Naming simple compounds?
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Huge order. Let's see how far it can be served.\n\n1. Monoatomic negative ions: take the element name (sometimes shortened) and add "-ide" (as in hydride, nitride, oxide, sulphide, phosphide, chloride...)\nPositive ions: element-name, charge (if several charges are possible), ion (sodium ion, iron II ion...)\n\n2. Polyatomic ions:\nComplexes with various ligands list the ligands and the central ion/atom.\nOxygen as ligands has its own nomenclature, depending on oxidation state. E.g. Sulphate, sulphite, perchlorate, chlorate, chlorite, hypochlorite...\n\n3. Binary molecular compounds: Halogen, oxygen and sulphur compounds usually have the correspondent "-ide" as if you had ionic compounds. Usually the more electropositive element is used as center.\n\n4. Acids: Oxygen acids have a similar nomenclature to oxygen ions.
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Lithium nitride\nGallium oxide\nRubidium chloride\nBarium sulfide\nFor binary ionic compounds, you just write the name of the first element, then take the second element and just change the ending to -ide.
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I can't tell you the name because i can't remember that stuff but the product will be K(NO3) PbI2\nif you're writing it in the long form it will be\n2KI + Pb(NO3)2 yeilds (arrow) 2K(NO3) + PbI2
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1. Crystals\n\n2. Covalent bonds\n\n3.  Molecules\n\n4.  Vasoline\n\nCrossword = nucleuss\n\nH- Ion
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CnHnx2\n\nFor instance, the simplest alkene is ethene, or C2H4.
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Bromocyclohexane. You don't need to add the "1-" because it's assumed to be 1 by IUPAC convention.
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google it and type 'periodic table, first twenty elements'\nn u'll get sumthing, far quicker than lettin sum1 write them up 4 u.
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SrSe\nK2O\nCa3N2\nCoI3\n\nthe numbers should be subscripts
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You have to do this by analogy to other molecules.\nFor instance Se is in the same column as S and therefore SeO3 and SeO2 will look like SO3 and SO2.  Similarly SiF4 will have the structure of CF4. As comes two periods after N.\n\nFinally, the structure of simple molecules like SO2 can often be found on Wikipedia or here:\n http://www.3dchem.com/table.asp
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NH3OH\nPbO\nKBr\nPCl4\nAl(NO3)3\nBa3(PO4)2\nSpelling error?? C4H10 ??? (not sure here)\nSn(OH)4\nNH4NO3\nLi3P
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acetylene. usually any carbon compound with two carbons gets the 'nick name' starting with acetyl-  like u take acetic acid for example .. it's got CH3-COOH two carbons hence ACETic-acid
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an easy example you can remember is H2O(water).\nif u want a more difficult one, u can use CH3COOH(acetic acid)!\n\nALL DE BEST!
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Fundamental concepts\nNomenclature\nNomenclature refers to the system for naming chemical compounds. There are well-defined systems in place for naming chemical species. Organic compounds are named according to the organic nomenclature system. Inorganic compounds are named according to the inorganic nomenclature system.\n\nRelated Topics:\nChemical compound - Organic compound - Organic nomenclature - Inorganic compound - Inorganic nomenclature\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nSee also: IUPAC nomenclature\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nAtoms\nMain article: Atom.\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nAn atom is a collection of matter consisting of a positively charged core (the nucleus) which contains protons and neutrons, and which maintains a number of electrons to balance the positive charge in the nucleus.\n\nRelated Topics:\nNucleus - Protons - Neutrons - Electron\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nElements\nMain article: Chemical element.\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nAn element is a class of atoms which have the same number of protons in the nucleus. This number is known as the atomic number of the element. For example, all atoms with 6 protons in their nuclei are atoms of the chemical element carbon, and all atoms with 92 protons in their nuclei are atoms of the element uranium.