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Saturday, November 24, 2012

FLUORIDE BATTLE RAGING IN AIKEN, SC..


Subject: FLUORIDE BATTLE RAGING IN AIKEN, SC...11-22-12
FORWARDED for Education, Edification, and Information Purposes Only
Not spam - contact: becworks@gmail.com   
++++++++++++++++++++

Scott:
[Responding]

Below is a sixth grade level of information on fluoride, with references to the industrial chemistry you lack...grow up...the nation poisoned entire generations of children...to gain control over the future...that was what Goals 2000 was all about.  I know, because I studied it at the University of South Carolina in my graduate studies in the 1990s.  You lack science knowledge. The universities are hell-bent on protecting the agenda, as is evident in the tweaked info on safety in public documents...it is safe but toxic...we are playing Russian Roulette with children's lives...and you are an accomplice to that agenda.

READ the following and learn.  Then, read the MSDS for sodium fluoride.  Then, read chemistry on fluoride, the most aggressive element in the periodic chart, because it replaces all elements beneath it on the chart.  Fluoride is not meant for human bodies.

Sincerely,
R.E. Sutherland
QUOTE:

Sodium fluoride

From Wikipedia, the free encyclopedia
Jump to: navigation, search
Sodium fluoride
http://en.wikipedia.org/wiki/File:Sodium-fluoride-3D-ionic.png
IUPAC name[hide]
Sodium fluoride
Other names[hide]
Florocid
Identifiers
5045 Yes
1690
WB0350000
[show]
Properties
NaF
41.988173 g/mol
Appearance
White solid
odorless
2.558 g/cm3
993 °C, 1266 K, 1819 °F
1704 °C, 1977 K, 3099 °F
36.4 (0 °C); 40.4 (20 °C); 50.5 (100 °C) g/L[1]
soluble in HF
insoluble in alcohol
1 mmHg @ 1077 C°[2]
1.336
Structure
cubic
Hazards
EU Index
009-004-00-7
http://en.wikipedia.org/wiki/File:Hazard_T.svgT - Toxic
http://en.wikipedia.org/wiki/File:Hazard_X.svg
Xi - Irritant
http://en.wikipedia.org/wiki/File:NFPA_704.svg
0
3
0
Non-flammable
52–200 mg/kg (oral in rats, mice, rabbits)[3]
Related compounds
Other anions
Other cations
Related compounds
  (verify) (what is: Yes/?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Sodium fluoride is an inorganic chemical compound with the formula NaF. A colorless solid, it is a source of the fluoride ion in diverse applications. Sodium fluoride is less expensive and less hygroscopic than the related salt potassium fluoride.

Contents

Structure, general properties, occurrence

Sodium fluoride is an ionic compound, dissolving to give separated Na+ and F ions. Like sodium chloride, it crystallizes in a cubic motif where both Na+ and F occupy octahedral coordination sites;[4][5] its lattice spacing, approximately 462 pm, is somewhat smaller than that of sodium chloride.
The mineral form of NaF, villiaumite, is moderately rare. It is known from plutonic nepheline syenite rocks.[6]

Production

NaF is prepared by neutralizing hydrofluoric acid or hexafluorosilicic acid (H2SiF6), byproducts of the production of superphosphate fertilizer. Neutralizing agents include sodium hydroxide and sodium carbonate. Alcohols are sometimes used to precipitate the NaF:
HF + NaOH → NaF + H2O
From solutions containing HF, sodium fluoride precipitates as the bifluoride salt NaHF2. Heating the latter releases HF and gives NaF.
HF + NaF NaHF2
In a 1986 report, the annual worldwide consumption of NaF was estimated to be several million tonnes.[7]

Applications

http://en.wikipedia.org/wiki/File:Sodium_fluoride_tablets.jpg
http://en.wikipedia.org/wiki/File:Sodium_fluoride_tablets.jpg
Sodium fluoride is sold in tablets for cavity prevention.
Fluoride salts are used to enhance the strength of teeth by the formation of fluorapatite, a naturally occurring component of tooth enamel.[8][9] Although sodium fluoride is also used to fluoridate water and, indeed, is the standard by which other water-fluoridation compounds are gauged, hexafluorosilicic acid (H2SiF6) and its salt sodium hexafluorosilicate (Na2SiF6) are more commonly used additives in the U.S.[10] Toothpaste often contains sodium fluoride to prevent cavities.[11] Alternatively, sodium fluoride is used as a cleaning agent, e.g. as a "laundry sour".[7] A variety of specialty chemical applications exist in synthesis and extractive metallurgy. It reacts with electrophilic chlorides including acyl chlorides, sulfur chlorides, and phosphorus chloride.[12] Like other fluorides, sodium fluoride finds use in desilylation in organic synthesis. The fluoride is the reagent for the synthesis of fluorocarbons.
In medical imaging, fluorine-18-labelled sodium fluoride is used in positron emission tomography (PET). Relative to conventional bone scintigraphy carried out with gamma cameras or SPECT systems, PET offers more sensitivity and spatial resolution. A disadvantage of PET is that fluorine-18 labelled sodium fluoride is less widely available than conventional technetium-99m-labelled radiopharmaceuticals.

