1. Development of a Modern Atomic Theory

2. John Dalton 1766-1844 Dalton’s Atomic Theory
Suggested that particles which make up matter are actually like small, hard spheres, different for each different element. He brought back the idea of an atom being the smallest particle of an element.
Dalton’s Atomic Theory
All matter are made up of small particles called atoms
Atoms cannot be created, destroyed or subdivided during chemical changes
Atoms of the same element are identical, those of different atoms are different.
each element has its own kind of atom, with its own particular mass
Compounds are created when atoms of different elements
link together in definite proportions

3. Dalton’s Symbols John Dalton 1808
Jons Jakob Berzelius ( ) Swedish chemist who invented modern chemical symbols.
Berzelius discovered the elements silicon, selenium, cerium, and thorium.
John Dalton
1808

4. Daltons’ Models of Atoms
Carbon dioxide, CO2
Water, H2O
Dalton would have shown water with a single hydrogen and a single oxygen. Dalton did not know that hydrogen was diatomic and had a mass of 1 amu.
Methane, CH4

5. J.J. Thomson
In 1897, J.J. determined that currents were streams of negatively charged particles, later called electrons. He found that every substance he tested produced these particles.
Based on his experiments, he theorized that all atoms must have these particles; he proposed that atoms were actually formed by even smaller particles.
Thomson proposed the raisin bun model, where an atom would be a positively charged ball with negative particles embedded in it like raisins.

6. Thomson’s Revision to the Atomic Theory: Electrons
Atoms contains electrons.
The electrons have a negative charge and a very small mass
The rest of the atom has a positive charge
The electrons are embedded randomly in the positive part of the atom
Electrons can be removed from, or added to atoms to create charged atoms

7. Ernest Rutherford (1871-1937) Learned physics in J.J. Thomson’ lab.
PAPER
Learned physics in J.J. Thomson’ lab.
Noticed that ‘alpha’ particles were sometime deflected by something in the air.
Gold-foil experiment
Ernest Rutherford received the Nobel Prize in chemistry (1908) for his work with radioactivity.
Ernest Rutherford ( ) was born in Nelson, New Zealand in He began work in J.J. Thompson’s laboratory in He later moved to McGill University in Montreal where he became one of the leading figures in the field of radioactivity. From 1907 on he was professor at the University of Manchester where he worked with Geiger and Marsden. He was awarded the Nobel Prize for Chemistry in 1908 for his work on radioactivity. In 1910, with co-workers Geiger and Marsden he discovered that alpha-particles could be deflected by thin metal foil. This work enabled him to propose a structure for the atom. Later on he proposed the existence of the proton and predicted the existence of the neutron. He died in 1937 and like J.J. Thompson is buried in Westminster Abbey. He was one of the most distinguished scientists of his century.
Is the Nucleus Fundamental?
Because it appeared small, solid, and dense, scientists originally thought that the nucleus was fundamental. Later, they discovered that it was made of protons (p+), which are positively charged, and neutrons (n), which have no charge.

8. Ernest Rutherford
Designed an experiment to probe inside atoms.
He exposed a very thin sheet of gold to a stream of high speed, heavy, positively charged particles, called alpha particles.
He noticed that when they were shot through the gold, the particles mostly went through, but some bounced in unexpected directions. This was the discovery of the nucleus.
A decade later, he also established that the nucleus must have at least two kinds of particles: a positive proton, and a neutral neutron.

