How is effective nuclear charge related to the electron affinity of oxygen and fluorine?
Q. (more than one answer is possible) The fluorine has a larger effective nuclear charge than oxygen. The electron affinity becomes more exothermic (negative) as the effective nuclear charge increases. The electron affinity becomes more endothermic (positive) as the effective nuclear charge increases. The fluorine has a less exothermic electron affinity than oxygen. The fluorine has a more exothermic electron affinity than oxygen.
Asked by domican - Thu Nov 13 14:39:43 2008 - - 1 Answers - 0 Comments
A. The fluorine has a larger effective nuclear charge than oxygen. NO The electron affinity becomes more exothermic (negative) as the effective nuclear charge increases. YES The electron affinity becomes more endothermic (positive) as the effective nuclear charge increases. NO The fluorine has a less exothermic electron affinity than oxygen. YES The fluorine has a more exothermic electron affinity than oxygen. NO
Answered by Ezra - Thu Nov 13 18:36:08 2008
Q. (more than one answer is possible) The fluorine has a larger effective nuclear charge than oxygen. The electron affinity becomes more exothermic (negative) as the effective nuclear charge increases. The electron affinity becomes more endothermic (positive) as the effective nuclear charge increases. The fluorine has a less exothermic electron affinity than oxygen. The fluorine has a more exothermic electron affinity than oxygen.
Asked by domican - Thu Nov 13 14:39:43 2008 - - 1 Answers - 0 Comments
A. The fluorine has a larger effective nuclear charge than oxygen. NO The electron affinity becomes more exothermic (negative) as the effective nuclear charge increases. YES The electron affinity becomes more endothermic (positive) as the effective nuclear charge increases. NO The fluorine has a less exothermic electron affinity than oxygen. YES The fluorine has a more exothermic electron affinity than oxygen. NO
Answered by Ezra - Thu Nov 13 18:36:08 2008
Why is the radius of a fluoride ion similar to that of a fluorine atom?
Q. Aren't radii of anions larger than their corresponding atoms? Why is the radius of a fluoride ion(0.133 nm) similar to that of a fluorine atom?(that's a question from my textbook) Is there something to do with its electronegativity?
Asked by twister - Mon Dec 1 06:57:13 2008 - - 1 Answers - 0 Comments
A. fluorine ion is larger than the fluorine atom because fluorine ion has a stronger positive charge on its nucleus than fluorine atom.=] hope it will help=]
Answered by scientific - Tue Dec 2 01:51:59 2008
Q. Aren't radii of anions larger than their corresponding atoms? Why is the radius of a fluoride ion(0.133 nm) similar to that of a fluorine atom?(that's a question from my textbook) Is there something to do with its electronegativity?
Asked by twister - Mon Dec 1 06:57:13 2008 - - 1 Answers - 0 Comments
A. fluorine ion is larger than the fluorine atom because fluorine ion has a stronger positive charge on its nucleus than fluorine atom.=] hope it will help=]
Answered by scientific - Tue Dec 2 01:51:59 2008
What's the difference between fluorine and fluoride?
Q. If the question asks to write the word, what is KF? Is it potassium fluorine or fluoride? Is fluorine the element and fluoride when mixed with oxygen? Please help!
Asked by imsiedaisy - Wed Sep 2 04:45:48 2009 - - 2 Answers - 0 Comments
A. Fluorine is an element, existing as F2. It is a dangerous, explosive, toxic gas. Fluoride is a form of fluorine, that has gained an electron, to form an anion, it is F-. It is the most commonly encountered form of fluorine, as in salts, like Potassium FluorIDE (KF). the ending IDE implies a negative ion, that does not contain oxygen. The type of negative anion that does contains oxygen ends in ATE, ie., Fluorate is the FO- anion. Fluorine and oxygen mixed in the right proportions, under the right conditions can form Oxygen fluorides, like Dioxygen difluoride, which is a mightily powerful oxidising agent. Also, oxidising salts like hypofluorites are known. The ending ITE is an old fashioned term for ATE's. For example, HYPOfluorITE is… [cont.]
