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Early History Early Greeks (Circa 400 BC)

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Presentation on theme: "Early History Early Greeks (Circa 400 BC)"— Presentation transcript:

1 AP Chemistry Unit 2: Atoms, Molecules, Ions History of Atomic Theory – Classic Atomic Experiments

2 Early History Early Greeks (Circa 400 BC)
Theorized of Existence of Atoms (“atomos”)

3 Dark Ages of Chemistry . . . Alchemists

4 AGE OF EXPERIMENTATION
Mid-Late 1700’s AGE OF EXPERIMENTATION

5 Antoine Lavoisier French Chemist Law of Conservation of Mass
“Father of Modern Chemistry”

6 Joseph Proust 1754-1826 French Chemist Law of Definite
Composition/Proportions

7 John Dalton 1766 – 1844 English Chemist
& School Teacher Believed that atoms were not divisible, and that atoms of each element are identical to each other. The Law of Multiple Proportions

8 Dalton’s Atomic Theory
All matter is composed of extremely small particles called atoms. Atoms of a given element are identical in size, mass, and other properties; atoms of different elements differ in size, mass, and other properties. Atoms cannot be subdivided, created, or destroyed. Atoms of different elements can combine in simple, whole-number ratios to form chemical compounds. In chemical reactions, atoms are combined, separated, or rearranged. **The Atomic Theory was not accepted until the late 1800s. **There are two errors with The Atomic Theory.

9 Models of The ATOM Dalton: Solid Sphere

10 JJ. Thomson ( ) English Physicist Cathode Ray Tube Experiment

11 Thompson: Was able to deflect the cathode ray in an electric field (1897) Found the mass to charge ratio of an electron (-1.76 x 108 C/g) Credited with discovery of electron

12 Robert Milliken (1868-1953) Oil Drop Experiment American Physicist
Measured minimum electric charge that could be carried by a particle (1905) (This enabled him to find the mass of an electron) Determined it to be 1/1837 as massive as a H atom

13 The Discovery of the Electron
“Could anything at first sight seem more unpractical 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

14 Thompson’s Model of the Atom

15 Rutherford (1871-1953) Performed the Au foil experiment
New Zealand born physicist Performed the Au foil experiment

16 Rutherford (1871-1953) Discovered the nucleus (1910)
Discovered the proton (1918)

17 James Chadwick ( ) Discovered the neutron in 1932

18 Rutherford’s Model of the Atom

19 SUBATOMIC PARTICLES Electron 9.11 x 10-31 kg -1 (-1.60 x 10-19C)
Proton 1.67 x kg +1 (+1.60 x 10-19C) Neutron None

20 Basic Terms/Concepts:
Atom Element Compound

21 What gives an element it’s identity?
Atomic Number (Z) Mass Number (A) Average Atomic Mass Atomic Weight

22 Nuclide Symbol Isotope

23 Bonding Basics Types of Bonds Molecule vs. Formula Unit Structural vs.
Space-filling vs. Ball-and-Stick Models

24 Ion Cation Anion Monoatomic vs. Polyatomic

25 THE PERIODIC TABLE Vertical Columns Horizontal Rows Metals & Nonmetals
Where Found? General Properties? Types of Ions formed when react?

26 Periodic Families Alkali Metals Alkaline Earth Metals
Transition Metals Halogens Noble Gases

27 CHEMICAL FORMULAS CHEMICAL NOMENCLATURE

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