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Atomic Structure Complete Chapter in One Shot | B.Sc 1st Year Chemistry‎️‍🔥

Padhai Ka Safar・2 minutes read

The video on Physical Chemistry delves into organic chemistry topics like End Bonding and Stereochemistry, providing essential calculations and formulas for solving numerical problems. Concepts like De Broglie's hypothesis, Quantum Mechanics, and the Quantum Mechanical Model of the atom are detailed, emphasizing the wave nature of electrons and the energy levels in orbitals.

Insights

  • Louis de Broglie's hypothesis in 1924 introduced the concept that matter particles exhibit wave-like behavior, with the wavelength inversely proportional to momentum.
  • The Quantum Mechanical Model of the atom emphasizes the wave nature of electrons, quantized energy levels, and the uncertainty in electron position, challenging the fixed orbit concept.
  • The energy levels of orbitals in atoms follow specific rules such as the Aufbau principle, Pauli exclusion principle, and Hund's rule, with orbitals arranged by increasing energy levels and electron occupancy based on spin and energy considerations.

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Recent questions

  • What is the significance of Louis de Broglie's hypothesis?

    Louis de Broglie's hypothesis in 1924 proposed that matter particles have associated waves, with the wavelength dependent on momentum. This idea revolutionized the understanding of the dual nature of particles, linking wave and particle characteristics. The wavelength of matter waves is expressed as lambda = h/p, inversely proportional to particle momentum. De Broglie's hypothesis laid the foundation for quantum mechanics, providing a crucial insight into the wave-particle duality of matter.

  • How does the Uncertainty Principle impact atomic behavior?

    The Uncertainty Principle, introduced in quantum mechanics, states the impossibility of determining position and momentum simultaneously for small moving particles like electrons. This principle has significant implications for atomic behavior, highlighting the inherent uncertainty in the position and momentum of electrons within an atom. The mathematical representations of uncertainty in position and momentum, along with the mention of Planck's constant, underscore the limitations of precise measurements at the atomic level.

  • What are the key aspects of the Quantum Mechanical Model of the atom?

    The Quantum Mechanical Model of the atom emphasizes the wave nature of electrons, uncertainty in their position, and quantized energy levels. This model challenges the fixed orbit concept of electrons, suggesting they move in a spread-out manner around the nucleus. Understanding the quantum nature of electrons is crucial for a comprehensive grasp of atomic behavior, with the model highlighting the wave-particle duality and the importance of quantized energy levels in determining electron behavior within an atom.

  • How are orbitals and orbits differentiated in atomic structure?

    In atomic structure, orbitals are regions where electrons are likely to be found, while orbits are well-defined circular paths. Orbitals do not represent the position and momentum of electrons with complete certainty, unlike orbits. The concept of orbitals allows for a more accurate depiction of electron behavior within an atom, emphasizing the probability distribution of electron locations rather than fixed circular paths.

  • What principles govern the arrangement of electrons in orbitals?

    The arrangement of electrons in orbitals follows the Aufbau principle, Pauli exclusion principle, and Hund's rule. Electrons fill orbitals in increasing energy order, with the value of N + L determining the energy levels of orbitals. The Pauli Exclusion Principle dictates that each orbital can hold a maximum of two electrons with opposite spins, while the maximum number of electrons in an energy level is determined by the formula 2n². These principles guide the orderly filling of orbitals and the distribution of electrons within an atom.

Related videos

Summary

00:00

"Physical Chemistry Video: End Bonding, Quantum Mechanics"

  • The video on Physical Chemistry focused on organic chemistry, particularly on End Bonding and Stereochemistry.
  • The link to the video can be found in the description box, along with the atomic Structure link.
  • Effective nuclear charge, radial Angular wave function, and probability distribution were discussed as extra topics.
  • The video covers important topics from previous years, including questions related to Di Broglie and uncertainty.
  • The Scrollinger equation for atomic orbitals (s, p, f) was mentioned, with derivation to be covered in B.Sc Six Semester.
  • Quantum mechanics topics like Scrollinger equation and energy diagrams are crucial in B.Sc Fifth and Sixth Semesters.
  • Louis de Broglie's hypothesis in 1924 suggested that matter particles have associated waves, with wavelength dependent on momentum.
  • The wavelength of matter waves is expressed as lambda = h/p, inversely proportional to particle momentum.
  • Numerical problems can be solved using the formula lambda = h/p, with values like mass of electron and helium provided for calculations.
  • Practical applications involve calculating momentum and Broglie wavelength using the formula P = h/lambda, with the Planck constant value given.

17:27

Quantum Mechanics: Wave Nature of Electrons

  • The formula to find frequency is discussed, involving calculations like 5.65*10^Mins on 25th June.
  • The concept of energy particles and the formula for energy calculation are explained.
  • De Broglie's hypothesis on the dual nature of particles is detailed, linking wave and particle characteristics.
  • The Uncertainty Principle is introduced, stating the impossibility of determining position and momentum simultaneously for small moving particles.
  • Mathematical representations of uncertainty in position and momentum are provided, with Planck's constant mentioned.
  • The Uncertainty Principle's application to electrons and the limitations of Bohr's Atomic Model are discussed.
  • The Quantum Mechanical Model of the atom is presented, emphasizing the wave nature of electrons and the uncertainty in their position.
  • Three key aspects of the new Atomic Model are highlighted, including the wave nature of electrons, uncertainty in their position, and fixed energy states.
  • The model challenges the fixed orbit concept, suggesting electrons move in a spread-out manner around the nucleus.
  • The importance of understanding the quantum nature of electrons in the new Atomic Model is underscored for a comprehensive understanding of atomic behavior.

