thebackalleys

lets go Zabimaru

nobody here likes bleach. Talk about something else or fuck off.

chew a shitbrick bitch

This is someone's alt, and it's not even funny.

wrong all wrong

this is ........

Since bleaches are strong oxidizing agents, they can be quite hazardous, especially when reacted with other common household chemicals.

Mixing sodium hypochlorite with acids like vinegar or drain cleaners containing sodium bisulfate (sodium hydrogen sulfate), or even lemon juice can release chlorine. Hypochlorite and chlorine are in equilibrium in water, the position of the equilibrium is pH dependant and low pH (acidic) favors chlorine,[1]

Cl2 + H2O  H+ + Cl- + HClO

Chlorine is a respiratory irritant that attacks mucous membranes and burns the skin. As little as 3.5 ppm can be detected as an odour, and 1000 ppm is likely to be fatal after a few deep breaths. Exposure to chlorine has been limited to 0.5 ppm (8-hour time-weighted average—40 hour week) by OSHA in the U.S.[2]

Sodium hypochlorite and ammonia react to form a number of products, depending on the temperature, concentration, and how they are mixed. [3]. The main reaction is chlorination of ammonia, first giving chloramine (NH2Cl), then NHCl2 and finally nitrogen trichloride (NCl3). These materials are very irritating to eyes and lungs and are toxic above certain concentrations.

NH3 + NaOCl --> NaOH + NH2Cl

NH2Cl + NaOCl --> NaOH + NHCl2

NHCl2 + NaOCl --> NaOH + NCl3

Additional reactions produce hydrazine, in a variation of the Olin Raschig process.

NH3 + NH2Cl + NaOH --> N2H4 + NaCl + H2O

The hydrazine generated can further react with the monochloramine in an exothermic reaction:[1]

2 NH2Cl + N2H4 --> 2 NH4Cl + N2

Industrial bleaching agents can also be sources of concern. For example, the use of elemental chlorine in the bleaching of wood pulp produces organochlorines, persistent organic pollutants, including dioxins. According to an industry group, the use of chlorine dioxide in these processes has reduced the dioxin generation to under detectable levels.[4] However, respiratory risk from chlorine and highly toxic chlorinated byproducts still remain.

^ what\\\'s so great about that???

someone has been paying attention in science class. PS tthe anime show bleach

Bleach is just another overrated anime fad about bitch ass 14 year old schoolboy with nothing interesting about him, no animation and a lame story that's dragged out over 900 episodes of talking and powering up. Fuck ya Naruto, Fuck ya Ichigo and fuck ya lil' Zabimaro too. There's so much better anime to watch.

^fuck you*

burned.

As cliche as Bleach is I think it has some of the better character designs from trendy anime

Such as this guy
(https://thebackalleys.com/forum/proxy.php?request=http%3A%2F%2Fimg255.imageshack.us%2Fimg255%2F2397%2F3nf5.png&hash=0473b8f714ad9ca65adbebefbbbd90af883fc74a)

Or maybe Im just gay!

A bleach is a chemical that removes color or whitens, often via oxidation. Common chemical bleaches include household "chlorine bleach", a solution of approximately 3-6% sodium hypochlorite (NaOCl), and "oxygen bleach", which contains hydrogen peroxide or a peroxide-releasing compound such as sodium perborate or sodium percarbonate. To bleach something is to apply bleach, sometimes as a preliminary step in the process of dyeing. Bleaching powder is calcium hypochlorite.
Contents
[hide]

   * 1 Other types of bleaches
   * 2 Hazards and concerns
   * 3 Chemistry
   * 4 Mechanism of bleach action
   * 5 See also
   * 6 References
   * 7 Further reading
   * 8 External links

[edit] Other types of bleaches

Chlorine dioxide is used for the bleaching of wood pulp, fats and oils, cellulose, flour, textiles, beeswax, skin and in a number of other industries.

In the food industry, some organic peroxides (benzoyl peroxide, etc.) and other agents (e.g. bromates) are used as flour bleaching and maturing agents.

Peracetic acid, ozone and hydrogen peroxide and oxygen are used in bleaching sequences in the pulp industry to produce totally chlorine free (TCF) paper.

Not all bleaches have to be of an oxidizing nature. Sodium dithionite is used as a powerful reducing agent in some bleaching formulas. It is commonly used to bleach wood pulp used to make newsprint.

[edit] Hazards and concerns

Since bleaches are strong oxidizing agents, they can be quite hazardous, especially when reacted with other common household chemicals.

Mixing sodium hypochlorite with acids like vinegar or drain cleaners containing sodium bisulfate (sodium hydrogen sulfate), or even lemon juice can release chlorine. Hypochlorite and chlorine are in equilibrium in water, the position of the equilibrium is pH dependant and low pH (acidic) favors chlorine,[1]

Cl2 + H2O \rightleftharpoons H+ + Cl- + HClO

Chlorine is a respiratory irritant that attacks mucous membranes and burns the skin. As little as 3.5 ppm can be detected as an odour, and 1000 ppm is likely to be fatal after a few deep breaths. Exposure to chlorine has been limited to 0.5 ppm (8-hour time-weighted average—40 hour week) by OSHA in the U.S.[2]

Sodium hypochlorite and ammonia react to form a number of products, depending on the temperature, concentration, and how they are mixed. [3]. The main reaction is chlorination of ammonia, first giving chloramine (NH2Cl), then NHCl2 and finally nitrogen trichloride (NCl3). These materials are very irritating to eyes and lungs and are toxic above certain concentrations.

NH3 + NaOCl --> NaOH + NH2Cl

NH2Cl + NaOCl --> NaOH + NHCl2

NHCl2 + NaOCl --> NaOH + NCl3

Additional reactions produce hydrazine, in a variation of the Olin Raschig process.

NH3 + NH2Cl + NaOH --> N2H4 + NaCl + H2O

The hydrazine generated can further react with the monochloramine in an exothermic reaction:[1]

2 NH2Cl + N2H4 --> 2 NH4Cl + N2

Industrial bleaching agents can also be sources of concern. For example, the use of elemental chlorine in the bleaching of wood pulp produces organochlorines, persistent organic pollutants, including dioxins. According to an industry group, the use of chlorine dioxide in these processes has reduced the dioxin generation to under detectable levels.[4] However, respiratory risk from chlorine and highly toxic chlorinated byproducts still remain.

