1. DEVELOPMENT OF THE ATOMIC MODEL From Democritus to Rutherford Dr, Anilkumar R. Koppalkar S.S.Margol College Shahabad S.S.Margol College Shahabad

2. c.400 B.C. Ancient Greek Philosopy Everything in the universe is made of one or more of the basic “elements:” Everything in the universe is made of one or more of the basic “elements:” Earth, Fire, Water, Air Earth, Fire, Water, Air

3. What makes up the elements? ARISTOTLE ARISTOTLE Matter is infinitely divisible; no matter how small a piece is, it can always be divided into smaller pieces Matter is infinitely divisible; no matter how small a piece is, it can always be divided into smaller pieces DEMOCRITUS DEMOCRITUS There exists a “smallest piece” of matter, which cannot be divided any further. These pieces are called “ατομοσ,” or “atoms” Aristotle Democritus

4. Whose Argument Prevails? Aristotle’s viewpoint enjoyed the support of most of the world because he was more well-known and because Democritus had no evidence to back up his claim since these “atoms” would be too small to see. Aristotle’s viewpoint enjoyed the support of most of the world because he was more well-known and because Democritus had no evidence to back up his claim since these “atoms” would be too small to see.

5. 1803: John Dalton Dalton was an English schoolteacher Dalton was an English schoolteacher Began teaching mathematics and chemistry at the age of 12 Began teaching mathematics and chemistry at the age of 12 Revived the idea of Democritus’ “smallest piece” of matter Revived the idea of Democritus’ “smallest piece” of matter

6. Dalton’s Atomic Model All matter is made of tiny particles called “atoms” All matter is made of tiny particles called “atoms” Atoms are indivisible and indestructible Atoms are indivisible and indestructible Atoms of the same element are identical Atoms of the same element are identical Atoms of different elements differ in some fundamental way Atoms of different elements differ in some fundamental way Atoms combine in simple whole number ratios to form compounds Atoms combine in simple whole number ratios to form compounds

7. Why did people believe Dalton? He had EVIDENCE! He had EVIDENCE! Dalton found that compounds always contained the same mass ratio of one element to another Dalton found that compounds always contained the same mass ratio of one element to another This is now known as the “Law of Definite Proportions” This is now known as the “Law of Definite Proportions” Elements could combine in different ratios, but when they did, they would make different compounds Elements could combine in different ratios, but when they did, they would make different compounds This is now known as the “Law of Multiple Proportions” This is now known as the “Law of Multiple Proportions”

8. So what? These results could only be explained by assuming that matter was made of atoms – tiny building blocks – and that these atoms only came in certain sizes. These results could only be explained by assuming that matter was made of atoms – tiny building blocks – and that these atoms only came in certain sizes. Dalton’s View of an atom

9. Hooray, Dalton! Besides giving us his Atomic Theory, Dalton did much more in the newly- emerging field of chemistry: Besides giving us his Atomic Theory, Dalton did much more in the newly- emerging field of chemistry: He worked with mixtures of gases and determined how the pressure was related to their proportions He worked with mixtures of gases and determined how the pressure was related to their proportions He made a list of all the known elements from lightest to heaviest He made a list of all the known elements from lightest to heaviest

10. 1869: Dmitri Mendeleev Russian chemist Russian chemist Arranged elements in tabular form so that elements with similar properties were in the same column Arranged elements in tabular form so that elements with similar properties were in the same column When listed in order by mass, elements generally repeat properties in groups of 8 (Law of Octaves) When listed in order by mass, elements generally repeat properties in groups of 8 (Law of Octaves)

11. The First Periodic Table Most tables at the time listed elements by mass Most tables at the time listed elements by mass Mendeleev also arranged elements by mass, but left several “holes” in his table and occasionally reversed the order of elements to fit the properties of others in that column Mendeleev also arranged elements by mass, but left several “holes” in his table and occasionally reversed the order of elements to fit the properties of others in that column The “holes” were later filled in with newly discovered elements that had the properties predicted by Mendeleev’s table. The “holes” were later filled in with newly discovered elements that had the properties predicted by Mendeleev’s table. The reason for the reversal of elements was explained later by Henry Moseley, who noted that the elements were in order by atomic number (number of protons) rather than by mass The reason for the reversal of elements was explained later by Henry Moseley, who noted that the elements were in order by atomic number (number of protons) rather than by mass

12. 1897: J.J. Thomson English physicist English physicist Worked with Cathode-Ray Tubes (CRTs) Worked with Cathode-Ray Tubes (CRTs) Credited with the discovery of the electron Credited with the discovery of the electron

13. CRTs Mysterious particles emanated from the cathode end Mysterious particles emanated from the cathode end These particles were deflected by magnetic and electric fields These particles were deflected by magnetic and electric fields They were very small and negatively charged They were very small and negatively charged These particles were called “electrons” and were assumed to be a part of all matter

14. Thomson’s Atomic Model Electrons Positively charged “goo” “Plum-Pudding Model”

15. 1909-11: Robert Millikan Set out to discover the charge of a single electron Set out to discover the charge of a single electron Famous experiment called the “oil-drop experiment” Famous experiment called the “oil-drop experiment” Using his results and the charge-to-mass ratio from Thomson, the mass of an electron was found Using his results and the charge-to-mass ratio from Thomson, the mass of an electron was found

16. Procedure: (1) Oil drop is placed on the dry glass substrate; (2) Solution of surfactant + NaCl is poured in the cuvette; (3) The process of oil drop detachment is recorded by horizontal microscope and video-camera. Scheme of the experimental cell: 1 – glass plate; 2 – oil droplet  1  l; 3 – glass holders; 4 – surfactant solution; 5 – syringe; 6 – cuvette. The Oil Drop Experiment

17. 1910: Ernest Rutherford Expert in radiation Expert in radiation Famous “Gold-Foil Experiment” Famous “Gold-Foil Experiment” Discovered the presence of the nucleus by firing alpha particles at a sheet of gold foil Discovered the presence of the nucleus by firing alpha particles at a sheet of gold foil

18. Ernest Rutherford (movie: 10 min.) Most particles passed through. So, atoms are mostly empty. Some positive  -particles deflected or bounced back! Thus, a “nucleus” is positive & holds most of an atom’s mass. Radioactiv e substance path of invisible  -particles Rutherford shot alpha (  ) particles at gold foil. Rutherford shot alpha (  ) particles at gold foil. Lead block Zinc sulfide screen Thin gold foil

19. Rutherford’s Atomic Model Electrons Nucleus Positively charged Made of “protons” Empty Space

20. 1932: James Chadwick A fellow researcher with Rutherford, Chadwick discovered years later that the nucleus was not made of only one particle – the proton – but of two particles. A fellow researcher with Rutherford, Chadwick discovered years later that the nucleus was not made of only one particle – the proton – but of two particles. This second particle was called the “neutron” because it had no electrical charge This second particle was called the “neutron” because it had no electrical charge

21. HISTORY OF THE ATOM 1913 Niels Bohr studied under Rutherford at the Victoria University in Manchester. Bohr refined Rutherford's idea by adding that the electrons were in orbits. Rather like planets orbiting the sun. With each orbit only able to contain a set number of electrons.

22. Bohr’s Atom electrons in orbits nucleus

23. HELIUM ATOM + N N + - - proton electron neutron Shell What do these particles consist of?

24. ATOMIC STRUCTURE Particle proton neutron electron Charge + ve charge -ve charge No charge 1 1 nil Mass

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