36:54

Quantum Mechanics: Wave Model and Orbitals

  • The mechanical model of the atom is also known as the wave model.
  • The equation describing the mechanics of particles as waves is crucial.
  • The equation includes terms like Dell Square 5/dx² and Delta Square Plus Dell Square / Dell s squared plus 8y².
  • The mass of an electron is 9.1 * 10^-31 kg.
  • The wave function represents the amplitude of the electron.
  • Quantum numbers, such as principal quantum number and magnetic quantum number, are essential for solutions.
  • The quantum mechanical model of the atom emphasizes quantized energy levels for electrons.
  • The wave nature of electrons in orbitals is a key feature.
  • Atomic orbitals can only hold a maximum of two electrons.
  • Orbitals are regions where electrons are likely to be found, while orbits are well-defined circular paths.

55:15

Electron Orbitals: Position, Momentum, and Quantum Numbers

  • Orbitals do not represent d positions in Momentum of electron with complete certainty.
  • In circularity orbital case, position and Momentum of Electron with Certility are found.
  • Maximum Electrons Wear and Use Number of Orbit.
  • 2n² can accommodate electrons in orbitals.
  • Opposite spin is required for most electrons.
  • Four differences between orbiter orbital are explained.
  • Quantum details with four types of numbers are covered.
  • Shapes, function, sign, and probability distribution in orbitals are studied.
  • Principal energy diagram structure is discussed.
  • Spin quantum number represents two types of motion for electrons.

01:08:57

Electron Arrangement and Subshell Calculations

  • Total of 10 electrons, with 2, 6, and 10 electrons in different scenarios.
  • Formula for total electrons: 16 + 2 = 18, 80 electrons calculated using 2n².
  • Determining total electrons on subshell using the formula 2n².
  • Calculating values of N, with examples like 2 * 3² = 18.
  • Explaining the values of L based on N, such as L being zero for N = 4.
  • Understanding the values of L for different scenarios, like -1, 0, +1 for L = 0.
  • Explaining the number of orbitals in different subshells, like 7 orbitals in total.
  • Describing the arrangement of electrons in F orbitals.
  • Calculating the total number of electrons in 7 orbitals.
  • Discussing the concept of degenerate orbitals and their energy differences.

01:23:45

Orbital Energy Determined by Quantum Numbers

  • The energy of the orbital is determined by the ratio of 2s and 2p, with S and P present.
  • The energy of the orbital is similar to the principal quantum number (n) you have.
  • The energy of orbitals remains consistent with the principal quantum number, such as 4s, 4p, 4d, and 4f.
  • For hydrogen and hydrogen-like atoms, the energy of orbitals corresponds to your principal quantum number.
  • In multi-electron atoms, the energy of orbitals may differ based on the principal quantum number.
  • The energy level of orbitals follows a specific order: S orbital has the lowest energy, followed by P and then D orbitals.
  • Comparing energy levels at n=3 and n=4, the 3D orbital has slightly higher energy than the 4s orbital.
  • The energy of orbitals is influenced by the sum of the principal and azimuthal quantum numbers (N + L).
  • The relative energy of orbitals is determined by the N + L rule, where higher values indicate higher energy levels.
  • The arrangement of electron energy levels in atoms follows the Aufbau principle, Pauli exclusion principle, and Hund's rule, with electrons filling orbitals in increasing energy order.

01:37:41

Orbital Energy Levels and Electron Capacity

  • The value of N + L determines the energy levels of orbitals, with higher values indicating higher energy.
  • The energy of 2p orbitals is greater than that of 2s orbitals.
  • For N = 3, the value of L is zero, leading to the formation of 3s, 3p, and 3d orbitals.
  • The value of N + L for 3s, 3p, and 3d orbitals is 3, 4, and 5 respectively.
  • The order of orbitals based on increasing energy levels is 1s, 2s, 2p, 3s, 3p, 3d, 4s, 4p, 4d.
  • For N = 4, the value of L is zero, resulting in the formation of 4s, 4p, 4d, and 4f orbitals.
  • The value of N + L for 4s, 4p, 4d, and 4f orbitals is 4, 5, 6, and 7 respectively.
  • The energy levels of orbitals follow a specific order, with 2s, 2p, 3s, 3p, 3d, 4s, 4p, 4d, 4f being arranged in increasing energy.
  • The Pauli Exclusion Principle states that each orbital can hold a maximum of two electrons with opposite spins.
  • The maximum number of electrons in an energy level is determined by the formula 2n², where n is the principal quantum number.

01:52:23

Electron Orbitals: Structure, Filling, and Multiplicity

  • If n goes up to -1, it becomes zero; van at n = 2 means an orbital and a p orbital.
  • In an S orbital, two electrons spread, while in a p orbital, six electrons are present.
  • With two lost electrons, the total electrons are 8, calculated by the formula 2n².
  • The topic discussed is the structure and maximum multiplicity, following Holmes' rule.
  • Orbitals are filled based on increasing energy, with equal energy orbitals filled first.
  • Electrons occupy orbitals singly with parallel spin, pairing only after all orbitals are singly occupied.
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