1. Old Dead Guys

2. Democritus ( BC)
Was the first person to come up with
the idea of atom
Believed that all matter was composed of indivisible particles he called “ATOMS”
Which is derived from the Greek word “Atomos” – meaning indivisible
He also believed that different atoms:
Are different sizes
Have different properties
Other philosophers of that time did not agree with his theories.

3. John Dalton (1766-1844) Dalton is the “Father of Atomic Theory”
Dalton’s ideas were so brilliant that they have remained essentially intact up to the present time and has only been slightly corrected.

4. Dalton’s Atomic Theory (1803) aka: 5 Postulates
All matter is composed of extremely small particles called atoms. (I agree with Democritus!)
2. All atoms of a given element are identical, having the same:
- size
- mass
- chemical properties.
3. All atoms of different elements are different.

5. Dalton’s Atomic Theory (1803) aka: 5 Postulates
Atoms cannot be created, divided into smaller particles, or destroyed.
**In a chemical reaction, atoms of different elements are separated, joined or rearranged. They are never changed into the atoms of another element. We will learn more later**
5. Atoms combine in definite whole number ratios to make compounds (you can’t have a ½ of a Carbon bonding with Oxygen; it’s a whole atom or no atom)

6. Dalton’s Atomic Laws 1. Law of Conservation of Mass
Matter cannot be created or destroyed in any physical or chemical process, just transferred.
2.     Law of Constant Composition
When atoms combine to form molecules, the ratio of atoms is constant.
Example – H2O will always have 2 times as many Hydrogen atoms as Oxygen.

7. Dalton’s Atomic Laws
3.     Law of Multiple Proportions – if two elements can combine to form more than one compound, then the ratio of the second element combined with a certain mass of the first element is always a ratio of small whole numbers.

8. JJ Thomson ( )
Used cathode rays to prove that Dalton’s Solid-ball model could be broken into smaller particles
Thomson is credited with discovering electrons

9. Cathode Ray Tubes
Cathode rays had been used for some time before Thompson’s experiments.
A cathode ray is a tube that has a piece of metal, called an electrode, at each end. Each electrode is connected to a power source (battery).
When the power is turned on, the electrodes become charged and produce a stream of charged particles. They travel from cathode, across the tube to the anode.

10. -----------------------------
Cathode Ray Tubes
Thomson put the tube in a magnetic field. He predicted that the stream would travel in a straight path.
Instead, he found that the path curved away from a negatively charged plate and toward a positively charged plate
Why?
Like charges repel each other, and objects with unlike charges attract each other, Thomson concluded that the stream of charged particles had electrons in them.

11. Cathode Ray Tube Experiment
Thompson Concluded:
Cathode rays are made up of invisible, negatively charged particles called Electrons.
These electrons had to come from the matter (atoms) of the negative electrode.
Since the electrodes could be made from a variety of metals, then all atoms must contain electrons!

12. Thomson’s Plum Pudding Model
Thomson’s Plum Pudding model is a + charge sphere that has (- )charged electrons scattered inside, like “raisins” in “plum pudding”.
Overall, the atom is neutral atom because the atom had the same number of positive and negative charges.
From Thomson’s experiments, scientists concluded that atoms were not just neutral spheres, but somehow were composed of electrically charged particles.
The balance of positive and negative charge supports the neutral atom.

13. Rutherford ( )
Took Thomson’s Plum Pudding Model and added to it
Used the “Gold Foil Experiment” to discover the existence of:
An atomic Nucleus
Protons (in later experiments)

14. Gold Foil Experiment
Rutherford directed a narrow beam of alpha particles (+ charges) at a thin piece of gold foil.
Based on observations from other experiments involving alpha particles, he predicted that the (+) charges would go through the foil

15. Results from Gold Foil Experiment
Rutherford found that every once and a while, a + particle was deflected bounced back. (about 1% of the time)
Why?
Because the + charge hit a central mass of positive charge and was repelled.

16. Conclusions from Rutherford’s Gold Foil Experiment (memorize this!)
The atom contains a positively charged “nucleus”
This nucleus contains almost all of the mass of the atom, but occupies a very small volume of the atom.
The negatively charged electrons occupied most of the volume of the atom.
 The atom is mostly empty space.

17. Bohr (1885-1962) Worked in Rutherford’s lab
Wondered why – electrons are not attracted to the + nucleus and cluster around it
Disproved Rutherford’s Planetary Model
Experimented with light and its interaction with matter to develop a new model.

18. Bohr’s Energy Level Model
Energy Level Model: Electrons are arranged in circles around the nucleus. Each circle has a different energy.
Electrons are in constant motion, traveling around the circle at the speed of light.
Electrons can “jump” from one circle to the next
But they can’t go to the nucleus they traveling too fast to be fully attracted.

19. Bohr’s Energy Level Model
·  He proposed the following:
1. Protons and neutrons are in the nucleus
2. Electrons can only be certain distances from the nucleus.
3. The electrons orbit the nucleus at fixed energy levels.
4. The electrons must absorb or emit a fixed amount of energy to travel between these energy levels

20. Isotopes of an element have different mass numbers because they have
different numbers of neutrons,
but they have
the same atomic number.

21. C Isotopes Mass # Atomic# 12 6
Atoms of the same element with different mass numbers.
Nuclear symbol: 12 6 C
Mass #
Each isotope has a different number of neutrons.
Atomic#
Hyphen notation: carbon-12
Courtesy Christy Johannesson

22. What is average atomic mass?
Average atomic mass is the weighted average of the atomic masses of the naturally occurring isotopes of an element

23. Calculating Average Atomic Mass
EXAMPLE
Boron has two isotopes:
B-10 (mass amu) 19.8% abundance
B-11 (mass amu) 80.2% abundance
Calculate the average atomic mass.
(.198) (10.013) + (.802) ( ) =
1.98 amu amu = amu

24. Calculating Average Atomic Mass
Calculate the average atomic mass of Mg.
Isotope amu (78.99%)
Isotope amu (10.00%)
Isotope 3 – amu (11.01%)
(23.985)(.7899)+(24.986)(.1000)+(25.982)(.1101)
18.95 amu amu amu = amu