Back Back The Discovery of Atomic Structure Assign. #4 Bires, 2002 Anyone who says that they can contemplate quantum mechanics without becoming dizzy has not understood the concept in the least. -Niels Bohr Slide 1 Atomic History Back Back
The Greek philosopher Democritus (400BC) coined the term atomon which means that which cannot be divided. Idea of an indivisible thing that made up all matter was refined by colorblind chemist John Dalton in 1803. Bires, 2002 Slide 2 Daltons Atomic Theory Back Back
1. All matter is made of indestructible and indivisible atoms. 2. Atoms of a given element have identical physical and chemical properties. (all atoms of X will behave the same anywhere) 3. Different atoms have different properties. (X behaves differently than Y) 4. Atoms combine in whole-number ratios to form compounds. (two Hs and one O = Water (H2O) 5. Atoms cannot be divided, created or destroyed in chemical reactions. Bires, 2002 Slide 3 Daltons Atom
Bires, 2002 Back Back Slide 4 The Laws: Back Back Constant Composition: Ratios of atoms in a compound is constant for that compound. Conservation of Mass: Mass is not created or destroyed in a chemical reaction. Multiple Proportions: Since atoms bond in
small, whole number ratios to form compounds, their masses are small whole number ratios. Bires, 2002 Slide 5 J. J. Thomson Back Back Dalton had no experimental evidence for his theory, so scientists began working to provide evidence for the existence of atoms. J. J. Thomson set up a cathode ray tube and began using magnets to study the charge that was being emitted in the tube.
The beam bent when placed next to a magnet, so the atom must have negative charges, which Thomson called electrons. Bires, 2002 Slide 6 Back Back Beam is attracted to positive magnet and repelled by a negative magnet Bires, 2002
Slide 7 Back Back Thomsons Plum Pudding Model Thomsons negative charges in a sea of positive charge Bires, 2002 Slide 8
Millikans Oil Drop Experiment Back Back We now know the existence of the electron, but what is its charge? Millikans Oil Drop Experiment was engineered to precisely tell us the charge of a single electron. Thomsons experiment had determined the charge to mass ratio (1.76 x 108 C/g), but the exact charge was still
unknown. Bires, 2002 Slide 9 Millikans Experiment By varying the voltage and the amount of electrons, he was able to determine the specific charge of the Bires, 2002
Back Back Slide 10 Back Back Bires, 2002 Slide 11 Millikans Discovery Back Back
Millikans classic oil-drop experiment allowed the charge of a single electron to be determined: 1.60 x 10-19 C. Knowing the charge and the charge to mass ratio from Thomson, the mass could be determined: 19 1.60 x10 C 28 melectron 9.10 x10 g 8 1.76 x10 C / g Bires, 2002
Slide 12 Ernest Rutherford Back Back While studying radioactive elements, New Zealander Physicist Ernest Rutherford found that radioactive alpha particles deflected when fired at a very thin gold foil. This was known as the gold foil experiment, and it suggested that the atom was not a hard sphere as thought, but was mostly space, with a small concentration of mass. This concentration of mass became known as
the nucleus. Link to experiment Bires, 2002 Slide 13 The Bohr Model Back Back Niels Bohr, (a student of Rutherford) rebuilt the model of the atom placing the electrons in energy levels. Bohr was one of the founders of quantum physics a discipline that states that energy can be given off in small packets or quanta of
specific size. More of this theory and the Bohr model to come in future chapters! Bires, 2002 Slide 14 Adding the Neutrons Back Back James Chadwick, proved the existence of massive, neutral particles. These particles came to be called neutrons. This completed our model of the atom that still
remains the accepted model (with more modifications to come!). Bires, 2002 Slide 15 The Modern Model Back Back Democritus and Daltons atom electron
Thompsons electrons neutron Rutherfords space proton Bohrs energy levels (not to scale) Bires, 2002 Chadwicks neutrons Slide 16
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