Answered by Filpi - Wed Sep 2 07:39:18 2009
Q. If the question asks to write the word, what is KF? Is it potassium fluorine or fluoride? Is fluorine the element and fluoride when mixed with oxygen? Please help!
Asked by imsiedaisy - Wed Sep 2 04:45:48 2009 - - 2 Answers - 0 Comments
A. Fluorine is an element, existing as F2. It is a dangerous, explosive, toxic gas. Fluoride is a form of fluorine, that has gained an electron, to form an anion, it is F-. It is the most commonly encountered form of fluorine, as in salts, like Potassium FluorIDE (KF). the ending IDE implies a negative ion, that does not contain oxygen. The type of negative anion that does contains oxygen ends in ATE, ie., Fluorate is the FO- anion. Fluorine and oxygen mixed in the right proportions, under the right conditions can form Oxygen fluorides, like Dioxygen difluoride, which is a mightily powerful oxidising agent. Also, oxidising salts like hypofluorites are known. The ending ITE is an old fashioned term for ATE's. For example, HYPOfluorITE is… [cont.]
Answered by Filpi - Wed Sep 2 07:39:18 2009
Element that forms with Fluorine to form covalent bond?
Q. I need to know of any covalent bonds including fluorine for a chemistry project. Thanks!
Asked by Brittany C - Sun Mar 15 14:35:34 2009 - - 1 Answers - 0 Comments
A. Try an Alkaline metal.
Answered by Will - Sun Mar 15 14:42:37 2009
Q. I need to know of any covalent bonds including fluorine for a chemistry project. Thanks!
Asked by Brittany C - Sun Mar 15 14:35:34 2009 - - 1 Answers - 0 Comments
A. Try an Alkaline metal.
Answered by Will - Sun Mar 15 14:42:37 2009
What is the equilibrium concentration of fluorine?
Q. The equilibrium constant for the reaction of fluorine gas with bromine gas at 300 K is 54.7 and the reaction is: Br2(g) + F2(g) 2BrF(g) What is the equilibrium concentration of fluorine if the initial concentrations of bromine and fluorine were 0.119 moles/liter in a sealed container and no product was present initially?
Asked by physicsnerd - Sun Apr 22 19:58:21 2007 - - 3 Answers - 0 Comments
A. this is a typical gas equilibrium problem. im going to take u through it step by step since it is important that u no how to do these. u can email me if u want. Br2 + F2 --> 2BrF we know that the Br and F started as 0.119M and we assume that there was no BrF. we will call what Br2 went down X. that means that F2 also goes down X and BrF goes up 2X. Br2 + F2 --> 2BrF 0.119M...0.119M...0M -X...-X...+2X 0.119-X...0.119-X...2X now lets right the equiliblium expression. [BrF]^2 ___ = K [Br2] [F2] [2x]^2 ___ = 54.7 [0.119-x]^2 we can take the square root of both sides. 2X ___ = 7.396 0.119-X cross multiply 2X= 7.396(0.119-X) 2X= 0.88 - 7.396X add 7.396X to both sides 9.396X = 0.88 divide by 9.396 X= 0.094M the eq… [cont.]
Answered by Ari - Sun Apr 22 20:12:38 2007
Q. The equilibrium constant for the reaction of fluorine gas with bromine gas at 300 K is 54.7 and the reaction is: Br2(g) + F2(g) 2BrF(g) What is the equilibrium concentration of fluorine if the initial concentrations of bromine and fluorine were 0.119 moles/liter in a sealed container and no product was present initially?
