1. The History of Atomic Theory
Chapter 4 Section 1 Notes
The History of Atomic Theory

2. Who are these men?
In this lesson, we’ll learn about the men whose quests for knowledge about the fundamental nature of the universe helped define our views.

3. Democritus
B.C.E.
This is the Greek philosopher Democritus who began the search for a description of matter more than 2400 years ago.
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?”
He had no way of knowing what atoms looked like!

4. The word “atom” comes from a Greek word that means “unable to be cut”
Imagine you had a piece of gold that you then cut in half…
… and you kept on cutting the leftover piece in half…
…and then you cut one of these smaller pieces in half…
Gold Go ld

5. The word “atom” comes from a Greek word that means “unable to be cut”
Eventually you would have 1 piece of gold left. If you cut it in half, you wouldn’t have gold any more – you’d have something else. This tiny, tiny single piece of gold is called an atom of gold. An atom is the smallest particle of an element that acts like the element.
…and kept going…
…and kept going…
An atom of gold

6. Atomos
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. Atomos
To Democritus, atoms were small, hard particles that were all made of the same material but were different shapes and sizes.
Atoms were infinite in number, always moving and capable of joining together.

8. This theory was ignored and forgotten for more than 2000 years!

9. Can matter be divided into smaller and smaller pieces forever?
A Big Debate
Can matter be divided into smaller and smaller pieces forever?
What do you think?
YES!
NO!

10. Democritus But no one believed him! He hypothesized that atoms were:
Small & Hard
Different in shape & size
Infinite
Always moving
Capable of joining
But no one believed him!

11. The atomos idea was buried for approximately 2000 years.
Why?
The eminent philosophers of the time, Aristotle and Plato, had a more respected, (and ultimately wrong) theory.
Aristotle and Plato favored the earth, fire, air and water approach to the nature of matter.
The atomos idea was buried for approximately 2000 years.

12. Time Goes By…
1600s-1700s: Key experiments occur which support Democritus’s ideas.
Robert Boyle ( )
Antoine Lavoisier ( )

13. Dalton (1766-1844) Dalton’s Model
English chemist and school teacher
In the early 1800s, the English Chemist John Dalton performed a number of experiments that eventually led to the acceptance of the idea of atoms.

14. His model was called the Billiard Ball!
Dalton’s Theory (1803)
All elements are 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.
His model was called the Billiard Ball!

15. .
This theory became one of the foundations of modern chemistry.

16. Thomson’s Plum Pudding Model
In 1897, the English scientist J.J. Thomson provided the first hint that an atom is made of even smaller particles.

17. Atomic Model: Thomson => Electrons! Click here for more on the
Passed electricity through an uncharged gas
The gas gave off rays to show it was NEGATIVELY charged
How?
Negative charges must come from inside the atom!
=> Electrons!
Click here
for more
on the
Discovery of
the electron

19. But wait…
How can an atom be NEUTRAL if it is full of negatively charged particles (electrons?)

20. Atomic Models: Thomson
The atoms are neutral… How?
+ charges must be present to balance - charges
+ & - lumped in a cluster he said looked like “plum pudding”

21. Thomson Model
He proposed a model of the atom that is sometimes called the “Plum Pudding” model.
Atoms were made from a positively charged substance with negatively charged electrons scattered about, like raisins in a pudding.

22. Thomson Model
Where did they come from?
This surprised Thomson, because the atoms of the gas were uncharged. Where had the negative charges come from?

23. Thomson concluded that the negative charges came from within the atom.
A particle smaller than an atom had to exist.
The atom was divisible!
Thomson called the negatively charged “corpuscles,” today known as electrons.
Since the gas was known to be neutral, having no charge, he reasoned that there must be positively charged particles in the atom.
But he could never find them.

24. Rutherford’s Gold Foil Experiment
In 1908, the English physicist Ernest Rutherford was hard at work on an experiment that seemed to have little to do with unraveling the mysteries of the atomic structure.

