How are ionic compounds formed?
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In chemistry, an ionic compound is a chemical compound in which ions are held together in a lattice structure by ionic bonds. The positively charged ion is usually a metal ion and the negatively charged ion is non-metallic element or molecule.\n\nIons can be single atoms, as in common table salt sodium chloride, or more complex groups such as calcium carbonate. But to be considered ions, they must carry a positive or negative charge.\n\nThus, in an ionic bond, one 'bonder' must have a positive charge and the other a negative one. By sticking to each other, they resolve, or partially resolve, their separate charge imbalances. Positive to positive and negative to negative ionic bonds do not occur. (For a real world analogy, experiment with a pair of bar magnets.)
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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
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Since the reaction is between two ionic compounds, it will be double replacement.  In that case, the positive ion of one compound switches places with the positive ion from the other.  The two products will then be sodium chloride (NaCl) and Calcium Carbonate (CaCO3).  Sodium Chloride is soluble, as are all ionic compounds with group 1 ions present, however, carbonate compounds are almost never soluble in water.  The only water-soluble carbonate compoounds that I can think of are ammonium carbonate and group 1 carbonate compounds.
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1)  At the centre, you have the nucleus (positively charged) and, around that, there are the electronic orbitals (negatively charged).\n2)  By losing one or more electrons, to produce a cation (positively charged), e.g. Na+, Ca++, Al+++\nOr by gaining one or more electrons, to produce an anion (negatively charged), e.g. Cl-, O--, N---\n3)  An ion.
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It depends of the type of substance. When an ionic substance, such as NaCl (table salt), melts the bonds between Na and Cl in the lattice break. These are strong bonds so Na Cl melts at a very high temperature. When it melts, you are left with free Na and free Cl. \n\nWhen a molecular substance melts, such as solid water, things are different.  In water there are only very weak bonds holding each water molecule together,(ie. one water with its neighbour) thus requires a little bit of heat to break.  When it melts, the water molecule has not broke up just the bond to it neighbour (within each water there is strong bonds holding the H to the O and these do not break when melted), therefore in the liquid form there is still H2O around.
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Ionic precipitation is when two ions say Ba+2 and a S-2 get together and precipitate into BaS2 (ppt) which in insoluble. Which is different if two organic molecules react to form an insoluble substance.
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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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Ionic bonds are comprised of a metal and a non-metal.\nCovalent bonds are comprised of two bonded non-metals.
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Positive ions (Cation) are formed by a neutral atom losing electron(s), and Negative ions (Anion) are formed by atom gaining electron(s).  \n\nThe exact number of electrons an atom gains or loses are predictable.  Atoms gain or lose electrons so that they turn isoelectric with the closest neighboring Noble Gas.
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Technically, there are no ions on the periodic table, only elements.\n\nWhen an atom becomes an ion, it either looses to gains an eletron to develop a charge.  When this happens, the atom no longer behaves the way it normally would, it now has a charge and is attracted to other atoms with opposite charges.\nTo distinguish between normal atoms and atoms with charges, we change their names slightly (but I wouldnt call it "wierd").  For example, when a Chlorine atom gains an extra electron to fill its octet, we call it the Chloride ion.  However, we do not change the names of the cations (+), we just add the number of the charge to the end of the same.  For example, then Iron metal looses 3 electrons to develop a +3 charge, we call it Iron (III) or Fe+3.\n\nThere are also such things as polyatomic ions, or groups of covalently bondded atoms that have an over all charge on them.  For example, the Ammonium ion is made up of a Nitrogen atom and 4 Hydrogen atoms with an overall charge of +1 (NH4+1).  These polyatomic ions can have some odd names, but they too still follow a partern.\n\nTake the many forms of this type of ion,\nClO-, HYPOchlorITE\nClO2-, chlorITE\nClO3-, chlorATE\nClO4-, PERchlorATE\nThs capitilized letters are the pattern it follows.
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I'm sorry...my answer to this question, will either sound really smart or really stupid. \n\nMy AP Chemistry class just finished the chapter on bonding. We learned of Ionic bonds, Covalent Bonds, and Hydrogen bonds. \n\nAn ionic bond is a bond between a metal and non-metal and involves the transferring of electrons so that both atoms will become stable but with opposite charges, become attracted to each other, and form a molecule. An example is NaCl or table salt. Na is a metal, Cl is a non-metal.\n\nThe next is covalent bonding between two non-metals or non-metal and metal and involves sharing electrons. An example is O2 - oxygen.\n\nFinally hydrogen bonding is self-explanatory consisting of hydrogen and another element.\n\nBecause of the above, it is chemically impossible for two metals to bond as they will not have enough electrons to stabilize each other in the first place. \n\nI even performed this experiment in class. When a metal is heated it "oxidizes". Its atoms fuse with the oxygen atoms in the air and form the gas. For this reason a metal starts turning brown, as you are simply speeding up the process of rusting.\n\nSo your question is kind of impossible from what I have learned in class. \n\nI'm sorry if I am completely of the point in this answer (if there is something I am not getting and that two metals can actually bond) and I apologize for my ignorance and stupidity in advance. haha
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Ionic bonds are created by attraction of separated charges or differences in electronegativity.  This results in a dipole moment, which is a vector property, hence it is directional.
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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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It's a bond where electrons are shared between elements.  As opposed to ionic bonds where the charges make the bond.
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if it forms a 2- ion it is from the Chalcogen (group V1(A) or 16) family (Oxygen, Sulphur, ...).  The two bonds between two Oxygen atoms are Covalent.  It has 6 valence electrons and takes two to complete the valence shell (noble configuration).\n\nThe reaction of X with Sodium (Na) will require twice as many Na atoms as Sodium only has 1 valent electron to give (to make the Na+ ion)\n\nSo\n\n2Na + X -> Na2X which in a polar solvent (e.g. water) will become 2Na+ +X2- \n\nFYI, the Halogens are Fluorine, Chlorine etc and only have one single space left to take an electron to reach Noble configuration hence they form singly charged anions F-, Cl-...
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If the ionic compound is soluble, no precipitate is formed.\n\nOn the other-hand, if an ionic compound is not very soluble in the solvent, then it will precipitate out of solution.\n\nFor example, Sodium chloride is soluble and Silver nitrate is soluble, but if these solutions are mixed, some of the Silver ions will react with chloride ions and form solid Silver chloride precipitate.
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when an atom loses an electon from its outermost shell then it forms an electropositive ion while when an atom gains an electron it forms an electronegative elctron.\n\nfor e.g. during the formation of nacl na atom loses an elcron to the cl atom to form a +ve ionwhile the cl atom which gains that electon forms a -ve ion.