2. Models of the Atom a Historical Perspective simple atom structure atomic history song

3. Aristotle Early Greek Theories 400 B.C. - Democritus thought matter could not be divided indefinitely. 350 B.C - Aristotle modified an earlier theory that matter was made of four “elements”: earth, fire, water, air. Democritus Aristotle was wrong. However, his theory persisted for 2000 years. fire air water earth This led to the idea of atoms in a void.

4. John Dalton 1800 -Dalton proposed a modern atomic model based on experimentation not on pure reason. All matter is made of atoms. Atoms of an element are identical. Each element has different atoms. Atoms of different elements combine in constant ratios to form compounds. Atoms are rearranged in reactions. His ideas account for the law of conservation of mass (atoms are neither created nor destroyed) and the law of constant composition (elements combine in fixed ratios).

5. Adding Electrons to the Model 1)Dalton’s “Billiard ball” model (1800-1900) Atoms are solid and indivisible. 2)Thompson “Plum pudding” model (1900) Negative electrons in a positive framework. 3)The Rutherford model (around 1910) Atoms are mostly empty space. Negative electrons orbit a positive nucleus. Materials, when rubbed, can develop a charge difference. This electricity is called “cathode rays” when passed through an evacuated tube (movie).movie These rays have a small mass and are negative. Thompson noted that these negative subatomic particles were a fundamental part of all atoms.

6. Ernest Rutherford (movie1, movie2)movie1movie2 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. Radioactive substance path of invisible  -particles Rutherford shot alpha (  ) particles at gold foil. Lead block Zinc sulfide screenThin gold foil

7. Bohr’s model ( movie ) movie Electrons orbit the nucleus in “shells.” Electrons can be bumped up to a higher shell if hit by an electron or a photon of light.

8. Bohr’s model There are 2 types of spectra: continuous spectra and line spectra. It’s when electrons fall back down that they release a photon. sun H He Hg U These jumps down from “shell” to “shell” account for the line spectra seen through spectroscopes (and the colors of neon lights and fireworks).

9. Schrödinger and Heisenberg You can never know exactly where an electron is, but you can predict the orbital using probability (Heisenberg’s Uncertainty Principle). Different energy clouds have different shapes. Quantum mechanical model – electrons are not circling the nucleus like planets, but can be found somewhere in a ‘cloud’ of energy (Bohr’s ‘shells’ = ‘orbitals’) (movie)movie X

10. Models of the Atom Review atomic history song 1900 Thompson electron, cathode ray tube, Plum Pudding Model 1800 Dalton Atomic Theory, Billiard Ball Model 1910 Rutherford nucleus, gold foil experiment 1913 Bohr Electron Shell (planetary) Model 1930 Schrödinger and Electron Cloud Model Heisenberg 400 BC Democritus ‘atom’ = ‘indivisible’ 350 BC Aristotle earth, air, fire, water Timeline of Atomic Structure

12. Atomic numbers, Mass numbers There are 3 types of subatomic particles. We already know about electrons (e – ) & protons (p + ). Neutrons (n 0 ) were also shown to exist (1930s). They have: no charge, a mass similar to protons Elements are often symbolized with their mass number and atomic number E.g. Oxygen: O 16 8 These values are given on the periodic table. For now, round the mass # to a whole number. These numbers tell you a lot about atoms. # of protons = # of electrons = atomic number # of neutrons = mass number – atomic number Calculate # of e –, n 0, p + for Ca, Ar, and Br.

13. 3545358035Br 1822184018Ar 20 4020Ca e–e– n0n0 p+p+ MassAtomic

14. 3 p + 4 n 0 2e – 1e – Li shorthand Bohr - Rutherford diagrams Putting all this together, we get B-R diagrams To draw them you must know the # of protons, neutrons, and electrons (2,8,8,2 filling order) Draw protons (p + ), (n 0 ) in circle (i.e. “nucleus”) Draw electrons around in shells 2 p + 2 n 0 He 3 p + 4 n 0 Li Draw Be, B, Al and shorthand diagrams for O, Na

15. 11 p+ 12 n° 2e – 8e – 1e – Na 8 p+ 8 n° 2e – 6e – O 4 p+ 5 n° Be 5 p+ 6 n° B 13 p+ 14 n° Al

16. Isotopes and Radioisotopes Atoms of the same element that have different numbers of neutrons are called isotopes. Due to isotopes, mass #s are not round #s. Li (6.9) is made up of both 6 Li and 7 Li. Often, at least one isotope is unstable. It breaks down, releasing radioactivity. These types of isotopes are called radioisotopes Q- Sometimes an isotope is written without its atomic number - e.g. 35 S (or S-35). Why? Q- Draw B-R diagrams for the two Li isotopes. A- The atomic # of an element doesn’t change Although the number of neutrons can vary, atoms have definite numbers of protons.

17. 3 p + 3 n 0 2e – 1e – 6 Li 7 Li 3 p + 4 n 0 2e – 1e – For more lessons, visit www.chalkbored.com www.chalkbored.com