Structure of atom

SHARDA PUBLIC SCHOOL, ALMORA
1
Structure of Atom
Class XI
Subject Expert
Dr. Tanuja Nautiyal

Structure of Atom
Atom is the smallest indivisible particle of the
matter.
Atom is made of
Electron (e)
Proton (p)
Neutrons (n)
SHARDA PUBLIC SCHOOL, ALMORA 2

Structure of Atom
Discovery J. J. Thomson (1869) Goldstein (1886) Chadwick (1932)
Nature of charge Negative Positive Neutral
Amount of charge 1.6 × 10−19 C 1.6 × 10−19 C −
Mass 9.11 × 10−31kg 1.672 × 10−27 kg 1.674 × 10−27 kg
ELECTRON PROTON NEUTRON

Structure of Atom
 Nucleus was discovered by Rutherford in 1911.
 Atomic number (Z) : the number of protons or electrons
present in the nucleus (Moseley 1913).
 Mass Number (A) : Sum of the number of protons or
electrons and neutrons present in the nucleus.
2He4
No. of electrons or protons (Z)= 2
No. of electrons and neutrons (A) = 4

Structure of Atom
Wavelength, frequency and wave velocity are
related to each other by
c = vλ
where c = velocity in light = 3.0 × 10−8 m/s
v = frequency of s−1 or Hz
λ = wavelength in metres
Wave number ( 𝑣) is the reciprocal of wavelength
𝑣 = 1/λ

Planck’s quantum theory
According to Planck’s quantum theory, the energy is emitted or
absorbed not continuously but discontinuously in the form of
energy packets called quanta.
A quantum of light is called photon. The energy of a quantum is
where h = Planck’s constant,
v = frequency of radiation.
E = hv

The line spectrum of hydrogen consists of
 Lyman Series (in UV region)
 Balmer series (visible region)
 Paschen,
 Brackett
 Pfund series (IR region).

The wave number of lines can be calculated by the following
relation :
 R = Rydberg’s constant = 109677 cm−1
 For, Lyman series : n1 = 1, n2 = 2, 3, 4, ..........
 Balmer series : n1 = 2, n2 = 3, 4, 5, ..........
 Paschen series : n1 = 3 and n2 = 4, 5, 6 ..........
 Brackett series : n1 = 4 and n2 = 5, 6, 7, ..........
 Pfund series : n1 = 5 and n2 = 6, 7, 8, ..........
𝒗= R.
𝟏
𝒏
𝟐
𝟏
−
𝟏
𝒏
𝟐
𝟐

The energy of electron in hydrogen atom is given by :
m = mass of electron, e = charge on electron, Z = atomic number
of element
The radius of the nth orbital
𝐫 =
𝟐𝛑 𝟐 𝐦𝐙 𝟐 𝐞 𝟒
𝐧 𝟐 𝐡 𝟐
𝒓 𝒏 =
𝟎. 𝟓𝟐𝟗 𝑨 𝟎 2
𝒁

For hydrogen atom, energy of electron in nth orbit is
E=
−1.312 𝑋 106 𝑍2
𝑛2 J mol-1 =
−2.178 𝑋 10−18 𝑍2
𝑛2 atom-1 =
−13.60 𝑍2
𝑒
𝑛2
The lowest energy state of an electron in atom is called ground state (n
= 1), when an electron absorb energy, it jumps to higher energy level
called excited state, (first excited state n = 2 for H).
• The energy absorbed or emitted during electronic transition is given
by the difference of the energies of two levels, i.e.,
E2 – E1 = – 2.18 × 10–18 1
𝑛12 −
1
𝑛22 J/ atom such as n2 > n1

