1. Discovering the Atom (Chapters 4 and 5) Dr. Walker

2. Objectives
Understand how experiments shaped our understanding of the modern atom:
Subatomic particles (protons, neutrons, electrons)
Models of the atom (solid sphere, planetary, quantum)
Know scientists who contributed to atomic theory
Democritus
Dalton
Thomson
Rutherford
Bohr

3. Chemistry Over Time…
Our understanding of the atom is based on experimental evidence, not conjecture
Our understanding of the atom has changed over time based upon new evidence, and may continue to change
All science is subject to peer review and repetition of experiments --- science deals with what can be proven!!

4. Democritus ( BC)
Believed there had to be a basic building block of matter which could not be subdivided.
A more famous philosopher, Aristotle, opposed this theory
Called these building blocks “atomos”
Greek for “uncuttable” or “indivisible”

5. John Dalton (1766-1844) Credit with “atomic theory”
Believed atoms were solid blocks (like a billiard ball) – known as the “solid sphere” model

6. John Dalton Elements are made of tiny particles called atoms.
The atoms of a given element are different from those of any other element; different elements can be distinguished by their distinct atomic weights.
All atoms of a given element are identical.
Atoms of one element can combine with atoms of other elements to form chemical compounds; a given compound always has the same relative numbers of types of atoms.
In chemical reaction, atoms cannot be created, destroyed, or divided.

7. JJ Thomson ( )
Performed cathode ray tube experiment, discovering the electron
Pumped most of the air from a glass tube and applied a voltage to two electrodes placed at each end of the tube (1897)
Anode---attached to positive terminal.
Cathode—attached to negative terminal.

8. JJ Thomson
Thomson observed a glowing beam coming out of the cathode, striking the anode and the nearby glass walls of the tube.
Called them cathode rays.
The glass tube used by Thomson is known as a cathode-ray tube (CRT) which is currently used in television sets, computer monitors, and radar displays.

9. http://upload. wikimedia

10. JJ Thomson
Because he had pumped most of the air of the tube, the rays must have come from the cathode.
Because the ray came from the negatively charged cathode, the ray must have been negatively charged.
He confirmed his prediction by bending the cathode ray with a magnet.

11. JJ Thomson
He also observed that when he placed a small paddle wheel in the path of the rays, the wheel turned.
Something must’ve been hitting the wheel---this suggested that the rays of the cathode were tiny particles that had mass.
Later experiments with cathodes of different metals showed electrons were present in all atoms.

12. What did this mean?
Atoms are uncharged, electrons have a negative charge.
Scientists realized that there must be particles with a positive charge within the atom to balance the negative charge.
Scientists also found that electrons are much less massive than atoms so other subatomic particles must exist.

13. JJ Thomson’s Atomic Model
Thomson proposed that electrons of the atom were embedded in a positively charged ball-of-matter, which led to the name “plum-pudding model”.

15. Robert Millikan Performed experiments with charged oil drops
Known (oddly enough) as the “Millikan oil drop experiment”
Allowed him to calculate magnitude of charge of an electron
1.592 × 10−19 Coulombs (unit of charge)

16. Robert Millikan

17. Ernest Rutherford ( )
Performed experiments (gold foil) disproving the plum pudding model of the atom (1909)
Focused a beam of positively charged particles (“alpha particles”) at a thin gold foil.
The team measured the angles at which the particles deflected after hitting the foil.

19. Ernest Rutherford
However, his team found that most of the particles went straight through the foil.
Others went completely backwards. Rutherford’s model didn’t predict this----Thomson’s model had solid atoms and all of the atoms would have deflected.
What happened in this experiment?

20. Ernest Rutherford
The mass of this positively charge space, which he called the nucleus, must be larger than the mass of the alpha particle. Otherwise, the particle would have deflected rather than moving backward.
The particles that went through the gold foil did so because most of the volume of the gold atoms were empty space (the electron cloud).

21. Okay… From Rutherford’s experiments, we know…
The nucleus has most of the mass of an atom
The nucleus is positively charged
The nucleus has protons and something else…
The atom is mostly empty space
The “plum-pudding” model is invalid
So now what does the atom look like???

22. Rutherford’s Model Rutherford proposed:
The nucleus is positively charged
Electrons orbit around the nucleus
Known as the “nuclear model”
Rutherford’s model was incomplete. It would later be expanded upon by Niels Bohr

23. Nuclear Model Notice there are no defined paths for the electrons….yet

24. Niels Bohr Bohr expanded upon this theory by proposing
Electrons travel only in successively larger circular orbits
The outer orbits could hold more electrons than the inner ones, and that these outer orbits determine the atom's chemical properties

25. Planetary Model
If opposite charges attract, what keeps the negatively charged electrons from moving into the positively charged nucleus?

26. The Solution…
Max Planck (1901) found that when matter is heated, it gives off energy at specific wavelengths.
This energy is known as a “quantum” of energy
These specific wavelengths mean that electrons can only exist at specific energy levels, like the rungs of a ladder.
This led Bohr to the planetary model of the atom (1913)

27. Bohr’s Planetary Model

28. The Quantum Model
Bohr was the first to theorize the quantum model in a planetary arrangement
Bohr’s model = PLANETARY MODEL!!
Bohr’s original planetary arrangement didn’t work (due to physics beyond the scope of this class)
His idea only worked for hydrogen
Electrons DO NOT move around the nucleus in fixed circular orbits
Electrons ARE contained in discrete energy levels with distinct differences between them.
You’ve seen these in the electron configuration section.

29. The Quantum Model
Louis de Broglie discovered that electrons act like waves (wave-particle duality)
Matter acts like a particle (solid) AND a wave (radio waves, water)
Frequencies of electrons correspond to the energy levels around the nucleus
Werner Heisenberg is credited with the uncertainty principle
Uncertainty principle – we can’t know EXACTLY where an electron is or how fast it’s moving
Both (along with Erwin Schrodinger) are credited with the discovery of the quantum model of the atom

30. Quantum Model

31. Atomic Models Through Time
Thomson model (Plum-Pudding)
In the nineteenth century, Thomson described
the atom as a ball of positive charge containing
a number of electrons.
Rutherford model
In the early twentieth century, Rutherford
showed that most of an atom's mass is
concentrated in a small, positively charged
region called the nucleus.
Bohr model (Planetary)
After Rutherford's discovery, Bohr proposed
that electrons travel in definite orbits around
the nucleus.
Quantum mechanical model
Modern atomic theory described the
electronic structure of the atom as the
probability of finding electrons within
certain regions of space.

32. Terms to Know People Democritus Dalton Thomson Rutherford Millikan
Planck
Bohr
deBroglie
Heisenberg

33. Terms to Know Experiments – Terms Solid sphere model
Cathode ray tube experiment
Plum pudding model
Gold foil experiment
Oil drop experiment
Planetary model
Quantum model
Uncertainty principle