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NE 105 - Introduction to Nuclear EngineeringSpring 2011
Classroom Session 2 - Fundamental Concepts
•Molecular weight•Mole•Isotopic Abundances•Classic and Relativistic Calculations
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Solution to Quiz #0:
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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.
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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.…
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611
1001mor
000,101
1001mor
1001m 1m100cm
impunity. with "1"by multipy alwayscan you --- 1196.1
1196.11
cmem
cmcmm
cmcm
JeeVJeeV
or suffer the consequences.Show at least first complete calculation including units.Box answersStaple homeworkBe mindful of significant digitsNumber all your pages
Please work neat…
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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 AX.e.g. 235U, 16O, 3H, 14C
ZAX
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Chart of the Nuclides
Z
N
IsobarsIsotopes
Isotones
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Isobars = A
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Atomic Mass Unit1/12 of the mass of 12C 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 1023
6.02e23 atoms of carbon weight 12 g
Notice the mole concept let you convert from mass to number of atoms/molecules