Atomic Structure: The Journey from Ancient Philosophers to Modern Theories
Arts,Science and Commerce College Mokhada
ATOMIC STRUCTURE
A
T
O
M
I
C
S
T
R
U
C
T
U
R
E
1.
INTRODUCTION
The
word
atom
in
Greek
means
indivisible,
i.e.
an
ultimate
particle which cannot be further
subdivided.
This
idea
of
all
matter ultimately
consisting
of
extremely small
particles was
conceived
by ancient
Indian
and
Greek
philosophers. The old
concept
was put on
firm
footing by John
Dalton
with his
atomic
theory
that
was
developed
by
him during the
years 1803–1808.
Dalton’s
Atomic
Theory
Every
element
is
composed
of
extremely
small
indestructible
particles
called
atoms
Atoms
of
any
one
element
are
all
similar
but
they
differ
from atoms
of
another
element.
Atoms
of
each element
are
fundamental particles,
have
a
characteristic
mass
but do not
have
any
structure.
Atoms
of
various
elements
take
part
in
a chemical
reaction
to
form
compound.
In
any
compound,
the
relative
number
and
kinds
of
atoms are
constant.
Emission
spectrum
Absorptions
spectrum
It
gives
bright
lines
(colored
on
the
dark
background.
Radiations
from
emitting
source
are
analyzed
by
the
spectroscope.
It
may
be
continuous
(if
source
emits
white
light)
and
may
be
discontinuous
(if
the
source
emits
colored
light).
It
gives
dark
lines
on
the
bright
background.
It is
observed when the
white
light is passed through
the
substance
and the
transmitted
radiations
are
analyzed by
the
spectroscope
These
are
always
discontinuous.
ATOMIC
SPECTRA
OF
HYDROGEN
Atomic Spectra of Hydrogen
BOHR’S
ATOMIC
MODEL
The
atom
has a nucleus
where
all the
protons
and
neutrons are present.
The
size
of
the nucleus
is
very
small.
It
is present
at the
center
of
the
atom.
Negatively charged electrons are revolving around
the nucleus.
When
the
electron
remains
in
any
one
of
the
stationary
orbits,
it
does
not
lose
energy.
Each
stationary
orbit
is
associated
with
a
definite
amount
of
energy
Limitations
of
Bohr’s
Model
It
does
not
explain
the
spectra
of
multi-electron
atoms.
.
Bohr’s
theory
does not explain the
fine
spectra
of
even
the
hydrogen
atom.
Spectral lines split into
a
group
of
inner lines
under
the
influence
of
magnetic field
(Zeeman effect) and
electric
field
(Stark
effect); but,
Bohr’s
theory
does
not explain this.
Bohr’s
theory
is
nt
in
agreement
with
Heisenberg’s
uncertainty
principle.
Principal Quantum
Number
This
is
denoted
by
n, an
integer.
The
values
of
n
are from
1
to
n.
n
=
1 K Shell
n’
represents
the
major
energy
shell
to
which
an
electron
belongs.
The
values
of
‘n’
signify
the
size
and
energy
level
of
major energy
shells.
Angular
momentum
can be
calculated
using
principal
quantum
number.
As
the
value
of
‘n’
increases,
the
energy
of
the
electron
increases
and
thus,
the
electron
is
less
tightly
held
with
nucleus.
Azimuthal
Quantum
Number
This
is
denoted
by
l
.
The
values
of
l
are
from
0
to
(n
−
1)
l
=
0,
s-sub-shell,
spherical
l
=
1,
p-sub-shell,
dumbbell
For
a
given value
of
n,
total values
of
‘
l
’
are
n.
The
values
of
l
signify
the
shape
and
energy level
of
sub-shells in
a
major energy
shell.
The
angular
momentum
of
an
electron in
an
orbital
is
given
by
nh/2
.
The
energy
level
for
sub-shells
of
a
shell shows
the
order:
s
<
p <
d <
f
Magnetic
Quantum
Number
Denoted
by
m
l
,
an
integer.
The
values
of
m
l
lie
from
±
l
through
zero.
Total
values
of
m
l
for
a
given
value
of
n
=
n
2
.
