Скачать или смотреть Chromium & Copper - Electronic Configuration Abnormality | Structure of Atom | Chemistry Class 11

🔬 STABILITY OF HALF & COMPLETELY FILLED SUBSHELLS | STRUCTURE OF ATOM | CHEMISTRY CLASS 11 | QUANTUM CLASSES

Download Notes of This Lecture:
Google Drive Link: https://drive.google.com/file/d/1OlM1...

Welcome to Quantum Classes!
In this detailed video, we explore one of the most important and conceptually rich topics from Chapter – Structure of Atom (Class 11 Chemistry): Stability of Half and Completely Filled Subshells.

📘 What You’ll Learn in This Video:

In this session, you will learn:
✅ The concept of electronic configuration and the order of filling of orbitals (Aufbau Principle).
✅ The Pauli Exclusion Principle and Hund’s Rule of Maximum Multiplicity.
✅ The scientific explanation behind the extra stability of half-filled (like 3d⁵) and completely filled (like 3d¹⁰) subshells.
✅ Quantum mechanical reasons for stability — symmetrical distribution and exchange energy.
✅ Examples of exceptional electronic configurations such as:
Chromium (Cr): 3d⁵ 4s¹
Copper (Cu): 3d¹⁰ 4s¹
✅ The energy difference between orbitals and how this affects electron distribution.
✅ The importance of exchange energy and symmetry in achieving stable atomic structures.

🧠 Key Concepts Discussed:
1. Subshells and Orbitals: Understanding s, p, d, f orbitals.
2. Half-Filled & Completely Filled Configurations: Why they are more stable.
3. Exchange Energy Concept: How exchange of electrons with parallel spins increases stability.
4. Symmetrical Distribution: Role of symmetry in energy minimization.
5. Exceptional Configurations: Chromium, Copper, Niobium, Molybdenum, etc.
6. Electronic Configuration of Elements (Z = 1 to 30): Understanding patterns and exceptions.
7. Comparison Between Normal and Anomalous Configurations.

📚 Chapter: Structure of Atom
Subject: Chemistry
Class: 11 (CBSE + JEE + NEET Foundation)

⚡Why This Topic is Important:
Frequently asked in CBSE Board Exams, JEE Main, and NEET.
Builds the foundation for understanding periodic trends and chemical bonding.
Helps in predicting valence electrons, oxidation states, and magnetic properties of elements.
Strengthens conceptual clarity on atomic structure and quantum mechanics.

💡 Why Watch Quantum Classes?
At Quantum Classes, we make complex concepts simple and logical!
We focus on concept-based learning to help students of Class 11 & 12 prepare for:
CBSE Board Exams
JEE Main & Advanced
NEET
Foundation Courses for Class 9–10

Our goal is to make every student understand the **“why” behind science**, not just memorize facts.

📖 Watch Next:
🎥 Electronic Configuration of Elements – Step-by-Step Explained
🎥 Quantum Numbers – n, l, m, s with Examples
🎥 Aufbau Principle, Pauli Exclusion & Hund’s Rule – Complete Guide
🎥 Energy Level Diagram & Filling of Orbitals

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🏷️ Tags:
Stability of Half Filled and Completely Filled Subshells, Class 11 Chemistry, Structure of Atom, Electronic Configuration, Aufbau Principle, Hund’s Rule, Exchange Energy, Pauli Exclusion Principle, Extra Stability of Half Filled Orbitals, Copper and Chromium Configuration, Exceptional Electronic Configurations, Chemistry Class 11, Quantum Classes, JEE Main Chemistry, NEET Chemistry, Class 11 CBSE Chemistry, Half Filled and Fully Filled Stability, Structure of Atom Class 11 Notes, Chemistry Explained in Hindi, Concept Based Chemistry, Quantum Numbers and Configuration.

🎯 Keywords:
Stability of half-filled and completely filled orbitals explained
Chromium and copper electronic configuration exceptions
Exchange energy concept chemistry class 11
Aufbau principle anomalies
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Electronic configuration class 11 important concept

✨ Final Note:
Understanding why some atoms prefer half-filled or fully filled subshells gives deep insight into atomic behavior and periodic trends. This topic not only strengthens your understanding of atomic structure but also builds the base for future topics like Periodic Classification, Chemical Bonding, and Coordination Chemistry.

So, sit back, take notes, and watch the video till the end to master this crucial concept in Chemistry!
📚 Learn Smart. Learn Deep. Learn with Quantum Classes.