Asked by physicsnerd - Sun Apr 22 19:58:21 2007 - - 3 Answers - 0 Comments
A. this is a typical gas equilibrium problem. im going to take u through it step by step since it is important that u no how to do these. u can email me if u want. Br2 + F2 --> 2BrF we know that the Br and F started as 0.119M and we assume that there was no BrF. we will call what Br2 went down X. that means that F2 also goes down X and BrF goes up 2X. Br2 + F2 --> 2BrF 0.119M...0.119M...0M -X...-X...+2X 0.119-X...0.119-X...2X now lets right the equiliblium expression. [BrF]^2 ___ = K [Br2] [F2] [2x]^2 ___ = 54.7 [0.119-x]^2 we can take the square root of both sides. 2X ___ = 7.396 0.119-X cross multiply 2X= 7.396(0.119-X) 2X= 0.88 - 7.396X add 7.396X to both sides 9.396X = 0.88 divide by 9.396 X= 0.094M the eq… [cont.]
Answered by Ari - Sun Apr 22 20:12:38 2007
Why is bromine a liquid and fluorine a gas?
Q. Really need help with this, don't particularly get it... Fluorine, F , is a gas, and Bromine, Br , is a liquid at room temperature. Discuss the different states of these elements at room temperature. Please include in your answer information on particle separation, energy, particle motion and the attractive forces between the particles.
Asked by R S - Wed Dec 19 21:14:40 2007 - - 3 Answers - 0 Comments
A. Bromine simply has more electrons than fluorine, so there is more chance of there being a polar imbalance, thus resulting in stronger dispersion forces between molecules. To become a gas, a substance must break these combined Van Der Waals forces, so if the forces are stronger, it requires more energy to break them. Bromine is a liquid because room temperature is not hot enough to overcome the strong dispersion forces. This also accounts for the fact that iodine is solid at room temperature.
Answered by unknown - Wed Dec 19 21:53:47 2007
Q. Really need help with this, don't particularly get it... Fluorine, F , is a gas, and Bromine, Br , is a liquid at room temperature. Discuss the different states of these elements at room temperature. Please include in your answer information on particle separation, energy, particle motion and the attractive forces between the particles.
Asked by R S - Wed Dec 19 21:14:40 2007 - - 3 Answers - 0 Comments
A. Bromine simply has more electrons than fluorine, so there is more chance of there being a polar imbalance, thus resulting in stronger dispersion forces between molecules. To become a gas, a substance must break these combined Van Der Waals forces, so if the forces are stronger, it requires more energy to break them. Bromine is a liquid because room temperature is not hot enough to overcome the strong dispersion forces. This also accounts for the fact that iodine is solid at room temperature.
Answered by unknown - Wed Dec 19 21:53:47 2007
How much fluorine is formed in this problem?
Q. The mass ratio of sodium to fluorine in sodium fluoride is 1.21:1. A sample of sodium fluoride produced 26.5 of sodium upon decomposition. Could you please explain how you got the answer too? Thanks
Asked by ~Princess~ - Wed Sep 23 14:37:41 2009 - - 1 Answers - 0 Comments
A. This isn't complicated. Say the question said that the mass ratio of a compound was 3:2, and you got 9 grams of the first out, you'd get 6 grams of the second. Divide by the sodium side (1.21) and multiply by the fluoride/fluorine side (um, 1).
Answered by Tweek - Wed Sep 23 15:22:36 2009
Q. The mass ratio of sodium to fluorine in sodium fluoride is 1.21:1. A sample of sodium fluoride produced 26.5 of sodium upon decomposition. Could you please explain how you got the answer too? Thanks
Asked by ~Princess~ - Wed Sep 23 14:37:41 2009 - - 1 Answers - 0 Comments
A. This isn't complicated. Say the question said that the mass ratio of a compound was 3:2, and you got 9 grams of the first out, you'd get 6 grams of the second. Divide by the sodium side (1.21) and multiply by the fluoride/fluorine side (um, 1).
Answered by Tweek - Wed Sep 23 15:22:36 2009
What's a common, everyday material with fluorine (the element) in it?
Q. I'm doing a project for Chemistry on fluorine and I have to bring something to class with fluorine in it. I know toothpaste has it, but do any foods? Gum, for example? Thanks for your help!