9. Hit moth driving car – no change in car direction
Hit deer – car changes direction
Alpha particle
moth
deer
Gold Atom

10. Rutherford’s Gold-Leaf Experiment Conclusions: Atom is mostly empty space Nucleus has (+) charge Electrons float around nucleus
“Rutherford’s Gold-Leaf Experiment”
Description
This slide illustrates Ernest Rutherford’s experiment with alpha particles and gold foil and his interpretation of the results.
Basic Concepts
When charged particles are directed at high speed toward a metal foil target, most pass through with little or no deflection, but some particles are deflected at large angles.
Solids are composed of atoms that are closely packed. The atoms themselves are mostly empty space.
All atoms contain a relatively small, massive, positively charged nucleus. The nucleus is surrounded by negatively charged electrons of low mass that occupy a relatively large volume.
Teaching Suggestions
Use this slide to describe and explain Rutherford’s experiment. Rutherford designed the apparatus shown in figure (A) to study the scattering of alpha particles by gold. Students may have difficult with the concepts in this experiment because they lack the necessary physics background. To help students understand how it was determined that the nucleus is relatively massive, use questions 3 and 4 to explain the concept of inertia.
Explain that the electrostatic force is directly proportional to the quantity of electric charge involved. A greater charge exerts a greater force. (Try comparing the electrostatic force to the foce of gravity, which is greater near a massive object like the sun, but smaller near an object of lesser mass, such as the moon.) The force exerted on an alpha particle by a concentrated nucleus would be much greater that the force exerted on an alpha particle by a single proton. Hence, larger deflections will result from a dense nucleus than from an atom with diffuse positive charges.
Point out that Rutherford used physics to calculate how small the nucleus would have to be produce the large-angle deflections observed. He calculated that the maximum possible size of the nucleus is about 1/10,000 the diameter of the atom. Rutherford concluded that the atom is mostly space.
Questions
If gold atoms were solid spheres stacked together with no space between them, what would you expect would happen to particles shot at them? Explain your reasoning.
When Ernest Rutherford performed the experiment shown in diagram (A) he observed that most of the alpha particles passed straight through the gold foil. He also noted that the gold foil did not appear to be affected. How can these two observations be explained?
Can you explain why Rutherford concluded that the mass of the f\gold nucleus must be much greater than the mass of an alpha particle? (Hint: Imagine one marble striking another marble at high speed. Compare this with a marble striking a bowling ball.)
Do you think that, in Rutherford’s experiment, the electrons in the gold atoms would deflect the alpha particles significantly? Why or why not? (Hint: The mass of an electron is extremely small.)
Rutherford experimented with many kinds of metal foil as the target. The results were always similar. Why was it important to do this?
A friend tries to convince you that gold atoms are solid because gold feels solid. Your friend also argues that, because the negatively charged electrons are attracted to the positively charged nucleus, the electrons should collapse into the nucleus. How would you respond?
As you know, like charges repel each other. Yet, Rutherford determined that the nucleus contains all of an atom’s positive charges. Invent a theory to explain how all the positive charges can be contained in such a small area without repelling each other. Be creative!
Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3rd Edition, 1990, page 120

11. Rutherford’s Revisions to the Atomic Theory: The Nucleus
The nucleus contains all of the positive charge and most of the mass of the atom.
The nucleus contains positively charged protons and uncharged neutrons.
Neutrons have the same mass as protons.
The nucleus is very small, compared with the size of the atom.
The electrons orbit the nucleus, like satellites around the planet.
The mass of an electron is 1/1800 the mass of a proton.
The size of the atom is determined by the size of the orbit of the electrons.
There is only empty space between the electrons and the nucleus.

12. Niels Bohr
Bohr worked under Ernest Rutherford, and focused on the regions around the nucleus, which was known to contain electrons.

13. Niels Bohr
He proposed that the electrons were organized into specific energy levels, or shells. The placement of each electron would depend on how much energy they have. The more energy an electron has, the closest they will be to the outer shell.

14. Bohr’s Model
Nucleus
Electron
Orbit
Energy Levels

15. Bohr’s Revisions to the Atomic Theory: Electrons in Specific Orbits
Electrons are located in defined shells, which are located certain distances from the nucleus.
Electrons cannot exist between the defined shells.
Electrons can gain energy to move up to a higher shell, or they can lose energy to move down to a lower shell.
Electrons are more stable( have less energy) when they are closer to the nucleus.

16. What is an atom?
An atom is the smallest particle of an element that retains the properties of the element.
An atom is composed of subatomic particles: protons, electrons and neutrons.
The nucleus is tiny, dense and composed of protons and neutrons. They have much more mass than electrons, about 1800 times more.
Electrons are arranged around the nucleus in specific levels.
A neutral atom has the same number of protons and electrons.

17. Electric Charge
Electric charge comes in two types: positive and negative.
Protons are positive, and electrons are negative; since positive and negative attract each other, protons and electrons are attracted together.
Each proton counts as +1 and each electron counts as -1.
All neutral atoms have the same amount of protons and electrons; this means that the charge will add up to zero.
Example: Oxygen has 8 electrons and 8 protons; the overall charge is zero.

18. Nucleus
The nucleus has a positive charge because of the protons. For any atom more complicated than Hydrogen, the nucleus must contain neutrons. Neutrons keep the protons separated from each other. The number of neutrons varies depending on how many are necessary to keep the nucleus stable.
Electrons
Electrons occupy special regions called energy levels, or shells, which surround the nucleus.
The region occupied by electrons account for way over 99.99% of the volume of the atom.
Each electron occupies the whole energy level at a time.