Post by russjensenutah on Jan 15, 2014 8:06:02 GMT
Not a great video explanation of the general elements involved. So I am asking for confirmation or correction of this information. Sorry I have to redo this video. The show will resume momentarily, head up to the snack bar and get some goodies! 
Fukushima Fission or Hydrofluoric Acid??
Why are the creatures in the Pacific dying? The radiation levels are not that high?
Does not matter, it is still lethal to all biological life
Sourced from the following fukushimatruths.freeforums.net/thread/392/links-uranyl-nitrate-scientific-stuff
Uranium Dioxide/Uranium Hexafluoride (UF6) to Uranyl Fluoride to Hydrogen Fluoride aka Hydrofluoric Acid
Uranium dioxide or uranium(IV) oxide (UO2), also known as urania or uranous oxide, is an oxide of uranium, and is a black, radioactive, crystalline powder that naturally occurs in the mineral uraninite. It is used in nuclear fuel rods in nuclear reactors. A mixture of uranium and plutonium dioxides is used as MOX fuel.
Enrichment methods
Isotope separation is difficult because two isotopes of the same elements have very nearly identical chemical properties, and can only be separated gradually using small mass differences. (235U is only 1.26% lighter than 238U.) This problem is compounded by the fact that uranium is rarely separated in its atomic form, but instead as a compound UF6 Uranium Hexaflouride (235UF6 is only 0.852% lighter than 238UF6.) A cascade of identical stages produces successively higher concentrations of 235U. Each stage passes a slightly more concentrated product to the next stage and returns a slightly less concentrated residue to the previous stage.
Uranium Hexafluoride (UF6), referred to as "hex" in the nuclear industry, is a compound used in the uranium enrichment process that produces fuel for nuclear reactors and nuclear weapons. It forms solid grey crystals at standard temperature and pressure, is highly toxic, reacts violently with water and is corrosive to most metals. It reacts mildly with aluminium, forming a thin surface layer of AlF3 that resists further reaction.
Preparation
Milled uranium ore—U3O8 or "yellowcake"—is dissolved in nitric acid, yielding a solution of uranyl nitrate UO2(NO3)2. Pure uranyl nitrate is obtained by solvent extraction, then treated with ammonia to produce ammonium diuranate ("ADU", (NH4)2U2O7). Reduction with hydrogen gives UO2, which is converted with hydrofluoric acid (HF) to uranium tetrafluoride, UF4. (Green Salt) Oxidation with fluorine yields UF6.
During nuclear reprocessing, uranium is reacted with chlorine trifluoride to give UF6:
U + 2 ClF3 → UF6 + Cl2
About 95% of the depleted uranium produced to date is stored as uranium hexafluoride, DUF6, in steel cylinders in open air yards close to enrichment plants. Each cylinder contains up to 12.7 tonnes (or 14 US tons) of solid UF6. In the U.S. alone, 560,000 tonnes of depleted UF6 had accumulated by 1993. In 2005, 686,500 tonnes in 57,122 storage cylinders were located near Portsmouth, Ohio, Oak Ridge, Tennessee, and Paducah, Kentucky.[12][13] The long-term storage of DUF6 presents environmental, health, and safety risks because of its chemical instability.
When Uranium hexafluoride (UF6), is exposed to moist air, it reacts with the water in the air to produce UO2F2 (uranyl fluoride) and HF (hydrogen fluoride) both of which are highly corrosive and toxic. Storage cylinders must be regularly inspected for signs of corrosion and leaks. The estimated lifetime of the steel cylinders is measured in decades.[14]
Uranyl fluoride (UO2F2), a compound of uranium, is an intermediate in the conversion of uranium hexafluoride UF6 to an uranium oxide or metal form and is a direct product of the reaction of UF6 with moisture in the air. It is very soluble in water. Uranyl fluoride also is hygroscopic and changes in color from brilliant orange to yellow after reacting with water.
Uranyl fluoride is reported to be stable in air to 300 °C, above which slow decomposition to U3O8 occurs. When heated to decomposition, UO2F2 emits toxic fluoride fumes.
In accidental releases of UF6, UO2F2, as a solid particulate compound, may deposit on the ground. The overall chemical reaction of this event can be represented as:
UF6 + 2 H2O → UO2F2 + 4 HF.
These reactions can take place whether the uranium hexafluoride is a solid or a gas, but will take place almost instantaneously when the UF6 is in a gaseous state. The resulting hydrofluoric acid and the presence of additional water results in formation of solids (primarily Hydrofluoric adducts of hydrated uranyl fluoride (UO2F2−nH2O). Bucky Balls
Toxicology
Chemical hazards are far more significant than radioactive hazards, though there is a radioactivity concern if prepared with enriched uranium. Material is corrosive, and harmful by inhalation, ingestion or skin absorption. Ingestion or inhalation may be fatal. Effects of exposure may be delayed.
