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Chpt. 2: The Atom.

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Presentation on theme: "Chpt. 2: The Atom."— Presentation transcript:

1 Chpt. 2: The Atom

2 - first proposed that matter was composed of minute particles
History of the Atom Greek Philosophers (400BC): - first proposed that matter was composed of minute particles - believed that the tiny particles of which all matter was composed were so small that nothing smaller was possible ‘Atomos’ Greek word for indivisible - ATOM

3 2. John Dalton (1808): Dalton’s Atomic Theory - All matter is made up of very small particles called atoms All atoms are indivisible. They cannot be broken down into simpler particles Atoms cannot be created or destroyed

4 What is inside the atom???

5 Discovery of the Electron
3. William Crookes – cathode ray tube (1875): - passed electric current through gases at low pressure invisible radiation that caused the glass to glow came from *cathode (-) called cathode rays showed existence of this radiation by placing Maltese Cross inside the tube *Note: Cathode = plate connected to negative end of battery Anode = plate connected to positive end of battery ,


7 4. J.J Thomson – cathode ray tube experiments (1897):
devised experiment to investigate if cathode rays consisted of charged particles cathode rays attracted up towards positive plate (anode) => consisted of negatively charged particles hence cathodes are streams of negatively charged particles called electrons Definition: cathode rays are streams of negatively charged particles called electrons

8 + Thomson’s Experiment Voltage source
Passing an electric current makes a beam appear to move from the negative to the positive end

9 Thomson’s Experiment Voltage source
+ - By adding an electric field he found that the moving pieces were negative

10 Further experiment: - he found electrons were also deflected in magnetic field found ratio of charge to mass of the electron (e/m): (electrical charge of electron) (mass of electron) = 1.76 x 108 coulombs = 1 gram of electrons *Note: In 1891 George Stoney proposed that the smallest amount of electric charge be called an electron.


12 Dough = positive charge
Thomson's ‘Plum Pudding Model’ of the Atom (1898): Proposed that since atoms are neutral each one consists of: - a sphere of positive charge - electrons embedded randomly Dough = positive charge Raisins = electrons

13 5. Robert Millikan (1909): - Experiment to measure size of charge on electron – Oil Drop Experiment - Charge of one electron = 1.6 x coulomb THUS…. Mass of e- = x 10-31g

14 Discovery of radiation led to the use of alpha particles in experiments
Alpha particles are positively charged particles produced by certain radioactive substances

15 Rutherford discovered the nucleus and the proton
6. Ernest Rutherford (1909): Rutherford discovered the nucleus and the proton

16 Rutherford's Gold Foil Experiment
- bombarded tin foils of gold with alpha (α) particles - If plum pudding model was correct he expected: The alpha particles to pass through without changing direction very much Fluorescent Screen Gold Foil Lead block Uranium

17 What He Got!!!!! *Note: Detector flashes - of light produced when α particles strike zinc/sulphite screen

18 Rutherford’s Gold Foil Experiment
Results Most alpha particles passed straight through undeflected Some were deflected at wide angles Few deflected back along own path Explanation/Conclusion Atom mainly empty space occupied by electrons (negative) Both the mass and positive charge were concentrated in a small dense core which he called the nucleus

19 Rutherford – discovery of protons (1924):
Light atoms (oxygen, nitrogen) were bombarded with alpha particles - small POSITIVE charged particles were given off This did not occur with heavier metals e.g. gold Explanation – alpha particles were breaking up the nuclei of the lighter atoms to release positively charged particles referred to these small positive particles as protons

20 7. James Chadwick (1932): Search for a neutral particle to cement the nucleus Bombarded beryllium with alpha particles Produced neutral particles – neutron

21 Properties of Sub-Atomic Particles
Name Relative Charge Relative Mass Location Proton +1 1 nucleus Electron -1 1/1836 (no mass) outside nucleus Neutron

22 Dalton Model of the Atom
Small, indivisible spheres

23 J.J. Thompson’s Model of Atom
Plum Pudding Model, 1896 Thought an atom was like plum pudding

24 Rutherford’s Model of the Atom
Rutherford Model, 1911 Thought atom was mostly empty space: - Nucleus - Electrons (negatively charged) revolving around nucleus

25 Bohr’s Model of the Atom
Neils Bohr, 1913 Similar to Rutherford’s model Thought atom was mostly empty space: - Nucleus in center is dense, positively charge - Electrons in orbits around nucleus

26 (Modern) Quantum Mechanical Model of the Atom
Heisenberg, Schrodinger, many others, ~1926 Think atom is mostly empty space: Nucleus in center is dense, positively charge - Electrons cannot locate

27 Evidence for the existence of small particles!!!
Why is it possible to smell the perfume that someone is wearing from several metres away?

28 Diffusion The process by which molecules of a substance
spread through a solid, liquid or gas. Some examples which can be demonstrated in the lab:- Gas Jar full of air

29 Demonstration Diffusion of ink in water Diffusion of NH3 and HCl
Diffusion of smoke in air

30 Diffusion of NH3 and HCl

31 Ammonia + Hydrogen chloride = Ammonium chloride
Diffusion of NH3 and HCl Word Equation: Ammonia + Hydrogen chloride = Ammonium chloride (Gas) (Gas) (White powdered ring) Chemical Equation: NH3 + HCl = NH4Cl

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