1. Models of the Atom a Historical Perspective

2. Early Greek Theories
Democritus
400 B.C. - Democritus thought matter could not be divided indefinitely.
This led to the idea of atoms in a void.
fire
air
water
earth
Aristotle
350 B.C - Aristotle modified an earlier theory that matter was made of four “elements”: earth, fire, water, air.
Aristotle was wrong. However, his theory persisted for 2000 years.

3. John Dalton 1800 -Dalton proposed a modern atomic model
based on experimentation not on pure reason.
All matter is made of atoms.
Atoms of an element are identical.
Each element has different atoms.
Atoms of different elements combine in constant ratios to form compounds.
Atoms are rearranged in reactions.
His ideas account for the law of conservation of mass (atoms are neither created nor destroyed) and the law of constant composition (elements combine in fixed ratios).

4. Adding Electrons to the Model
Materials, when rubbed, can develop a charge difference. This electricity is called “cathode rays” when passed through an evacuated tube.
These rays have a small mass and are negative.
Thompson noted that these negative subatomic particles were a fundamental part of all atoms.
Dalton’s “Billiard ball” model ( )
Atoms are solid and indivisible.
Thompson “Plum pudding” model (1900)
Negative electrons in a positive framework.
The Rutherford model (around 1910)
Atoms are mostly empty space.
Negative electrons orbit a positive nucleus.

5. Sir J.J. Thomson (Late 1800’s)

6. Sir J.J. Thomson (Late 1800’s)
Evidence:
When cathode rays traveled through an electric field they were repelled from the negative side of the field and attracted to the positive side.
From measuring the deflection of the cathode rays in combinations of electric and magnetic fields, Thomson was able to determine that cathode rays had charge and mass.
The same results were obtained no matter what the cathode was made from.

7. Electrons
Claim:
Cathode rays were composed of a stream of negatively charged particles.
These particles were fundamental to all atoms.
Cathode rays were composed of a stream of negatively charged particles.
(Because they were repelled from negative and attracted to positive)
These particles were fundamental to all atoms.
(Because they were the same no matter which material was used in the cathode)

8. Electrons
Reasoning:
The particles were negative because they were repelled by negative charges and attracted towards positive charges.
The particles were fundamental to all atoms because the same results were found no matter what material was used to produce the electrons.

9. Electrons These particles were given the name electrons.
Later Robert Millikan, in the USA, determined the charge on an electron.
His results, when combined with Thomson’s, allowed scientists to calculate the mass of an electron.
Evidence:
Thomson had determined that atoms contained negative particles called electrons.
However, atoms were electrically neutral.

10. Thomson’s “Plum Pudding” Model
(Early 20th century)
Claim:
Atoms contain an equal amount of positive charge as negative charge
Thomson suggested that the electrons in an atom were embedded in a positively charged, diffuse sphere.
Atoms contain an equal amount of positive charge as negative charge
(Because atoms have no overall charge but are known to contain negatively charged electrons)

11. Thomson’s “Plum Pudding” Model
(Early 20th century)
Reasoning:
Thomson had no experimental evidence for his model but built on the idea that positive charge in an atom was spread evenly and diffusely throughout a spherical shape.

12. Ernest Rutherford Rutherford shot alpha () particles at gold foil.
Zinc sulfide screen
Thin gold foil
Lead block
Radioactive substance
path of invisible -particles
Most particles passed through. So, atoms are mostly empty.
Some positive -particles deflected or bounced back!
Thus, a “nucleus” is positive & holds most of an atom’s mass.

13. Bohr’s model Electrons orbit the nucleus in “shells”
Electrons can be bumped up to a higher shell if hit by an electron or a photon of light.
There are 2 types of spectra: continuous spectra & line spectra. It’s when electrons fall back down that they release a photon. These jumps down from “shell” to “shell” account for the line spectra seen in gas discharge tubes (through spectroscopes).