Outline

• Introduction

• History

• Physical properties

• Nature sources of element

• Methods of purification

• Commercial and industrial uses

• Characteristics

• Fluorine’s effect in human body

• Environmental effects of fluorine

• Citation

Self introduce of fluorine

Hey everyone! I am so glad have this opportunity to introduce my self to you all. My name is Fluorine, usually people use the symbol F stand for me, and my atomic number is 9. Tell you a secret, my weight is 18.9984. My address in periodic table is period 2, group 17, located in P block. I am also a family member of halogens. And this is my Electron configuration

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I got to say that I am not a good boy, I thought I am one of the toughest elements. There is a thing that make me really proud of myself-- I am the most electronegative element,It makes me almost can react with anyone! So people do need lots of care to handle me duo to my extremely reactive and poisonous. So after a brief introduce, do you have interest on me? I believe you do, just keep reading and you gonna know more things about me!

HISTORY

Around 1670 Fluorine compound was first record to used. They found out that bohemian emerald(CaF2) can etch glass. So Chemists start wonder what cause the material have the ability of etching glass. The first report was made by Andreas Sigismund Marggraf in 1764. He found out when fluorite was heated with sulfuric acid, the resulting solution is able to corrode its glass container.

What really interested me was the isolation part, because the F2 is toxic a lot of scientists injury or get killed while they trying to isolate F. "Fluorine martyrs" is how people describe how danger and how hard to isolate fluorine. They were lots of scientists attempt to isolate fluorine though different way, like Edmond Frémy tried to passing electric current through pure hydrofluoric acid, but electric current could not pass through hydrogen fluoride. Even though he was failed, His student Henri Moissan (French chemist) continued the search. Moissan devised a new ideas that can make the reaction in to a really low temperature environment in a special bath, though this strategy can slow the rate of corrosion. He also made a lot of corrosion-resistant equipment like a special container made by mixture of platinum and iridium, which is more chemically resistant. Finally in 1886 Moissan succeeded in isolating elemental fluorine—the pale yellow gas, He ended the work of almost 74 years that many chemists had done effort on it even sacrifice. In 1906, Moissan received the Nobel Prize in chemistry. I do want to share the honor word for him by the Nobel prize community, for the great scientist.

in recognition of the great services rendered by him in his investigation and isolation of the element fluorine...The whole world has admired the great experimental skill with which you have studied that savage beast among the elements.

It’s a good story of chemistry, it encourage people at chemistry filed, because there is no problems that cannot be beaten.

Physical properties

Phase gas

Density (0 °C, 101.325 kPa) 1.696[2] g/L

Liquid density at b.p. 1.505[3] g·cm−3

Melting point 53.48 K, −219.67 °C, −363.41[4] °F

Boiling point 85.03 K, −188.11 °C, −306.60[4] °F

Triple point 53.48 K, 90[4] kPa

Critical point 144.41 K, 5.1724[4] MPa

Heat of vaporization 6.51[2] kJ·mol−1

Molar heat capacity (Cp) (21.1 °C) 31[3] J·mol−1·K−1

(Cv) (21.1 °C) 23[3] J·mol−1·K−1

Vapor pressure

P (Pa) 1 10 100 1 k 10 k 100 k

at T (K) 38 44 50 58 69 85

Nature sources of element

Fluorine has an abundance of 0.65% in earth’s cryst. There are more than 300 minerals that fluorine can be found as well as in the biosphere. In nature, fluorine occurs mainly in the minerals fluorspar (CaF2) and cryolite (Na3AlF6),Cryolite is also known as Greenland spar.. Lowest one is Fluorapatite (Ca5(PO4)3F). (3.5%).

Abundance earth's crust:585 parts per million by weight, 104 part per million by moles

Abundance solar system:500 parts per billion by weight, 30 parts per billion by moles

Cost, pure:$190 per 100g

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Methods of purification

I found lots of methods to purify fluorine. At my paper I think I just choose a simple one, It’s a method relate to our daily life, a method that can remove fluorine from water.

This technique can remove fluoride from water through the addition of calcium and phosphate compound. After that let the water pass through an saturated bone charcoal medium. As pictures show below.

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After doing research I found out this is a broad used method which contain a lot of water purifier.

