Atomic Theory. Developing the Nuclear Model of the Atom. Saturday, January 20, 18
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1 Atomic Theory Developing the Nuclear Model of the Atom
2 Democritus Theory: Atom, the indivisible particle c. 300 BC
3 Democritus Problem: No scientific evidence c. 300 BC
4 Dalton Theory: The solid sphere model Atoms are seen as solid indestructible spheres c. 1800
5 Dalton Supports the law of conservation of mass, matter cannot be created or destroyed. Problem: Doesn t explain the behavior of substances in chemical reactions c. 1800
6 J. J. Thomson Theory: The Raisin Bun Model Atoms are positively charged spheres with negatively charged electrons distributed throughout c. 1850
7 J. J. Thomson Experiments using a cathode ray tube lead to the discovery of the negative particles (later termed electrons) c. 1850
8 Rutherford and Chadwick Theory: The Planetary Model Existence of a nucleus containing positively charged protons surrounded mostly by empty space and electrons c c. 1932
9 Rutherford s Gold Foil Experiment Directed a single beam of alpha particles towards a piece of gold foil.
10 Rutherford s Gold Foil Experiment Expected Results: High speed alpha particle will pass straight through the gold foil.
11 Rutherford s Gold Foil Experiment Achieved Results: Majority of the alpha particles pass through but a small number are deflected at large angles or even reflected.
12
13 Rutherford s Gold Foil Experiment Conclusion: The atom is made up of mainly empty space with a small massive region of concentrated positive charge.
14 Rutherford s Gold Foil Experiment This dense core was termed the nucleus.
15 Rutherford s Gold Foil Experiment Problem: A core made up of only positives should break apart due to repulsion.
16 Chadwick In 1932 using radiation from polonium discovered the neutrons. Neutrons act as the glue holding the nucleus together.
17 Electromagnetic Radiation The visible section of the electromagnetic spectrum (the part that we can see) is called the continuous spectrum because the colours are indistinct.
18 Atomic Spectra Instead of emitting energy as a continuous spectrum, when electrons give off energy they do so in the form of a distinct line spectra.
19 Bohr s Model Bohr proposed a new model to explain the line spectra of hydrogen. It was similar to Rutherford s but imposed restrictions on electrons. c. 1913
20 Bohr s Model 1) The atom has only specific allowable energy levels (termed stationary sites). 2) While in one of it s stationary sites an electron does not emit energy. 3) An atom changes stationary sites by emitting or absorbing specific amounts of energy.
21 Bohr s Model Bohr based some of his theory on the research by Planck. Planck stated that matter emitted energy in distinct indivisible packets called quanta.
22 Bohr s Model Therefore the energy associated with the line spectrum of hydrogen corresponds to the energy of an electron as it moves to higher or lower energy levels.
23 Bohr s Model When an atom is exposed to energy the electron absorbs photons and is said to move to an excited state.
24 Bohr s Model An atom has all electrons in the lowest energy levels, it is said to be in the ground state.
25 Bohr s Model These energy transitions were used to designate allowed levels of hydrogen.
26 Bohr s Model n is referred to as the principal quantum number.
27 Bohr s Model Problem: Bohr s model can only explain the line spectra produced by one electron systems.
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