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Atomic Structure
        ….a brief overview…..
Important Highlights
•   INTRODUCTION
•   RUTHERFORD’S ATOMIC MODEL
•   BOHR’S ATOMIC MODEL
•   DISTRIBUTION OF EXTRA-NUCLEAR
    ELECTRONS IN SHELLS & SUB-SHELLS
•   ELECTRONIC CONFIGURATION OF ATOM
•   WAVE-NATURE OF AN ATOM
•   ATOMIC NUMBER
•   MASS NUMBER BESU SHIBPUR,HOWRAH
Introduction
• ATOM : An atom is the smallest particle of an element, which
    Can not be subdivided.
    Does not exist in free state. But,
    Participate in chemical reaction.

The structure of an atom can be broadly divided into two parts
    Nuclear Parts
    Extra-Nuclear Parts
   Nuclear part basically consist of 2 major particles– protons &
     neutrons. Apart from this there are some more tiny particles
     such as deuteron, neutrino, positron etc.
   Extra-Nuclear parts consists of mainly electrons.
                         BESU SHIBPUR,HOWRAH
Rutherford’s Atomic Model
• Also known as “Planetary Model” of Atom.
K e y F e a tu re s :
• An atom consists of a central nucleus.  This nucleus is
  composed of positively charged protons, and electrically
  uncharged (neutral) neutrons.
• Negatively charged electrons revolve around the nucleus
  in definite orbits.
• The orbits themselves can be at any distance from the
  nucleus.
• In any atom, the number of protons is equal to the number
  of electrons, and hence it is electrically neutral.


                      BESU SHIBPUR,HOWRAH
Drawbacks of Rutherford’s Model
•    It could not explain the stability of the atom. A/c to
    classical theory of mechanics, during uniform revolution, any
    body accelerates, & an accelerating charged particle must
    emit radiation, and lose energy. Due to the fact, the electron
    must emit radiation and lose energy. As a result, the
    electron will follow a spiral path, and ultimately fall into
    nucleus .So, Rutherford has given concept of unstable atom.

• The Rutherford’s model of atom does not say anything about
  the arrangement of electrons in an atom.



                         BESU SHIBPUR,HOWRAH
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                                                     ’
                                    DE             HR
                                         L      BO


                               BESU SHIBPUR,HOWRAH
Bohr’s Atomic Model
The main points of Bohr’s atomic model are….
• Electrons revolve around the nucleus in orbits that have
  fixed radius and energy. So, such orbits are also known
  as stationary orbit ,Energy shells etc.
• The energy of the orbit is related to its size. The lowest
  energy is found in the smallest orbit and its vice-versa.
• Radiation is absorbed or emitted when an electron jumps
  from one orbit to another.




                     BESU SHIBPUR,HOWRAH
Bohr postulated that the angular momentum of the electron is
  quantized as shown…

Where, h=6.626*10^(-34) Js


Then by using simple physical equation he deduced the
  expression for energy,velocity,radius,wavelength,wave-no. etc.

 L=nh/2ᴨ= mvr
 F= Ze*e/r*r=mv*v/r

 Where,L=Angular accn., Z=Atomic number, v=Orbital velocity
         m=mass of electron, n=Principal Quantum Number
         r=Radius of Orbit, h=Planck’s constant=6.626*10^34Js
                             BESU SHIBPUR,HOWRAH
Deduced Formulae:

• Radius, r= (n^2/Z)*0.529 Å

• Energy, E= -(Z^2/n^2)* 13.6 eV

• Wave No.=1/wave-length=R(1/nf2-1/ni2)

• Velocity, v=(Z/n)*21.88*10^5 m/s




                    BESU SHIBPUR,HOWRAH
e.g. Emission of a Quantum:1st Balmer Transition




                    -3.4eV




                  BESU SHIBPUR,HOWRAH
Limitation of Bohr’s Atomic Model
• The Bohr atomic model is applicable only for one-electron
  system. e.g. H, He+, Li++, Be+++ etc.
• The Bohr Model provides an incorrect value for the ground
  state orbital angular momentum.
• It does not predict the relative intensities of spectral lines.
• The Bohr Model does not explain fine structure and hyperfine
  structure in spectral lines.
• It violates the Heisenberg Uncertainty Principle because it
  considers electrons to have both a known radius and orbit.
• It does not explain the Stark’s & Zeeman’s Effect.