Hydrofluoric acid (HF) is a solution of hydrogen fluoride in water. It is a valued source of fluorine and is a precursor to numerous pharmaceuticals such as fluoxetine (Prozac) and diverse materials such as PTFE (Teflon).
Hydrofluoric acid is a highly corrosive acid, capable of dissolving many materials, especially oxides. Its ability to dissolve glass has been known since the 17th century, even before Carl Wilhelm Scheele prepared it in large quantities in 1771.[2] Because of its high reactivity toward glass and moderate reactivity toward many metals, hydrofluoric acid is usually stored in plastic containers (although PTFE is slightly permeable to it).[3]
Hydrogen fluoride gas is an acute poison that may immediately and permanently damage lungs and the corneas of the eyes.
Aqueous hydrofluoric acid is a contact-poison with the potential for deep, initially painless burns and ensuing tissue death. By interfering with body calcium metabolism, the concentrated acid may also cause systemic toxicity and eventual cardiac arrest and fatality, after contact with as little as 160 cm2 (25 square inches) of skin.
www.laka.org/nieuws/bijlagen/2003/07/uranyl_fluoride.pdf
Uranyl Fluoride (U02F2) Uranium hexafluoride (UF6),
The presence of U02F2 is characterized by a cloud of white. smoke like vapor. A nuclear scientist from a French enriched fuel fabrication plant warns that
"... even a slow leakage of UF6 will give rise to the formation of an opaque and toxic cloud of uranyl
fluoride (U02F2), which would rule out any possibility of local remedial action unless gas-tight safetyequipment including self-contained breathing apparatus is available. "15
U02F2 is formed as a very fine powder with a particle size of 0.5 microns.1B Such small particles settle very slowly, leading to greatest deposition away from the accident site if a wind is blowing. Concentrations of about one mg/m3 U02F2 are visible,11and visibility does not exceed 90 cm at concentrations of one g/m3.1s
www.iaea.org/inis/collection/NCLCollectionStore/_Public/12/626/12626650.pdf?origin=publication_detail
ie.lbl.gov/fission/endf349.pdf
onlinelibrary.wiley.com/doi/10.1002/9783527618798.app5/pdf
sti.srs.gov/fulltext/dpms6862/dpms6862.pdf
en.wikipedia.org/wiki/Buckminsterfullerene
Fukushima Fission or Hydrofluoric Acid??
Why are the creatures in the Pacific dying? The radiation levels are not that high?
Does not matter, it is still lethal to all biological life
Sourced from the following fukushimatruths.freeforums.net/thread/392/links-uranyl-nitrate-scientific-stuff
Uranium Dioxide/Uranium Hexafluoride (UF6) to Uranyl Fluoride to Hydrogen Fluoride aka Hydrofluoric Acid
Uranium dioxide or uranium(IV) oxide (UO2), also known as urania or uranous oxide, is an oxide of uranium, and is a black, radioactive, crystalline powder that naturally occurs in the mineral uraninite. It is used in nuclear fuel rods in nuclear reactors. A mixture of uranium and plutonium dioxides is used as MOX fuel.
Enrichment methods
Isotope separation is difficult because two isotopes of the same elements have very nearly identical chemical properties, and can only be separated gradually using small mass differences. (235U is only 1.26% lighter than 238U.) This problem is compounded by the fact that uranium is rarely separated in its atomic form, but instead as a compound UF6 Uranium Hexaflouride (235UF6 is only 0.852% lighter than 238UF6.) A cascade of identical stages produces successively higher concentrations of 235U. Each stage passes a slightly more concentrated product to the next stage and returns a slightly less concentrated residue to the previous stage.
Uranium Hexafluoride (UF6), referred to as "hex" in the nuclear industry, is a compound used in the uranium enrichment process that produces fuel for nuclear reactors and nuclear weapons. It forms solid grey crystals at standard temperature and pressure, is highly toxic, reacts violently with water and is corrosive to most metals. It reacts mildly with aluminium, forming a thin surface layer of AlF3 that resists further reaction.
Preparation
Milled uranium ore—U3O8 or "yellowcake"—is dissolved in nitric acid, yielding a solution of uranyl nitrate UO2(NO3)2. Pure uranyl nitrate is obtained by solvent extraction, then treated with ammonia to produce ammonium diuranate ("ADU", (NH4)2U2O7). Reduction with hydrogen gives UO2, which is converted with hydrofluoric acid (HF) to uranium tetrafluoride, UF4. (Green Salt) Oxidation with fluorine yields UF6.
