What are the chemical symbols of chromite and iron ore?
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Chromite is iron magnesium chromium oxide: (Fe,Mg)Cr2O4\n\nIron ores are rocks and minerals from which metallic iron can be economically extracted. The ores are usually rich in iron oxides and vary in colour from dark grey to rusty red. The iron itself is usually found in the form of magnetite (Fe3O4), hematite (Fe2O3), limonite or siderite.
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Ferric sulfite, or iron (III) sulfite
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They are different terms for talking about the same thing.  Many elements have several valences. Iron, for instance has common valences of 0, +2 and +3.  You can say that iron metal exhibits a valence of 0 or that iron as metal is in the 0 oxidation state.\n\nSimilarly, iron (II) oxide  (FeO) exhibits a valence of 2 or is in the +2 oxidation state.\n\nI guess there is a fine point here: iron always has valences of 0, 2, 3 etc. but it doesn't exhibit them all at once.  Note that it can exhibit more that one valence at a time.  Iron in Fe3O4 exhibits +2 and +3 valences at the same time and so has a mixed oxidation state.
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weak organic acid= vinegar\nTitanium Oxide = sun block\nalkaline earth hydroxide= milk of magnesia\nalkali metal= NaCl\npaper chromatography= a penny and iron vinegar mixture\ntransition element= iron or copper\nnonmetal=sugar\nelectrolyte= NaCl\na noneletrolyte solution= sugar and water\noxide  of a element = rust or sun block
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A. Pyrite and magnetite are both from the same crystal system. That means they form crystals in a similar shape or pattern. They are both from the isometric system. They will both be blocky crystals but may not be exactly the same. Perfect pyrite crystals are cube shaped or diploidal (see:http://webmineral.com/data/Pyrite.shtml), and magnetite is an octahedron (see: http://webmineral.com/data/Magnetite.shtml).\n\nHardness of magnetite is 5 1/2-6 on Mohs scale and pyrite is 6- 6 1/2.  \n\nBoth have conchoidal fracture. (Quartz has conchoidal fracture in case you need to picture this)\n\nBoth have a similar density. Pyrite has a density of 4.8-5 g/cc and magnetite has a density of 4.95 gm/cc.\n\nBoth have a metallic luster. \n\nB. The best way to distinguish between them is to use a streak test. Magnetite will be grayish-black and pyrite will be greenish-black.\n\nThe other major difference is that magnetite will be naturally magnetic, and pyrite will not be. \n\n\nThe lesson here is to learn think of your different properties as sort of a tool kit. Decide which properties are useful and which ones will not be useful for the particular samples you are testing. Be sure to be familiar with all of the properties you can use. A list would be:\na. cleavage\nb. color (one of the least reliable)\nc. density\nd. luster\ne. fracture\nf. crystal habit (can be confusing because some minerals have several possible)\ng. hardness (know the hardness of common tests like a penny, a knife, a quartz crystal, glass, etc.)\nh. streak\ni. magnetism\nj. taste (best test for Halite or sylvite)\nk. There are lots more that involve using thin sections in a microscope, and X-ray diffractometer, etc.
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In acidic solutions, dichromate is the predominant species.  When the pH rises, as it would when you're adding ammonia to your acidic solution, the predominant form for chromium(VI) is the chromate ion, CrO4(2-), which is yellow.
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Magnetite or AKA 'lodestone' - an iron containing mineral that is slightly magnetic. The orientation of the iron in the mineral is lined up much like we think of normal man-made magnets. This allows it to be attracted to earth's magnetic field.
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If you assume Iron(III) oxide (ferric oxide, Hematite, red iron oxide, synthetic maghemite, colcothar), then no.
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Stainless steel contains chromium that was put there by diffusing it in there with high heat and a concentration difference.  Metals corrode because they get converted from neutral, solid form to ions (they are oxidized, that's why oxidation is a synonym for corrosion) that combine with negatively charged ions (usually oxides or chlorides) and are no longer metal, and many times soluble, hence taking a chunk out of your original metal.  Chromium is a more active metal than the iron that makes up most of the steel.  This means when both are present on the same surface, the chromium is more likely to dissolve into ions and electrons than the iron.\n\nWhen stainless is exposed to dissolved oxygen in water (for example) the chromium atoms will dissolve their way towards the surface of the steel. Then, they will be oxidized:\n\nCr(s)-->Cr3+ + 3e-\n\nWhat little iron that may have been oxidized before the chromium reached the surface can gain these 3 electrons and join the surface as solid iron again.  Otherwise, once the Cr reaches the surface, it'll corrode to form chromium oxide, a greenish black powdery ceramic that doesn't stick well to the surface, and can be easily rinsed away or knocked off.  And while the Cr will be oxidized, the iron will not because the Cr is more active. The steel itself remains shiny and well, stainless (without rust).  However, when the steel runs out of Cr atoms to sacrifice to protect the iron (once they become chromium oxide, they won't go back to being regular Cr metal, and the oxide does NOT stick to the surface to protect it), the iron will rust.
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The official English name for the element in question is Iron.\n\nThe official symbol for the element is Fe, which comes from the Latin name for iron: "Ferrum."\n\nThe latest international convention of naming iron compounds (using English) is to  call the compound Iron and use Roman numerals to indicate the oxidation state of the iron.  Therefore, FeCl3 is Iron (III) Chloride, while FeS is Iron (II) Sulfide.\n\nOlder methods called Iron (III) compounds "Ferric" and Iron (II) compounds "Ferrous," so that the examples above would be called Ferric Chloride and Ferrous Sulfide.
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ferric oxide, or rust, is the product
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Nickel (II) oxide, sulphur dichloride, and chlorine\n\n2NiCl2 + S02 ---> SCl2 + 2NiO + Cl2
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Dichromate ion is: Cr2072-.\n \nhybrid state is:sp3d.\none lp on each Cr atom\n4 pi bonds\n2 0- so overall charge is 2-\nstructure not possible to be shown here.\nBye
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Iron (II) SulfIDE\n\nSodium ChlorIDE\n\nSodium HydroxIDE\n\nand Lead...umm...something. *lol*\n\nThe answer is evidently (A). =D\n\n\n\nPS okay, so yea, someone already wrote what i wrote when i was typing it. sorry!
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Sodium is +1 times 2 =+2\nSo the chromate is -2\nOxygen is -2 times 4 = -8\nSo the chromium is +6
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Copper, Iron, Chromium, Aluminium
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PH3:                           Phosphine\nAg2SO3:                    Silver Phosphite\nFeCO3:                      Iron(II) Carbonate\nN2O4:                        Dinitrogen tetroxide\nPb(OH)2:                   Lead(II) Hydroxide