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Atomic Structure – Complete Chapter | Class 11 Chemistry
Understand Atomic Structure from the basics through simple explanations, diagrams, important formulas, and step-by-step problem-solving.
About this course
This course covers the essential aspects of atomic structure, focusing on the discovery of subatomic particles, atomic models, and quantum mechanics. Students will learn about the characteristics of electrons, protons, and neutrons, and how these particles contribute to the behavior of elements. The course will delve into Thomson, Rutherford, and Bohr's atomic models, highlighting their significance and limitations. Additionally, students will explore the quantum mechanical model of the atom, electromagnetic radiation, and the principles governing electron configurations. By the end of the course, students will have a solid understanding of atomic theory and its applications in chemistry.
What you will learn
- Understand the discovery and characteristics of subatomic particles.
- Describe and compare different atomic models.
- Explain the quantum mechanical model of the atom.
- Understand electromagnetic radiation and its properties.
- Write electronic configurations for various elements.
Who it is for
Class 11 students studying Chemistry, beginners who want to understand Atomic Structure from the basics, and students who need help with concepts, formulas, diagrams, and numerical problems.
Before you start:
- Basic understanding of chemistry concepts
- Familiarity with scientific notation
Course content
- The Discovery of Subatomic Particles · free preview · 30 min
Learn about electrons, protons, and neutrons and their characteristics. - Historical Atomic Models · 45 min
Explore Thomson, Rutherford, and Bohr's atomic models.
- Understanding Quantum Mechanics · 40 min
Introduce the quantum mechanical model and its significance. - Electromagnetic Radiation · 35 min
Discuss the nature of electromagnetic radiation and Planck’s theory.
- Principles of Electron Configuration · 50 min
Learn about quantum numbers and atomic orbitals. - Writing Electron Configurations · 45 min
Practice writing electronic configurations for various elements.
- De Broglie Relation and Heisenberg Principle · 40 min
Understand the de Broglie relation and Heisenberg uncertainty principle. - Spectroscopy and Atomic Spectra · 45 min
Explore the concept of atomic spectra and spectroscopy.
Free preview
1. Atoms are made of three fundamental particles: electrons, protons, and neutrons. 2. J.J. Thomson discovered the electron in 1897; it has a negative charge and very small mass (9.109 × 10^-31 kg). 3. Protons were discovered shortly after; they have a positive charge and are about 1840 times heavier than electrons (1.672 × 10^-27 kg). 4. Neutrons were discovered by James Chadwick in 1932; they are neutral particles with a mass similar to protons (1.675 × 10^-27 kg). 5. The charge of an electron is -1.602 × 10^-19 C, while the charge of a proton is +1.602 × 10^-19 C. 6. In a neutral atom, the number of protons equals the number of electrons, balancing the charges. 7. The atomic number (Z) is the number of protons in an atom's nucleus and determines the element's identity. 8. The mass of an atom is mainly concentrated in its nucleus, which contains protons and neutrons, collectively known as nucleons. 9. The discovery of these particles led to the development of various atomic models to explain atomic structure. 10. Thomson's model suggested electrons were embedded in a positively charged sphere, but this was later replaced by Rutherford's model, which proposed a central nucleus with electrons orbiting around it.
How it is taught
Interactive, student-friendly teaching with simple explanations, diagrams, real-life examples, and step-by-step numerical problem-solving. Each topic will be taught from the basics, followed by practice questions, doubt-clearing sessions, and short revision exercises.