[Chemistry4me]

Is that something that you have studied? I'm wondering why you think I am a student [] []
I don't blame you, its probably because of my poor knowledge of science... [] []

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Is that something that you have studied? I'm wondering why you think I am a student [] []
I don't blame you, its probably because of my poor knowledge of science... [] []

Ok, indeed I thought you were studying chem at university..
Those things are taught during the qualitative analysis courses.

[Chemistry4me]

I am humbled... [] [] [:I] [:I]

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I am humbled... [] [] [:I] [:I]

Why? You would have a reason if you had already studied these things but you wouldn't know them the same... []

[Chemistry4me]

I am humbled... [] [] [:I] [:I]

Why? You would have a reason if you had already studied these things but you wouldn't know them the same... []

Huh? I'm not sure what you mean.

[Chemistry4me]

Chlorine, greenish-yellow gaseous element, in group 17 of the periodic table. The gas has an irritating odour and in large concentrations is dangerous; it was the first substance used as a poison gas in World War I. Free chlorine does not occur in nature, but its compounds are common minerals, and it is the 20th most abundant element in the Earth's crust. Chlorine is an active element, reacting with water, organic compounds, and many metals. Four oxides have been prepared: Cl2O, ClO2, Cl 2O6, and Cl2O7. Chlorine will not burn in air, but it will support the combustion of many substances; an ordinary paraffin candle, for example, will burn in chlorine with a smoky flame. Chlorine and hydrogen can be kept together in the dark, but react explosively in the presence of light. Chlorine solutions in water are familiar in the home as bleaching agents, or in weaker solutions as a sterilizing agent, for example in swimming pools and public water systems. A few parts per million of chlorine can be added to drinking water to kill bacteria, and the chlorine then removed with sodium sulphite prior to distribution to homes. Industrial chlorine is produced by treating salt with nitrogen oxides or by oxidizing hydrogen chloride. Chlorine is shipped as a liquid in steel bottles.

[Chemistry4me]

Argon, inert gaseous element that is the third most prevalent gas in the Earth's atmosphere. In group 18 of the periodic table, argon is one of the noble gases. Argon was discovered in 1894 by the British scientists Sir William Ramsay and Baron John William Strutt Rayleigh. They were led to this discovery by a discrepancy between the density of supposedly pure nitrogen, prepared from air, and actually pure nitrogen, prepared from ammonium nitrate. Argon is composed of monatomic molecules and is colourless and odourless. It constitutes 0.93 per cent of the atmosphere. Argon is produced commercially by the fractional distillation of liquid air. It is used in large quantities to fill electric light bulbs. If air is left in incandescent bulbs, the filament burns; if the bulb is evacuated, as was formerly done, the tungsten filament tends to evaporate, blackening the inside of the bulb. To prevent this evaporation, the bulb can be filled with nitrogen, which is the least expensive gas for the purpose, or argon, which is better, as it is a poorer conductor of heat and so cools the filament less. Argon is also used in one type of neon lamp. Whereas pure neon gives a red light, argon gives a blue light. Argon tubes require a lower voltage than neon tubes, and for this reason small amounts of argon are sometimes mixed with neon. Argon is also used in electric-arc technology, in gas lasers, and in arc welding.

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I am humbled... [] [] [:I] [:I]

Why? You would have a reason if you had already studied these things but you wouldn't know them the same... []

Huh? I'm not sure what you mean.

Do you have a degree in Chemistry?

[Chemistry4me]

Ok, it seem that I have been taken out of context, what I should have said was "I am humbled that you think I am a university student [] [] [:I] [:I]"

Do you have a degree in Chemistry?

No  [:I]

[Chemistry4me]

Potassium, (from Latin kalium, “alkali”), chemically reactive, extremely soft metallic element. In group 1 of the periodic table. Potassium exists in three natural isotopic forms, with mass numbers 39, 40, and 41. Potassium-40 is radioactive and has a half-life of 1.28 billion years. The most abundant isotope is potassium-39. Several radioactive isotopes have been artificially prepared. Potassium is found in nature in large quantities, ranking eighth in order of abundance of the elements in the crust of the Earth, in various minerals such as carnallite, feldspar, saltpetre, greensand, and sylvite. Potassium bromide (KBr), a white solid formed by the reaction of potassium hydroxide and bromine, is used in photography, engraving, and lithography, and in medicine as a sedative. Potassium chromate (K2CrO4), a yellow crystalline solid, and potassium dichromate, or potassium bichromate (K2Cr2O7), a red crystalline solid, are powerful oxidizing agents used in matches and fireworks, in textile dyeing, and in leather tanning. Potassium iodide (KI), a white crystalline compound that is very soluble in water, is used in photography for preparing gelatin emulsions and in medicine for the treatment of rheumatism and overactivity of the thyroid gland. Potassium nitrate (KNO3), a white solid prepared by fractional crystallization of sodium nitrate and potassium chloride solutions, is used in matches, explosives, and fireworks, and in pickling meat.