[edit] Chemistry

The process of bleaching can be summarised in the following set of chemical reaction:

Cl2(aq) + H2O(l) \rightleftharpoons H+(aq) + Cl-(aq) + HClO(aq)

The H+ ion of the hypochlorous acid then dissolves into solution, and so the final result is effectively:

Cl2(aq) + H2O(l) \rightleftharpoons 2H+(aq) + Cl-(aq) + ClO-(aq)

[edit] Mechanism of bleach action

Color in most dyes and pigments is produced by molecules, such as beta carotene, which contain chromophores. Chemical bleaches work in one of two ways:

   * An oxidizing bleach works by breaking the chemical bonds that make up the chromophore. This changes the molecule into a different substance that either does not contain a chromophore, or contains a chromophore that does not absorb visible light.

   * A reducing bleach works by converting double bonds in the chromophore into single bonds. This eliminates the ability of the chromophore to absorb visible light.[5]

Sunlight acts as a bleach through a process leading to similar results: high energy photons of light, often in the violet or ultraviolet range, can disrupt the bonds in the chromophore, rendering the resulting substance colorless. Extended exposure often leads to massive discoloration usually reducing the colors to white and typically very faded blue spectrums.[6]

[edit] See also

   * Household chemicals
   * Tooth bleaching
   * Bleaching of wood pulp
   * Bleachfield

[edit] References

  1. ^ a b Cotton, F.A; G. Wilkinson (1972). Advanced Inorganic Chemistry. John Wiley and Sons Inc. ISBN 0-471-17560-9.
  2. ^ Occupational Safety & Health Administration (2007). and peroxide/recognition.html OSHA -- Chlorine. OSHA. Retrieved on 2007-08-26.
  3. ^ Rizk-Ouaini, Rosette & Ferriol, Michel; Gazet, Josette; Saugier-Cohen Adad, Marie Therese (1986), "Oxidation reaction of ammonia with sodium hypochlorite. Production and degradation reactions of chloramines.", Bulletin de la Societe Chimique de France 4: 512–21
  4. ^ ECF: The Sustainable Technology. Alliance for Environmental Technology. Retrieved on 2007-09-19.
  5. ^ Field, Simon Q (2006). Ingredients -- Bleach. Science Toys. Retrieved on 2006-03-02.
  6. ^ Bloomfield, Louis A (2006). Sunlight. How Things Work Home Page. Retrieved on 2006-03-02.

[edit] Further reading

   * Bodkins, Dr. Bailey. Bleach. Philadelphia: Virginia Printing Press, 1995.
   * Trotman, E.R. Textile Scouring and Bleaching. London: Charles Griffin & Co., 1968. ISBN 0852640676.
   * Book in numerical format Knew you that?

[edit] External links
Look up bleach in
Wiktionary, the free dictionary.

   * American Chemistry Council, Chlorine Chemistry Division

Retrieved from "http://en.wikipedia.org/wiki/Bleach"
Categories: Bleaches | Disinfectants | Dyes | Household chemicals | Laundry
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   * This page was last modified on 4 May 2008, at 20:04.
   * All text is available under the terms of the GNU Free Documentation License. (See Copyrights for details.)
     Wikipedia® is a registered trademark of the Wikimedia Foundation, Inc., a U.S. registered 501©(3) tax-deductible nonprofit charity.
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Chlorine dioxide is a chemical compound with the formula ClO2. This reddish-yellow gas crystallizes as orange crystals at −59 °C. As one of several oxides of chlorine, it is a potent and useful oxidizing agent used in water treatment and in bleaching.
Contents
[hide]

   * 1 Uses
   * 2 Preparation
   * 3 Handling properties
   * 4 References
   * 5 External links

[edit] Uses

Chlorine dioxide is used primarily (>95%) for bleaching of wood pulp, but is also used for the bleaching of flour and for the disinfection of municipal drinking water. The Niagara Falls, New York water treatment plant first used chlorine dioxide for drinking water treatment in 1944 for phenol destruction. Chlorine dioxide was introduced as a drinking water disinfectant on a large scale in 1956, when Brussels, Belgium, changed from chlorine to chlorine dioxide. Its most common use in water treatment is as a pre-oxidant prior to chlorination of drinking water to destroy natural water impurities that produce trihalomethanes on exposure to free chlorine. Trihalomethanes are suspect carcinogenic disinfection by-product associated with chlorination of naturally occurring organics in the raw water. Chlorine dioxide is also superior to chlorine when operating above pH7, in the presence of ammonia and amines and/or for the control of biofilms in water distribution systems. Chlorine dioxide is used in many industrial water treatment applications as a biocide including cooling towers, process water and food processing. Chlorine dioxide is less corrosive than chlorine and superior for the control of legionella bacteria.

It is more effective as a disinfectant in most circumstances than chlorine against water borne pathogenic microbes such as viruses, bacteria and protozoa – including the cysts of Giardia and the oocysts of Cryptosporidium.

The use of chlorine dioxide in water treatment leads to the formation of the by-product chlorite which is currently limited to a maximum of 1 ppm in drinking water in the USA. This EPA standard limits the use of chlorine dioxide in the USA to relatively high quality water or water which is to be treated with iron based coagulants. (Iron can reduce chlorite to chloride.)

Protective effect of low-concentration chlorine dioxide gas against influenza A virus infection Ogata N, Shibata T. J Gen Virol 89 (2008), 60-67; DOI 10.1099/vir.0.83393-0 http://vir.sgmjournals.org/cgi/content/abstract/89/1/60 (http://vir.sgmjournals.org/cgi/content/abstract/89/1/60)

It can also be used for air disinfection, and was the principal agent used in the decontamination of buildings in the United States after the 2001 anthrax attacks. Recently, after the disaster of Hurricane Katrina in New Orleans, Louisiana and the surrounding Gulf Coast, chlorine dioxide has been used to eradicate dangerous mold from houses inundated by water from massive flooding.

Chlorine dioxide is used as an oxidant for phenol destruction in waste water streams, control of zebra and quagga mussels in water intakes and for odor control in the air scrubbers of animal byproduct (rendering) plants.

Stabilized chlorine dioxide can also be used in an oral rinse to treat oral disease and malodor, but its adverse side-effects are still being investigated.[1]

[edit] Preparation

Chlorine dioxide is a highly endothermic compound that can decompose extremely violently when separated from diluting substances. As a result preparation methods that involve producing solutions of it without going through a gas phase stage are often preferred.

