1. Basic Laws and Important People
Intro to Chemistry

2. Fundamental Chemical Laws
1. Law of Conservation of Mass
States that matter cannot be created or destroyed
Its just rearranged through chemical processes
Total mass of reactants must be equal to the total mass of the products

4. 2. Law of Definite Proportion
A given compound always contains the same proportions of elements by mass
Compounds do not have a changing form
Compounds have a fixed ratio of components

5. Law of Multiple Proportions
When two elements form a series of compounds (Homologous series in organic) the ratio of masses of the elements can always be reduced to the smallest whole number
Also it is important to note that sometimes two elements can produce a series that is not able to be reduced
CO, CO2, CO3, etc…

6. ImPortant people and what they did
Early Experiments to Characterize the Atom
ImPortant people and what they did

7. J.J Thomson and Electrons
Determined the charge to mass ratio of the electron
x 108 C/g
Reasoned that all atoms must contain at least 1 electron
Reasoned that atoms must have a positive charge as well although he didn’t “find” the particle
Used the cathode ray tube experiment to determine this information

10. Robert Milikan and the oil drop
Used this experiment to determine the magnitude of the charge of an electron
Along with Thomson he determines the mass of an electron to be 9.11 x kg

12. Radioactivity
Gamma Rays
Beta Particles
Alpha Particles

13. Rutherford and the Gold Foil Experiment
Uses this experiment to determine that all atoms are composed of mostly empty space
All atoms also have a positive dense core that he calls a nucleus
Makes an attempt to develop an atomic model but was incorrect with his placement of particles
Considered the ground breaking experiment in the fields of chemistry and physics with regards to atoms

18. 2.5 Modern View of The Atom 1. Nucleus---center of mass
Contains protons and neutrons
Positive charge that is indicated by the atomic number of an element
Small size, large density
2. Electrons
Source of reactivity
Negative charge
1/2000th the mass of a proton

19. Parts of an atom Continued
3. Atomic Number– same as number of protons
Identifying feature of all elements
Number cannot be changed for an individual atom
4. Mass Number
Protons + Neutrons
Can be different for isotopes of the same element
Number on periodic table is a weighted average of all known isotopes for the element

20. Parts….
5. Isotopes----same element with a different number of neutrons
Gives this version a different mass

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