Safety

The lethal dose for a 70 kg (154 lb) human is estimated at 5–10 g.[7] Sodium fluoride is classed as toxic by both inhalation (of dusts or aerosols) and ingestion.[13] In high enough doses, it has been shown to affect the heart and circulatory system.
In the higher doses used to treat osteoporosis, plain sodium fluoride can cause pain in the legs and incomplete stress fractures when the doses are too high; it also irritates the stomach, sometimes so severely as to cause ulcers. Slow-release and enteric-coated versions of sodium fluoride do not have gastric side effects in any significant way, and have milder and less frequent complications in the bones.[14] In the lower doses used for water fluoridation, the only clear adverse effect is dental fluorosis, which can alter the appearance of children's teeth during tooth development; this is mostly mild and is unlikely to represent any real effect on aesthetic appearance or on public health.[15]

See also

References

1.     ^ Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. p. 5.194. ISBN 1439855110.
2.     ^ Lewis, R.J. Sax's Dangerous Properties of Industrial Materials. 10th ed. Volumes 1–3 New York, NY: John Wiley & Sons Inc., 1999., p. 3248
3.     ^ Martel, B.; Cassidy, K. (2004), Chemical Risk Analysis: A Practical Handbook, Butterworth–Heinemann, p. 363, ISBN 1-903996-65-1
4.     ^ Wells, A.F. (1984), Structural Inorganic Chemistry, Oxford: Clarendon Press, ISBN 0-19-855370-6
5.     ^ "Chemical and physical information" (PDF), Toxicological profile for fluorides, hydrogen fluoride, and fluorine, Agency for Toxic Substances and Disease Registry (ATDSR), September 2003, pp. 187, retrieved 2008-11-01
6.     ^ (PDF) Mineral Handbook, Mineral Data Publishing, 2005.
7.     ^ a b c Aigueperse, Jean; Paul Mollard, Didier Devilliers, Marius Chemla, Robert Faron, RenĂ©e Romano, Jean Pierre Cuer (2005), "Fluorine Compounds, Inorganic", in Ullmann, Encyclopedia of Industrial Chemistry, Weinheim: Wiley-VCH, doi:10.1002/14356007.a11_307
8.     ^ Bourne, Geoffrey Howard (1986), Dietary research and guidance in health and disease, Karger, p. 153, ISBN 3-8055-4341-7, Snippet view from page 153
9.     ^ Klein, Cornelis; Hurlbut, Cornelius Searle; Dana, James Dwight (1999), Manual of Mineralogy (21 ed.), Wiley, ISBN 0-471-31266-5
10.  ^ Division of Oral Health, National Center for Prevention Services, CDC (1993) (PDF), Fluoridation census 1992, retrieved 2008-12-29.
11.  ^ "Sodium fluoride, Molecule of the week". American Chemical Society. 2008-02-19. Retrieved 2008-11-01.
12.  ^ Halpern, D.F. (2001), "Sodium Fluoride", Encyclopedia of Reagents for Organic Synthesis, John Wiley & Sons, doi:10.1002/047084289X.rs071
15.  ^ National Health and Medical Research Council (Australia). A systematic review of the efficacy and safety of fluoridation [PDF]. 2007. ISBN 1-86496-415-4. Summary: Yeung CA. A systematic review of the efficacy and safety of fluoridation. Evid Based Dent. 2008;9(2):39–43. doi:10.1038/sj.ebd.6400578. PMID 18584000. Lay summary: NHMRC, 2007.
[show]
Sodium compounds

[show]
Stomatological preparations (A01)
[show]
Mineral supplements (A12)
END QUOTE
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On Thu, Nov 22, 2012 at 11:57 PM, Scott Bergeson <scottb@xmission.com> wrote:
Quoting R.E. Sutherland on Thu, 22 Nov 2012 19:09:05 -0500:

Hello Scott,

The element Fluoride is different from the compound Sodium Fluoride.

Apparently you are lacking in science knowledge.

The compound form of fluoride called sodium
fluoride is found in drinking water and toothpaste.

Now, go look up the MSDS for "SODIUM FLUROIDE" ... and get better educated.

Sincerely,
R.E. Sutherland, M.Ed.
-----

Thank you for your vote of confidence.
The attached PDF file came up first in a startpage search.
https://www.sciencelab.com/msds.php?msdsId=9927595
Zero occurrences. As it should be. MSDS writers have better
science education than you. And while not relevant to
whether fluoride be a "toxin"* (really weird theology you
have there, to not only call stars living organisms, but
hold they make and secrete fluorine for their biological
defense), ions are ions. Fluoride is an anion formed
when a fluorine atom (½ of a fluorine molecule) takes
an additional electron to complete its valence octet.
When dissociated, the counterion makes no difference.

* Toxin: a toxic substance - poison - an organism makes and secretes.

Now, if you expect people to take concerns about such bad actors as
fluoride seriously, it would help to lose the fringy misdefinitions.

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