In the laboratory, ClO2 is prepared by oxidation of sodium chlorite:[2]

   2NaClO2 + Cl2 → 2ClO2 + 2 NaCl

Over 95% of the chlorine dioxide produced in the world today is made from sodium chlorate and is used for pulp bleaching. It is produced with high efficiency by reducing sodium chlorate in a strong acid solution with a suitable reducing agent such as hydrochloric acid and sulfur dioxide. The reaction of sodium chlorate with hydrochloric acid proceeds in one reactor via the following pathway:

   HClO3 + HCl → HClO2 + HOCl
   HClO3 + HClO2 → 2ClO2 + Cl2 + 2H2O
   HOCl + HCl → Cl2 + H2O

A much smaller but important market for chlorine dioxide is for use as a disinfectant. Since 1999 a growing proportion of the chlorine dioxide made globally for water treatment and other small scale applications has been made using the chlorate, hydrogen peroxide and sulfuric acid method which can produce a chlorine free product at high efficiency. Traditionally, chlorine dioxide for disinfection applications has been made by one of three methods using sodium chlorite or the sodium chlorite - hypochlorite method:

   2NaClO2 + 2HCl + NaOCl → 2ClO2 + 3NaCl + H2O

or the sodium chlorite - hydrochloric acid method:

   5NaClO2 + 4HCl → 5NaCl + 4ClO2 + 2H2O

All three sodium chlorite chemistries can produce chlorine dioxide with high chlorite conversion yield, but unlike the other processes the chlorite-HCl method produces completely chlorine free chlorine dioxide but suffers from the requirement of 25% more chlorite to produce an equivalent amount of chlorine dioxide.

Very pure chlorine dioxide can also be produced by electrolysis of a chlorite solution:

   2NaClO2 + 2H2O   →   2ClO2 + 2NaOH + H2

High purity chlorine dioxide gas (7.7% in air or nitrogen) can be produced by the Gas:Solid method, which reacts dilute chlorine gas with solid sodium chlorite.

   2NaClO2 + Cl2   →   2ClO2 + 2NaCl

These processes and several slight variations have been reviewed.[3]

[edit] Handling properties

At concentrations greater than 15% volume in air at STP, ClO2 explosively decomposes into chlorine and oxygen. The decomposition is initiated by light. Thus, it is never handled in concentrated form, but is almost always used as a dissolved gas in water in a concentration range of 0.5 to 10 grams per liter. Its solubility increases at lower temperatures: it is thus common to use chilled water (5 °C or 41 °F) when storing at concentrations above 3 grams per liter. In many countries, such as the USA, chlorine dioxide gas may not be transported at any concentration and is almost always produced at the application site using a chlorine dioxide generator. In some countries, chlorine dioxide solution below 3 grams per liter in concentration may be transported by land, but are relatively unstable and deteriorate quickly.

A number of products are marketed as "stabilized chlorine dioxide" (SCD). These solutions do not actually contain chlorine dioxide but consist of solutions of buffered sodium chlorite. A weak acid can be added to SCD to "activate" it and make chlorine dioxide in-situ without a chlorine dioxide generator. The use of SCD is effective when the demand for chlorine dioxide is low and when impurities, such as small amounts of sodium, can be tolerated. For application requiring above 5 kg day−1 ClO2, chlorine dioxide produced by a generator with either sodium chlorite or sodium chlorate is typically more economical.

[edit] References

  1. ^ US patent 4689215
  2. ^ Derby, R. I.; Hutchinson, W. S. "Chlorine(IV) Oxide" Inorganic Syntheses, 1953, IV, 152-158.
  3. ^ White, G. C. "Handbook of Chlorination and Alternative Disinfectants", 4th Edition (Wiley, 1999).

[edit] External links

   * Catalytic Chlorine Dioxide Generation
   * Catalytic Chlorine Dioxide Generation and Applications
   * Stabilized Chlorine Dioxide used for oral hygiene
   * Chlorine Dioxide Applications
   * National Pollutant Inventory: Chlorine dioxide
   * An Interview with Chlorine Dioxide, Kevin McCue/The American Chemical Society

[hide]
v • d • e
E numbers

Colours (E100–199) • Preservatives (E200–299) • Antioxidants & Acidity regulators (E300–399) • Thickeners, stabilisers & emulsifiers (E400–499) • pH regulators & anti-caking agents (E500–599) • Flavour enhancers (E600–699) • Miscellaneous (E900–999) • Additional chemicals (E1100–1599)

Waxes (E900–909) • Synthetic glazes (E910–919) • Improving agents (E920–929) • Packaging gases (E930–949) • Sweeteners (E950–969) • Foaming agents (E990–999)

L-cysteine (E920) • L-cystine (E921) • Potassium persulfate (E922) • Ammonium persulfate (E923) • Potassium bromate (E924) • Chlorine (E925) • Chlorine dioxide (E926) • Azodicarbonamide (E927) • Carbamide (E927b) • Benzoyl peroxide (E928)
Retrieved from "http://en.wikipedia.org/wiki/Chlorine_dioxide"
Categories: Oxides | Chlorine compounds | Bleaches | Disinfectants

Quote from: topcatyoA bleach is a chemical that removes color or whitens, often via oxidation. Common chemical bleaches include household "chlorine bleach", a solution of approximately 3-6% sodium hypochlorite (NaOCl), and "oxygen bleach", which contains hydrogen peroxide or a peroxide-releasing compound such as sodium perborate or sodium percarbonate. To bleach something is to apply bleach, sometimes as a preliminary step in the process of dyeing. Bleaching powder is calcium hypochlorite.
Contents
[hide]

   * 1 Other types of bleaches
   * 2 Hazards and concerns
   * 3 Chemistry
   * 4 Mechanism of bleach action
   * 5 See also
   * 6 References
   * 7 Further reading
   * 8 External links

[edit] Other types of bleaches

Chlorine dioxide is used for the bleaching of wood pulp, fats and oils, cellulose, flour, textiles, beeswax, skin and in a number of other industries.

In the food industry, some organic peroxides (benzoyl peroxide, etc.) and other agents (e.g. bromates) are used as flour bleaching and maturing agents.

Peracetic acid, ozone and hydrogen peroxide and oxygen are used in bleaching sequences in the pulp industry to produce totally chlorine free (TCF) paper.

Not all bleaches have to be of an oxidizing nature. Sodium dithionite is used as a powerful reducing agent in some bleaching formulas. It is commonly used to bleach wood pulp used to make newsprint.

[edit] Hazards and concerns

Since bleaches are strong oxidizing agents, they can be quite hazardous, especially when reacted with other common household chemicals.

