1. NE 105 - Introduction to Nuclear Engineering Spring 2011 Classroom Session 2 - Fundamental Concepts Molecular weight Mole Isotopic Abundances Classic and Relativistic Calculations

2. 2 Solution to Quiz #0:

3. 3

4. 4

5. 5

6. 6 Solving Problems, working with units and doing calculations. 1. Stop! Think. Read again. Inventory given data, and equations known. 2. Make a diagram. 3. Write equations, do the algebra. 4. Replace values with the units included. 5. Simplify if possible and compute (including UNITS). 6. Make sense of answer/Review process.

7. 7 Strong Suggestion: Use conversion factors as a “1” factor. Example: Use Quad-Lock Converter – If desired Use Mathematica/Maple/etc programs or practice using your calculator.…

8. or suffer the consequences. Show at least first complete calculation including units. Box answers Staple homework Be mindful of significant digits Number all your pages Please work neat…

9. 9 Atomic and Nuclear Nomenclature X, the atomic symbol (H, He, Na, Xe, U, etc.) represents the number of charges in the nucleus (thus electrons, thus chemical behavior). A = Mass number = protons + neutrons = Nucleons. Z = atomic number = protons. X and Z are redundant and normally we only write A X. e.g. 235 U, 16 O, 3 H, 14 C

10. 10 Chart of the Nuclides Z N Isobars Isotopes Isotones

11. Isobars = A 11

12. 12 Atomic Mass Unit 1/12 of the mass of 12 C Units are: AMU (1 AMU= 1.66e-27 kg) or g/mole How much a Mole of something weights Mole (mol) = Avogadro # of entities. Atomic and molecular weights are given in grams/mole Concept similar to a “dozen” except it is: 6.022 x 10 23 6.02e23 atoms of carbon weight 12 g Notice the mole concept let you convert from mass to number of atoms/molecules