STRUCTURE OF ATOM

Name: STRUCTURE OF ATOM
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Cathode Rays, Anode Rays

Created byVinay Arya

Last updated 10/2019

English

English [Auto],

What you'll learn

CATHODE RAYS, ANODE RAY, THOMSON MODEL OF ATOM, RUTHERFORD’S MODEL OF THE ATOM, BOHR’S THEORY

Course content

1 section • 9 lectures • 1h 47m total length

4.1. CONTENTS12:45
Explore the structure of the atom from atomic number and mass to electrons, protons, and neutrons, and review cathode ray experiments, Thomson’s and Rutherford’s models, isotopes, and electronic configuration principles.
4.2. INTRODUCTION TO STRUCTURE9:08
Explore the introduction to atomic structure: electrons, protons, neutrons, the nucleus, and how atomic number equals protons (and electrons) while mass number sums protons and neutrons.
4.3. CATHODE RAYS9:33
Explore the discovery of the electron through cathode ray experiments in a discharge tube, showing rays deflected by electric and magnetic fields and revealing negatively charged particles.
4.4. ANODE RAY8:55
Explore anode rays and canal rays, reveal that positively charged particles arise from hydrogen, identify protons, and discuss their electric and magnetic deflection and e/m ratio.
4.5. THOMSON MODEL OF ATOM8:13
Describe Thomson's plum pudding model as a uniform positive sphere with embedded electrons. Note drawbacks: even mass distribution and a static model that cannot explain electron movement or stability.
4.6. RUTHERFORD’S MODEL OF THE ATOM11:04
Rutherford's gold foil experiment reveals most of the atom is empty space, with mass and positive charge concentrated in a tiny nucleus, while electrons orbit it.
4.7. BOHR’S THEORY11:39
Bohr’s theory depicts atoms with a nucleus of protons and neutrons and electrons in fixed energy levels. It explains transitions via energy absorption or emission and notes valence electrons.
4.8. ISOTOPES22:43
Explain isotopes, their mass numbers, and applications from carbon dating to uranium-238 as nuclear fuel. Apply Aufbau principle, Pauli exclusion principle, and Hund's rules to electron configurations and isotopes.
4.9. HUND’S RULE13:43
Understand Hund’s rule and how it maximizes unpaired electrons with the same spin, guiding the electronic configuration by filling s, p, d, and f orbitals under Aufbau and Pauli principles.
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Requirements

Basics of Atomic Structure.

Description

Atom was considered as the smallest particle up to 19th century. A series of experiments were performed to explore the structure of atom. We shall discuss the structure of an atom and study the characteristics of atomic spectra and chemical properties of various atoms. An atom is made up of three subatomic particle electron, proton & neutrons. These three particle are called fundamental particle of matter.The size of nucleus of atom is very small in which neutron and protons are present so the entire mass of the atom is situated in nucleus. Protons and neutrons present in the nucleus are collectively termed an nucleons. Number of neutrons is called mass number of the element.

The neutron and proton have approximately equal masses of 1 amu and the electron is about 1836 times lighter; its mass can sometimes be neglected as an approximation. The electron and proton have equal, but opposite, electric charges; the neutron is not charged. The electron and proton have equal, but opposite, electric charges; the neutron is not charged. The existence of electrons in atoms was first suggested, by J.J. Thomson, as a result of experimental work on the conduction of electricity through gases at low pressures, which produces cathode rays and x-rays, and a study of radioactivity by Becquerel, the Curies and Rutherford.

Who this course is for:

Beginners, 9 grade students and research Scholars.