2. Atomic Structure www.lab-initio.com

3. Section 4-1 Greek Philosophers (cont.) Many ancient scholars believed matter was composed of such things as earth, water, air, and fire. Many believed matter could be endlessly divided into smaller and smaller pieces.

4. Section 4-1 Greek Philosophers (cont.) Democritus (460–370 B.C. ) was the first person to propose the idea that matter was not infinitely divisible, but made up of individual particles called atomos. Aristotle (484–322 B.C. ) disagreed with Democritus because he did not believe empty space could exist. Aristotle’s views went unchallenged for 2,000 years until science developed methods to test the validity of his ideas.

5. Section 4-1 Greek Philosophers (cont.)

6. Section 4-1 Greek Philosophers (cont.) John Dalton revived the idea of the atom in the early 1800s based on numerous chemical reactions. Dalton’s atomic theory easily explained conservation of mass in a reaction as the result of the combination, separation, or rearrangement of atoms.Dalton’s atomic theory

7. Section 4-1 Greek Philosophers (cont.)

8. Modern Atomic Theory  All matter is composed of atoms  Atoms cannot be subdivided, created, or destroyed in ordinary chemical reactions. However, these changes CAN occur in nuclear reactions!  Atoms of an element have a characteristic average mass which is unique to that element.  Atoms of any one element differ in properties from atoms of another element  All matter is composed of atoms  Atoms cannot be subdivided, created, or destroyed in ordinary chemical reactions. However, these changes CAN occur in nuclear reactions!  Atoms of an element have a characteristic average mass which is unique to that element.  Atoms of any one element differ in properties from atoms of another element

9. Discovery of the Electron In 1897, J.J. Thomson used a cathode ray tube to deduce the presence of a negatively charged particle. Cathode ray tubes pass electricity through a gas that is contained at a very low pressure.

10. Conclusions from the Study of the Electron  Cathode rays have identical properties regardless of the element used to produce them. All elements must contain identically charged electrons.  Atoms are neutral, so there must be positive particles in the atom to balance the negative charge of the electrons  Electrons have so little mass that atoms must contain other particles that account for most of the mass  Cathode rays have identical properties regardless of the element used to produce them. All elements must contain identically charged electrons.  Atoms are neutral, so there must be positive particles in the atom to balance the negative charge of the electrons  Electrons have so little mass that atoms must contain other particles that account for most of the mass

11. Thomson’s Atomic Model Thomson believed that the electrons were like plums embedded in a positively charged “pudding,” thus it was called the “plum pudding” model.

12. Rutherford’s Gold Foil Experiment  Alpha (  ) particles are helium nuclei  Particles were fired at a thin sheet of gold foil  Particle hits on the detecting screen (film) are recorded

13. Rutherford’s Findings  The nucleus is small  The nucleus is dense  The nucleus is positively charged  Most of the particles passed right through  A few particles were deflected  VERY FEW were greatly deflected “Like howitzer shells bouncing off of tissue paper!” Conclusions:

14. Atomic Particles

15. Atomic Number Atomic number (Z) Atomic number (Z) of an element is the number of protons in the nucleus of each atom of that element.

16. Mass Number Mass number Mass number is the number of protons and neutrons in the nucleus of an isotope. Mass # = p + + n 0 8818 Arsenic753375 Phosphorus1531 16

17. Isotopes Isotopes are atoms of the same element having different masses due to varying numbers of neutrons.

18. Atomic Masses Atomic mass Atomic mass is the average of all the naturally occurring isotopes of that element. Carbon = 12.011

19. Nuclear Chemistry Bravo – 15,000 kilotons

20. Nuclear Symbols Element symbol Mass number (p + + n o ) Atomic number (number of p + )

21. Types of Radioactive Decay  alpha production (  He): helium nucleus  beta production (  e): gamma ray production (  ):  gamma ray production (  ):  alpha production (  He): helium nucleus  beta production (  e): gamma ray production (  ):  gamma ray production (  ):

22. Nuclear Stability Decay will occur in such a way as to return a nucleus to the band (line) of stability.

23. Alpha Radiation Alpha decay is limited to VERY large, nuclei such as those in heavy metals.

24. Beta Radiation Beta decay converts a neutron into a proton.

26. CA Standards

27. Fission Fission Fission - Splitting a heavy nucleus into two nuclei with smaller mass numbers.

28. Deuterium – Tritium Fusion Reaction Fusion Fusion - Combining two light nuclei to form a heavier, more stable nucleus.

29. Energy and Mass mass defect Nuclear changes occur with small but measurable losses of mass. The lost mass is called the mass defect, and is converted to energy according to Einstein’s equation:  E =  mc 2  m = mass defect  E = change in energy c = speed of light mass defect Nuclear changes occur with small but measurable losses of mass. The lost mass is called the mass defect, and is converted to energy according to Einstein’s equation:  E =  mc 2  m = mass defect  E = change in energy c = speed of light Because c 2 is so large, even small amounts of mass are converted to enormous amount of energy.

31. A Fission Reactor