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86 Cards in this Set
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Mendelecv
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orginized periodic table by atomic mass
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mosley
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organized periodic table by atomic number
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periodic law
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similiarities in elements are the result of the number of outermost valence electrons
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how much of the periodic table is metal
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2/3
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structure
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small section called metalloids
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metalloids
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elements with both metallic and non matallic properties
(B, Si, Ge, As, Sb, Te, Po) *Po = raidoactive |
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all elements with atom numbers greater than 83 are...
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raidoactive isotopes
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trend
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as you move left ---> to right you go from
Metal---> to metalloid ---> to non metal |
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groups
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18 of them
vertical columns of elements with similar properties because they have the same number of valence electrons AKA "Family" |
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group 1
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alkali metals
- most raidoactive mentals - do not exist free in nature - hydrogen although in group 1 is NOT an alkali metal |
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Group 2
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alkali earth metals
- very raidoactive metals - do not exist free in nature |
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Group 13
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- Boron = metalloid
- {Al - Te} Metals |
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group 14
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*Carbon* has allotropes
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allotropes
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any element which can exist in more than one form
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group 15
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contains nitrogen-- tripple bond
- tripple bond makes nitrogen almost unreactive |
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group 16
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halogens
- contains oxygen-- double bond - double bond makes oxygen somewhat unreactive |
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oxygen- allotropes
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has 2 allotropes
1= O2 (Gas) 2= O3 (gas) = ozone |
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group 17
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halogens
* most reactive non-metals * do not exist free in nature - contains (4) of the (7) HOFBrINCl2 --diatomic molecules H²- (g) O²- (g) F²- (g) Br²-(l) I²- (s) N²- (g) Cl²-(g) |
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Group 18
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noble/ inert gases
- monoatomic molecules -unreactive -some rare Xe & Kr compounds do exist (He, Ne, Ar, Kr, Xe, Rn) |
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periods
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7 of them
horizontal rows of elements |
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transition metals
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groups 3-11
periods 4-7 - some what unreactive metals - some transition metals can form colored solutions or solids (C4 = Blue) |
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lanthanide series
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(period 6) (57-71)(Can be found naturally on earth)
AKA: Rare earth elements or inner-transition elements * only one element in the series is raidoactive* |
top row of the section of the periodic table taken out
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actinide series
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(period 7) (89-103)
- all are raidoactive - not found in nature |
bottom row of the section take out of the periodic table
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symbols
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either single uppercase letter of an uppercase letter with and lowercase letter
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rutherford
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- credited with the discovery of the atomic nucleus
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rutherford's gold (Au) foil experiment
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rutherford "bombarded" a think gold foil with (alpha)particles which are positivly charged
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What does it mean??:
many particles moved passed the gold foil |
the atom is mostly EMPTY space
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What does it mean??:
some of the (+)alpha particles deflected back off the foil |
the Nucleus of an atom is (+) charged and that most of the mass of an atom is in the nucleus
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planets revolve around the sun like _____ revolves around the _____
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ELECTRONS revolves around the NUCLEUS
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electrons
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negative particle that is found OUTSIDE ther nucleus and has a mass of zero
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nucleus
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AKA: Nuclide or Nucleons
Protons and neutrons |
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proton
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symbol: P= :H (each . = 1)
charge: +1 Mass: 1g Location: inside nucleus |
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neutron
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symbol: n= ;1 (.=1 ,=0)
charge: +1 Mass:1g Location: inside nucleus |
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electron
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symbol: eˉ¹= ;e =ß
(.=1 ,=0)(ß= beta) charge: -1 Mass: 0 Location: outside nucleus |
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atomic number of protons
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never changes
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neutral atom
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# of particles = # of electrons
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ion
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an atom with an electron charge
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(+) Ion
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AKA: Cation
- an atom that has lost electrons |
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(-) Ion
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AKA: Anion
- an atom that has gained electrons |
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protons + neutrons =
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mass number
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symbol formate
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top left corner = mass #
top right corned = charge middle = element symbol bottom left = atomic number |
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isotope
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an atom with the same number of protons (atomic #) but a different number of neutrons (mass #)and thus a different mass
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Mass Number
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NOT EQUAL TO ATOMIC MASS!!
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atomic mass
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the weighted average, by mass of all know isotopes for a given element
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atomic mass is based on...
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the relative % abundance of each isotope in the element
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atomic mass unit (amu)
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a unit of mass based on the carbon- 12 isotope = 12.000 amu
* 1 amu = 1/12th mass of carbon-12 * |
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atomic mass formula
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atomic mass= (% abundance)(mass of isotope) + (% abundance)(mass of isotope)
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Boron has (2) isotopes.
