Quiz 2 Unit 2 Flashcards
Chemical VS Nuclear Reactions Same
Atoms attain stability, mass and change must be balanced
Radioactivity
Process by which an unstable nucleus spontaneously emits high energy particles or rays from the nucleus in order to attain stability
Radioactive Isotope/Radioisotope
Isotope with an unstable nucleus
Strong Nuclear Force/Strong Force
An attractive force that binds protons and neutrons together in the nucleus, stronger than the four fundamental forces
Electrostatic Force
Causes protons to repel other protons
Nuclear Force
Created by neutrons and holds nucleus together
Unstable and Radioactive Elements
Above #83 or found by finding neutron to proton ratio
Finding Neutron to Proton Ratio
Subtract mass number and atomic number then divide by atomic number
Majority of Isotopes
Are unstable and decay over time
Elements Below #20
Have 1:1 neutron to proton ratio
Band of Stability
Relationship between nuclear force and electrostatic forces between protons
Decay Occurs in Order To
Return nucleus to band of stability
Nuclear Reaction
Affects the nucleus of the atom, giving off large amounts of energy
Alpha Particle
4/2 He, +2 charge, 4 amu, heavy, low penetration, low danger
Beta Particle
0/-1 e, -1 charge, 0 amu, light, medium penetration, medium danger
Gamma Ray
0/0 y, 0 charge, 0 amu, no mass, high penetration, high danger
Radiation Changes to Nucleus
Alpha mass number -4 atomic number -2
Beta neutron to proton atomic number +1
Gamma no change
Positron
Particle that has same mass as electron but opposite charge
Positron Emission
0/+1 e
Neutron Emission
1/0 n
Proton Emission
1/1 p
Emission
Top mass bottom charge
K-Capture
When a nucleus captures an electron from their inner most energy level
Proton and Electron Form
A neutron
Alpha Particle is A
Helium nucleus
Beta Particle is An
Electron
Quarks
Protons are made of two up and one down
Neutrons are made of two down and one up
In Beta Decay
Electron leaves which adds a proton
In Electron Capture or Positron Emission
Proton leaves which adds an electron
Large Atom VS Small Atom
Alpha VS beta
Bombardment/Capture
Radiation taken in
Nuclear VS Chemical Reactions Different
Nucleus VS electrons
In nuclear elements change, isotopes matter, spontaneous, can not be sped up/slowed/stopped, decay chain
Transmutation
Elements change to other elements
Decay Chain
If the product of a nuclear reaction is unstable, it will decay as well
Alpha Decay
4 He + mass number -4 new symbol
2 atomic number -2
Radioactive/Parent Isotope
Isotope in reactant
Daughter Isotope
Isotope in product
Beta Decay
0 e + mass number new symbol
-1 atomic number +1
Capture VS Decay
Follow the signs VS opposite
Artificial Radioactive Nuclides
Made by artificial transmutations through the bombardments of nuclei with charged and uncharged particles
Transuranium Elements
Elements produced by artificial transmutations, beyond uranium #92
Bombardment Reactions
Induced by accelerating a particle and colliding it with a nuclei
Particle Accelerators
Make particles race towards each other a little less than the speed of light than collide
Nuclear Fission
Very heavy nucleus splits into more stable nuclei
Chain Reaction
Self propagating reaction or the material that starts is also the product and creates another reaction
Critical Mass
The mass required to sustain a chain reaction
Nuclear Fusion
Combining two light nuclei to form a heavier, more stable nucleus, deuterium-tritium fusion reaction
Deuterium
Stable isotope of hydrogen with an added neutron
Tritium
Radioactive isotope of hydrogen with two neutrons
Fission VS Fusion
1) Uranium-235 is limited, fuel is abundant
2) Danger of meltdown, none
3) Toxic waste, none
4) Thermal pollution, not yet sustainable
Fusion Requires
Material in plasma state
Radon Daughters
Short lived, very radioactive radon progeny
Decay Series
Series of radioactive isotopes produced by successive radioactive decay until a stable isotope is reached
Radioactive Isotopes Have
Too many or too few neutrons
Half-Life
(t1/2) The time required for half of the atoms in a radioactive isotope to decay
During Each Half-Life
Half of the remaining radioactive atoms decay into atoms of a new element
Shorter Half-Life Indicates
A less stable nucleus
Formula
mf = mi/2^n
mf = final mass
mi = initial mass
n = number of half-lives, the length of one is the total time passed
