IB Physics 12 Nuclear Physics 5 Mr. Jean

The plan: Video clip of the day –Example of fission energies –Example of fusion energies –Recap of nuclear physics

Conservation Laws For any nuclear reaction, there are three conservation laws which must be obeyed: Conservation of Charge: The total charge of a system can neither be increased nor decreased. Conservation of Nucleons: The total number of nucleons in a reaction must be unchanged. Conservation of Mass Energy: The total mass-energy of a system must not change in a nuclear reaction.

Nuclear Reactions: yQhttp:// yQ Nuclear reactions (Yelling Guy)

Example 7: Use conservation criteria to determine the unknown element in the following nuclear reaction: Charge before = = +4 Charge after = +2 + Z = +4 Z = 4 – 2 = 2 Nucleons before = = 8 Nucleons after = 4 + A = 8 (Helium has Z = 2) (Thus, A = 4)

Conservation of Mass-Energy There is always mass-energy associated with any nuclear reaction. The energy released or absorbed is called the Q-value and can be found if the atomic masses are known before and after. Q is the energy released in the reaction. If Q is positive, it is exothermic. If Q is negative, it is endothermic.

Example 8: Calculate the energy released in the bombardment of lithium-7 with hydrogen- 1. Substitution of these masses gives: Q = u(931.5 MeV/u) Q =17.3 MeV The positive Q means the reaction is exothermic.

Radioactive Decays: ssentialchemistry/flash/radioa7.swfhttp:// ssentialchemistry/flash/radioa7.swf –Alpha –Beta –Gamma –Compare Check out this page:

Mass-energy: LBRqjQhttp:// LBRqjQ

Chain Reactions: Chain Reaction – neutrons released from one fission reaction go on to initiate further reactions.

Nuclear Fission: Controlled nuclear fission: –nuclear power production some material absorbs excess neutrons before striking nucleus. –leaving only one neutron from each reaction to produce another reaction.

Controlled Reaction:

Uncontrolled Reaction:

Demonstration: 10.1 Chain reaction of elements

Chernobyl Today:

Nuclear Fission: Critical Mass: if mass of uranium is too small, too many neutrons escape without causing further fission in uranium so the reaction cannot be sustained Thermal Neutron: low-energy neutron (≈1eV) that favors fission reactions – energy comparable to gas particles at normal temperatures

Nuclear Reactions:

Natural Isotopes: Naturally Occurring Isotopes of Uranium: Uranium-238: most abundant, 99.3%, very small probability of fissioning when it captures a neutron, not used for fuel, more likely to capture high energy neutron than low energy one Uranium-235: 0.3%, 500 times greater probability of fissioning when captures a neutron but must be a low-energy (thermal) neutron, used for fuel

Fuel Enrichment: This process of increasing proportion of uranium-235 in a sample of uranium –1) formation of gaseous uranium (uranium hexafluoride) from uranium ores –2) Separated in gas centrifuges by spinning – heavier U-238 moves to outside –3) increases proportion of U-235 to about 3% to be used as fuel in nuclear reactors

Fuel Enrichment: Advantage: more uranium is available for fission and reaction can be sustained Disadvantage: enriched fuel can be used in the manufacture of nuclear weapons – threat to world peace – 85% = weapons grade

Inside the reactor: Moderator: material (water, graphite) used to slow down high-energy neutrons emitted from fission reactions to thermal levels for use in further fission reactions to sustain the chain reaction - slow neutrons by collisions Control Rods: inserted between fuel rods – made of neutron-absorbing cadmium or boron - used to control reactor temperature to prevent overheating – lowered if too many neutrons/reactions and excess thermal neutrons are absorbed

Nuclear Waste: Low-level waste: radioactive material from mining, enrichment and operation of plant – must be disposed of – left untouched or encased in concrete High-level waste: disposal of spent fuel rods- some isotopes have ½ lives of thousands of years – plutonium 240,000 years stored under water at reactor site for several years to cool of then sealed in steel cylinders, buried underground reprocessed to remove any plutonium and useful uranium, remaining isotopes have shorter ½ lives and long-term storage need is reduced

Nuclear Weapons Manufacture: –Enrichment technology could be used to make weapons grade uranium (85%) rather than fuel grade (3%) –Plutonium is most used isotope in nuclear weapons and can be gotten from reprocessing spent fuel rods

Example Question: Suppose the average power consumption for a household is 500 W per day. Estimate the amount of uranium-235 that would have to undergo fission to supply the household with electrical energy for a year. Assume that for each fission, 200 MeV is released.

Nuclear Fission: 7U41M (Yelling guy) 7U41M ob9s8 (Non-yelling) ob9s8

Example Question #2: A fission reaction taking place in a nuclear power station might be –Estimate the initial amount of uranium-235 needed to operate a 600 MW reactor for one year assuming 40% efficiency and 200 MeV released for each fission reaction.

Nuclear Fusion:

Nuclear Fusion: Two light nuclei combine to form a more massive nucleus with the release of energy. Write the reaction equation for the fusion reaction shown below.

To calculate how much energy is released in this fusion reaction we would need to again use the change in mass vs. energy relationship.

Plasma: fuel for reactor – high energy ionized gas (electrons and nuclei are separate) – if energy is high enough (hot enough), nuclei can collide fast enough to overcome Coulomb repulsion and fuse together Magnetic confinement: charged particles are contained via magnetic fields – travel in a circle in a doughnut shaped ring (tokamak) Heating Plasma: accelerate nuclei by means of magnetic fields and forces = high temperatures (high kinetic energies)

Problems with current fusion technology: –Maintaining and confining very high-density and high-temperature plasmas – very difficult to do – uses more energy input than output – not commercially efficient

Fusion Reactions:

Summary ParticleFig.SymMassChargeSize Electron e 9.11 x kg -1.6 x C  Proton p x kg +1.6 x C 3 fm Neutron n x kg 0 3 fm Fundamental atomic and nuclear particles The mass number A of any element is equal to the sum of the protons (atomic number Z) and the number of neutrons N : A = N + Z

Summary Definitions: A nucleon is a general term to denote a nuclear particle - that is, either a proton or a neutron. The mass number A of an element is equal to the total number of nucleons (protons + neutrons). Isotopes are atoms that have the same number of protons (Z 1 = Z 2 ), but a different number of neutrons (N). (A 1  A 2 ) A nuclide is an atom that has a definite mass number A and Z-number. A list of nuclides will include isotopes.

Summary (Cont.) Symbolic notation for atoms Mass defect m D Binding Energy per nucleon E B = m D c 2 where c 2 = MeV/u Binding energy

Summary (Decay Particles) An alpha particle  is the nucleus of a helium atom consisting of two protons and two tightly bound neutrons. A beta-minus particle    is simply an electron that has been expelled from the nucleus. A beta positive particle    is essentially an electron with positive charge. The mass and speeds are similar. A gamma ray  has very high electromagnetic radiation carrying energy away from the nucleus.

Summary (Cont.) Alpha Decay: Beta-minus Decay: Beta-plus Decay:

Summary (Radioactivity) Nuclei Remaining Activity R Mass Remaining Number of Half-lives: The half-life T 1/2 of an isotope is the time in which one-half of its unstable nuclei will decay.

Summary (Cont.) Conservation of Charge: The total charge of a system can neither be increased nor decreased. Conservation of Nucleons: The total number of nucleons in a reaction must be unchanged. Conservation of Mass Energy: The total mass- energy of a system must not change in a nuclear reaction. (Q-value = energy released) Nuclear Reaction:x + X  Y + y + Q