Conservapedia - User contributions [en]

Cesium

2012-04-01T01:11:13Z

SallyReilly: minor change

{{Element | name=Cesium | symbol=Cs | anumber=55 | amass=132.9 amu | state=solid, but very easily melts | class=[[alkali metal]] | cstructure=Body-Centered Cubic | color=silver with slight gold tinge | date=1860 | discname=[[Bunsen, R.W. and Kirchoff, G.]] | origname=From the Latin ''Caesius'', meaning "sky blue" | uses=removing air traces in vacuum tubes | obtained=lepidolite, pollucite }}

'''Cesium''' is an element<ref>Wile, Dr. Jay L. ''Exploring Creation With Physical Science''. Apologia Educational Ministries, Inc. 1999, 2000</ref> in the [[alkali metal]] class of the periodic table. It is so chemically active that it is never found free (in elemental form) in nature, and catches fire on mere exposure to air and almost explodes on contact with water.
Cesium is a key component in atomic clocks. <ref>http://physicsworld.com/cws/article/news/25595</ref>

It was discovered by Robert Bunsen and Gustav Kirchoff, using their newly invented spectroscope, and was the first element to be discovered spectroscopically. It (along with [[rubidium]]) was identified by a previously unseen blue spectral line in the analysis of mineral water from a German spa. The name comes from that color.

==References==
<references/>

[[Category:Metals]]
[[Category:Elements]]

Francium

2012-04-01T00:24:38Z

SallyReilly: Expanding.

{{Element | name=Francium | symbol=Fr | anumber=87 | amass=223 amu | state=Solid | class=Alkali Metals | cstructure=Cubic Body Centered | color=silver if able to be isolated | date=1939 | discname=Marguerite Perey | origname=Named after France. | uses=None (far too short lived for any application). | obtained=Not commercially available, it is formed by the decay of [[actinium]]. }}
'''Francium''' is an [[element]], it is the heaviest discovered [[Alkali metal]]. It is very unstable and radioactive. It lasts for a very short time period (half life of approximately 22 minutes<ref>http://www.chemicool.com/elements/francium.html#appear</ref>) before decaying into [[Astatine]] via alpha decay or [[Radium]] via Beta Decay.

It is estimated that only between 20 and 30 grams of it exist in the earth's crust at any given point in time <ref>http://www.webelements.com/francium/</ref> and is in fact the second rarest naturally occurring element after Astatine. The only reason it exists is because of its part in the decay chain of [[Uranium]].

==Properties==
Francium would presumably be more reactive than [[Cesium]], reacting violently with Water to produce Francium Hydroxide and Hydrogen Gas. It would also react with Oxygen rapidly in the air. It has an esitmated melting point of 27 degrees Celsius, which would make it [[liquid]] in a warm room. None of these are confirmed owing to the rarity of the element and are based on the reactivity of the rest of the series.

==References==
{{reflist}}
[[Category:Metals]]

Alkali metals

2012-04-01T00:00:10Z

SallyReilly: Redirected page to Alkali metal

#REDIRECT [[Alkali metal]]

User:SallyReilly

2012-03-31T23:59:13Z

SallyReilly:

hello.

I like chemistry related stuff, I aim to improve chemistry related articles here. I am also interested in Christianity.

Benzene

2012-03-31T23:49:58Z

SallyReilly: actually it melts at quite a low temperature (melting point only a few degrees above freezing)

'''Benzene''' is an [[organic]] [[chemical compound]] (an [[aromatic ring]]) with formula C6H6. It is sometimes abbreviated Ph-H. Benzene is a [[carcinogen]] which is a colorless and flammable liquid that has a pleasant, aromatic odor and a low [[melting point]].

A [[hydrocarbon]], benzene is present in small proportion in some [[crude oil]]s and made commercially from [[petroleum]] by the [[catalyst|catalytic]] reforming of naphthenes in petroleum naphtha. It is also made from [[coal]] in the manufacture of coke. Benzene is used as a [[solvent]] in the manufacture of detergents, synthetic fibers, petrochemicals, and is a component of high-octane gasoline.

==See also==
*[[BTX]]

[[Category:Organic Chemistry]]
[[Category:Chemical Compounds]]

User:SallyReilly

2012-03-31T23:44:01Z

SallyReilly: Created page with "hello."

hello.

Alcohol

2012-03-31T23:42:57Z

SallyReilly: correction to general formula

''This is an article about the chemical [[functional group]]. For the beverage, see [[alcoholic drink]]s''

'''Alcohols''' are a group of organic compounds consisting of a hydrocarbon or group with an -OH group; CnH2n+1OH.

Commonly, the word alcohol refers to [[ethanol]] (C2H5OH), which is the alcohol found in [[alcoholic drink]]s. Ethanol is produced by yeast during the [[anaerobic]] [[metabolism]], comparable to the production of [[lactic acid]] in [[mammals]].

==Methanol==
[[Methanol]] consists of a single [[carbon]] atom, with three [[hydrogen]] atoms and a hydroxyl group (-OH). Traditionally, methanol was produced by the fermentation of wood, leading to the term 'wood alcohol'. Industrially, methanol can be produced by the reaction of [[carbon monoxide]] and [[hydrogen]] (CO + 2 H2 = CHO3OH). For this industrial process, copper, zinc oxide and aluminum oxide may be used as catalysts at 250°C and a pressure of 50-100 atm.

The primary use of methanol is its addition to ethanol to make it undrinkable. It has also been used as a [[biofuel]].

Methanol is highly toxic to humans. This toxicity is largely indirect, as alcohol dehydrogense metabolises methanol to form [[formaldehyde]], which causes blindness and death. Small amounts of methanol may be present in alcohol drinks are can cause a burning sensation of the eyes.

==Ethanol==
[[Ethanol]] (C2H5OH) is a major industrial spirit widely used in laboratories and household applications. It is also the type used in all [[alcoholic drink|alcoholic beverages]].

==Oxidation of Alcohols==
By heating a primary alcohol with an oxidising agent, such as acidified potassium dichromate, an [[aldehyde]] is formed. If the oxidation is down under reflux, the aldehyde will then itself oxidise to a carboxylic acid.

Secondary alcohols also oxidise, forming a [[ketone]]. Ketones, unlike aldehydes, cannot be oxidised further.

[[Category:Organic Chemistry]]