Atomic Models
Schrodinger’s
Equation
CHAPTER 2 – QUANTUM MECHANICS
Learning Objectives
By the end of the discussion the students
should be able to:
a) a. provide an overview of atomic models;
b) b. explain Schrödinger's equation and
its significance; and
c) c. discuss its applications in the field of
quantum mechanics.
Learning contents
01
03
Introduction to
Atomic Models
Schrödinger's Equation
and its Significance
02
The Need for
Quantum Mechanics
04
Applications of
Schrödinger's Equation
in Quantum Mechanics
INTRODUCTION TO
ATOMIC MODELS
Introduction
Atomic models are mathematical
models used to describe the
behavior of atoms, which are the
fundamental building blocks of
matter. Atoms consist of a nucleus,
which contains positively charged
protons and neutral neutrons, and
negatively
charged
electrons
orbiting around the nucleus in
discrete energy levels.
SOLID SPHERE MODEL
In 1803,1803, John Dalton developed a theory of the
structure of matter. The main postulates of this theory are:
The matter is composed of a large number of extremely
small particles called an atom.
2. Atoms are indivisible and cannot be destroyed in a
chemical reaction.
3. All the atoms of an element are alike, i.e., identical in
mass, size and every other aspect.
4. Atoms of different elements possess different properties,
size, mass, etc.
5. Compounds are formed by the combination of atoms in a
simple whole-number ratio.
6. In a given compound, the relative number and kinds of
atoms are constant.
1.
SOLID SPHERE MODEL
PLUM PUDDING MODEL
J.J Thomson made the first attempt at
explaining the fine structure of the atom. He
proposed that atoms were uniform, positively
charged spheres. Along with all the positive
charges, most of the mass of the atom was
thought to be uniformly distributed in this
uniform ‘cloud’ of positive charge.
The tiny negatively charged electrons
were believed to be embedded in these
positively charged cloud-like seeds in a
watermelon or like the plums in a pudding, and
hence, it was named the plum pudding model.
NUCLEAR MODEL
The major contribution in knowing
the relative positions of electrons and
protons in an atom was by Ernest
Rutherford.
According to Rutherford Model of an
Atom
1. There is a positively charged centre in
an atom called the nucleus.
2. The electrons revolve around the
nucleus in circular paths.
3. The size of the nucleus is very small
as compared to the size of the atom.
PLANETARY MODEL
In 1913, Neils Bohr, a student
of Rutherford's, developed a new model of the
atom. He proposed that electrons are arranged
in concentric circular orbits around the
nucleus.
1. Electrons occupy only certain orbits around
the nucleus.
2. Each orbit has an energy associated with it.
3. Energy is absorbed when an electron jumps
from a lower orbit to a higher one.
4. The energy and frequency of light emitted or
absorbed can be calculated.
QUANTUM MODEL
In 1926 Erwin Schrödinger proposed quantum model of
atom. The quantum mechanical model does not define the exact
path of an electron, but rather, predicts the odds of the location
of the electron. This model can be portrayed as a nucleus
surrounded by an electron cloud.
QUANTUM
MECHANICS
QUANTUM MECHANICS
 In the 19th Century most
physicists agreed that light is a
wave.
 Quantum mechanics is based on
the wave-particle duality of
quantum particles, meaning that
particles can exhibit both wavelike and particle-like behavior.
SCHRÖDINGER'S
EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
SCHRÖDINGER'S EQUATION
APPLICATIONS OF
SCHRÖDINGER'S
EQUATION
APPLICATIONS OF
SCHRÖDINGER'S EQUATION
Schrödinger's equation is a fundamental equation
in quantum mechanics that describes how the wave
function of a physical system changes with time. It has
many applications in quantum mechanics, including:
Predicting the behavior of atomic and subatomic
particles.
2. Understanding the properties of materials.
3. Designing and developing new materials.
1.
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