Asked by asister20 - Sun Mar 8 21:24:31 2009 - - 4 Answers - 0 Comments
A. Here is a nice list of its uses in day-to-day life:
Answered by Thomas - Sun Mar 8 21:28:30 2009
Q. I'm doing a project for Chemistry on fluorine and I have to bring something to class with fluorine in it. I know toothpaste has it, but do any foods? Gum, for example? Thanks for your help!
Asked by asister20 - Sun Mar 8 21:24:31 2009 - - 4 Answers - 0 Comments
A. Here is a nice list of its uses in day-to-day life:
Answered by Thomas - Sun Mar 8 21:28:30 2009
What is a compound between Fluorine and sodium?
Q. Science: Naming compounds What is a compound between Fluorine and sodium? What is the chemical formula and the compound name using the naming rules?
Asked by unknown - Thu Jul 8 16:41:15 2010 - - 3 Answers - 0 Comments
A. the formula is NaF and the name is sodium flouride and it's the sodium salt of hydroflouric acid (HF).
Answered by Eldy - Thu Jul 8 17:09:58 2010
Q. Science: Naming compounds What is a compound between Fluorine and sodium? What is the chemical formula and the compound name using the naming rules?
Asked by unknown - Thu Jul 8 16:41:15 2010 - - 3 Answers - 0 Comments
A. the formula is NaF and the name is sodium flouride and it's the sodium salt of hydroflouric acid (HF).
Answered by Eldy - Thu Jul 8 17:09:58 2010
What are the allotropes of fluorine, if any?
Q. I need to know all the allotropes of fluorine. If it doesn't have any, just say so. Name the isotopes of fluorine also please.
Asked by allstarbri22 - Wed Dec 13 23:40:49 2006 - - 4 Answers - 0 Comments
A. I would have to say none, never heard of any. Plus, it's rarely found in nature alone since it is the most reactive nonmetal. However, we can find allotropes for carbon, sulfur, phosphorus, and oxygen.
Answered by Math-Chem-Physics Teacher - Thu Dec 14 00:05:49 2006
Q. I need to know all the allotropes of fluorine. If it doesn't have any, just say so. Name the isotopes of fluorine also please.
Asked by allstarbri22 - Wed Dec 13 23:40:49 2006 - - 4 Answers - 0 Comments
A. I would have to say none, never heard of any. Plus, it's rarely found in nature alone since it is the most reactive nonmetal. However, we can find allotropes for carbon, sulfur, phosphorus, and oxygen.
Answered by Math-Chem-Physics Teacher - Thu Dec 14 00:05:49 2006
What does the element Fluorine look like?
Q. I need to write a children's book to teach them about Fluorine and I was wondering how I could turn Fluorine into a fun character What does it exactly look like?
Asked by Christine Murai - Sat Sep 13 16:42:17 2008 - - 2 Answers - 0 Comments
A.
Answered by Hannah - Sat Sep 13 16:46:04 2008
Q. I need to write a children's book to teach them about Fluorine and I was wondering how I could turn Fluorine into a fun character What does it exactly look like?
Asked by Christine Murai - Sat Sep 13 16:42:17 2008 - - 2 Answers - 0 Comments
A.
Answered by Hannah - Sat Sep 13 16:46:04 2008
What is the raw material for obtaining Fluorine?
Q. I also need to know how Fluorine is extracted from it.
Asked by unknown - Wed Oct 21 16:37:57 2009 - - 2 Answers - 0 Comments
A. wikipedia, do your own research with something so trivial
Answered by unknown - Wed Oct 21 16:42:25 2009
Q. I also need to know how Fluorine is extracted from it.
Asked by unknown - Wed Oct 21 16:37:57 2009 - - 2 Answers - 0 Comments
A. wikipedia, do your own research with something so trivial
Answered by unknown - Wed Oct 21 16:42:25 2009
In a molecule of fluorine how many shared electrons are there in each fluorine atom in the outer energy level?
