What are the differences between an ionic bond and a covalent bond?
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Ionic bonds are a type of chemical bond based on electrostatic forces between two oppositely-charged ions.\n\nCovalent bonding is a description form of chemical bonding that is characterized by the sharing of one or more electrons between two atoms. In general bonds are defined by a mutual attraction that holds the resultant molecule together. Often bonding occurs in such a way that the the outer electron shells of the participating atoms becomes filled. Such bonds are always stronger than the intermolecular hydrogen bond and similar in strength to or stronger than the ionic bond......;
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Covalent bond: bond in which one or more pairs of electrons are shared by two atoms.\n\nIonic bond: bond in which one or more electrons from one atom are removed and attached to another atom, resulting in positive and negative ions which attract each other.
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Determining structure of molecules.\nIonic structures- The Alkali metal halides are ionic compounds e.g NaCl. Na has a positive charge whereas Cl has a negative charge.\n\nMolecular solids- are held by weak bonds called Van Der waals forces. \n\nMacromolecular structures or giant molecular- have covalent bonds between atoms, these bind all the atoms into a giant molecule e.g Diamond
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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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covalent bonds are called the directional bonds.because the orbitals involved in bonding have specific direction where they bond.
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A coordination bond is a bond where one molecule gives both electrons to form a covalent bond. It differs from an ionic bond because the electrons are "shared" not given (e.g. the bond consists of a wavefunction, instead of discrete cations and anions)
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Ionic bonds have really different electronegativity to the point where one atom really takes the electron and the other atom readily gives the electron.  Therefore, 2 ions (or more) are formed with opposing charges.  Since they are opposing, what happens is that they will be really stuck together at a fixed position.  Therefore, no sliding will occur.  The material will be brittle.  Fine examples are salts and rust.  If and when dissolved in a solvent, the ions seperate and yet maintain their charge.  Ions can come from a group of atoms (molecule) like CN or a single atom H.  But the results are not atoms, but ions such as CN- and Na+ (NaCN), which individually C and N of the CN- are not the ions, but the CN- is considered the ion.  Other examples of this is CO3 2- and Ca 2+ which together is CaCO3, a salt; again, the Carbon and the three Oxygen atoms are not the ions, but the group itself is considered an ion.\n\nCovalent bonding occurs between two atoms that are willing to share the electrons.  Sometimes, due to difference in electronegativity, there are unequal sharing but nonetheless sharing; note the difference cannot be to high or you'll get an ion.  Atoms are can be easier to slide like in a metal or be really difficult to move (like in silicate oxides and diamond).  It all depends.  Since there's a sharing of electrons, it is possible to have a dipole-dipole moment where electrons could concentrate themselves at one end or the other of the molecule; that is why I2 exists as a liquid, because of the looser valence electrons, there is a tenadancy for the electron density to shift from one to the other atom causing a propagative effect to other neighboring I2 molecules, which is the reason why it's the only diatomic molecule to be a liquid from all halides.  CN- has a covalent bond (triple bond).  CO3 2- also have covalent bonds.\n\nLooking at the periodic table, the electronegativity of a an element increases from the bottom to the top row and from the left to the right column (w/ exception of noble gases).  That means that the halides are extremely electronegative, which means they love electrons.  But, as you go down the list of halides, they love electrons less and less due to electron shielding - there are other electrons that are closer to the nucleus lessening the effective nuclear charge that is reaching the valence electrons.  Therefore, those electrons can be stripped from those heavier halides (like Iodine) as opposed to the halides that have less orbitals filled (like Fluorine).
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ok listen if u have a compound formed by 2 atoms u take the electronegativity of the second atom and u substract the electronegativity of the first one if the number that u get is between 0 and 0.3 its non polar covalent if its 0.4-1.7 then its polar covalent and if its 1.7 or more than it is ionic
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a.)ionic b.)covalent c.)covalent d.)metallic
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Ionic compounds are basically defined as compounds where two or more ions are held next to each other by electrical attraction. One of the ions has a positive charge (called a "cation") and the other has a negative charge ("anion"). Cations are usually metal atoms, and anions are either nonmetals or polyatomic ions (ions with more than one atom).\n\nA molecular compound is made up of all non-metals. The bond that forms between the atoms is by the sharing of electrons, unlike ionic compounds, which are made by the transfer of electrons.\n\nIn the case of NaH, this is a ionic compount and this is a strong base. \n\nAcid is defined as a compound which donates a hydrogen ion (H+) to another compound (called a base). You can also see it this way: An acid is a proton donor and a base is a proton acceptor. The acid is said to be dissociated after the proton is donated.\n\nAbout naming of compounds, read the book. It's a long discussion.
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Ionic bond, hydrogen bonds, covalent bond, ionic interactions, van der waals interaction, non-polar interaction ... the list goes on.\n\nA bit more on covalent bonds:\nThere are sigma and pi covalent bonds, mainly. Pi bonds are usually the double bonds, while sigma are single bonds. Pi bonds can have resonance!\n.\nAlso there are often non-bonding electrons and anti-bonding electrons in molecules, but they aren't really "bonds"\n.\nCheers.\n.\nP.S.: If you share "chemistry" with a girl / boy you could also call that a "chemical bond"! He he he he.
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-molecular:it is a double replacement reaction.  i.e.:ab+cd=ad+bc.  \n-net ionic: you find the one that becomes the solid, and you remove all the other spectator ions.\n\nno way, i have to do the same exact thing for homework tonight.  writing net ionic, gross ionic, and molecular formulas. damn.  are you doing molarity too?  are you a sophomore?  damn science.  i hate science.
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A covalent bond\nThe other is an Ionic Bond which is when one atom gives an electron to another atom.
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Covalent bonds are where two (or more) atoms "share" outer layer electrons in order to achieve stability. Polar molecules are where the electronegativity of the atoms do not cancel each other out, and hence the molecule forms a charge.\n\nA carbon and a hydrogen forms a covalent bond. The carbon has 12 protons while the hydrogen has only one. Hence, the carbon will draw the shared electron from hydrogen towards itself more than that of the hydrogen drawing the electron shared by the carbon, and hence the carbon becames negatively charged because the electron from hydrogen spends more of its time around carbon while the hydrogen, left with its single proton, becomes positively charged.\n\nAn example of a polar covalent bond is water. \n- O---H +\n    /\n    H\n   +
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Something called ionic bonding occurs, when one covalent electron in sodium is given to the atom in the chlorine atom. The two ions are now bonded, hence the name ionic bonding.
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I2 is has a covalent molecular bond, that forms into the solid crystal.  So, that would be molecular. (Molecules make up the crystal structure).\n\nNi(s) is a crystal made up of atoms, so that's atomic.\n\nNone are ionic, b/c all the atoms in the crystal are the same, so they share electrons, they don't transfer them.
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If the difference in the electronegativity between the two elements is less than 1.67, the bond will be covalent.\n\nNote: As to the statement that electronegative atoms don't form covalent bonds, that's nonsense.  ALL atoms are electronegative to some extent.  Just go look up the electronegativity series in any general chem. text.  Or check out this:\nhttp://dbhs.wvusd.k12.ca.us/webdocs/Bonding/Electroneg-Bond-Polarity.html