Mixing sodium hypochlorite with acids like vinegar or drain cleaners containing sodium bisulfate (sodium hydrogen sulfate), or even lemon juice can release chlorine. Hypochlorite and chlorine are in equilibrium in water, the position of the equilibrium is pH dependant and low pH (acidic) favors chlorine,[1]

Cl2 + H2O \rightleftharpoons H+ + Cl- + HClO

Chlorine is a respiratory irritant that attacks mucous membranes and burns the skin. As little as 3.5 ppm can be detected as an odour, and 1000 ppm is likely to be fatal after a few deep breaths. Exposure to chlorine has been limited to 0.5 ppm (8-hour time-weighted average—40 hour week) by OSHA in the U.S.[2]

Sodium hypochlorite and ammonia react to form a number of products, depending on the temperature, concentration, and how they are mixed. [3]. The main reaction is chlorination of ammonia, first giving chloramine (NH2Cl), then NHCl2 and finally nitrogen trichloride (NCl3). These materials are very irritating to eyes and lungs and are toxic above certain concentrations.

NH3 + NaOCl --> NaOH + NH2Cl

NH2Cl + NaOCl --> NaOH + NHCl2

NHCl2 + NaOCl --> NaOH + NCl3

Additional reactions produce hydrazine, in a variation of the Olin Raschig process.

NH3 + NH2Cl + NaOH --> N2H4 + NaCl + H2O

The hydrazine generated can further react with the monochloramine in an exothermic reaction:[1]

2 NH2Cl + N2H4 --> 2 NH4Cl + N2

Industrial bleaching agents can also be sources of concern. For example, the use of elemental chlorine in the bleaching of wood pulp produces organochlorines, persistent organic pollutants, including dioxins. According to an industry group, the use of chlorine dioxide in these processes has reduced the dioxin generation to under detectable levels.[4] However, respiratory risk from chlorine and highly toxic chlorinated byproducts still remain.

[edit] Chemistry

The process of bleaching can be summarised in the following set of chemical reaction:

Cl2(aq) + H2O(l) \rightleftharpoons H+(aq) + Cl-(aq) + HClO(aq)

The H+ ion of the hypochlorous acid then dissolves into solution, and so the final result is effectively:

Cl2(aq) + H2O(l) \rightleftharpoons 2H+(aq) + Cl-(aq) + ClO-(aq)

[edit] Mechanism of bleach action

Color in most dyes and pigments is produced by molecules, such as beta carotene, which contain chromophores. Chemical bleaches work in one of two ways:

   * An oxidizing bleach works by breaking the chemical bonds that make up the chromophore. This changes the molecule into a different substance that either does not contain a chromophore, or contains a chromophore that does not absorb visible light.

   * A reducing bleach works by converting double bonds in the chromophore into single bonds. This eliminates the ability of the chromophore to absorb visible light.[5]

Sunlight acts as a bleach through a process leading to similar results: high energy photons of light, often in the violet or ultraviolet range, can disrupt the bonds in the chromophore, rendering the resulting substance colorless. Extended exposure often leads to massive discoloration usually reducing the colors to white and typically very faded blue spectrums.[6]

[edit] See also

   * Household chemicals
   * Tooth bleaching
   * Bleaching of wood pulp
   * Bleachfield

[edit] References

  1. ^ a b Cotton, F.A; G. Wilkinson (1972). Advanced Inorganic Chemistry. John Wiley and Sons Inc. ISBN 0-471-17560-9.
  2. ^ Occupational Safety & Health Administration (2007). and peroxide/recognition.html OSHA -- Chlorine. OSHA. Retrieved on 2007-08-26.
  3. ^ Rizk-Ouaini, Rosette & Ferriol, Michel; Gazet, Josette; Saugier-Cohen Adad, Marie Therese (1986), "Oxidation reaction of ammonia with sodium hypochlorite. Production and degradation reactions of chloramines.", Bulletin de la Societe Chimique de France 4: 512–21
  4. ^ ECF: The Sustainable Technology. Alliance for Environmental Technology. Retrieved on 2007-09-19.
  5. ^ Field, Simon Q (2006). Ingredients -- Bleach. Science Toys. Retrieved on 2006-03-02.
  6. ^ Bloomfield, Louis A (2006). Sunlight. How Things Work Home Page. Retrieved on 2006-03-02.

[edit] Further reading

   * Bodkins, Dr. Bailey. Bleach. Philadelphia: Virginia Printing Press, 1995.
   * Trotman, E.R. Textile Scouring and Bleaching. London: Charles Griffin & Co., 1968. ISBN 0852640676.
   * Book in numerical format Knew you that?

[edit] External links
Look up bleach in
Wiktionary, the free dictionary.

   * American Chemistry Council, Chlorine Chemistry Division

Retrieved from "http://en.wikipedia.org/wiki/Bleach"
Categories: Bleaches | Disinfectants | Dyes | Household chemicals | Laundry
Views

   * Article
   * Discussion
   * Edit this page
   * History

Personal tools

   * Log in / create account

Navigation

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   * Contents
   * Featured content
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   * Random article

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Powered by MediaWiki
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   * This page was last modified on 4 May 2008, at 20:04.
   * All text is available under the terms of the GNU Free Documentation License. (See Copyrights for details.)
     Wikipedia® is a registered trademark of the Wikimedia Foundation, Inc., a U.S. registered 501©(3) tax-deductible nonprofit charity.
   * Privacy policy
   * About Wikipedia
   * Disclaimers

You can support Wikipedia by making a tax-deductible donation.

Chlorine dioxide is a chemical compound with the formula ClO2. This reddish-yellow gas crystallizes as orange crystals at −59 °C. As one of several oxides of chlorine, it is a potent and useful oxidizing agent used in water treatment and in bleaching.
Contents
[hide]

   * 1 Uses
   * 2 Preparation
   * 3 Handling properties
   * 4 References
   * 5 External links

[edit] Uses

Chlorine dioxide is used primarily (>95%) for bleaching of wood pulp, but is also used for the bleaching of flour and for the disinfection of municipal drinking water. The Niagara Falls, New York water treatment plant first used chlorine dioxide for drinking water treatment in 1944 for phenol destruction. Chlorine dioxide was introduced as a drinking water disinfectant on a large scale in 1956, when Brussels, Belgium, changed from chlorine to chlorine dioxide. Its most common use in water treatment is as a pre-oxidant prior to chlorination of drinking water to destroy natural water impurities that produce trihalomethanes on exposure to free chlorine. Trihalomethanes are suspect carcinogenic disinfection by-product associated with chlorination of naturally occurring organics in the raw water. Chlorine dioxide is also superior to chlorine when operating above pH7, in the presence of ammonia and amines and/or for the control of biofilms in water distribution systems. Chlorine dioxide is used in many industrial water treatment applications as a biocide including cooling towers, process water and food processing. Chlorine dioxide is less corrosive than chlorine and superior for the control of legionella bacteria.