                        BESU SHIBPUR,HOWRAH
Concept of shells and subshells
• Shells, n, represents the distance of an electron from
  Nucleus. It is represented by K,L,M,N,O,…for n=1,2,3,4,..
• Shell no., n, also represents the maximum no. of electrons
  accommodated by a particular shell, which is 2n(2). i.e. for
  n=1, First Shell, maximum no. of electrons=2.
  Similarly, for n=2, it’s 8.
              n=3, it’s 18 and so on.

• Subshell represents the traversal path of any electron in
  3D view or, shape of the Orbital. For any Orbit ,n, it’s
  value ranges from 0 to(n-1). It is represented by s,p,d,f,…
  for l=0,1,2,3,…

                       BESU SHIBPUR,HOWRAH
Quantum Numbers of Wave funtions
Quantum #   Symbol     Values              Description

Principal   n          1,2,3,4,…           Size & Energy of orbital

Angular     l          0,1,2,…(n-1)        Shape of orbital
Momentum                for each n

Magnetic    ml         -l…,0,…+l           Relative orientation of orbitals within
                        for each l         same l
Spin        ms         +1/2 or –1/2        Spin up or Spin down

            Angular Momentum Quantum # l           Name of Orbital
                        0                             s (sharp)

                        1                             p (principal)
                        2                             d (diffuse)
                        3                             f (fundamental)
                        4                             g
                                BESU SHIBPUR,HOWRAH
Electronic Configuration
The electrons gather around the nucleus in quantum orbitals
  following four basic rules, called the Aufbau principle.
• no two electrons in the atom will share the same four quantum
  numbers n, l, m, and s. (Pauli’s Exclusion Principle)
• electrons will first occupy orbitals of the lowest energy level.
• orbitals will be filled with the same spin number until all the
  orbitals are filled, before it will begin to fill in the opposite spin.
  (Hund’s Rule of maximum multiplicity)
• (n+l) Rule: electrons will fill orbitals by the sum of the
  quantum numbers n and l. In case equal values of (n+l), orbitals
  with the lower value of n, will be filled first.


                           BESU SHIBPUR,HOWRAH
Electronic Configuration contd.
Hence, Aufbau Principle  Gives order of filling of electrons in
  different subshells. It can be shown as follows….

•   1s2
•   2s22p6
•   3s23p63d10
•   4s24p64d104f14
•   5s25p65d105f14(5g18)
•   6s26p66d106f14(6g18)(6h22)
•   7s27p67d106f14(6g18)(6h22)(7i26)


                            BESU SHIBPUR,HOWRAH
Electronic Configuration contd.
• The electronic configuration of elements generally follows
  Aufbau principle.
• except some cases viz. Cu,Cr type d-block elements(due
  to some stability factor).




                       BESU SHIBPUR,HOWRAH
Wave Nature of an Atom
• Wave–particle duality postulates that, all particles exhibits
  both particle as well as wave characteristics.

• Louis-Victor de Broglie describes the atom considering
  "Dual Properties of Matter”.

• He formulated a hypothesis, claiming that all matter, not just
  light, has a wave-like nature; he related wavelength (denoted
  as λ), and momentum (denoted as p):

                          λ =h/p
This is the generalization of Einstein’s and Planck’s Equation.


                           BESU SHIBPUR,HOWRAH
Atomic Number
• Atomic Number, Z: The number of protons in an atom.
• As atoms are neutral,
So,
    N(p)=N(e)=Z
Where,
 N(p)= number of protons
 N(e)=number of electrons
 Z=Atomic Number



.                  BESU SHIBPUR,HOWRAH
Mass Number
Mass Number: The total numbers of neutrons and
protons in an atom.
So, if we know mass no. and atomic number, we can
find out the number of neutrons in an atom .

Mass Number - Atomic Number=Number of neutrons




                       BESU SHIBPUR,HOWRAH
Notation of an Atom
  Mass Number


                     65
                       Cu
                     29
   Atomic Number




                   BESU SHIBPUR,HOWRAH
References…...
• http://www.answers.com/topic/electron-configuration

• http://www.sparknotes.com/chemistry/fundamentals/atomicstr




                     BESU SHIBPUR,HOWRAH
Thanking You…!
Presented By………
 Navin Kumar
 COMPUTER SCIENCE & TECHNOLOGY
 BENGAL ENGINEERING & SCIENCE UNIVERSITY SHIBPUR, HOWRAH




                     BESU SHIBPUR,HOWRAH
….question please….!!




