1. History of the Atom

2. Why study the history of the atom?
"If I have seen further, it is by standing on the shoulders of giants.“ – Isaac Newton, 1676

3. Aristotle
We are what we repeatedly do. Excellence, then, is not an act, but a habit.
Happiness depends upon ourselves.
The educated differ from the uneducated as much as the living from the dead.

4. Aristotle
Ideas on Nature:
Four Elements

5. Democritus
He asked: Could matter be divided into smaller and smaller pieces forever, or was there a limit to the number of times a piece of matter could be divided?

6. Democritus His theory:
Matter could not be divided into smaller and smaller pieces forever; eventually the smallest possible piece would be obtained.
This piece would be indivisible.
He named the smallest piece of matter “atomos,” meaning “not to be cut.”

7. Democritus His theory:
Matter is composed of “atoms” which move through empty space.
Atoms are solid, homogeneous, indestructible and indivisible.
Different kinds of atoms have different shapes and sizes.
The properties of matter are determined by the sizes, shapes, and movement of atoms.

8. Dalton His theory: He deduced that all matter is composed of atoms.
Atoms are indivisible and indestructible particles.
Atoms of the same element are exactly alike.
Atoms of different elements are different.
Compounds are formed by the joining of atoms of two or more elements.

9. Thomson
He found that there were even smaller particles inside atoms.

10. Thomson
His theory:
When he passed an electric current through an almost empty glass tube, he saw a green flash.
This radiation was called a cathode ray.
It was negatively charged.
Now called electrons.

11. Thomson
His theory:
Since all matter is neutral, it has no electric charge.
If there are negatively charged particles in side atoms, there must be a positive charge too.
Plum Pudding Model of the Atom
Spherical atom of uniform positive charge, with negative electrons studded in it.

12. Rutherford
Rutherford’s experiment Involved firing a stream of tiny positively charged particles at a thin sheet of gold foil (2000 atoms thick)

13. Rutherford

14. Rutherford
Most of the positively charged “bullets” passed right through the gold atoms in the sheet of gold foil without changing course at all.
Some of the positively charged “bullets,” however, did bounce away from the gold sheet as if they had hit something solid. He knew that positive charges repel positive charges.

15. Rutherford His Theory: Most of the space of an atom must be empty.
There must be a small, positively charged area in the center of the atom.  called the nucleus.
The nucleus is tiny compared to the atom as a whole.

16. Bohr
His Theory:
The electrons “live” in specific energy levels around the nucleus.
The energy levels were like “orbits”

17. Wave Model
Today’s atomic model is based on the principles of wave mechanics.
According to the theory of wave mechanics, electrons do not move about an atom in a definite path, like the planets around the sun.
In fact, it is impossible to determine the exact location of an electron. The probable location of an electron is based on how much energy the electron has.
A space in which electrons are likely to be found is called the electron cloud.

18. Wave Model: The Electron Cloud
Electrons whirl about the nucleus billions of times in one second
They are not moving around in random patterns.
Location of electrons depends upon how much energy the electron has.
Depending on their energy they are locked into a certain area in the cloud.
Electrons with the lowest energy are found in the energy level closest to the nucleus
Electrons with the highest energy are found in the outermost energy levels, farther from the nucleus.