During nuclear reprocessing, uranium is reacted with chlorine trifluoride to give UF6:
U + 2 ClF3 → UF6 + Cl2
About 95% of the depleted uranium produced to date is stored as uranium hexafluoride, DUF6, in steel cylinders in open air yards close to enrichment plants. Each cylinder contains up to 12.7 tonnes (or 14 US tons) of solid UF6. In the U.S. alone, 560,000 tonnes of depleted UF6 had accumulated by 1993. In 2005, 686,500 tonnes in 57,122 storage cylinders were located near Portsmouth, Ohio, Oak Ridge, Tennessee, and Paducah, Kentucky.[12][13] The long-term storage of DUF6 presents environmental, health, and safety risks because of its chemical instability.
When Uranium hexafluoride (UF6), is exposed to moist air, it reacts with the water in the air to produce UO2F2 (uranyl fluoride) and HF (hydrogen fluoride) both of which are highly corrosive and toxic. Storage cylinders must be regularly inspected for signs of corrosion and leaks. The estimated lifetime of the steel cylinders is measured in decades.[14]
Uranyl fluoride (UO2F2), a compound of uranium, is an intermediate in the conversion of uranium hexafluoride UF6 to an uranium oxide or metal form and is a direct product of the reaction of UF6 with moisture in the air. It is very soluble in water. Uranyl fluoride also is hygroscopic and changes in color from brilliant orange to yellow after reacting with water.
Uranyl fluoride is reported to be stable in air to 300 °C, above which slow decomposition to U3O8 occurs. When heated to decomposition, UO2F2 emits toxic fluoride fumes.
In accidental releases of UF6, UO2F2, as a solid particulate compound, may deposit on the ground. The overall chemical reaction of this event can be represented as:
UF6 + 2 H2O → UO2F2 + 4 HF.
These reactions can take place whether the uranium hexafluoride is a solid or a gas, but will take place almost instantaneously when the UF6 is in a gaseous state. The resulting hydrofluoric acid and the presence of additional water results in formation of solids (primarily Hydrofluoric adducts of hydrated uranyl fluoride (UO2F2−nH2O). Bucky Balls
Toxicology
Chemical hazards are far more significant than radioactive hazards, though there is a radioactivity concern if prepared with enriched uranium. Material is corrosive, and harmful by inhalation, ingestion or skin absorption. Ingestion or inhalation may be fatal. Effects of exposure may be delayed.
Hydrofluoric acid (HF) is a solution of hydrogen fluoride in water. It is a valued source of fluorine and is a precursor to numerous pharmaceuticals such as fluoxetine (Prozac) and diverse materials such as PTFE (Teflon).
Hydrofluoric acid is a highly corrosive acid, capable of dissolving many materials, especially oxides. Its ability to dissolve glass has been known since the 17th century, even before Carl Wilhelm Scheele prepared it in large quantities in 1771.[2] Because of its high reactivity toward glass and moderate reactivity toward many metals, hydrofluoric acid is usually stored in plastic containers (although PTFE is slightly permeable to it).[3]
Hydrogen fluoride gas is an acute poison that may immediately and permanently damage lungs and the corneas of the eyes.
Aqueous hydrofluoric acid is a contact-poison with the potential for deep, initially painless burns and ensuing tissue death. By interfering with body calcium metabolism, the concentrated acid may also cause systemic toxicity and eventual cardiac arrest and fatality, after contact with as little as 160 cm2 (25 square inches) of skin.
www.laka.org/nieuws/bijlagen/2003/07/uranyl_fluoride.pdf
Uranyl Fluoride (U02F2) Uranium hexafluoride (UF6),
The presence of U02F2 is characterized by a cloud of white. smoke like vapor. A nuclear scientist from a French enriched fuel fabrication plant warns that
"... even a slow leakage of UF6 will give rise to the formation of an opaque and toxic cloud of uranyl
fluoride (U02F2), which would rule out any possibility of local remedial action unless gas-tight safetyequipment including self-contained breathing apparatus is available. "15
U02F2 is formed as a very fine powder with a particle size of 0.5 microns.1B Such small particles settle very slowly, leading to greatest deposition away from the accident site if a wind is blowing. Concentrations of about one mg/m3 U02F2 are visible,11and visibility does not exceed 90 cm at concentrations of one g/m3.1s
www.iaea.org/inis/collection/NCLCollectionStore/_Public/12/626/12626650.pdf?origin=publication_detail
ie.lbl.gov/fission/endf349.pdf
onlinelibrary.wiley.com/doi/10.1002/9783527618798.app5/pdf
sti.srs.gov/fulltext/dpms6862/dpms6862.pdf
en.wikipedia.org/wiki/Buckminsterfullerene
so whats happening in the Solomons, is haarp missing its mark?