Total
values
of
m
l
for
a
given
value
of
l
=
(2
l
+
1)
The
values
of
m
l
signify
the
possible
numbers
of
orientations
of
a
sub-shell.
In
the absence
of
magnetic field,
the
three
p-orbitals
are equivalent in energy
and
are said to
be
threefold
degenerate, i.e. sub sub-shell
(orbitals) having
same
energy
level
are
known
as
degenerate
orbitals
.
Spin Quantum
Number
The
v
alues
o
f
m
s
a
r
e
+ half and
–
half.
The
values
of
ms signify
the
direction
of
rotation
or
spin
of
an
electron
in
its
axis during
its motion.
Number
of
radial
nodes
=
(n
−
l
−
1)
Number
of
angular
nodes
=
l
Total
number
of
nodes
=
(n
−
l
)
Number
of
nodal
planes
=
l
PAULI’S
EXCLUSION
PRINCIPLE
The
principle
states
that
no
two
electrons
in
an
atom
can
have
the
same
set
of
all
the
numbers.
In
other
words,
no
orbital
can have
more
than two electrons.
Conclusion:
(a)
The
maximum capacity
of
a
main energy
shell is
equal
to
2n
2
electrons.
(b)
The
maximum capacity
of
a
sub-shell is
equal
to
2(2
l
+
1) electrons.
(c)
Number
of
sub-shells in
a
main energy shell
is
equal
to
the
value
of
n.
(d)
Number
of
orbitals
in
a
main
energy
shell
is
equal
to
n
2
.
(e)
One
orbital
cannot
have
more
than
two
electrons.
If
two
electrons
are
present,
their
spins
should
be
in
opposite directions.
AUFBAU
PRINCIPLE
.
The
sub-shell
of the
lowest
energy
is filled
up
first,
then the next
sub-shell
of higher energy
starts
filling.
The
sequence in
which
various
sub-shells
are
filled
is
the following:
1s,
2s, 2p, 3s, 4s, 3d, 5s, 4d, 5s, 4d,
5p, 6s, 4d, 5d,
6p, 7s, 5f, 6d, 7p
HUND’S
RULE
OF
MAXIMUM
MULTIPLICITY
It states
that electrons are distributed among the
orbitals
of
sub-shell in such
a way as to give the
maximum
number
of
unpaired
electrons
with
parallel
spins.
This
means
that
the
orbitals
available
in
a
sub-shell
are
first
filled
singly
before they
begin to pair
i.e.
the pairing of electrons occurs
with the
introduction
of the
second
electron
in
the
s-orbital,
the
fourth
electron
in
the
p-orbitals,
the
sixth
electron
in
the
d-orbitals
and
the
eighth
electron
in
the
f-orbitals.
THANK YOU
Exploring the evolution of atomic theory from ancient times to John Dalton's contributions, the concept of indivisible atoms forming elements, atomic spectra of hydrogen, and Bohr's atomic model. Delve into the limitations of Bohr's model and the complexities of multi-electron atoms.
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Arts,Science and Commerce College Mokhada ATOMIC STRUCTURE
ATOMIC STRUCTURE 1.INTRODUCTION The word atom in Greek means indivisible, i.e. an ultimate particle which subdivided. This idea of all matter ultimately consisting of extremely conceived by ancient philosophers. The old concept was put on firm footing by John Dalton with his atomic theory that was developed by him during the years 1803 1808. cannot be further small Indian particles and was Greek
Daltons Atomic Theory Every element is composed of extremely small indestructible particles called atoms Atoms of any one element are all similar but they differ from atoms of another element. Atoms of each element are fundamental particles, have a characteristic mass but do not have any structure. Atoms of various elements take part in a chemical reaction to form compound. In any compound, the relative number and kinds of atoms are constant.
ATOMIC SPECTRA OF HYDROGEN Emission spectrum Absorptions spectrum It gives bright lines (colored on the dark background. Radiations from emitting source are analyzed by the spectroscope. It gives dark lines on the bright background. It is observed when the white light is passed through the substance and the transmitted radiations are analyzed by the spectroscope These are always discontinuous. It may be continuous (if source emits white light) and may be discontinuous (if the source emits colored light).