Q. In a molecule of fluorine how many shared electrons are there in each fluorine atom in the outer energy level? Choices: a)1 b)2 c)8 d)32
Asked by seaworldfan2010 - Sun Nov 18 10:23:37 2007 - - 3 Answers - 0 Comments
A. We only concern ourselves here with the p electrons. Each Fluorine atom has five electrons on its outermost shell. Only one electron is available for bonding. The others are paired. The key word to see is 'shared'. The bonding electron pair is shared between two atoms in each fluorine molecule. Each fluorine atom has that bonding pair in a p orbital. Paradoxically, each fluorine atom has two shared electrons as specified in the question, even though the total of shared electrons is two. Drawing a picture would make this easier to follow.
Answered by Sciman - Sun Nov 18 10:33:24 2007
Q. In a molecule of fluorine how many shared electrons are there in each fluorine atom in the outer energy level? Choices: a)1 b)2 c)8 d)32
Asked by seaworldfan2010 - Sun Nov 18 10:23:37 2007 - - 3 Answers - 0 Comments
A. We only concern ourselves here with the p electrons. Each Fluorine atom has five electrons on its outermost shell. Only one electron is available for bonding. The others are paired. The key word to see is 'shared'. The bonding electron pair is shared between two atoms in each fluorine molecule. Each fluorine atom has that bonding pair in a p orbital. Paradoxically, each fluorine atom has two shared electrons as specified in the question, even though the total of shared electrons is two. Drawing a picture would make this easier to follow.
Answered by Sciman - Sun Nov 18 10:33:24 2007
According to the octet rule, which of the following are possible combinations of nitrogen and fluorine?
Q. According to the octet rule, which of the following are possible compounds of nitrogen and fluorine? Select all that apply NF2 NF3 N2F2 NF Could you also explain how this works? I thought I understood it but I can't get the correct answer.
Asked by DefyGravity44 - Wed Nov 19 19:59:44 2008 - - 1 Answers - 0 Comments
A. NF3,because N has 5 and F has 7 so use that to do the Lewis and Dot Formula. Trust me it is the right answer.
Answered by Cubs Fan - Wed Nov 19 22:44:23 2008
Q. According to the octet rule, which of the following are possible compounds of nitrogen and fluorine? Select all that apply NF2 NF3 N2F2 NF Could you also explain how this works? I thought I understood it but I can't get the correct answer.
Asked by DefyGravity44 - Wed Nov 19 19:59:44 2008 - - 1 Answers - 0 Comments
A. NF3,because N has 5 and F has 7 so use that to do the Lewis and Dot Formula. Trust me it is the right answer.
Answered by Cubs Fan - Wed Nov 19 22:44:23 2008
Is there an Electropositive Gas like Fluorine is the Most electronegative gas?
Q. Is there an electropositive gas that can cancel out Fluorine, a highly electronegative gas?
Asked by confuzzled88 - Fri Jan 1 23:48:37 2010 - - 4 Answers - 0 Comments
A. Don't listen to the moron that said chlorine, Electro negativity increases as you go from the bottom left hand side of the periodic table to the upper right, but remeber, noble gasses have a full valence shell so they have no electro negativity or positivity. No, there are no very electro positive gasses, some of the alkali metals (caesium, rubidium, francium if it wouldn't decay in .0001 seconds) that have low melting and boiling points, but those are metals. There is no strongly electronegative substance that is a gas at room temperature, there is hydrogen which has an electro negativity of 2.2 out of 4, making it the most electropositive gas. But in the whole scheme of things, hydrogen is not very electropositive, stick to the alkali… [cont.]
Answered by unknown - Sat Jan 2 00:09:55 2010
Q. Is there an electropositive gas that can cancel out Fluorine, a highly electronegative gas?
Asked by confuzzled88 - Fri Jan 1 23:48:37 2010 - - 4 Answers - 0 Comments
A. Don't listen to the moron that said chlorine, Electro negativity increases as you go from the bottom left hand side of the periodic table to the upper right, but remeber, noble gasses have a full valence shell so they have no electro negativity or positivity. No, there are no very electro positive gasses, some of the alkali metals (caesium, rubidium, francium if it wouldn't decay in .0001 seconds) that have low melting and boiling points, but those are metals. There is no strongly electronegative substance that is a gas at room temperature, there is hydrogen which has an electro negativity of 2.2 out of 4, making it the most electropositive gas. But in the whole scheme of things, hydrogen is not very electropositive, stick to the alkali… [cont.]