[Chemistry4me]

Calcium, reactive, silvery-white metallic element. In group 2 of the periodic table. Calcium has six stable and several radioactive isotopes. A malleable and ductile metal, calcium rapidly tarnishes to yellow on exposure to air. Calcium is fifth in abundance among the elements in the Earth's crust, but it is not found uncombined in nature. It occurs in many highly useful compounds, such as calcium carbonate (CaCO3), of which calcite, marble, limestone, and chalk are composed; calcium sulphate (CaSO4) in alabaster or gypsum; calcium fluoride (CaF2) in fluorite; calcium phosphate (Ca3(PO4)2) in rock phosphate; and in many silicates. In cold, dry air, calcium is not readily attacked by oxygen, but when heated it unites vigorously with the halogens, oxygen, sulphur, phosphorus, hydrogen, and nitrogen. Calcium reacts violently with water, forming the hydroxide Ca(OH)2 and releasing hydrogen. The metal is obtained mainly by electrolysis of fused calcium chloride, a costly process. Until recently the pure metal had little use in industry. It is being used to an increasing extent as a deoxidizer for copper, nickel, and stainless steel. Because calcium hardens lead when alloyed with it, lead-calcium alloys are excellent for bearings, superior to ordinary lead antimony for grids in storage batteries, and more durable as sheathing for lead-covered cable. Calcium is present in teeth and bones (as a calcium hydroxyphosphate), and in many body fluids essential to muscle contraction, the transmission of nerve impulses, and the clotting of blood.

[miriam0920]

Since you are studying chemistry you have to know that the flame's colour it's not blue but lilac:

Lilac?  Do you want to debate with me too?

[Chemistry4me]

Since you are studying chemistry you have to know that the flame's colour it's not blue but lilac:
Lilac?  Do you want to debate with me too?

Are you addressing me?

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Since you are studying chemistry you have to know that the flame's colour it's not blue but lilac:

Lilac?  Do you want to debate with me too?

No, no, it was just to give you some more informations. (Maybe I said it badly because of my not perfect knowledge of english language). They could ask you this at an exam.

I know of a teacher of analythical chemistry at university in Florence, who one day (many years ago) asked a student which colour is Ni⁺⁺ in water solution. The student replied "green". The teacher: just "green"? The student replied yes, and he didn't pass the exam. The correct answer for the teacher was "apple green"!  []
(It's not a joke).

http://www.uncp.edu/home/mcclurem/ptable/ni.htm

[Chemistry4me]

Scandium, soft silver-white metallic element with an atomic number of 21. Scandium is one of the transition elements in the periodic table. Scandium was discovered in 1879 by the Swedish chemist Lars Fredrik Nilson, eight years after the Russian chemist Dmitry Ivanovich Mendeleyev had predicted, on the basis of the periodic law, that the element exists in nature and that its properties resemble those of the element boron. Scandium is sometimes regarded as one of the rare earth elements. Scandium occurs in rare minerals such as wolframite. It is 31st in order of abundance of the elements in the Earth's crust. It forms trivalent, colourless salts.

