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SH📘 Class 9 Chemistry | Chapter 4 – Structure of the Atom ⚛️✨
Handwritten ✍️ colorful 🎨 realistic notes with easy language, doodles 🖍️ and diagrams 🧪
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MAChemistry class - atomic structure👌🏽 #rappingscienceteacher #gcse #science
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IIAtomic Structure Topper’s Short Notes for IIT JEE 2026 - PDF(Link in Bio)
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GL✨️What does an atom look like?✨️
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Did you know?
The structure of the atom, according to Bohr's model and other early 20th-century models, can be described in physical terms quite simply:
Atomic Nucleus: At the center of the atom is the nucleus, composed of protons (positively charged particles) and neutrons (neutral particles). This nucleus contains most of the atom's mass.
Electrons: Electrons are negatively charged particles that orbit the nucleus in specific layers or energy levels. In Bohr's model, these levels are well-defined, and electrons can move between levels by absorbing or emitting energy in the form of photons.
Quantum Models: Following Bohr's model, more advanced models incorporating quantum mechanics principles were developed.
Let's start discussing atomic orbitals, wave functions, eigenstates, Hilbert space, Heisenberg's uncertainty principle, radial distribution functions, etc. Etc.
All of these were introduced following Bohr's atomic model and Scattering Rutherford .
These models treat the positions of electrons not as precise orbits but as "probability clouds" that indicate where an electron is most likely to be found at any given time.
These initial physical models of the atom laid the groundwork for modern understanding of atomic structure, which continues to evolve with further research and technological developments.
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SO"Structure of Atom in 90 seconds ⏱️ | All important formulas at one place – Save this reel before you forget!"
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QUInside every atom, electrons do not follow fixed paths. They exist as quantum probability clouds, governed by wave behavior and fundamental physical laws.
#QuantumPhysics #AtomicStructure #Electrons #ModernPhysics #scienceeducation
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OL.
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Imagine drawing shrödinger's model on paper 😭
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John Dalton proposed that matter is composed of indivisible particles called atoms, laying the foundation for modern atomic theory in the early 1800s.
J.J. Thomson discovered electrons in 1897, leading to the "plum pudding" model, which described atoms as spheres of positive charge with embedded electrons (just like a plum pudding!). Subsequent experiments would prove this model wrong.
Ernest Rutherford, through his gold foil experiment in 1911, introduced the concept of a dense, positively charged nucleus at the center of the atom, around which electrons orbit. However his model couldn't explain the stability of the electron orbits (since electrons are attracted to protons, why doesn't the electrons collapse into the nucleus?)
In 1913, Niels Bohr developed a model where electrons travel in specific energy levels or shells around the nucleus, explaining atomic emission spectra. Bohr's model addressed the stability and spectral lines but only for simple atoms like Hydrogen.
Erwin Schrödinger, in 1926, introduced wave mechanics, describing electrons as wave functions, leading to probability distributions and orbitals. This approach resolved many of the previous model issues by providing the most accurate and comprehensive description of atom models even today.
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CHStructure of Atom
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SCFrom 1 proton… to 118.
This animation moves through different elements on the periodic table, showing how atomic number shapes the entire structure of an atom.
Add more protons to the nucleus → add more electrons → build more shells → change the chemistry completely.
Same rules.
Same physics.
Completely different behaviour.
The periodic table isn’t just a list, it’s a map of how matter builds complexity.
#ScienceKind #Chemistry #PeriodicTable #AtomicStructure #STEM
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MAChemistry class - atomic structure #rappingscienceteacher #gcse #science
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BEATOMIC MODEL THROUGH HISTORY
1. John Dalton’s Model (1803) – Solid Sphere Model
Overview:
Dalton proposed that all matter is made up of indivisible particles called atoms.
He imagined atoms as tiny, solid spheres—like billiard balls.
Key Ideas:
Atoms of the same element are identical in mass and properties.
Atoms cannot be created, divided, or destroyed.
Compounds form when atoms of different elements combine in fixed ratios.
Importance:
First scientific model of the atom based on experimental evidence (like gas laws).
Laid the groundwork for modern chemistry.
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2. J.J. Thomson’s Model (1904) – Plum Pudding Model
Overview:
After discovering the electron, Thomson proposed that atoms are made of a positively charged substance with negatively charged electrons scattered within it—like raisins in pudding.
Key Ideas:
Atoms are divisible.
Electrons are negatively charged subatomic particles.
The rest of the atom is a blob of positive charge to balance the electrons.
Importance:
First model to show that atoms have internal structure.
Introduced the idea of subatomic particles.
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3. Ernest Rutherford’s Model (1911) – Nuclear Model
Overview:
Conducted the gold foil experiment where alpha particles were fired at a thin sheet of gold.
Most passed through, but some were deflected at large angles.
Key Ideas:
Atoms are mostly empty space.
A small, dense, positively charged nucleus is at the center.
Electrons orbit around this nucleus.
Importance:
Disproved the plum pudding model.
Introduced the concept of a nucleus.
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4. Niels Bohr’s Model (1913) – Planetary Model
Overview:
Bohr expanded on Rutherford’s model using discoveries from quantum theory.
Key Ideas:
Electrons orbit the nucleus in fixed paths or “energy levels.”
Each level has a specific amount of energy.
Electrons can jump to higher levels when energy is absorbed and fall back down when energy is released (as light).
Importance:
Explained why atoms emit light in specific colors (atomic spectra).
Added the concept of quantized energy levels.
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5. Erwin Schrödinger’s Model (1926) – Quantum Mechanical Model (Electron Cloud Model)
Overview:
Schrödinger used complex
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QUCan you imagine visualizing a single atom scaled up to the size of Earth? Now, think about what the size of the nucleus would be in comparison to Earth.Comment down below.
The atom, the fundamental building block of matter, is a marvel of complexity and simplicity combined. At the heart of every atom lies the nucleus, a dense core composed of protons, which are positively charged particles, and neutrons, which carry no charge.
This nucleus holds nearly all the atom’s mass, despite being minuscule in size compared to the overall atom.
Surrounding the nucleus are electrons, negatively charged particles that occupy regions known as electron orbitals.
Unlike the neat orbits of planets around the sun, these orbitals are better described as “probability clouds” due to the principles of quantum mechanics. Electrons don’t have precise paths; instead, they exist in regions where they are most likely to be found.
Initially, John Dalton proposed that atoms were indivisible spheres. This idea evolved with J.J. Thomson’s discovery of the electron, suggesting atoms were divisible and included smaller particles.
Ernest Rutherford’s gold foil experiment revealed the existence of a dense nucleus at the atom’s center, surrounded by electrons. Niels Bohr refined this model, proposing that electrons orbit the nucleus in defined energy levels.
Modern quantum mechanics further revolutionized our understanding by introducing the concept of electron orbitals as “probability clouds” rather than fixed paths. These advancements highlighted the nucleus, composed of protons and neutrons, and the electrons that occupy regions based on quantum numbers: principal (n), angular momentum (l), and magnetic (m).
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