2. Atom Definition: the smallest particle of any element that retains the properties of that element. Definition: the smallest particle of any element that retains the properties of that element.

3. Practice quiz question: What is the smallest particle of magnesium that retains the properties of magnesium?

4. Interesting side note… Atoms are fantastically durable. Because they last so long, atoms really get around! Atoms are fantastically durable. Because they last so long, atoms really get around! Every atom you possess has almost certainly passed through several stars and been part of millions of organisms on its way to becoming you. Every atom you possess has almost certainly passed through several stars and been part of millions of organisms on its way to becoming you.

5. Interesting side note… It has been suggested that up to a billion of each person’s atoms once belonged to Shakespeare. Another billion came from Beethoven. You probably have some atoms from any historical figure you can think of! It has been suggested that up to a billion of each person’s atoms once belonged to Shakespeare. Another billion came from Beethoven. You probably have some atoms from any historical figure you can think of!

6. Nowadays, with the use of tunneling electron microscopes, we can sort of “see” atoms… image of copper atoms

7. This is an image of silicon atoms arranged on a face of a crystal. It is impossible to "see" atoms this way using ordinary light. The image was made by a Scanning Tunneling Microscope, a device that "feels" the cloud of electrons that form the outer surface of atoms, like a phonograph needle feels the grooves in a record.

8. These electron microscopes were invented in the mid-1900’s. How did scientists figure out atomic structure without being able to look at any atoms?

9. The History of Atomic Theory

10. But first… What is a theory in science? A theory is a well-tested explanation of what happens in nature. In layman’s terms, if something is said to be “just a theory,” it usually means that it is a mere guess, or is unproven. But in scientific terms, a theory implies that something has been well-tested and verified many times by multiple groups of scientists.

11. And while we’re at it… A scientific law is a statement of something that seems to be true in the natural world. Example: The Law of Gravity. Newton could use this law to predict the behavior of a dropped object, but he couldn't explain why it happened.

12. Einstein’s Theory of Relativity explains gravity as a curve in the fabric of space-time:

13. Remember! A law states or describes what happens in nature. A theory explains what happens. Both are well-tested by experiments. Memory hint: “explanation starts with an “e” and “theory” has an “e”.

14. True or False? The difference between a scientific law and a scientific theory is that a law has been proven, but a theory has not been proven.

15. The History of Atomic Theory

16. Democritus ancient Greek philosopher, not scientist ancient Greek philosopher, not scientist first to suggest that matter is made of tiny particles called “atomos” first to suggest that matter is made of tiny particles called “atomos” “atomos” = Greek for “indivisible” “atomos” = Greek for “indivisible” ideas were rejected by Aristotle, who was very influential, and therefore forgotten for two thousand years. ideas were rejected by Aristotle, who was very influential, and therefore forgotten for two thousand years.

17. Democritus’ atomic model: atoms were small, hard particles that were different shapes and sizes

18. John Dalton: First to propose an atomic theory based on science: 1. Each element is composed of small particles called atoms. 2. All atoms of a given element are identical*; the atoms of different elements are different. 3. Atoms are not created or destroyed in chemical reactions. 4. Compounds are formed when atoms of more than one element combine.

19. John Dalton: First to propose an atomic theory based on science: 1. Each element is composed of small particles called atoms. 2. All atoms of a given element are identical*; the atoms of different elements are different. 3. Atoms are not created or destroyed in chemical reactions. 4. Compounds are formed when atoms of more than one element combine. * We now know this part is not true!

20. Dalton’s atomic model: a tiny sphere that is indivisible

21. 1. All matter is composed of extremely small particles called atoms 2. Atoms of a given element are identical in size, mass, and other properties; atoms of different elements differ in size, mass, & other properties ELEMENT 2 ELEMENT 2 ELEMENT 3 ELEMENT 3 ELEMENT 1 ELEMENT 1 ELEMENT 4 ELEMENT 4 Atomic Theory

22. 3. Atoms cannot be created or destroyed 4. Atoms of different elements combine to form compounds 5. In chemical rxns, atoms are combined, separated, or rearranged ++ ++ Atomic Theory

23. J.J. Thomson: First to suggest that there were particles smaller than the atom. First to suggest that there were particles smaller than the atom. Discovered the electron. Discovered the electron. Developed the “plum pudding model.” Developed the “plum pudding model.”

24. Thomson’s “plum-pudding” model: the atom is composed of electrons surrounded by a cloud of positive charge to balance the electron's negative charge

25. Ernest Rutherford gold foil experiment gold foil experiment discovered the nucleus, and realized that it was very dense and positively charged discovered the nucleus, and realized that it was very dense and positively charged suggested that most of the atom is empty space suggested that most of the atom is empty space

26. Gold Foil Experiment: Rutherford shot tiny positively-charged alpha particles through a thin sheet of gold foil What Rutherford expected: What really happened:

27. Gold Foil Experiment: Some of the alpha particles bounced back. “It was as if you fired a 15-inch cannon ball at a piece of tissue paper and it came back and hit you.” What Rutherford expected: What really happened:

28. Such huge deflections could mean only one thing: some of the alpha particles had run into massive concentrations of positive charge and, since like charges repel, had been hurled straight back by them.

29. Rutherford’s atomic model: All of the positive charge is crammed inside a tiny, massive nucleus about ten thousand times smaller than the atom as a whole. The atom is mostly empty space. nucleus

30. Animation of Rutherford’s experiment http://www.mhhe.com/physsci/chem istry/essentialchemistry/flash/ruther 14.swf http://www.mhhe.com/physsci/chem istry/essentialchemistry/flash/ruther 14.swf http://www.mhhe.com/physsci/chem istry/essentialchemistry/flash/ruther 14.swf http://www.mhhe.com/physsci/chem istry/essentialchemistry/flash/ruther 14.swf

31. James Chadwick Scientists were looking for Scientists were looking for missing mass – the protons and electrons in the atom didn’t weigh enough to account for the mass of the atom proved the existence of proved the existence ofneutrons

32. Chadwick’s model of the atom: Protons and neutrons are in the nucleus, which only takes up one millionth of a billionth of the volume of the atom. The electrons are in the electron cloud, which constitutes almost all of the volume of the atom.

33. In fact, if an atom were expanded to the size of a cathedral, the nucleus would be about the size of a housefly!

34. Subatomic Particles to Know Subatomi c ParticleLocationMassCharge ProtonNucleus 1 amu +1 NeutronNucleus 0 ElectronElectronCloudPracticallyzero