s, 2s, or 2p orbitals are not fully occupied before electrons are placed in higher orbitals such as 3s or 3p.

Step 4: Pay attention to the number of electrons in each orbital and ensure that the Pauli Exclusion Principle and Hund's Rule are also followed. For example, electrons in the same orbital must have opposite spins.

Step 5: Once the violation is identified, note the specific orbital arrangement that breaks the Aufbau Principle, such as skipping a lower energy orbital or incorrectly filling orbitals.