What's the name of these polyatomic compounds? How do you know? I really want to learn and I need help! Thanks
814096
in order:\nammonium chloride\ncalcium nitrate\nIron(III)hydroxide(this will turn to Fe2O3 fast which is rust)\nSodium carbonate\npotassium sulfate\nammonium sulfate\nI think you mean: Ca(NO3) with this one which is calcium nitrate\nand the last one is magnesium nitrite(not nitrate)
1133019
There are a lot of sites that have info.  Search for "formula writing polyatomic ions".\nIf you have a list of polyatomic ions like "SO4", "SO3", "PO4", etc. you will see that they have specific charges associated with them.  SO4 and SO3 both have a negative 2 charge.  Hydrogen has a +1 charge.  A compound must be neutral so you need 2 H to pair with one SO4.  +2-2=0.\nPO4 has a negative 3 charge, so you'd need 3 H+ to offset the 3 negatives.  H3PO4.\n\nAs far as naming them, search for "naming chemical compounds"  The examples you are asking about are actually acids, so you might need to look up "naming acids".
116719
What can we do, though? You need to take a relatively pure sample of your compound and dissolve it in a deuterated solvent (say CDCl3). Then you can use an NMR to find the different peaks.
120958
TO name an compound you must first know what kind of compound it is. If it is an ionic compound you just name it by its element name and add ide to the last element (example: sodium chloride. If it is a binary molecular compound (two nonmetals bonded) you use prefixes to notate how many of each element there is in the compound (mono,di,tri,tetra,etc but never use mono on the first element name)(example: dinitrogen trioxide). If the element has hydrogen in it it is an acid. If it only has two elements it is a binary acid and you name it by saying hydro-(element name) acid, but you always add "ic" to the end ( example: hydrochloric acid). If the acid contains oxygen it is an oxyacid. You name it by "(ion name+ ic/ous) acid". To determine whether or not you say "ic" or "ous" use this rule: "ate" ions use "ic" ending "ite" ions use "ous" endings. Examples of each of these are chloric acid and chlorous acid.
200262
mono = 1\ndi = 2\ntri = 3\ntetra = 4\npent = 5\nhex = 6\nhept = 7\noct = 8\nnon = 9\n\nnonmetals:\nif there is no prefix for the first element, it is assumes to be one.\nTHe ening of the anion (the second one listed) is changed to -ide.\n\ncarbon - 1 \noxygen - 2\nCO2  <---The number is a subscript, but you cant do that on here\n\nPhosphorous - 1\nIodine - 3\nPI3\n\nHydrogen - 2\nOxygen - 1  (it should be monoxide)\nH2O\n\nHope that helps you.  Don't feel bad; you can't know what you haven't learned.
752782
There are a few methods, most of them require memorization, or a good chart.  For example, ionic compounds get named by adding the names of their ions, but molecular compounds get named by each individual element and a prefix of how many there are.  Then you have acids...  \n\nhere are some examples:\n\nNaCl - Sodium Chloride\nNa2CO3 - Soduum Carbonate\nNa3PO4 - Sodium Phosphate\n\nNotice that sodium is always sodium, not mono, di or tri.\n\nMolecular compounds are different, here are some examples:\n\nNF3- nitrogen trifluoride   \nNO - nitrogen monoxide OR nitric oxide (Ionic)\nNO2 - nitrogen dioxide  \nN2O - dinitrogen monoxide (laughing gas)\n\nI wont even go into acids, or Hydrocarbons\n\nI hope that gets you started anyway
1116509
analize an existing polymer with as many properties of the ones you are looking for, determine the formula ( possibly use a mass spectrometer for the recipe,)  experiment with the atomic structure of the elements in the formula. wouldn't it be great if you could manipulate the structure at subatomic level, i.e. at levels below protons and neutrons like quarks.\ntry changing the formula ( recipe?) at its basic level, with different proportions of at least carbon and hydrogen, possibly adding 'alloying' elements into the atomic structure.
54928
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.
83406
Ionic compounds (like NaCl) for lattice structures.  These lattice structures make up the crystaline arrangement of the compound.\n\nThe lattice of NaCl looks like a cube,\nhttp://zimmer.csufresno.edu/~davidz/Chem3AF97/ChB/IonicBond.html\nhttp://departments.kings.edu/chemlab/chemlab_v2/nacl.html
488364
Chemexper.com its super cool , type in the name of the compound and it will give you a ton of info about the thing you are looking at. I order chemicals off of it but it was really useful in researching for my Ochem labs as well.
565895
Your compound is not fully named...well type the compound name serach bar in www.google.com and see if you get the answer
776359
Methylamine\n\nNext time, just type the chemical formula into http://en.wikipedia.org/ and see if they have your compound documented.
1040448
ask your chem prof or tutor ..it's hard to explain over the internet!
838145
tetrahedral: 4\ntrigonal bipyramidal:  5\noctahedral:  6\n\nChemistry joke:\n \nName the compound: Ba(Na)2\nAnswer: Banana\n\nHahahahahahaha!
274092
All ionic compounds dissociate into respective +ve and -ve ions in aquous solutions.\n\nYou possibly want to know such compounds which give both +ve and -ve ions with more than 1 charge.\n\nYes salts of all alkline earth metals (+ve2) with ions of more than one atoms (CO3,PO4 etc) having more than 1 -ve charge dissociate in the way you need to know.
298587
Look up the site chemfinder.com.  its a good website if you have not heard of it already.
80472
I'm trying to work with this info:\n\nOctet Rule - atoms want to have eight electrons in their valence shell (two for H) (most will form octets, some will not)\n\nMultiple Bonds\nSingle bond - a covalent bond in which a single pair of electrons is shared by two atoms\ndouble bond - two pairs of electrons are shared by two atoms\ntriple bond  - three pairs of electrons are shared by two atoms\n-generally form with C, N, O, S\n-------\nOkay, oxygen might attach easily to one of the Cls, leaving no spaces, but I'm not sure if there is a doule bond or something weird like that. Same with C.\nIf I remember correctly, CO2 looks like this:\nO=C=O\n------\nWait, check this out- I found the following (and no further info) somewhere on the net.\n\nE) COCl2\n      (C is the \n       central atom)\n\n----------\nWait. No.\n_______\nCl- C -Cl\n___O___\nI'm going to try that...\nI don't know. It lacks the symmetry that you normally see and it's kinda weird looking. What do you think of what I got?\n__________\nI found a pic: http://www.chem.ox.ac.uk/inorganicchemistry3/C/COCl2.html\nLooks kinda like yours.\n______\nHoly Mother of God - http://www.chem.ox.ac.uk/inorganicchemistry3/C/COCl2.html\nI found the name of the compound- phosgene- and did an image search. *exclamation of glee*\n___\nLol, better be right. Later.