1. Concept of the Atom Democritus 400 B.C.E., Greece Democritus

2. Multiple Proportions O/C 2.39 1.27 O/N 0.58 1.27 2.39 Oxides of Carbon%C%O 2872 4456 Carbonic Acid (1801) Carbonous Acid (1789) Oxides of Nitrogen%N%O 63.3036.70 44.0555.95 29.5070.50 Nitrous Oxide (1810) Nitrous Gas (1810) Nitric Acid (1810) %err 4 5 2 11 5 (1) (~2) (~4) (~2) (1) Rel. integral values consistent with simple atomic ratios

3. Experimental Evidence for the Existence of Atoms John Dalton (1766-1844 ), British Put the pieces together to form the first atomic theory! If elements combined in whole-number ratios, there must be atoms! (matter is made of discrete particles!) Was the first to create a table of atomic weights He was a quaker school teacher at age 12 He was color-blind; never married More than 40 thousand people marched in his funeral procession. Dalton Dalton’s table of elements and their combinations

4. Dalton’s Atomic Theory 1. Elements are composed of atoms solid, tiny, hard, unbreakable, spheres 2. All atoms of a given element are identical all carbon atoms have the same chemical and physical properties 3. Atoms of a given element are different from those of any other element carbon atoms have different chemical and physical properties than sulfur atoms

5. Dalton’s Atomic Theory 4. Atoms of one element combine with atoms of other elements to form compounds (in simple ratios). Law of Constant Composition all samples of a compound contain the same proportions (by mass) of the elements 5. Atoms are indivisible in a chemical process. Reactions only cause a rearrangement of atoms. Law of Conservation of Mass: all atoms present at beginning are present at the end atoms are not created or destroyed, just rearranged atoms of one element cannot change into atoms of another element cannot turn Lead into Gold by a chemical reaction

6. Discovery of the electron “Could anything at first sight seem more impractical than a body which is so small that its mass is an insignificant fraction of the mass of an atom of hydrogen?" -- J.J. Thomson. Joseph John Thomson (1856-1940), British Used the cathode ray tube (modified by Crookes, 1850s) to do experiments that led to the idea of electrons. http://www.chem.uiuc.edu/clcwebsite/catho de.html Electrons are negatively charged particles that exist in an atom Thomson won the Nobel Prize in Physics, 1906 for evidence of electrons as particles. Ironically, his son won the Nobel in 1937 for evidence of electrons as waves (it has been accepted since then that electrons have both wave and particle properties).

7. Plum Pudding Model of the Atom Atoms (matter) is electrically neutral. If electrons are negatively charged, there must be positive charges to balance the electrons (later, protons were discovered by Goldstein). Lord Kelvin (William Thomson, no relation to JJ) JJ Thomson

8. Discovery of the nucleus “All science is either physics or stamp collecting” -Ernest Rutherford Ernest Rutherford (1871-1937), British His famous gold foil experiment proved the existence of the nucleus in atoms and that 1)The nucleus was composed of positive charge (protons). 2)Atoms are mostly empty space Born and raised on a farm in New Zealand Won scholarship to study at Cambridge Became a student of JJ Thomson Performed extensive research in radioactivity Nobel Prize in 1908 in Chemistry Was a great mentor—several of his students also won Nobel Prizes

9. Gold Foil Experiment Rutherford and JJ Thomson (horsing around?)

10. Bohr’s Model This model involves the idea of quantization (developed by Planck): Energy levels (orbits) increase in quantized amounts of energy (discrete—not continuous—amounts of energy) This means the light emitted from excited electrons are not continuous—only certain colors are seen (only QUANTA of energy can be absorbed and released) "We are tracing the description of natural phenomena back to combinations of pure numbers which far transcends the boldest dreams of the Pythagoreans." -- Bohr

11. Wave-Particle Duality Bohr’s model did not explain why electrons do not spiral into the nucleus. (It makes the assumption that this does not occur). It was accepted by physicists that light seemed to behave as both waves and as particles (called photons). This idea is called “Wave-Particle Duality.” Louis de Broglie asked “If light can be wave-like and particle-like, why can’t matter also be wave-like and particle-like?” This led to the concept that electrons can behave as waves and as particles. Prince Louis de Broglie first got a history degree, then went into science. Won the Nobel Prize in physics (1929). His work helped shape quantum mechanics.

12. Electrons as waves Electrons behave like standing (stationary) waves (not traveling waves, like light) Stationary waves are like the waves (vibrations) from plucking a guitar string. There are only certain areas where the waves (electrons) are allowed. The 3-D space where electrons might be is described by orbitals. This is one kind of orbital called a p-orbital

13. Werner Heisenberg, 1901-1976 (Nobel Prize, 1932) The Uncertainty Principle

14. Erwin Schrodinger (Quantum mechanical model of the atom) 1887-1961 (Nobel Prize, Physics, 1933)

15. Orbitals Wave functions determine the sizes and shapes of orbitals Four common orbital types are: s, p, d, f (theoretically, there are an infinite number of orbital types: g, h, I, j, k, etc…) Let’s look at the difference between Bohr’s atom and Schrödinger’s: http://www.colorado.edu/physics/2000/quantumzone/schroedinger.html

16. Light: Waves or Particles?

18. Joseph Louis Gay- Lussac (1809) Oxidation of Sugar, etc. with NaClO 3 Cleans up Lavoisier's Mass Balance 1.9989 volumes of hydrogen per 1.0000 volumes of oxygen Water gives 3.08163 volumes of hydrogen per 1 volume of nitrogen Ammonia gives Alternative to Dalton's Law of Greatest Simplicity http://www.bibliotheque.polytechnique.fr/associations/gaylussac/pages/AssofrGL.html 1804 - 7,016 m (1778-1850)