Does the element neon form compounds with any elements?
141567
The noble gasses are inert because they all have full electron orbitals, but the heavier noble gasses have so many electron shells that it is possible to strip some of the outer electrons off to get a reaction. Neon is going to be really tough to get a a reaction out of, but Xenon, a much heavier noble gas, will form compounds with Flourine under the right conditions. I'm thinking it's XeF4, but I can't recall exactly.\n\nLasers don't exactly require chemical reactions, as far as I know, so a Helium Neon laser could contain the two gasses unreacted with each other.
763705
No, no lead and silicon are elements, not compounds. Neither is made by combining carbon and chlorine. Please do not tell anyone they are, especially someone not very good at chemistry.\n\nCarbon tetrachloride, that's a carbon atom surrounded by four chlorine atoms is a chloride of carbon. It's sort of pyramid shaped. Here's some info on it.
964369
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.
825330
Ionic compound is usually non-metal reacting with metals.\nThat is positive ion forming a compound with negative ion.\nWe call the compound is ionic if the elements we've used have positive or negative charge.\n\nConvalent compunds have different story because they are sharing the electrons and they don't really have any charge.\n\nI don't know what you mean by exactly what kinds of elements make ionic compounds because almost all of them do! Except all the noble gases far right side of table will not react at all (Where there is argon).\n\nIt is that simple
67895
This has some info about neon with pics (scroll down on the page)\n\nhttp://ww.chem4kids.com/files/elements/010_shells.html
643847
1. Sodium will combine with Iodine, but Iodine never has a -3 charge. That would involving adding electrons to the 6st orbital, which would be considerably less stable than adding 1 electron to fill the 5p orbitals.\n\nSodium also doesn't form a +2 charge.\n\nBased on your data, it would be:\n\n3Na^+2 + 2I^-3 = Na3I2 \n\nI think it's:\n\nNa+ + I- ---> NaI or 2Na + I2 (solid) ---> 2NaI \n\nionic\n\n\n2. Protons will activately react with hydride donors to give hydrogen gas. That's why Lithium aluminium hydride is so reactive to water ... it considers the water's hydrogen atoms as a source for protons.\n\nH+ + H-1 ---> H2   covalent and non-polar.\n\n3.\nC^+4 + 20^-2 ---> CO2\n\nCovalent and non-polar
167726
potassium can form many compounds. such as KCN KCl KOH et cetera.
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.
839156
Generally Group I and Group II elements form ionic compounds with non-metals. Hence for all of the metals above, they should form ionic compounds with oxygen.\nSodium - Na+; oxide - O2-\nHence you need 2 sodium ions to calcen out the -2 charge on the oxide ion, and the formula of sodium oxide is Na2O.\nSimilarly for potassium oxide, K2O.\nCalcium - Ca2+, oxide - O2-\n1 of each is needed to cancel out the charges, hence the formula CaO.\nSimilarly for MgO.\nAns: Na2O, K2O, MgO and CaO\n\nHope this helps :)
83207
The only thing I can think of is a fullerene cage that is trapping the Neon...hmmm\nIf you were thinking Nitrogen...try any amino acid ...umm adesonine (if thats how its spelt)
857082
1.  Split up the elements and give them their original charges\n\nAg +\nNO3 -\nK +\nBr -\n\n2.  Combine an element with an element that they were not with, putting them side by side will help\n\nAg + with Br -\nNO3 - with K +\n\n3. So now you have 2 new compounds\n\nAgBr & KNO3-\n\n4.  Their should be a chart in your book that tells you which compound would be the precipitate but i don't think their is a precipitate for this reaction'\n\nso both will dissolve in a solution
802199
Hi,, hydrogen, oxygen, and nitrogen... \n\n good luck.....
712728
choose the noble gas that comes before the element.   in Mn(2+)'s case, that's Ar\n\nwrite the noble gas down in brackets, and continue on with the electron config. as normal\n\n[Ar}4s23d3\n\nFor O(2-), it turns into Neon so it would just be [Ne]
910584
Try this site:\nwww.webelements.com\nit should be on there this is the site I used for my chemistry report(interview with an element) on Neon
570696
It´s 10. Neon. \nIt has two energy levels, filled with 2 and 8 electrons respectively.
852794
dobereiner's like that mendeleev guy right? if my memory is right, all  of the elements above have similar chemical properties, that's why he placed them in his "triads". This means that all of them act similarly. Remember that it is the VALENCE electrons that causes the specific reaction of an element. So, as all three elemnts have the same number of valence electrons, they act similarly.
292657
Neon - it's inert and remains monoatomic ; whereas carbon, boron and fluorine combine with other elements to form compuonds.