         BESU SHIBPUR,HOWRAH

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Atomic structure

  • 1. Atomic Structure ….a brief overview…..
  • 2. Important Highlights • INTRODUCTION • RUTHERFORD’S ATOMIC MODEL • BOHR’S ATOMIC MODEL • DISTRIBUTION OF EXTRA-NUCLEAR ELECTRONS IN SHELLS & SUB-SHELLS • ELECTRONIC CONFIGURATION OF ATOM • WAVE-NATURE OF AN ATOM • ATOMIC NUMBER • MASS NUMBER BESU SHIBPUR,HOWRAH
  • 3. Introduction • ATOM : An atom is the smallest particle of an element, which  Can not be subdivided.  Does not exist in free state. But,  Participate in chemical reaction. The structure of an atom can be broadly divided into two parts  Nuclear Parts  Extra-Nuclear Parts Nuclear part basically consist of 2 major particles– protons & neutrons. Apart from this there are some more tiny particles such as deuteron, neutrino, positron etc. Extra-Nuclear parts consists of mainly electrons. BESU SHIBPUR,HOWRAH
  • 4. Rutherford’s Atomic Model • Also known as “Planetary Model” of Atom. K e y F e a tu re s : • An atom consists of a central nucleus.  This nucleus is composed of positively charged protons, and electrically uncharged (neutral) neutrons. • Negatively charged electrons revolve around the nucleus in definite orbits. • The orbits themselves can be at any distance from the nucleus. • In any atom, the number of protons is equal to the number of electrons, and hence it is electrically neutral. BESU SHIBPUR,HOWRAH
  • 5. Drawbacks of Rutherford’s Model • It could not explain the stability of the atom. A/c to classical theory of mechanics, during uniform revolution, any body accelerates, & an accelerating charged particle must emit radiation, and lose energy. Due to the fact, the electron must emit radiation and lose energy. As a result, the electron will follow a spiral path, and ultimately fall into nucleus .So, Rutherford has given concept of unstable atom. • The Rutherford’s model of atom does not say anything about the arrangement of electrons in an atom. BESU SHIBPUR,HOWRAH
  • 6. RU TH ER FO E L RD ’S MOD AT C OM O MI IC MO S AT ’ DE HR L BO BESU SHIBPUR,HOWRAH
  • 7. Bohr’s Atomic Model The main points of Bohr’s atomic model are…. • Electrons revolve around the nucleus in orbits that have fixed radius and energy. So, such orbits are also known as stationary orbit ,Energy shells etc. • The energy of the orbit is related to its size. The lowest energy is found in the smallest orbit and its vice-versa. • Radiation is absorbed or emitted when an electron jumps from one orbit to another. BESU SHIBPUR,HOWRAH
  • 8. Bohr postulated that the angular momentum of the electron is quantized as shown… Where, h=6.626*10^(-34) Js Then by using simple physical equation he deduced the expression for energy,velocity,radius,wavelength,wave-no. etc.  L=nh/2ᴨ= mvr  F= Ze*e/r*r=mv*v/r  Where,L=Angular accn., Z=Atomic number, v=Orbital velocity m=mass of electron, n=Principal Quantum Number r=Radius of Orbit, h=Planck’s constant=6.626*10^34Js BESU SHIBPUR,HOWRAH
  • 9. Deduced Formulae: • Radius, r= (n^2/Z)*0.529 Å • Energy, E= -(Z^2/n^2)* 13.6 eV • Wave No.=1/wave-length=R(1/nf2-1/ni2) • Velocity, v=(Z/n)*21.88*10^5 m/s BESU SHIBPUR,HOWRAH
  • 10. e.g. Emission of a Quantum:1st Balmer Transition -3.4eV BESU SHIBPUR,HOWRAH
  • 11. Limitation of Bohr’s Atomic Model • The Bohr atomic model is applicable only for one-electron system. e.g. H, He+, Li++, Be+++ etc. • The Bohr Model provides an incorrect value for the ground state orbital angular momentum. • It does not predict the relative intensities of spectral lines. • The Bohr Model does not explain fine structure and hyperfine structure in spectral lines. • It violates the Heisenberg Uncertainty Principle because it considers electrons to have both a known radius and orbit. • It does not explain the Stark’s & Zeeman’s Effect. BESU SHIBPUR,HOWRAH