Photoelectric effect
When radiation with certain minimum frequency (v0), called threshold
frequency, strike the surface of a metal, electrons (called photoelectrons) are
ejected from the surface. With this frequency, the kinetic energy of the
photoelectrons ejected is zero.
However, if the incident radiation having frequency v > v0, the difference of
energy (hv − hv0) is converted into kinetic energy of the photoelectrons i.e.,
The minimum energy hv0 required for emission of photoelectrons is called
threshold energy or work function. No photoelectric effect is shown if
incident frequency is less than v0 even if intensity of a radiation is increased.
However, number of photoelectrons ejected is proportional to the intensity of
incident radiation. mv = hv - hv0
𝟏
𝟐
𝐦𝐯 𝟐 = hv – hv0

de Broglie equation
According to de Broglie concept, all material particles (microscopic as
well as macroscopic) possess wave character as well as particle
character. The wave associated with a material particle is called de
Broglie wave or matter wave.
The relationship between the wavelength (λ) of the wave and the mass
(m) of the material particle moving with a velocity í is called de Broglie
equation. It is given by
where h is Planck’s constant and p is momentum of the particle.
The wave nature of electron has been confirmed by Davisson and
Germer’s experiment whereas the particle nature is confirmed by
scintillation method as well as by the photoelectric effect.
λ=
𝒉
𝒎𝒗
=
𝒉
𝑷

Heisenberg’s uncertainty Principle
It states that ‘‘It is impossible to measure simultaneously the position
and momentum of a microscopic particle with absolute accuracy. If
one of them is measured with greater accuracy, the other becomes
less accurate. The product of their uncertainties is always equal to or
greater than h/ 4π.
Mathematically
Where Δ x = uncertainty in position,
Δ p = uncertainty in momentum
de Broglie concept as well as uncertainty principle have no significance
in everyday life because they have significance only for microscopic
particles but we come across macroscopic bodies in everyday life.
Δ x.Δp ≥
𝒉
𝒎𝒗

Quantum Numbers
Principal Quantum Number
Azimuthal Quantum Number
Magnetic Quantum Number
Spin Quantum Number

Quantum numbers
The four quantum numbers provide the following
information :
Principal quantum number (n)
n = 1, 2, 3, 4, .........∞
It identifies shell, determines sizes and energy of
orbitals and number of orbitals in the nth shell
which is equal to n2.

Quantum numbers
Azimuthal quantum number (l)
For a given value of n, it can have n values ranging from 0 to (n − 1). It
identifies subshell, determines the shape of orbitals, energy of orbitals
in multi-electron atoms along with principal quantum number and
orbital angular momentum, i.e., ( 𝑙 𝑙 + 1 ) h/2π. The number of
orbitals in a subshell = 2l + 1.
Subshell notation s p d f g
Value of ‘l’ 0 1 2 3 4
Number of orbitals 1 3 5 7 9

(3) Magnetic orbital quantum number (ml)
For a given value of ‘l’, ml has a total of (2l + 1) values ranging
from −l to +l including ‘0’. It determines the orientation of
orbital.
(4) Spin quantum number (s)
It can take the values of +½ or −½ and determines the
orientation of spin.

Pauli’s Exclusion Principle
 Pauli’s Exclusion Principle states that ‘‘No two electrons in an
atom can have the same set of four quantum numbers.’’ Two
electrons can have same values for n, l and ml provided their
spins are opposite (ms is different). An orbital can have at the
most two electrons if they have opposite spins.

Hund’s Rule of maximum Multiplicity
Hund’s Rule of maximum Multiplicity states
that ‘‘The electrons start pairing only when all
the degenerate orbitals of a subshell are singly
occupied with parallel spins.’’
e.g., N : 1s2, 2s2, 2px
1, 2py
1, 2pz
1.

Aufbau Principle
Aufbau Principle states that ‘‘Orbitals are filled up in increasing order of their
energy with the help of Pauli principle and Hund’s rule.’’
1. Orbitals are filled up in the increasing order of their (n + 1) values.
2. If two orbitals have same (n + 1) values, then the one which has lower
value, will be filled up first.
Increasing order of energy :
1s < 2s < 2p < 3s < 3p < 4s < 3d < 4p < 5s < 4d < 5p < 6s
Exception of Aufbau principle : Extra stability is associated with the exactly
half-filled and fully-filled orbitals. Thus the p3, p6, d 5, d10, f 7, f 14 etc. have
extra stability, i.e., lower energy and therefore, more stable.

Presentation by
Dr. Tanuja Nautiyal
SHARDA PUBLIC SCHOOL

Structure of atom

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Structure of atom