[Chemistry4me]

Titanium, silver-white metallic element used principally to make light, strong alloys. Titanium is soluble in certain acids, and aqueous solutions of the metal can be prepared, but it is not directly dissolved by water. The metal is extremely brittle when cold, but is readily malleable and ductile at a low red heat. Titanium burns in oxygen to form titanium dioxide, and it burns in nitrogen to form titanium nitride, TiN. Titanium forms the salts titanium tetrachloride, TiCl4; titanium trichloride, TiCl3; and titanium dichloride, TiCl2. It ranks ninth in abundance among the elements in the crust of the Earth but is never found in the pure state. Because of its strength and light weight, titanium is used in metallic alloys and as a substitute for aluminium. Alloyed with aluminium and vanadium, titanium is used in aircraft for fire walls, outer skin, landing-gear components, hydraulic tubing, and engine supports. The compressor blades, discs, and housings of jet engines are also made of titanium. A supersonic transport, flying at speeds between 2,410 and 3,220 km/h, uses from 14 to 45 tonnes of titanium. Titanium is also widely used in missiles and space capsules. The relative inertness of titanium makes it available as a replacement for bone and cartilage in surgery and as a pipe and tank lining in the processing of foods. It is used in heat exchangers in desalination plants because of its ability to withstand salt-water corrosion.

[Chemistry4me]

Just type 'potassium flame colour' into Google images and you can decide whether it is blue or lilac.

[Chemistry4me]

Vanadium, silver-white metallic element . Vanadium takes a high polish and is one of the hardest of all metals. Vanadium is soluble in nitric and sulphuric acids and insoluble in hydrochloric acid, dilute sodium hydroxide, and dilute alcohol. Vanadium forms several acidic oxides, the most important of which are the dark green trioxide, V2O3, and the orange pentoxide, V2O5. Other important compounds include vanadium monosulphide, VS; vanadium trisulphide, V2S3; vanadium dichloride, VCI2; vanadium trichloride, VCI3; vanadium dihydroxide, V(OH)2; and metavanadic acid, HVO3.Vanadium ranks about 19th in abundance of the elements in the Earth's crust. It is never found in the pure state, but occurs in combination with various minerals throughout the world. Because of its hardness and great tensile strength, the metal is used in many alloys such as ferrovanadium, nickel vanadium, and chrome vanadium. Chrome-vanadium steels are used in the production of springs and in transmission gears and other engine parts. Titanium-vanadium alloys are used for missile cases, jet-engine housings, and nuclear-reactor components. As a catalyst, vanadium has largely replaced platinum in the manufacture of sulphuric acid and is employed widely as a photographic developer, as a reducing agent, and as a drying agent in various paints.

[Chemistry4me]

Chromium, grey metallic element that can take on a high polish. Chromium ranks about 21st in natural abundance among the elements in crustal rocks. Chromium can replace part of the aluminium or iron in many minerals, imparting to them their unique colours. Many precious gemstones owe their colour to the presence of chromium compounds. In chromites and chromic salts, chromium has a valence of +3. Most of these compounds are green, but some are red or blue. Chromic oxide (Cr2O3) is a green solid. Potassium dichromate (K2Cr2O7) is a red-orange, water-soluble solid that, when mixed with gelatin, gives a light-sensitive surface that is very useful in photographic processes. More than half the production of chromium goes into metallic products, and about another third is used in refractories. It is an ingredient in several important catalysts. The chief use of chromium is to form alloys with iron, nickel, or cobalt. The addition of chromium imparts hardness, strength, and corrosion resistance to the alloy. In the stainless steels, chromium makes up 10% or more of the final composition. Because of its hardness, an alloy of chromium, cobalt, and tungsten is used for high-speed metal-cutting tools. When deposited electrolytically, chromium provides a hard, corrosion-resistant, lustrous finish. For this reason it is widely used as body trim on cars and other vehicles.

[Chemistry4me]

Manganese, a silvery-white, brittle metallic element used principally in making alloys. Manganese metal corrodes in moist air and dissolves in acid. The metal does not occur in the free state, except in meteors, but is widely distributed over the world in the form of ores. It ranks about 12th in abundance among elements in the Earth's crust. Manganese is used principally in the form of alloys with iron, obtained by treating pyrolusite in a blast furnace with iron ore and carbon. The most important of these alloys, which are used in steelmaking, are ferromanganese, containing about 78% manganese, and spiegeleisen, containing from 12 to 33% manganese. Small amounts of manganese are added to steel as a deoxidizer; large amounts are used to produce a very tough alloy, resistant to wear. Safes, for example, are made of manganese steel containing about 12% cent manganese. Non-ferrous manganese alloys include manganese bronze (composed of manganese, copper, tin, and zinc), which resists corrosion from sea water and is used for propeller blades on boats and torpedoes, and manganin (containing manganese, copper, and nickel), used in the form of wire for accurate electrical measurements because its electrical conductivity does not vary appreciably with temperature.