  • 12. Concept of shells and subshells • Shells, n, represents the distance of an electron from Nucleus. It is represented by K,L,M,N,O,…for n=1,2,3,4,.. • Shell no., n, also represents the maximum no. of electrons accommodated by a particular shell, which is 2n(2). i.e. for n=1, First Shell, maximum no. of electrons=2. Similarly, for n=2, it’s 8. n=3, it’s 18 and so on. • Subshell represents the traversal path of any electron in 3D view or, shape of the Orbital. For any Orbit ,n, it’s value ranges from 0 to(n-1). It is represented by s,p,d,f,… for l=0,1,2,3,… BESU SHIBPUR,HOWRAH
  • 13. Quantum Numbers of Wave funtions Quantum # Symbol Values Description Principal n 1,2,3,4,… Size & Energy of orbital Angular l 0,1,2,…(n-1) Shape of orbital Momentum for each n Magnetic ml -l…,0,…+l Relative orientation of orbitals within for each l same l Spin ms +1/2 or –1/2 Spin up or Spin down Angular Momentum Quantum # l Name of Orbital 0 s (sharp) 1 p (principal) 2 d (diffuse) 3 f (fundamental) 4 g BESU SHIBPUR,HOWRAH
  • 14. Electronic Configuration The electrons gather around the nucleus in quantum orbitals following four basic rules, called the Aufbau principle. • no two electrons in the atom will share the same four quantum numbers n, l, m, and s. (Pauli’s Exclusion Principle) • electrons will first occupy orbitals of the lowest energy level. • orbitals will be filled with the same spin number until all the orbitals are filled, before it will begin to fill in the opposite spin. (Hund’s Rule of maximum multiplicity) • (n+l) Rule: electrons will fill orbitals by the sum of the quantum numbers n and l. In case equal values of (n+l), orbitals with the lower value of n, will be filled first. BESU SHIBPUR,HOWRAH
  • 15. Electronic Configuration contd. Hence, Aufbau Principle  Gives order of filling of electrons in different subshells. It can be shown as follows…. • 1s2 • 2s22p6 • 3s23p63d10 • 4s24p64d104f14 • 5s25p65d105f14(5g18) • 6s26p66d106f14(6g18)(6h22) • 7s27p67d106f14(6g18)(6h22)(7i26) BESU SHIBPUR,HOWRAH
  • 16. Electronic Configuration contd. • The electronic configuration of elements generally follows Aufbau principle. • except some cases viz. Cu,Cr type d-block elements(due to some stability factor). BESU SHIBPUR,HOWRAH
  • 17. Wave Nature of an Atom • Wave–particle duality postulates that, all particles exhibits both particle as well as wave characteristics. • Louis-Victor de Broglie describes the atom considering "Dual Properties of Matter”. • He formulated a hypothesis, claiming that all matter, not just light, has a wave-like nature; he related wavelength (denoted as λ), and momentum (denoted as p): λ =h/p This is the generalization of Einstein’s and Planck’s Equation. BESU SHIBPUR,HOWRAH
  • 18. Atomic Number • Atomic Number, Z: The number of protons in an atom. • As atoms are neutral, So, N(p)=N(e)=Z Where,  N(p)= number of protons  N(e)=number of electrons  Z=Atomic Number . BESU SHIBPUR,HOWRAH
  • 19. Mass Number Mass Number: The total numbers of neutrons and protons in an atom. So, if we know mass no. and atomic number, we can find out the number of neutrons in an atom . Mass Number - Atomic Number=Number of neutrons BESU SHIBPUR,HOWRAH
  • 20. Notation of an Atom Mass Number 65 Cu 29 Atomic Number BESU SHIBPUR,HOWRAH
  • 22. Thanking You…! Presented By……… Navin Kumar COMPUTER SCIENCE & TECHNOLOGY BENGAL ENGINEERING & SCIENCE UNIVERSITY SHIBPUR, HOWRAH BESU SHIBPUR,HOWRAH
  • 23. ….question please….!! BESU SHIBPUR,HOWRAH