Answered by unknown - Sat Jan 2 00:09:55 2010
Explain the benefits and any possible problems associated with the introduction of chlorine and fluorine into?
Q. Explain the benefits and any possible problems associated with the introduction of chlorine and fluorine into drinking water supplies.
Asked by Pegasus - Sun Dec 16 06:02:25 2007 - - 3 Answers - 0 Comments
A. Firstly, technically, you should be aware that it is not the elemental variety of either that applies here. Rather it is a fluoride or chloride complex involved. Chlorine gas, itself, is an excellent disinfecting agent, and will destroy a large amount of life. It is also very good at bleaching; though elemental oxygen that can be released adjacent to the material to be bleached is better and safer. Chlorination will usually involve a salt (such as the sodium one of) chorine/oxygen anionic complex; such as found in household bleach (sodium hypochlorite - NaOCl). Fluorine the element is plain dangerous. But simple salts of it are basically benign - e.g. KF, NaF. The form of fluoride used in drinking water is more complex, and its… [cont.]
Answered by big_george - Sun Dec 16 06:32:45 2007
Q. Explain the benefits and any possible problems associated with the introduction of chlorine and fluorine into drinking water supplies.
Asked by Pegasus - Sun Dec 16 06:02:25 2007 - - 3 Answers - 0 Comments
A. Firstly, technically, you should be aware that it is not the elemental variety of either that applies here. Rather it is a fluoride or chloride complex involved. Chlorine gas, itself, is an excellent disinfecting agent, and will destroy a large amount of life. It is also very good at bleaching; though elemental oxygen that can be released adjacent to the material to be bleached is better and safer. Chlorination will usually involve a salt (such as the sodium one of) chorine/oxygen anionic complex; such as found in household bleach (sodium hypochlorite - NaOCl). Fluorine the element is plain dangerous. But simple salts of it are basically benign - e.g. KF, NaF. The form of fluoride used in drinking water is more complex, and its… [cont.]
Answered by big_george - Sun Dec 16 06:32:45 2007
Which statement best explains why the fluorine atom is a good candidate for forming one bond to another atom?
Q. a. Fluorine has an atomic number of 9. b. Fluorine has an electron configuration of 1s2 2s2 2p5 and so it has one half-filled orbital. c. Fluorine has a high electronegativity. d. The 3s orbital has no electrons in it.
Asked by pinkgiraffe - Sat Feb 21 05:48:09 2009 - - 3 Answers - 0 Comments
Q. a. Fluorine has an atomic number of 9. b. Fluorine has an electron configuration of 1s2 2s2 2p5 and so it has one half-filled orbital. c. Fluorine has a high electronegativity. d. The 3s orbital has no electrons in it.
Asked by pinkgiraffe - Sat Feb 21 05:48:09 2009 - - 3 Answers - 0 Comments
How do i find the mass of fluorine in grams?
Q. Copper (II) fluoride contains 37.42 % F by mass.. Use this percentage to calculate the mass of fluorine in grams contained in 31.0 g of copper (II) fluoride. How would you calculate this? please provide steps. :) thanks!
Asked by bellla - Tue Mar 30 00:44:19 2010 - - 1 Answers - 0 Comments
A. 31.0g x .3742 = mass of Fluorine
Answered by Devon - Tue Mar 30 02:09:24 2010
Q. Copper (II) fluoride contains 37.42 % F by mass.. Use this percentage to calculate the mass of fluorine in grams contained in 31.0 g of copper (II) fluoride. How would you calculate this? please provide steps. :) thanks!
Asked by bellla - Tue Mar 30 00:44:19 2010 - - 1 Answers - 0 Comments
A. 31.0g x .3742 = mass of Fluorine
Answered by Devon - Tue Mar 30 02:09:24 2010
What is the name, formula, and uses for two compounds containing the element Fluorine?