Commercial and industrial uses

There are lots of uses of fluorine in industry and commercial area nowadays, It was start during the World WarⅡ when techniques were developed for the large scale production of of various inorganic fluorides. Basic raw materials such as fluorspar（CaF2）and elemental fluorine gas(F2) became commercially available form companies.

At here I want to introduce the fluorspar industry

The naturally-occurring mineral fluorspar, CaF2, is the principal source of fluorine, Fluorspar is classified according to its uses and purity Acid-grade fluorspar --used in the production of anhydrous hydrogen fluoride and aqueous hydrofluoric acid, is at a minimum 97% CaF2. Ceramic grade this material is 85-96% Caf2 and is used extensively by the ceramic industry to produce opaque enamels, for covering stell parts of appliances and fixtures.

Metallurgical grade -- also know as met-spar, is only 70-80% CaF2, and the least expensive fluorspar on the market, It is used by steel, alumium, magnesium and nonferrous metal industries as a smelting flux to refine alloys.

Characteristics

Unique characteristics that fluorine and its compound have is most reactive and electronegative of all elements, so its reacts happen vigorously with most of elements, oxygen, helium, neon and krypton are except.

Silicon dioxide can combustion in fluorine and produce oxygen

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The color of fluorine is pale yellow, its a diatomic, highly corrosive, also flammable gas, have a pungent odor.

Florine can react with water violently to produce oxygen and the really corrosive hydrofluoric acid.

The reaction is 2F2(g) + 2H2O(g) → O2(g) + 4HF(g)

2F2(g) + 2H2O(l) → O2(g) + 4HF(aq)

3F2(g) + 3H2O(l) → O3(g) + 6HF(aq)

Fluorine’s effect in human body

There are lots of discuss about fluorine’s effect in human body, some people saying that fluorine can done good job and is better to intake some fluorine, however others saying that fluorine is really harmful to our body so we should totally avoid take more fluorine in our body.

Some of elements that our body require to intake and to help maintain good situation, fluorine is one of them. Fluorine is important for the healthy teeth. Because it can protect teeth from tooth decay. And that’s is why fluorine also contain in the toothpaste and our daily water. And fluorine can also help firm a major part of salts from bones. That’s why fluorine is fairly important to human body.

But, we must should know that fluorine is a very danger element. With it toxicity, fluorine can severely damage any animal tissue with which it comes in contact and is really toxic when inhaled at the level of parts per million.

Even though we don’t intake fluorine directly but fluorides are also can do harmful in our body. They are cumulative with ingestion of fluoride from water, food, air, toothpaste all the sources. The problem is our body cannot eliminate all of them, that is mean fluoride will have accumulate in our body. With this situation, fluorides can distort protein structure causes the immune proteins cannot recognise body proteins and attack them. And may also cause thyroid disease. So as you can see there are lots of problems could happen because of taking fluorine.

Environmental effects of fluorine

Fluorine that in soil may accumulate in plants. Most of plants are sensitive for fluorine exposure that can cause damage of leave and a decline in growth.

Animals that eat those plants which contain fluorine may accumulate fluorine in their bodies. Finally cause animal exposed to high concentration of of fluorine. Too much fluorine could cause low birthweights.

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NAME:GEN LI

INSTRUCTOR: DR.Douglas

CITATION

Fluorine, the first hundred years (1886-1986). Elserier Science Publishing Co., Inc.,1986

Fluorine and the environment. Elsevier Publication, First edition, 2006

Organic fluorine chemistry, William A. Sheppard, New York, W.A benjamin, 1969.

2006, "Fluorine (revised)." Chemical Elements: From Carbon to Krypton., "fluorine." The Columbia Encyclopedia, 6th Ed.. 2013, and "fluorine." The Oxford Pocket Dictionary of Current English. 2009. "Fluorine (revised)." Encyclopedia.com. HighBeam Research, 01 Jan. 2006. Web. 10 Nov. 2013.

Fluorine." - Uses, Pictures, Characteristics, Properties, Periodic Table. N.p., n.d. Web. 10 Nov. 2013.

"Fluorine and Human Body." Bukisa. N.p., n.d. Web. 10 Nov. 2013.

"The Effects Of Fluoride On The Thyroid Gland." The Effects Of Fluoride On The Thyroid Gland. N.p., n.d. Web. 10 Nov. 2013.

Fluorine - F." Fluorine (F). N.p., n.d. Web. 10 Nov. 2013.