\n\nRelated Topics:\nProton - Nucleus - Atomic number - Carbon - Uranium\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nThe most convenient presentation of the elements is in the periodic table, which groups elements with similar chemical properties together. Lists of the elements by name, by symbol, and by atomic number are also available.\n\nRelated Topics:\nPeriodic table - By name - By symbol - Atomic number\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nSee also: isotope\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nCompounds\nMain article: Chemical compound\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nA compound is a substance with a fixed ratio of elements which determines the composition, and a particular organisation which determines chemical properties. For example, water is a compound containing hydrogen and oxygen in the ratio of two to one, with the Oxygen between the hydrogens, and an angle of 104.5° between them. Compounds are formed and interconverted by chemical reactions.\n\nRelated Topics:\nElement - Water - Hydrogen - Oxygen - Chemical reaction\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nMolecules\nMain article: Molecule.\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nA molecule is the smallest indivisible portion of a pure compound that retains a set of unique chemical properties. A molecule consists of two or more atoms bonded together.\n\nRelated Topics:\nCompound - Atom - Bonded\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nIons\nMain article: Ion.\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nAn ion is a charged species, or an atom or a molecule that has lost or gained an electron. Positively charged cations (e.g. sodium cation Na+) and negatively charged anions (e.g. chloride Cl-) can form neutral salts (e.g. sodium chloride NaCl). Examples of polyatomic ions that do not split up during acid-base reactions are hydroxide (OH-), or phosphate (PO43-).\n\nRelated Topics:\nCations - Sodium - Anions - Chloride - Salts - Sodium chloride - Polyatomic ion - Acid-base reactions - Hydroxide - Phosphate\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nBonding\nMain article: Chemical bond.\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nA chemical bond is the force which holds together atoms in molecules or crystals. In many simple compounds, valence bond theory and the concept of oxidation number can be used to predict molecular structure and composition. Similarly, theories from classical physics can be used to predict many ionic structures. With more complicated compounds, such as metal complexes, valence bond theory fails and alternative approaches which are based on quantum chemistry, such as molecular orbital theory, are necessary.\n\nRelated Topics:\nAtom - Molecule - Crystal - Valence bond theory - Oxidation number - Classical physics - Metal complexes - Quantum chemistry - Molecular orbital\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nStates of matter\nMain article: Phase (matter)
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(a) 2 NaClO3 -> 2 NaCl + 3 O2\n\n(b) 3 MnCl2 + 2 Al -> 3 Mn + 2 AlCl3\n\n(c) C4H10 + 13/2 O2 -> 5 H20 + 4 CO2 \n                  or\n(c) 2 C4H10 + 13 O2 -> 10 H20 + 8 CO2\n\nBalancing is quite simple for these simple equations. You just have to see the left hand side pick up an element, see how many atoms of that element are there in it and multiply the R.H.S compound containing that element with a number which will be equal to no. of atoms in the l.h.s. Then again repeat the procedure by picking another element.....see it's quite difficult to explain you with writing aneways i hope it helps u :)
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ethers: R-O-R (answer)\nPhenols: Ph-O-H\nAlcohols: R-O-H\nEsters: R-(C=O)-O-R
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1) MgCO3\n2) AlF3\n3) BF3\n4) NH4F\n5) SnO2\n6) HCL\n7) Ca(OH)2\n8) Na2S\n9) K2SO3\n\n1) do yo mean PbCl2? then Lead (II) Chloride\n2) Lithium Bromide\n3) Potassium Sulfate\n4) Megnesium Hydroxide\n5) don't know\n6) Hydrogen Nitrate\n7) Barium Phosphate\n8) Carbon Monoxide\n9) Copper Brimide\n10) Ammonium Chloride\n11) Tin (II) Hydroxide\n12) Calcium Nitrogide\n13) Strontium Oxide\n14) Tetraiodide prefix for 9 and oxide\n\nFe^+2\nNi^2\nAg^+1
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CoCl3.6NH3 yellow 3 [Co(NH3)6]Cl3 \nCoCl3.5NH3 purple 2 [Co(NH3)5Cl]Cl2 \nCoCl3.4NH3 green 1 [Co(NH3)4Cl2]Cl \nCoCl3.4NH3 violet 1 [Co(NH3)4Cl2]Cl \nThe green and violet compounds must have some further difference. \nAll have 6 ligands (coordination number = 6)