Q. I'm doing a chemistry project and need to know. Also, does anyone know how to make a pure sample of Fluorine? I'm not being asked to actually make it, I just need to know how it's done. Thanks :D
Asked by All<3 - Thu Sep 17 11:56:43 2009 - - 1 Answers - 0 Comments
A. Hydrofluoric Acid- Used to etch glass Polytetrafluoroethylene- Also known as Teflon. Used as nonstick coating for cooking utensils. Pure Fluorine gas is prepared by electrolysis of Hydrogen Fluoride in the presence of Potassium Fluoride. The basic reaction is: HF + KF ---> KHF2 2KHF2 --> 2KF +H2 + F2 The Fluorine gas is evolved at the anode, and Hydrogen gas is evolved at the cathode. Note: Fluorine and many of its compounds are extremely reactive and dangerous! Do not try this at home. Hope this helps
Answered by Civil - Thu Sep 17 12:10:06 2009
Q. I'm doing a chemistry project and need to know. Also, does anyone know how to make a pure sample of Fluorine? I'm not being asked to actually make it, I just need to know how it's done. Thanks :D
Asked by All<3 - Thu Sep 17 11:56:43 2009 - - 1 Answers - 0 Comments
A. Hydrofluoric Acid- Used to etch glass Polytetrafluoroethylene- Also known as Teflon. Used as nonstick coating for cooking utensils. Pure Fluorine gas is prepared by electrolysis of Hydrogen Fluoride in the presence of Potassium Fluoride. The basic reaction is: HF + KF ---> KHF2 2KHF2 --> 2KF +H2 + F2 The Fluorine gas is evolved at the anode, and Hydrogen gas is evolved at the cathode. Note: Fluorine and many of its compounds are extremely reactive and dangerous! Do not try this at home. Hope this helps
Answered by Civil - Thu Sep 17 12:10:06 2009
What is the normal phase of fluorine?
Q. Im doing a project for school and i need to know what the normal phase is for the element fluorine and if anyone could tell me what the cost is for fluorine that would be cool too...thanks!
Asked by Jamie - Wed Sep 9 16:06:59 2009 - - 1 Answers - 0 Comments
A. At room temp fluorine is a gas, and an exceptionally reactive and toxic one at that. Steel pipe, even stainless piping, can actually burn in fluorine, and must be rigorously cleaned and then 'passivated' before F2 can be put into it. Passivation is basically gently fluorinating the surface, with low low F2 pressure, so it reacts slowly without releasing a lot of heat. I have handled chlorine in cylinders a fair amount without great concern, but fluorine is a whole lot more dangerous. For one thing, usually we used it as a mix of 25% F2 in N2, simply diluted to make it less violently reactive. For pricing go to a vendor, eg, matheson, linde, praxair, air liquide, liquid carbonic, et al, and ask for a budget quote [if prices are not listed… [cont.]
Answered by redbeardthegiant - Thu Sep 10 14:21:27 2009
Q. Im doing a project for school and i need to know what the normal phase is for the element fluorine and if anyone could tell me what the cost is for fluorine that would be cool too...thanks!
Asked by Jamie - Wed Sep 9 16:06:59 2009 - - 1 Answers - 0 Comments
A. At room temp fluorine is a gas, and an exceptionally reactive and toxic one at that. Steel pipe, even stainless piping, can actually burn in fluorine, and must be rigorously cleaned and then 'passivated' before F2 can be put into it. Passivation is basically gently fluorinating the surface, with low low F2 pressure, so it reacts slowly without releasing a lot of heat. I have handled chlorine in cylinders a fair amount without great concern, but fluorine is a whole lot more dangerous. For one thing, usually we used it as a mix of 25% F2 in N2, simply diluted to make it less violently reactive. For pricing go to a vendor, eg, matheson, linde, praxair, air liquide, liquid carbonic, et al, and ask for a budget quote [if prices are not listed… [cont.]
Answered by redbeardthegiant - Thu Sep 10 14:21:27 2009
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