It is more effective as a disinfectant in most circumstances than chlorine against water borne pathogenic microbes such as viruses, bacteria and protozoa – including the cysts of Giardia and the oocysts of Cryptosporidium.

The use of chlorine dioxide in water treatment leads to the formation of the by-product chlorite which is currently limited to a maximum of 1 ppm in drinking water in the USA. This EPA standard limits the use of chlorine dioxide in the USA to relatively high quality water or water which is to be treated with iron based coagulants. (Iron can reduce chlorite to chloride.)

Protective effect of low-concentration chlorine dioxide gas against influenza A virus infection Ogata N, Shibata T. J Gen Virol 89 (2008), 60-67; DOI 10.1099/vir.0.83393-0 http://vir.sgmjournals.org/cgi/content/abstract/89/1/60 (http://vir.sgmjournals.org/cgi/content/abstract/89/1/60)

It can also be used for air disinfection, and was the principal agent used in the decontamination of buildings in the United States after the 2001 anthrax attacks. Recently, after the disaster of Hurricane Katrina in New Orleans, Louisiana and the surrounding Gulf Coast, chlorine dioxide has been used to eradicate dangerous mold from houses inundated by water from massive flooding.

Chlorine dioxide is used as an oxidant for phenol destruction in waste water streams, control of zebra and quagga mussels in water intakes and for odor control in the air scrubbers of animal byproduct (rendering) plants.

Stabilized chlorine dioxide can also be used in an oral rinse to treat oral disease and malodor, but its adverse side-effects are still being investigated.[1]

[edit] Preparation

Chlorine dioxide is a highly endothermic compound that can decompose extremely violently when separated from diluting substances. As a result preparation methods that involve producing solutions of it without going through a gas phase stage are often preferred.

In the laboratory, ClO2 is prepared by oxidation of sodium chlorite:[2]

   2NaClO2 + Cl2 → 2ClO2 + 2 NaCl

Over 95% of the chlorine dioxide produced in the world today is made from sodium chlorate and is used for pulp bleaching. It is produced with high efficiency by reducing sodium chlorate in a strong acid solution with a suitable reducing agent such as hydrochloric acid and sulfur dioxide. The reaction of sodium chlorate with hydrochloric acid proceeds in one reactor via the following pathway:

   HClO3 + HCl → HClO2 + HOCl
   HClO3 + HClO2 → 2ClO2 + Cl2 + 2H2O
   HOCl + HCl → Cl2 + H2O

A much smaller but important market for chlorine dioxide is for use as a disinfectant. Since 1999 a growing proportion of the chlorine dioxide made globally for water treatment and other small scale applications has been made using the chlorate, hydrogen peroxide and sulfuric acid method which can produce a chlorine free product at high efficiency. Traditionally, chlorine dioxide for disinfection applications has been made by one of three methods using sodium chlorite or the sodium chlorite - hypochlorite method:

   2NaClO2 + 2HCl + NaOCl → 2ClO2 + 3NaCl + H2O

or the sodium chlorite - hydrochloric acid method:

   5NaClO2 + 4HCl → 5NaCl + 4ClO2 + 2H2O

All three sodium chlorite chemistries can produce chlorine dioxide with high chlorite conversion yield, but unlike the other processes the chlorite-HCl method produces completely chlorine free chlorine dioxide but suffers from the requirement of 25% more chlorite to produce an equivalent amount of chlorine dioxide.

Very pure chlorine dioxide can also be produced by electrolysis of a chlorite solution:

   2NaClO2 + 2H2O   →   2ClO2 + 2NaOH + H2

High purity chlorine dioxide gas (7.7% in air or nitrogen) can be produced by the Gas:Solid method, which reacts dilute chlorine gas with solid sodium chlorite.

   2NaClO2 + Cl2   →   2ClO2 + 2NaCl

These processes and several slight variations have been reviewed.[3]

[edit] Handling properties

At concentrations greater than 15% volume in air at STP, ClO2 explosively decomposes into chlorine and oxygen. The decomposition is initiated by light. Thus, it is never handled in concentrated form, but is almost always used as a dissolved gas in water in a concentration range of 0.5 to 10 grams per liter. Its solubility increases at lower temperatures: it is thus common to use chilled water (5 °C or 41 °F) when storing at concentrations above 3 grams per liter. In many countries, such as the USA, chlorine dioxide gas may not be transported at any concentration and is almost always produced at the application site using a chlorine dioxide generator. In some countries, chlorine dioxide solution below 3 grams per liter in concentration may be transported by land, but are relatively unstable and deteriorate quickly.

A number of products are marketed as "stabilized chlorine dioxide" (SCD). These solutions do not actually contain chlorine dioxide but consist of solutions of buffered sodium chlorite. A weak acid can be added to SCD to "activate" it and make chlorine dioxide in-situ without a chlorine dioxide generator. The use of SCD is effective when the demand for chlorine dioxide is low and when impurities, such as small amounts of sodium, can be tolerated. For application requiring above 5 kg day−1 ClO2, chlorine dioxide produced by a generator with either sodium chlorite or sodium chlorate is typically more economical.

[edit] References

  1. ^ US patent 4689215
  2. ^ Derby, R. I.; Hutchinson, W. S. "Chlorine(IV) Oxide" Inorganic Syntheses, 1953, IV, 152-158.
  3. ^ White, G. C. "Handbook of Chlorination and Alternative Disinfectants", 4th Edition (Wiley, 1999).

[edit] External links

   * Catalytic Chlorine Dioxide Generation
   * Catalytic Chlorine Dioxide Generation and Applications
   * Stabilized Chlorine Dioxide used for oral hygiene
   * Chlorine Dioxide Applications
   * National Pollutant Inventory: Chlorine dioxide
   * An Interview with Chlorine Dioxide, Kevin McCue/The American Chemical Society

[hide]
v • d • e
E numbers

Colours (E100–199) • Preservatives (E200–299) • Antioxidants & Acidity regulators (E300–399) • Thickeners, stabilisers & emulsifiers (E400–499) • pH regulators & anti-caking agents (E500–599) • Flavour enhancers (E600–699) • Miscellaneous (E900–999) • Additional chemicals (E1100–1599)

Waxes (E900–909) • Synthetic glazes (E910–919) • Improving agents (E920–929) • Packaging gases (E930–949) • Sweeteners (E950–969) • Foaming agents (E990–999)

