1. Atomic Structure http://en.wikibooks.org/wiki/High_School_Che mistry/Further_Understanding_of_the_Atom

2. Subatomic Particles and the Nuclear Atom (4.2) I will distinguish between the subatomic particles in terms of relative charge and mass I will describe the structure of the nuclear atom, including the locations of the subatomic particles

3. Dalton's Atomic Theory Held up well to a lot of the different chemical experiments that scientists performed to test it. In fact, for almost 100 years, it seemed as if Dalton's Atomic Theory was the whole truth. As it turns out, Dalton had a lot right. He was right in saying matter is made up of atoms He was right in saying there are different kinds of atoms with different mass and other properties He was "almost" right in saying atoms of a given element are identical He was right in saying during a chemical reaction, atoms are merely rearranged He was right in saying a given compound always has atoms present in the same relative numbers. But he was wrong in saying atoms were indivisible or indestructible.

4. J.J. Thompson In 1897, a scientist named J. J. Thompson conducted some research which suggested that Atomic Theory wasn’t the entire story. As it turns out, atoms are divisible. In fact, atoms are composed of smaller subatomic particles.

5. Discovering Electrons In the mid-1800s, scientists were beginning to realize that the study of chemistry and the study of electricity were actually related. First, a man named Michael Faraday showed how passing electricity through mixtures of different chemicals could cause chemical reactions. Shortly after that, scientists found that by forcing electricity through a tube filled with gas, the electricity made the gas glow! Scientists didn't, however, understand the relationship between chemicals and electricity until a British physicist named J. J. Thomson began experimenting with what is known as a cathode ray tube. Cathode Ray Tube Experiment

8. J. J. Thomson made a radical proposal: Maybe atoms are divisible! J. J. Thomson suggested that the small, negatively charged particles making up the cathode ray were actually pieces of atoms. He called these pieces "corpuscles", although today we know them as "electrons". Thanks to his clever experiments and careful reasoning J. J. Thomson is credited with the discovery of the electron.

9. Thomson's Model of the Atom Thomson's "plum-pudding" model for the atom. Notice how the "plums" are the negatively charged electrons, while the positive charge is spread throughout the entire pudding batter.

10. Thomson's Model of the Atom Negative electrons = Pieces of Fruit-Plums (chocolate chips) Positive material = Pudding (cookie dough batter) How this fits Thompson’s Observations: – Isolated electrons using a cathode ray tube – Never managed to isolate positive particles Result: Thomson theorized that the positive material in the atom must form something like the "batter" in a plum pudding, while the negative electrons must be scattered through this "batter".

11. Disproving the "plum pudding" model A man named Ernest Rutherford used alpha particles (Helium atoms that lost their electrons and had a positive charge)as tiny bullets to fire at all kinds of different materials. One experiment in particular, however, surprised Rutherford, and everyone else. – Fired alpha particles at a very thin piece of gold foil – Almost all of the alpha particles went straight through the foil as if they'd hit nothing at all – Every so often, though, one of the alpha particles would be deflected slightly as if it had bounced off of something hard Structure of the Atom: The Rutherford Model

12. Discovering the Nucleus Rutherford Observation – Most alpha particles passed through the gold foil without hitting anything at all – Once in a while, though, the alpha particles would actually collide with a gold nucleus, causing the alpha particles to be deflected, or even to bounce right back in the direction they came from. Rutherford Explanation – The positive matter forming the gold atoms was not distributed like the batter in plum pudding – The positive matter was concentrated in one spot forming a small positively charged particle somewhere in the center of the gold atom. We now call this clump of positively charged mass the nucleus.

13. What about our “Batter” of electrons? Rutherford Suggestion – Electrons might be circling or "orbiting" the positively charged nucleus as some type of negatively charged cloud instead – Not much evidence at this time to suggest exactly how the electrons were held in the atom Modern Reconstruction of Rutherford's Experiment Modern Reconstruction of Rutherford's Experiment

14. Quick Think Without talking to a neighbor, write one fact about a scientist we recently studied Place your sticky note on the board

15. Quick- Vocab Review Electrons – Negatively charged sub atomic particles that are part of all forms of matter. Nucleus – Centrally located within the atom (very dense) – Contains all of an atom’s positive charge – Contains virtually all of an atom’s mass

16. Electrons

17. Completing the Atom-The Discovery of Protons and Neutrons 1920 (8 years after the Gold Foil Experiment) – Rutherford refines concept of nucleus Nucleus contained positively charged particles called protons – Proton » a subatomic particle carrying a charge equal to but opposite that of an electron » Protons have a positive charge +1

18. Completing the Atom-The Discovery of Protons and Neutrons 1932 James Chadwick (Rutherford’s Coworker and English Physicist) – Showed that the nucleus also contained another subatomic particle, a neutral particle called the neutron Neutron – Has a mass nearly equal to that of a proton – Carries NO electrical charge

19. Properties of Subatomic Particles ParticleSymbolLocationRelative Electrical charge Relative Mass Actual Mas (g) Electrone-e- In the space surrounding the nucleus 1-9.11x10 -28 Protonp+p+ In the nucleus 1+11.673x10 -24 Neutronn0n0 In the nucleus 011.675x10 -24

20. Atom Summary Spherically shaped Contains negative electron/s traveling through the empty space surrounding the nucleus Contains dense nucleus (99.97% of atom’s mass) – Neutral neurons – Positive protons Atom = electrically neutral – Number of electrons = number of protons NOTE: these 3 subatomic particles recently have been found to also contain quarks (yet smaller subatomic particles that we don’t understand quite yet if or how they affect chemical behavior)

21. Quick Think Describe the structure of a typical atom, be sure to identify where each subatomic particle is located. Briefly describe the experiments that led to the discovery of the electron and nucleus. Compare and Contrast Thompson’s Plum Pudding Model to Rutherford’s Nuclear Atomic Model

22. How Atoms Differ (4.3) I will explain the role of atomic number in determining the identity of an atom I will define an isotope and explain why atomic masses are not whole numbers I will calculate the number of electrons, protons, and neutrons in an atom given its mass number and atomic number

23. Atomic Number English Scientist Henry Moseley – Atoms of each element contain a unique positive charge in their nuclei Number of protons in an atom identifies it as an atom of a particular element Atomic Number – Number of protons in an element – Determines the element’s position on the periodic table

24. Quick Think How many protons does a gold atom contain? A silver atom?

25. Atomic Number Remember ALL atoms are neutral Atomic number = number of protons = number of electrons Atomic number = number of protons = number of electrons