B-10 has a mass of 10.013 amu and % abundance of 19.9% B-11 has a mass of 11.0093 amu and a % abundance of 80.1%what is the atomic mass of boron? |
atomic mass= (% abundance)(mass of isotope) + (% abundance)(mass of isotope)
X = (.199)(10.013) + (.801)(11.0093) X= 1.9925 + 8.8184 Atomic mass = 10.8109 |
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another name for nucleus
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nuclide
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natural radioactivity
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The spontaneous (decay) disintegration of “unstable” nuclei to “mere stable” nuclei through a transmutation of one element into another.
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transmutation
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one element change into another by releasing a sub atomic particle or proton of radiant energy
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why does transmutation occur?
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each radioactive isotope seeks to have a neutron proton ration of about 1:1 (n:p)
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lead block test
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separation of particles by magnetic and electric fields
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natural radioactive decay: General form
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A ---> B + C
A= unstable radioisotope B= stable isotope C= subatomic particle |
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law of conservation of charge and mass
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in nuclear process BOTH charge and mass are conserved
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Alpha decay
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releases an alpha particle
*mass # goes down by 4 and atomic # goes down by 2* |
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name the types of natural radioactive decay
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1- general
2- alpha 3- beta + 4- beta - |
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during alpha decay what is the change, if any, in mass # and/or Atomic #?
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Mass #- goes DOWN 4
Atomic # goes DOWN 2 |
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beta (-) decay
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releases a ß- = -1 e
(Beta negative = electron) |
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during Beta (-) decay what is the change, if any, in mass # and/or Atomic #?
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Mass #- remains the same
Atomic #- goes UP by 1 |
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Beta (+) decay
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releases the positron
(+1e) |
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during Beta (+) decay what is the change, if any, in mass # and/or Atomic #?
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Mass #- remains the same
Atomic #- goes DOWN 1 |
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artificial transmutation
(General form- formula) |
General form:
A+B --> C+D A= target nucleus B= bombarding particles C= new isotope D= subatomic particles |
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artifical transmutation
(definition) |
rediaisotopes are made in a lab when a target nucleus is bombarded with a high energy particle (proton, electron, neutron, positron)
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Particle accelerator
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mechines that speed up CHARGED particles so theat they can penetrate the target nucleus (series of electromagnetic fields)
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HALF LIFE of radioactive material
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the time it takes for a radioactive substance to decay to 1/2 its original mass
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does the half life ever change?
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NO!!! the half life NEVER changes- its uneffected by temperature, pressure or volume
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half life periods =
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total time
----------- (over) 1/2 life |
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use of radioisotopes
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1- chemical tracers : C-12
2- Medicine- short 1/2 life so that it will leave the body quickly 3- industry- to radiate food, to preserve it 4- geology/ archaeology- C-14/ U-238 ~ fossil dating |
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definition of Nuclear Energy
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the conversion of a small amount of mass into radiant energy
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nuclear energy
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~the starting materials (reactants) lose some mass and produce products that are more stable and lighter
~Enormous amounts of energy are produced |
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eintein called this the "Mass defect"
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E= MC²
E= energy M= mass C= speed of light |
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the two processes of nuclear energy
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nuclear fission and nuclear fusion
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definition of fission recations
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the "splitting" of HEAVY atomic nuclei into smaller, more stable "fission- fragments" and the release of a lot of energy
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process of fission reactions
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neutrons are "captured" by a target nucleus breaking a LARGE nucleus into smaller isotopes
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fission reactions result in
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1- energy
2- more radioisotopes 3- more neutrons |
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what is fission used for
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to produce electricity, radioisotopes used in medicein, and industry/research
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benefits of nuclear fission
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A- efficient source of energy without the air pollution associated with the burning of fossil fuels
B- produces useful radioisotopes used in medicine and research |
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Problems with nuclear fission
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A- Meltdown/Nuclear accident
B- coolant H2O is returned to its source over-heated killing fish and other animals C- the productiton of toxic raidoactive waste with long 1/2 lifes |
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fission fuel cells
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U-235
U-233 Pu-239 (breeder reactor) ** U-238, which comprises more than 99% of all natural Uranium is NOT fissionable fuel** |
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raidoactive waste with cause by fission
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its a problem becaus of its long 1/2 life and storage issues
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nuclear fusion
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the joining of (2) "light nuclei" to form a more stable and heavier nucleus
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nuclear fusion ________ energy compared to nuclear fission
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~*Produces greater*~
nuclear fusion PRODUCES GREATER energy compared to nuclear fission |
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why is it difficult for fusion to occur?
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A- b/c of the (+) charge of the small nuclei, a strong repulsive force exists between the nuclei making it difficult for them to react
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how do you make fusion happen?
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you need high temperatures
AKA: thermonuclear reactions |
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benefits of fusion
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could provide an unlimited source of energy without the pollution associated with the burning of fossil fuels and nuclear fission
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