L-cysteine (E920) • L-cystine (E921) • Potassium persulfate (E922) • Ammonium persulfate (E923) • Potassium bromate (E924) • Chlorine (E925) • Chlorine dioxide (E926) • Azodicarbonamide (E927) • Carbamide (E927b) • Benzoyl peroxide (E928)
Retrieved from "http://en.wikipedia.org/wiki/Chlorine_dioxide"
Categories: Oxides | Chlorine compounds | Bleaches | Disinfectants

no science again

Quote from: topcatyoA bleach is a chemical that removes color or whitens, often via oxidation. Common chemical bleaches include household "chlorine bleach", a solution of approximately 3-6% sodium hypochlorite (NaOCl), and "oxygen bleach", which contains hydrogen peroxide or a peroxide-releasing compound such as sodium perborate or sodium percarbonate. To bleach something is to apply bleach, sometimes as a preliminary step in the process of dyeing. Bleaching powder is calcium hypochlorite.
Contents
[hide]

   * 1 Other types of bleaches
   * 2 Hazards and concerns
   * 3 Chemistry
   * 4 Mechanism of bleach action
   * 5 See also
   * 6 References
   * 7 Further reading
   * 8 External links

[edit] Other types of bleaches

Chlorine dioxide is used for the bleaching of wood pulp, fats and oils, cellulose, flour, textiles, beeswax, skin and in a number of other industries.

In the food industry, some organic peroxides (benzoyl peroxide, etc.) and other agents (e.g. bromates) are used as flour bleaching and maturing agents.

Peracetic acid, ozone and hydrogen peroxide and oxygen are used in bleaching sequences in the pulp industry to produce totally chlorine free (TCF) paper.

Not all bleaches have to be of an oxidizing nature. Sodium dithionite is used as a powerful reducing agent in some bleaching formulas. It is commonly used to bleach wood pulp used to make newsprint.

[edit] Hazards and concerns

Since bleaches are strong oxidizing agents, they can be quite hazardous, especially when reacted with other common household chemicals.

Mixing sodium hypochlorite with acids like vinegar or drain cleaners containing sodium bisulfate (sodium hydrogen sulfate), or even lemon juice can release chlorine. Hypochlorite and chlorine are in equilibrium in water, the position of the equilibrium is pH dependant and low pH (acidic) favors chlorine,[1]

Cl2 + H2O \rightleftharpoons H+ + Cl- + HClO

Chlorine is a respiratory irritant that attacks mucous membranes and burns the skin. As little as 3.5 ppm can be detected as an odour, and 1000 ppm is likely to be fatal after a few deep breaths. Exposure to chlorine has been limited to 0.5 ppm (8-hour time-weighted average—40 hour week) by OSHA in the U.S.[2]

Sodium hypochlorite and ammonia react to form a number of products, depending on the temperature, concentration, and how they are mixed. [3]. The main reaction is chlorination of ammonia, first giving chloramine (NH2Cl), then NHCl2 and finally nitrogen trichloride (NCl3). These materials are very irritating to eyes and lungs and are toxic above certain concentrations.

NH3 + NaOCl --> NaOH + NH2Cl

NH2Cl + NaOCl --> NaOH + NHCl2

NHCl2 + NaOCl --> NaOH + NCl3

Additional reactions produce hydrazine, in a variation of the Olin Raschig process.

NH3 + NH2Cl + NaOH --> N2H4 + NaCl + H2O

The hydrazine generated can further react with the monochloramine in an exothermic reaction:[1]

2 NH2Cl + N2H4 --> 2 NH4Cl + N2

Industrial bleaching agents can also be sources of concern. For example, the use of elemental chlorine in the bleaching of wood pulp produces organochlorines, persistent organic pollutants, including dioxins. According to an industry group, the use of chlorine dioxide in these processes has reduced the dioxin generation to under detectable levels.[4] However, respiratory risk from chlorine and highly toxic chlorinated byproducts still remain.

[edit] Chemistry

The process of bleaching can be summarised in the following set of chemical reaction:

Cl2(aq) + H2O(l) \rightleftharpoons H+(aq) + Cl-(aq) + HClO(aq)

The H+ ion of the hypochlorous acid then dissolves into solution, and so the final result is effectively:

Cl2(aq) + H2O(l) \rightleftharpoons 2H+(aq) + Cl-(aq) + ClO-(aq)

[edit] Mechanism of bleach action

Color in most dyes and pigments is produced by molecules, such as beta carotene, which contain chromophores. Chemical bleaches work in one of two ways:

   * An oxidizing bleach works by breaking the chemical bonds that make up the chromophore. This changes the molecule into a different substance that either does not contain a chromophore, or contains a chromophore that does not absorb visible light.

   * A reducing bleach works by converting double bonds in the chromophore into single bonds. This eliminates the ability of the chromophore to absorb visible light.[5]

Sunlight acts as a bleach through a process leading to similar results: high energy photons of light, often in the violet or ultraviolet range, can disrupt the bonds in the chromophore, rendering the resulting substance colorless. Extended exposure often leads to massive discoloration usually reducing the colors to white and typically very faded blue spectrums.[6]

[edit] See also

   * Household chemicals
   * Tooth bleaching
   * Bleaching of wood pulp
   * Bleachfield

[edit] References

  1. ^ a b Cotton, F.A; G. Wilkinson (1972). Advanced Inorganic Chemistry. John Wiley and Sons Inc. ISBN 0-471-17560-9.
  2. ^ Occupational Safety & Health Administration (2007). and peroxide/recognition.html OSHA -- Chlorine. OSHA. Retrieved on 2007-08-26.
  3. ^ Rizk-Ouaini, Rosette & Ferriol, Michel; Gazet, Josette; Saugier-Cohen Adad, Marie Therese (1986), "Oxidation reaction of ammonia with sodium hypochlorite. Production and degradation reactions of chloramines.", Bulletin de la Societe Chimique de France 4: 512–21
  4. ^ ECF: The Sustainable Technology. Alliance for Environmental Technology. Retrieved on 2007-09-19.
  5. ^ Field, Simon Q (2006). Ingredients -- Bleach. Science Toys. Retrieved on 2006-03-02.
  6. ^ Bloomfield, Louis A (2006). Sunlight. How Things Work Home Page. Retrieved on 2006-03-02.

[edit] Further reading

   * Bodkins, Dr. Bailey. Bleach. Philadelphia: Virginia Printing Press, 1995.
   * Trotman, E.R. Textile Scouring and Bleaching. London: Charles Griffin & Co., 1968. ISBN 0852640676.
   * Book in numerical format Knew you that?

[edit] External links
Look up bleach in
Wiktionary, the free dictionary.

