NE 105 - Introduction to Nuclear EngineeringSpring 2011

Classroom Session 2 - Fundamental Concepts

•Molecular weight•Mole•Isotopic Abundances•Classic and Relativistic Calculations

2

Solution to Quiz #0:

3

4

5

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

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.…

3

33

2

22

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…

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 AX.e.g. 235U, 16O, 3H, 14C

ZAX

10

Chart of the Nuclides

Z

N

IsobarsIsotopes

Isotones

11

Isobars = A

12

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