What kinds of elements make ionic compounds?
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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
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um...  subtract???  hahaha\n\nThe higher the differences in electronegativity, the more ionic the compound.  The higher electronegative atom/ion will want to "hog" all the electrons.  They are greedy like that.  They don't want to share (which would be a covalent bond).
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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?
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You want us to calculate acitivites?\n\nYou need to determine the ionic strength and atomic radius in order to do that.
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as i have explained with the formation of ionic compounds. this is an ionic compound like table salt (NaCl)\nLithium gives up the one outermost electron to Chlorine which has a stable octet.\nLithium then has just two. Remember, this is the first orbital (s orbital) with a maximum of two electrons.
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In Ionic bond, elements looses or gains electron(s) and become ions and the electrostatic potential of these ions bind them\n\nIn covalent, the participating elements are bound by sharing electrons between them.
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complex ions - which then form ionic molecules
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http://www.chem1.com/CQ/ionbunk.html\n\nskim this article.
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You need to split the ionic compounds apart to find the individual ions you would find in these structures.\n\nMgO would produce Mg^2+ & O^2- ions.\n\nK2S would produce K^+ & S^2- ions.\n\nYou can find the charge values directly from the periodic table trends for the charges atoms assume when they are ionized.
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The main thing you need to know to figure out the ionic equation is whether the product is soluble or not.  In this case, PbSO4 and Mg(NO3)2 are your products, and lead salts are insoluble.  Thus, PbSO4 and any ion that is used to make this molecule is removed from the ionic equation:\n\nPb(+2) + 2(NO3)(-1) + Mg(+2) + (SO4)(-2) -> PbSO4 + Mg(NO3)2 (aq)\n\nbecomes:\n\n2(NO3)(-1) + Mg(+2) -> Mg(NO3)2 (aq)
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I'll make it easy for you.All the metals forms positive ions by losing electrons and all non-metals form negative ions by gaining electrons.\nExample:- NaCl  Na+ & Cl-
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In covalent bonds, elements actually lose and gain electrons to other elements in the compound.  Polar bonds are covalent bonds that don't require hybridization, and Non-Polar bonds do require hybridization.  Ionic bonds occur when elements share an electron but do not lose it.  Therefore, you can tell that NaCl is ionic because Sodium has an extra electron and Chlorine needs one, so Sodium shares it's electron with Chlorine, forming a very strong bond.  Ionic bonds, however are broken by Polar-Bonded liquids such as water, which is why NaCl dissolves.
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Well, obviously the donation of electrons from + to - atoms. Also, ionic compounds are soluble in water. Since ionic interactions are weak, they are weakly bound together.
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positive ions (a positively charged element in this case since you specified 'atoms')  To be compounds, different types of atoms must combine.
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Ionic bonds are comprised of a metal and a non-metal.\nCovalent bonds are comprised of two bonded non-metals.
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Basically, It is because water is polar. The positive Hydrogen atoms and the Negative Oxygen atoms pull apart the ionic compounds. This is because ionic compounds are made of a anion and cation, which are both charged. Then, just like a magnet, they are pulled apart, and not allowed back together.
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You need to know more than just the electron configuration.  There is contraction from left to right on the periodic table, plus additional periodic trends that must be considered.   \n\nEven more importantly, you need to define whether you are looking for the largest element IN ITS NATURAL  STATE (i.e. Cl2, Hg metal, etc) or AS THE ION.   Atomic and ionic radii differ.\n\nMore clarity is needed here.