   * American Chemistry Council, Chlorine Chemistry Division

Retrieved from "http://en.wikipedia.org/wiki/Bleach"
Categories: Bleaches | Disinfectants | Dyes | Household chemicals | Laundry
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Chlorine dioxide is a chemical compound with the formula ClO2. This reddish-yellow gas crystallizes as orange crystals at −59 °C. As one of several oxides of chlorine, it is a potent and useful oxidizing agent used in water treatment and in bleaching.
Contents
[hide]

   * 1 Uses
   * 2 Preparation
   * 3 Handling properties
   * 4 References
   * 5 External links

[edit] Uses

Chlorine dioxide is used primarily (>95%) for bleaching of wood pulp, but is also used for the bleaching of flour and for the disinfection of municipal drinking water. The Niagara Falls, New York water treatment plant first used chlorine dioxide for drinking water treatment in 1944 for phenol destruction. Chlorine dioxide was introduced as a drinking water disinfectant on a large scale in 1956, when Brussels, Belgium, changed from chlorine to chlorine dioxide. Its most common use in water treatment is as a pre-oxidant prior to chlorination of drinking water to destroy natural water impurities that produce trihalomethanes on exposure to free chlorine. Trihalomethanes are suspect carcinogenic disinfection by-product associated with chlorination of naturally occurring organics in the raw water. Chlorine dioxide is also superior to chlorine when operating above pH7, in the presence of ammonia and amines and/or for the control of biofilms in water distribution systems. Chlorine dioxide is used in many industrial water treatment applications as a biocide including cooling towers, process water and food processing. Chlorine dioxide is less corrosive than chlorine and superior for the control of legionella bacteria.

It is more effective as a disinfectant in most circumstances than chlorine against water borne pathogenic microbes such as viruses, bacteria and protozoa – including the cysts of Giardia and the oocysts of Cryptosporidium.

The use of chlorine dioxide in water treatment leads to the formation of the by-product chlorite which is currently limited to a maximum of 1 ppm in drinking water in the USA. This EPA standard limits the use of chlorine dioxide in the USA to relatively high quality water or water which is to be treated with iron based coagulants. (Iron can reduce chlorite to chloride.)

Protective effect of low-concentration chlorine dioxide gas against influenza A virus infection Ogata N, Shibata T. J Gen Virol 89 (2008), 60-67; DOI 10.1099/vir.0.83393-0 http://vir.sgmjournals.org/cgi/content/abstract/89/1/60 (http://vir.sgmjournals.org/cgi/content/abstract/89/1/60)

It can also be used for air disinfection, and was the principal agent used in the decontamination of buildings in the United States after the 2001 anthrax attacks. Recently, after the disaster of Hurricane Katrina in New Orleans, Louisiana and the surrounding Gulf Coast, chlorine dioxide has been used to eradicate dangerous mold from houses inundated by water from massive flooding.

Chlorine dioxide is used as an oxidant for phenol destruction in waste water streams, control of zebra and quagga mussels in water intakes and for odor control in the air scrubbers of animal byproduct (rendering) plants.

Stabilized chlorine dioxide can also be used in an oral rinse to treat oral disease and malodor, but its adverse side-effects are still being investigated.[1]

[edit] Preparation

Chlorine dioxide is a highly endothermic compound that can decompose extremely violently when separated from diluting substances. As a result preparation methods that involve producing solutions of it without going through a gas phase stage are often preferred.

In the laboratory, ClO2 is prepared by oxidation of sodium chlorite:[2]

   2NaClO2 + Cl2 → 2ClO2 + 2 NaCl

Over 95% of the chlorine dioxide produced in the world today is made from sodium chlorate and is used for pulp bleaching. It is produced with high efficiency by reducing sodium chlorate in a strong acid solution with a suitable reducing agent such as hydrochloric acid and sulfur dioxide. The reaction of sodium chlorate with hydrochloric acid proceeds in one reactor via the following pathway:

   HClO3 + HCl → HClO2 + HOCl
   HClO3 + HClO2 → 2ClO2 + Cl2 + 2H2O
   HOCl + HCl → Cl2 + H2O

A much smaller but important market for chlorine dioxide is for use as a disinfectant. Since 1999 a growing proportion of the chlorine dioxide made globally for water treatment and other small scale applications has been made using the chlorate, hydrogen peroxide and sulfuric acid method which can produce a chlorine free product at high efficiency. Traditionally, chlorine dioxide for disinfection applications has been made by one of three methods using sodium chlorite or the sodium chlorite - hypochlorite method:

   2NaClO2 + 2HCl + NaOCl → 2ClO2 + 3NaCl + H2O

or the sodium chlorite - hydrochloric acid method:

   5NaClO2 + 4HCl → 5NaCl + 4ClO2 + 2H2O

All three sodium chlorite chemistries can produce chlorine dioxide with high chlorite conversion yield, but unlike the other processes the chlorite-HCl method produces completely chlorine free chlorine dioxide but suffers from the requirement of 25% more chlorite to produce an equivalent amount of chlorine dioxide.

Very pure chlorine dioxide can also be produced by electrolysis of a chlorite solution:

   2NaClO2 + 2H2O   →   2ClO2 + 2NaOH + H2

High purity chlorine dioxide gas (7.7% in air or nitrogen) can be produced by the Gas:Solid method, which reacts dilute chlorine gas with solid sodium chlorite.

   2NaClO2 + Cl2   →   2ClO2 + 2NaCl

These processes and several slight variations have been reviewed.[3]

[edit] Handling properties

At concentrations greater than 15% volume in air at STP, ClO2 explosively decomposes into chlorine and oxygen. The decomposition is initiated by light. Thus, it is never handled in concentrated form, but is almost always used as a dissolved gas in water in a concentration range of 0.5 to 10 grams per liter. Its solubility increases at lower temperatures: it is thus common to use chilled water (5 °C or 41 °F) when storing at concentrations above 3 grams per liter. In many countries, such as the USA, chlorine dioxide gas may not be transported at any concentration and is almost always produced at the application site using a chlorine dioxide generator. In some countries, chlorine dioxide solution below 3 grams per liter in concentration may be transported by land, but are relatively unstable and deteriorate quickly.

A number of products are marketed as "stabilized chlorine dioxide" (SCD). These solutions do not actually contain chlorine dioxide but consist of solutions of buffered sodium chlorite. A weak acid can be added to SCD to "activate" it and make chlorine dioxide in-situ without a chlorine dioxide generator. The use of SCD is effective when the demand for chlorine dioxide is low and when impurities, such as small amounts of sodium, can be tolerated. For application requiring above 5 kg day−1 ClO2, chlorine dioxide produced by a generator with either sodium chlorite or sodium chlorate is typically more economical.