25. Atomic Models: Rutherford
Passed + Charged Particles through gold foil
Most passed right through
Atom is mostly empty space
Some bounced off at odd angles
Nucleus must be +
Calculate size of nucleus

26. Rutherford’s Gold Foil Experiment
start
experiment
DO NOT OPEN
RADIOACTIVE
MATERIAL
INSIDE + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + +
LOOK INSIDE
THE GOLD

27. Rutherford’s Work What's Different This Time??? start experiment
DO NOT OPEN
RADIOACTIVE
MATERIAL
INSIDE + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + +
LOOK INSIDE
THE GOLD

28. Rutherford’s experiment involved firing a stream of tiny positively charged particles at a thin sheet of gold foil (2000 atoms thick)
rutherford.mov

29. 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,” bounced away from the gold sheet as if they had hit something solid.
He knew that positive charges repel positive charges.

30. This could only mean that the gold atoms were mostly open space, not a pudding filled with a positively charged material.
Rutherford concluded that an atom had a small, dense, positively charged center that repelled his positively charged “bullets.”
He called the center of the atom the “nucleus”
The nucleus is tiny compared to the atom as a whole.

31. Rutherford
All of an atom’s positively charged particles were contained in the nucleus.
The negatively charged particles were scattered outside the nucleus.

32. So the atom is made up of positive and negative particles.
Okay…
So the atom is made up of positive and negative particles.
Where are the electrons found in the atom?

33. Bohr Model
In 1913, the Danish scientist Niels Bohr proposed an improvement. In his model, he placed each electron in a specific energy level.

34. Bohr’s Model

35. Bohr’s Model According to Bohr’s atomic model:
Electrons respond to light
Electrons move in definite orbits around the nucleus
Like planets around the sun
Electrons are found in specific energy levels
These orbits, or energy levels, are located at certain distances from the nucleus.
Electrons can jump from path to path (like a ladder)

36. The Electron Cloud Model (a.k.a. The 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.

37. Atomic Model: Electron Cloud (wave)
Electrons move so fast that it is impossible to determine their location
Move in all directions around the nucleus

38. Electron Cloud Model

39. The Electron Cloud Model
I 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.
In the electron cloud model, the atom has a small positively charged nucleus surrounded by a large region in which there are enough electrons to make an atom neutral.

40. Electron Cloud: A space in which electrons are likely to be found.
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.

41. Electron Cloud:
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.

42. Atomic Model Review

43. Dalton’s Atomic Model (1807)
The Billiard ball model.
Atoms were considered to be featureless, indivisible, spheres of uniform density

44. J. J. Thomson’s Atomic Model Plum Pudding Model
Atoms are not hard spherical balls.
Further experiments showed two particles in atoms
Protons (+) & electrons (-)
Electrons were like raisins stuck randomly inside a mass of positively charged “pudding”.
Negative electrons used to hold together the positively changed mass of pudding.

45. Rutherford’s Nuclear Model (1911)
Central nucleus composed of positively charged protons.
Negatively charged cloud of electrons surrounds the nucleus.
PROBLEM: As atoms lost energy why didn’t the electrons eventually spiral into the nucleus due to electrical attraction of + for -?
PROBLEM: How could all the positive protons stay packed together in the nucleus?

46. Neil Bohr’s Model of Hydrogen (1913)
Solves problem of why electrons to do fall into nucleus.
Used quantized orbits with specific energies.
Electron can only move between orbits by getting or losing the exact amount of energy required.
It could not take fractional steps.

47. Schrödinger Electron Cloud Model (1926)
According to Schrödinger atoms are composed of
Central nucleus
A fuzzy electron cloud

48. Summary of Atomic Models

49. Greek X Dalton Thomson Rutherford Bohr Indivisible Electron Nucleus
Orbit
Electron Cloud
Greek X
Dalton
Thomson
Rutherford
Bohr