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Why do covalent compounds share electrons?
A covalent compound forms when electrons are shared and this will happen when you have 2 nonmetals, or 2 anions, bonding together. The reason these elements share their electrons is because they have a small difference in...
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Unveiling the SECRETS of Atomic Structure!
In this video, students will learn about atomic theory, atomic structure and how the atom is put together. This will include learning about the different subatomic particles, protons, neutrons and electrons, that make up the atom! This...
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Determining the Number of protons, neutrons and electrons in an ATOM
In this video, we're going to learn about the number of p, n and e in an atom. We'll explore the atomic structure of different elements, and see how the number of protons, neutrons and electrons affects the properties of those elements....
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Protons, Neutrons and Electrons Explained - what's the difference?
In this video, we'll explore the differences between the proton, neutron, and electron. We'll learn about their characteristics, and how they interact with matter. This video is perfect for anyone who wants to learn more about subatomic...
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Molecules, compounds and types of chemical bonds
What is the difference between a molecule and a compound? What are the main types of chemical bonds? In this video, we will be answering those questions and more.
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Chemistry - Electron Configuration for Ions
Electron Configurations are essential to chemistry and they help us better understand and explain the position/location of electrons. Writing electron configurations can be daunting at first but once you see the pattern, you will be able...
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Pauli's Exclusion Principle: The rule of electrons
Wolfgang Pauli's Exclusion Principle, developed in 1925, is a crucial concept in quantum mechanics. It states that two electrons in the same atom cannot have the same set of quantum numbers, which are the principal quantum number (𝑻n),...
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Principal Quantum Number: The Key to Electron Shells
The principal quantum number (𝑛) is a fundamental parameter in quantum mechanics that determines the size and energy level of an electron's orbit within an atom. It is a positive integer that represents the main energy level or shell in...
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Stern-Gerlach Experiment and spin quantum number : Revealing Electron Spin
The Stern-Gerlach experiment, which took place in 1922, was the most important proof that electrons have spin and that they have a spin quantum number. A stream of silver atoms was sent through an experiment using a magnetic field that...
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Azimuthal Quantum Number: Shaping Electron Orbits
Characterised by the symbol 𝑙l, the azimuthal quantum number is a fundamental parameter in quantum mechanics that describes the angular momentum and form of an electron's orbital within an atom. The integer values it accepts range from 0...
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Negative Energy: Understanding Hydrogen's Electron
In a hydrogen atom, the electron is bound to the nucleus, so its energy is negative. This shows that it is in a bound state. When there is negative energy, it means that the electron is stable. It is inside the atom because its negative...
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Line Spectra: The Fingerprints of Atoms
Line spectra are unique patterns of light emitted or absorbed by atoms, resembling discrete lines. These patterns serve as the "fingerprints" of different elements, providing critical insights into atomic structure and composition....
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Bohr's Atomic Model: Electrons in Orbit
In 1913, Niels Bohr proposed an atomic model that dramatically altered our comprehension of atomic structure by establishing a novel framework for describing the arrangement and behaviour of electrons within an atom. The purpose of...
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Decoding the Photoelectric Effect: How It Works
The photoelectric effect is a phenomenon that occurs when light, consisting of photons, interacts with the inner structure of an atom. Photons carry a specific amount of energy proportional to their frequency, which is transferred to an...
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Drawbacks of Rutherford's Theory
Rutherford's Nuclear Model: Limitations and Developments • Stability of Electrons in Orbit: The model failed to account for the continuous emission of electromagnetic radiation, indicating a flaw in the model. • Inability to Explain...
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Millikan's Oil Drop Experiment : Tiny Drops, Big Discoveries
Millikan's Oil Drop Experiment: A Discovery and Impact Experimental Setup: • The experiment involved measuring the force on charged oil droplets suspended between two metal plates. • The apparatus included an atomizer, observation...
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Aufbau Principle: Building Electron Configurations
An important idea in atomic theory is the Aufbau Principle, which shows how electrons are arranged in an atom. It says that electrons fill atomic orbitals from least energetic to most energetic, starting with the least energetic orbitals...
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Heisenberg's Uncertainty principle : The Limits of Precision
Werner Heisenberg proposed Heisenberg's Uncertainty Principle in 1927, which states that measuring a particle's momentum and position at the same time with accuracy is not possible. One can know a property less precisely the more...
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Heisenberg's Thought Experiment: Exploring Uncertainty
The Uncertainty Principle is demonstrated by Heisenberg's thought experiment, which demonstrates that increasing uncertainty in a particle's momentum results from precisely measuring its position, such as through a narrow slit, and vice...
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De Broglie vs Bohr: A Quantum Debate
Niels Bohr's model of the atom introduced the idea of quantised orbits for electrons. In these, electrons occupy stable energy levels and either give off or take in photons when they move between these levels. This model was able to...
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De Broglie's Equation: Wave-Particle Duality
De Broglie's equation, formulated by Louis de Broglie in 1924, introduces the concept of wave-particle duality, suggesting that all matter exhibits both wave-like and particle-like properties. The equation is expressed as λ=h/p; λ is...
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Electron Energy: Deriving the Expression
Bohr's model of the atom says that an electron's energy is set by its orbit around the nucleus. Bohr said that electrons have specific, quantised levels of energy, and that the size of the orbit affects the energy level. An electron's...
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Atomic Orbits: Calculating the Radius
Bohr's atomic model postulates that the radius of an electron's orbit around the nucleus is determined by the concept that electrons travel in quantised orbits with distinct and well-defined radii. According to the model, the angular...
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Rutherford's Atomic Revelation: The Nuclear Model
Ernest Rutherford's Nuclear Model of the Atom: A Transformative Journey Background and Experiment • J.J. Thomson's Plum Pudding Model, a sphere of diffuse positive charge with negatively charged electrons, was the dominant model before...