[edit] References

  1. ^ US patent 4689215
  2. ^ Derby, R. I.; Hutchinson, W. S. "Chlorine(IV) Oxide" Inorganic Syntheses, 1953, IV, 152-158.
  3. ^ White, G. C. "Handbook of Chlorination and Alternative Disinfectants", 4th Edition (Wiley, 1999).

[edit] External links

   * Catalytic Chlorine Dioxide Generation
   * Catalytic Chlorine Dioxide Generation and Applications
   * Stabilized Chlorine Dioxide used for oral hygiene
   * Chlorine Dioxide Applications
   * National Pollutant Inventory: Chlorine dioxide
   * An Interview with Chlorine Dioxide, Kevin McCue/The American Chemical Society

[hide]
v • d • e
E numbers

Colours (E100–199) • Preservatives (E200–299) • Antioxidants & Acidity regulators (E300–399) • Thickeners, stabilisers & emulsifiers (E400–499) • pH regulators & anti-caking agents (E500–599) • Flavour enhancers (E600–699) • Miscellaneous (E900–999) • Additional chemicals (E1100–1599)

Waxes (E900–909) • Synthetic glazes (E910–919) • Improving agents (E920–929) • Packaging gases (E930–949) • Sweeteners (E950–969) • Foaming agents (E990–999)

L-cysteine (E920) • L-cystine (E921) • Potassium persulfate (E922) • Ammonium persulfate (E923) • Potassium bromate (E924) • Chlorine (E925) • Chlorine dioxide (E926) • Azodicarbonamide (E927) • Carbamide (E927b) • Benzoyl peroxide (E928)
Retrieved from "http://en.wikipedia.org/wiki/Chlorine_dioxide"
Categories: Oxides | Chlorine compounds | Bleaches | Disinfectants

no science again

Quote from: CoolDrMoneyAs cliche as Bleach is I think it has some of the better character designs from trendy anime

Such as this guy
(https://thebackalleys.com/forum/proxy.php?request=http%3A%2F%2Fimg255.imageshack.us%2Fimg255%2F2397%2F3nf5.png&hash=0473b8f714ad9ca65adbebefbbbd90af883fc74a)

Or maybe Im just gay!

i watched a few episodes of bleach and that guy was the only thing i liked because he told someone to die in a ditch

every other design is generally cliche and shit

ironic idiots are popping out of no where

Quote from: naruto102ironic idiots are popping out of no where

choke on a dick and die

Quote from: anigen

Quote from: naruto102ironic idiots are popping out of no where

choke on a dick and die

you don't know what a dick is

Quote from: anigenchoke on a dick and die

(https://thebackalleys.com/forum/proxy.php?request=http%3A%2F%2Fimg265.imageshack.us%2Fimg265%2F7791%2Fallplayer20071101141505tj8.png&hash=fe5f39d50018b888557f6e13d588d67c907ed5ef)
super generic.

(https://thebackalleys.com/forum/proxy.php?request=http%3A%2F%2Fwww.projectfirst.info%2Fbatenkaitos%2Fimages%2Fartwork_mizuti.jpg&hash=5ecb436e4158e2171843b680a7d5493a69c43729)
one of my favorite characters of all time.

I actually like over rated anime series like Naruto and D.Gray-Man, But Bleach is possibly one of the most irritating animes I've ever had the displeasure of watching.

The first season was actually straight, then they got to the spirit world and it turned into every other sucky anime after that. The 90's Scooby Doo movies had sicker animation than this cartoon, and frankly I'd much rather watch those, even Avatar has Bleach beat.

The animation of Doremi is amazing because I love the shading style:
(https://thebackalleys.com/forum/proxy.php?request=http%3A%2F%2Fen.wikivisual.com%2Fimages%2F2%2F2d%2FHarukazeDoremi.jpg&hash=ed26a6195fa9cd3485592f5dfeea6a0c914f323d)

are you serious Nicole what the fuck

(https://thebackalleys.com/forum/proxy.php?request=http%3A%2F%2Fusuarios.lycos.es%2Fcarmepatricia%2Fhpbimg%2Ftodas.jpg&hash=9530b923a81b1c0c2900472efe831a9bdea18bdb)

??

Why does the brown haired one not have fingers!?
(https://thebackalleys.com/forum/proxy.php?request=http%3A%2F%2Fi238.photobucket.com%2Falbums%2Fff229%2FKibakun16%2Fairgear.jpg&hash=a47014f28c2f647d8042000b99c4cae6fb351c2e)

Quote from: deadSTARWhy does the brown haired one not have fingers!?
(https://thebackalleys.com/forum/proxy.php?request=http%3A%2F%2Fi238.photobucket.com%2Falbums%2Fff229%2FKibakun16%2Fairgear.jpg&hash=a47014f28c2f647d8042000b99c4cae6fb351c2e)

Lost'em in Vietnam.

oh god airgear

????????????????????????????????????

Yeah, I know you're not a fan. It's probably one of my favorite series though.

okay here i go bye bye

Yup

^ That explains everythin.

Quote from: sakura102The animation of Doremi is amazing because I love the shading style:
(https://thebackalleys.com/forum/proxy.php?request=http%3A%2F%2Fen.wikivisual.com%2Fimages%2F2%2F2d%2FHarukazeDoremi.jpg&hash=ed26a6195fa9cd3485592f5dfeea6a0c914f323d)

more like glass shading hurhurhurhurHURHURHURHURHURHURHURHURHUR

i don't mind airgear i just am sick of hearing "freetown remindz me of air gear have u seen it????" i hadn't even heard of it until all those reviews
but the next episode won't have any rollerskates in it so TAKE THAT

Lmao, I looked it up on youtube and i was like wow... it's o.d. with sex... I WANNA SEE SOME ROLDERBLADERS!

airgear sucks, they got an episode where Doremi is learning how to use rollerskates in DoReMi, too.

What?

Rollerskates shouldn't be used in cartoons unless its that episode of Rocko's Modern Life with the roller disco.

I saw an old show from a long time ago called monster rancher, and the main character used his rollerskates for fighting all the time, mostly against dinosaurs and stuff.

Quote from: TomI saw an old show from a long time ago called monster rancher, and the main character used his rollerskates for fighting all the time, mostly against dinosaurs and stuff.

I remember that show it was pretty much ok if I remember correctly. Very boring.

Very cheesy.

That show was cool, I had one of the games  

I watched that show for several episodes then quit because I got annoyed with how many times they sad "baddie".

thanks for reminding me.
It was another one of those cartoons that ruined my saturdays.