1. Structure of the Atom Refer to: Science Probe 10 - Chapter 8

2. The idea of the atom goes back to Ancient Greece. We continue by looking at more “recent” ideas of the atom.

3. Dalton’s Atomic Theory (1808) All matter is made of atoms (particles to small to see). Each element has its own kind of atom. Atoms of the same element have the same mass, atoms of different elements have different masses.

4. Compounds are formed when different atoms link to form “compound atoms” (now called molecules). In a compound all “compound atoms” are alike. Atoms cannot be created or destroyed.

5. Modern Atomic Theory Even though Dalton’s work was 200 years ago, the basis of it is still valid with only a few modifications. Dalton thought atoms were solid spheres like billiard balls, but we know atoms are made up of smaller parts

6. Sub Atomic Particles (smaller than atoms) Atoms are made up of three main type of particles: Protons Found in nucleus (center part) of atom Positive charge (+1) Mass 1 atomic mass unit (a.m.u.)

7. Neutrons Found in nucleus of atom Neutral ( 0 charge) Mass 1 a.m.u. Electrons Found moving outside the nucleus Negative charge (-1) Mass approx 1/1800 a.m.u.

8. Atomic Number Number of protons in the atom Each atomic number is unique and defines each atom E.g. If there are 8 protons, the element is… oxygen! If the element is oxygen, there must be 8 protons

9. The atomic number is found at the top of each square on the periodic table. Atomic number See Periodic Table HereSee Periodic Table Here (or text p. 516) If you have a periodic table you can instantly find the number of protons.

10. Number of Electrons In any neutral (uncharged) atom the number of protons is always equal to the number of electrons. The number of electrons, therefore, is also equal to the atomic number. If there are 8 protons, there will be 8 electrons.

11. Mass Number Total number of all protons and neutrons in an element always a whole number Note - electrons are too small to effect total mass An element with 3 protons and 4 neutrons will have a mass number of 7

12. Mass Number To find mass number from a periodic table, look under the symbol (or name) Round off to a whole number (decimals will be explained soon!) See periodic table Mass number = 12 (rounded off)

13. Number of Neutrons Can be determined from the periodic table. If mass number = protons + neutrons, then: Neutrons = mass number - protons or Neutrons = mass number - atomic number

14. Calculating Protons, Neutrons and Electrons Find number of protons, neutrons and electrons for each of the following. Carbon Na Element #5

15. Assignment Do PNE Worksheet

16. Isotopes Isotopes are atoms of the same element that have different masses. Why are these masses different?? Since number of protons doesn’t change, the change in mass must be due to different number of neutrons. 16 amu17 amu 8 protons 8 neutrons 8 protons 9 neutrons

17. Example Hydrogen exists in 3 different isotopes Most hydrogen atoms have one proton, (one electron) and no neutrons Mass is 1 a.m.u. This is also called Hydrogen-1 or Protium

18. Some Hydrogen atoms have one neutron as well as the one proton and electron. This is a different isotope - it is still hydrogen, but it has a mass of 2 a.m.u. This isotope is called Hydrogen-2 Also called Deuterium

19. A third form of hydrogen has 2 neutrons with 1 proton and 1 electron. This gives a mass of 3 a.m.u. This is called Hydrogen-3 Also called Tritium

20. Atomic Mass (Decimal Number) The mass reported on the periodic table is actually a weighted average of the masses of all the isotopes of an element. This is why the periodic table show decimal number. For most atoms, one isotope is much more common than the other(s).

21. Assignment Do Isotope Worksheet