what is an example of an alkaline earth halide?
152932
alkaline earth metals are group 2A in the periodic table, they are Be, Mg, Ca, Sr, Ba, Ra.\nhalide is the name of salt that has halogen group (group 7A).they are F, Cl, I, Br, At.\nSince the valence of alkaline is 2 and that of halogen is 1, we'll have this chemical formula: MX2 (can't type subscript :P ) (2 should be typed in subscript).\nFor example: MgCl2, MgI2, BaCl2, CaBr2,....
677407
Astatine and iodine are both halogens and presumably have the chemical properties of that group. (Available quantities of At are of the order of 0.001 mg, with a half-life of 7 hours, so not much chemistry has been done on it!)\n\nAs a group is descended, halogens (and other non-metals for that matter) become less reactive. This is because halogens react by completing their outer shell of electrons, however, the attraction between outer electrons and the nucleus gets less down the group, even thought the number of protons increases, as the outer shell is further away and inner electrons shield outer electrons from the full nuclear charge.\n\ni hope this helps.
455088
Alkaline earth elements are the elements of the 2nd group in the periodic table. The hydroxides formed by Calcium(Ca),Magnesium(Mg),Beryllium(Be),Strontium(Sr),Barium(Ba  \n\nSo the chemical formula for alkaline earth hydroxides can be:\nCa(OH)2-Calcium hydroxide\nMg(OH)2-Magnesium hydroxide\nBe(OH)2-Berellium hydroxide(unstable)
233865
Generally, the elements that form ionic bonds tend to have either very high or very low electronegativity. This means the Alkali metals, Alkaline Earth metals, and the Halogens, especially when reacting with each other.
215105
yes ................see this for more info\n\n\nhttp://en.wikipedia.org/wiki/Alkali_metal
697035
this page has all your answers about ionic compounds\nhttp://misterguch.brinkster.net/ionic.html\n\nthis link give the answer to q2\nhttp://www.uncp.edu/home/mcclurem/lattice/halite1.gif
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.
1121228
I don't see any example of Metallic or network covalent solid materials in the compounds you listed.  \n\nBaCl2 is called Barium Chloride because it is an ionic compound.  You only use Mono, Di, Tri, etc prefixes for molecular compounds.  \n\nLiCl = Ionic\nBaCl2 = Ionic\nBCl3 = molecular\nCCl4 = molecular\nNCl3 = molecular\n\nAlthough Boron can possibly form network covalent bonds much like Carbon and Silicon, the fact that Boron Trichloride has very low melting point as well as boiling point clearly indicates that it does not have network covalent bonds.  A network covalent compound is very stable and has very high M.P and B.P like diamond and quarts. \n\nMetallic bonding is the is the bonding within metals. It involves the localized sharing of free electrons among a lattice of metal atoms.  Which means that to have metallic bonding the compound can not have any nonmetals in it.  In your list of compounds, they all have nonmetals in the compound, therefore non of them are metallic.
171909
IgDs that naturally have a neutral to alkaline ph
248245
Iodine is the least likely to form an iodide anion because it is the lest electronegative of the halogens. \n \nTHe halogens tend to want to draw and electron towards their neucleus.  Fluorine has the highest electronegativity.  It has a small electron cloud, so the outer most electrons are close to the nucleus and are more strongly pulled there.  Iodine has a large electron cloud.  The outer most electrons of iodine are much further away from the neuleus, so it can't pull electrons in as close.\n\nHope that helps.\n\nPS.  F, Cl, Br, and I all are diatomic, so they all form F2, Cl2, Br2, and I2.
922294
1) NH(4)Cl - Ammonium chloride\n\n2) HClO(2) - Chlorous acid\n\n3) Ca(BrO(3))2 - Calcium Bromate\n\n4) BeSO(4) - Beryllium sulphate\n\n5) (NH(4)) (3)N - Ammonium nitride\n\n6) RbI - Rubidium iodide
481911
H2, or hydrogen gas.\n\nFor example, take magnesium metal and hydrochloric acid.\n\nMg + 2HCl -> H2 + MgCl2\n\nThis is a displacement reaction, in which a free element (Mg) breaks the bond between a compound (HCl) and then bonds to the ion with the opposite charge (Cl-) forming a new compound (MgCl2).  The ion left over (H+) loses its charge and becomes a pure element (H2).
127454
If such a compound existed, it would be ionic. Calcium (IV) Chloride.\n\nBut it won't exist, particularly as an ionic compound. You're not going to be able to pull the p electrons from the calcium without a fight and chlorine isn't strong enough (or even fluorine, for that matter). Maybe you can achieve the species in the gas phase ... I don't know.\n\nIf it's covalent, what possible structure could it have? What do the bonding orbitals look like?
927969
alkaline earth metals are elements of group 2 in periodic table, so they have 2 electrons in outermost orbit. so to become stable they will try to loose 2 electrons to have stable electronic configuration. so they all have +2 oxidation states.\n\ni hope this will help you out
821226
1. sodium hypochlorite\n2. hydrogen chloride\n3. concentrated sulphuric acid\n4. oxidising it, for example with potassium manganate(VII).\n\nIf you've done the other 96, well done!
48646
CuI2 Copper (II) iodide\nSF6 sulfur hexafluoride\nNaOCl Sodium hypochlorite\nPb3(PO4)2 lead (II) phosphate\nHClO Hypochlorous acid\n\nChlorine triflouride  ClF3\nChromiumIII carbonate  Cr2(CO3)3\nPotassium Chlorate KCLO3\nSodium peroxide Na2O2 \nMercuryI chloride HgCl\n\nThanks You're welcome
556705
Ba(OH)2, MgBr2, CH3COOH, NH4OH\n\nFirst two are strong electrolytes, second two are weak (do not completely dissociate).