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66 Cards in this Set
- Front
- Back
Atomic Number |
The number of protons in the nucleus of an atom |
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Mass Number |
The total number of protons and neutrons in the nucleus of an atom |
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Isotope |
Two atoms that have the same number of protons but different number of neutrons |
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Nuclide |
Atom's nucleus |
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Nuclear Reaction |
A reaction that involves changes in the nucleus of an atom |
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Radioactive (nuclear) decay |
The spontaneous breakdown of an unstable nucleus of an atom |
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Nuclear Stability |
The ability of a nucleus to stay together and not fall apart |
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Alpha Particle |
A radioactive particle composed of 2 protons and 2 neutrons |
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Beta Particle |
A radioactive particle that is identical to an electron but is emitted from an atom's nucleus |
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Positron |
A radioactive particle that is identical to an electron but has a positive charge |
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Gamma Radiation |
A very high energy type of radiation that is often emitted from unstable nuclei |
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Ionizing Ability |
The ability of a subatomic particle to knock electrons off of an atom |
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Penetrating Ability |
The ability of a subatomic particle to pass through a material |
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Balanced Nuclear Equation |
An equation that describes the radioactive decay of an unstable nucleus. The total number of protons and neutrons in the reactants must equal the total number of protons and neutrons in the products |
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Zone of Stability |
The area on a neutron-proton graph where the nuclei are stable and do not emit radioactive particles. |
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Decay Rate |
A measure of how often an unstable nucleus emits a radioactive particle |
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Half Life |
The amount of time it takes for 1/2 of a sample of radioactive nuclei to decay = T1/2 |
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Mass Defect |
The difference in mass between the products and the reactants in a nuclear reaction. The products of a nuclear reaction usually weigh less than the reactants |
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Nuclear Binding Energy |
The energy between the protons and neutrons in a nucleus that binds these particles to each other. The more nuclear binding energy around each particle then the more stable the nucleus. |
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Nuclear Fission |
The splitting of a large unstable nucleus into two smaller nuclei |
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Chain Reaction |
This occurs when the neutrons emitted during a fission reaction cause other nearby nuclei to fission |
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Sub-critical Mass |
A sample of radioactive nuclei that does not contain enough nuclei to sustain a chain reaction. |
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Critical Mass |
A sample of radioactive nuclei with the number of nuclei required to produce a self sustaining chain reaction. |
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Super-critical Mass |
A sample of radioactive nuclei that contains too many nuclei resulting in a chain reaction that produces excessive fission reactions = nuclear bomb |
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Nuclear Reactor |
An electricity producing power plant that uses the heat released from fission reactions |
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Reactor Core |
The area of a nuclear power plant where the fission reaction occurs |
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Fuel Rods |
These contain unstable nuclei whose fission results in a significant mass defect. U-235 & Pu-239 serve as the unstable nuclei in the fuel rods |
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Control Rods |
These absorb the excess neutrons during the fission reaction and slow the chain reaction. They can be cadmium or boron atoms |
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Moderator - Graphite vs Heavy Water |
A material that surrounds the fuel rods and serves to slow down the neutrons so the U-235 or Pu-239 can capture them - Graphite - cheap but if caught on fire can not be put out - Heavy Water - expensive but will not catch on fire -- US standard |
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Coolant |
The water in the reactor core that removes the heat released by the fission process |
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Turbine |
A device that removes the kinetic energy from steam and then powers the generator |
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Generator |
A device that changes the kinetic energy of the turbine into electricity |
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Nuclear Fusion |
The combining of two small nuclei to form a larger nucleus |
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∆ G = ∆ H -t∆ S -- Gibbs Free Energy |
1) -∆H , -∆S = Spontaneous @ low temperatures 2) -∆H , ∆S = Always spontaneous regardless of temperature 3) ∆H , ∆S = Spontaneous @ high temperatures 4) ∆H, -∆S = Never spontaneous |
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Nuclear transformations involve the change of one _____ into another. |
Element |
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Who observed the first nuclear transformation? |
Lord Rutherford |
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A device that gives particles very high velocities |
Particle Accelerator |
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A Geiger counter is filled with ____ gas. |
Argon |
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A _______ counter involves the release of light by some compound when struck by high energy radiation. |
Scintillation |
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Ancient artifacts made from ______ can be dated by the C-14 dating method. |
Wood |
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The C-14 content of the atmosphere up to 10,000 years ago can be estimated by measuring the C-14 content inside ___. |
Trees |
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I-131 is useful to diagnose and treat diseases of the _____. |
Thyroid |
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Th-201 is useful to determine the amount of damage suffered by a person who has had a _____. |
Heart attack |
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Balanced equation showing the decay of C-14 |
C-14 --> N-14 + e- (beta particle)
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Balance equation showing how C-14 is created in the atmosphere |
1n + N-14 --> C-14 + 1p |
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Speed of Light Constant |
3 x 10^8 m/sec |
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System |
The chemical reaction on which we are focused |
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Surroundings |
The space around the chemical reaction on which we are focused |
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Energy |
Anything that has the ability to do work |
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Law of Conservation of Energy |
The total amount of energy in the universe remains constant. Energy can change location or energy can change form |
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Work |
The movement of an object against an opposing force |
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Expansion Work |
The work done by a gas on nearby objects as gas expands |
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Heat |
The type of energy that naturally moves from a warm object to a cooler object |
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Temperature |
A measure of the motion or kinetic energy of the atoms in a material |
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Calorimetry |
The science of measuring amounts of heat gained or lost by compounds
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Specific Heat |
The amount of heat needed to raise the temperature of 1 gram of material by 1 Celsius. Water Cp = 4.18 J/gdegC |
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Calorimeter |
A devise in which the heat needed to raise the temperature of a calorimeter by 1 Celsius |
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Heat of Combustion |
The amount of heat released when 1 gram of a material is burned |
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Enthalpy |
The heat stored in a compound |
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Standard states |
The form of a compound under standard room conditions, 1 atm and 25C |
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Standard Heat of Formation |
The amount of heat gained or released when 1 mole of a compound is synthesized from the elements in their standard states |
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Hess's Law |
The heat absorbed or released during a complex chemical reaction can be calculated by breaking the complex reaction down into a series of simple reactions. The heat absorbed or released by the complex reaction is the sum of the heats absorbed and released during simple reactions |
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Entropy |
The amount of disorder in a group of molecules |
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Second Law of Thermodynamics |
During a spontaneous chemical reaction the total entropy of the universe increases |
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Free Energy |
Energy not contained with any atoms or molecules |
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Spontaneous Reaction |
A chemical reaction that occurs on its own without any outside influence |