Atomic Spectra of Hydrogen Spectral Series Appearing Region Value of n1 Value ofn2 Lyman series Balmer series Paschen series Brackett series Pfund series Humphrey series Ultraviolet region Visible region Infrared region Infrared region Infrared region Far-infrared region 1 2 3 4 5 6 2, 3, 4, 5, .. 3, 4, 5, 6, .. 4, 5, 6, 7, .. 5, 6, 7, 8, .. 6, 7, 8, 9, .. 2, 3, 4, 5, ..
BOHRS ATOMIC MODEL The atom has a nucleus where all the protons and neutrons are present. The size of the nucleus is very small. It is present at the center of the atom. Negatively charged electrons are revolving around the nucleus. When the electron remains in any one of the stationary orbits, it does not lose energy. Each stationary orbit is associated with a definite amount of energy
Limitations of Bohrs Model It does not explain the spectra of multi-electron atoms. . Bohr s theory does not explain the fine spectra of even the hydrogen atom. Spectral lines split into a group of inner lines under the influence of magnetic field (Zeeman effect) and electric field (Stark effect); but, Bohr s theory does not explain this. Bohr s theory isnt in agreement with Heisenberg s uncertainty principle.
Principal Quantum Number This is denoted by n, an integer. The values of n are from 1 to n. n = 1 K Shell n represents the major energy shell to which an electron belongs. The values of n signify the size and energy level of major energy shells. Angular momentum can be calculated using principal quantum number. As the value of n increases, the energy of the electron increases and thus, the electron is less tightly held with nucleus.
Azimuthal Quantum Number This is denoted by l. The values of l are from 0 to (n 1) l = 0, s-sub-shell, spherical l = 1, p-sub-shell, dumbbell For a given value of n, total values of l are n. The values of l signify the shape and energy level of sub-shells in a major energy shell. The angular momentum of an electron in an orbital is given by nh/2 . The energy level for sub-shells of a shell shows the order: s < p < d < f
Magnetic Quantum Number Denoted by ml, an integer. The values of mllie from l through zero. Total values of mlfor a given value of n = n2. Total values of mlfor a given value of l = (2l + 1) The values of mlsignify the possible numbers of orientations of a sub-shell. In the absence of magnetic field, the three p-orbitals are equivalent in energy and are said to be threefold degenerate, i.e. sub sub-shell (orbitals) having same energy level are known as degenerate orbitals.
Spin Quantum Number The values of ms are + half and half. The values of ms signify the direction of rotation or spin of an electron in its axis during its motion. Number of radial nodes = (n l 1) Number of angular nodes = l Total number of nodes = (n l) Number of nodal planes = l
PAULIS EXCLUSION PRINCIPLE The principle states that no two electrons in an atom can have the same set of all the numbers. In other words, no orbital can have more than two electrons. Conclusion: (a)The maximum capacity of a main energy shell is equal to 2n2electrons. (b)The maximum capacity of a sub-shell is equal to 2(2l + 1) electrons. (c) Number of sub-shells in a main energy shell is equal to the value of n. (d)Number of orbitals in a main energy shell is equal to n2. (e)One orbital cannot have more than two electrons. If two electrons are present, their spins should be in opposite directions.
AUFBAU PRINCIPLE . The sub-shell of the lowest energy is filled up first, then the next sub-shell of higher energy starts filling. The sequence in which various sub-shells are filled is the following: 1s, 2s, 2p, 3s, 4s, 3d, 5s, 4d, 5s, 4d, 5p, 6s, 4d, 5d, 6p, 7s, 5f, 6d, 7p
HUNDS RULE OF MAXIMUM MULTIPLICITY It states that electrons are distributed among the orbitals of sub-shell in such a way as to give the maximum number of unpaired electrons with parallel spins. This means that the orbitals available in a sub-shell are first filled singly before they begin to pair i.e. the pairing of electrons occurs with the introduction of the second electron in the s-orbital, the fourth electron in the p-orbitals, the sixth electron in the d-orbitals and the eighth electron in the f-orbitals.
