Which of these nonelectrolytes are covelently bonded and why?
960296
only Sodium Chloride is not.\n\nsimple answer:\ncovalent bonds are between non-metals\nionic bonds are between a metal and a non-metal\n\nthis is because of the large difference in electronegativity between metals and non-metals.\n\nonly sodium chloride has a metal.  the rest are all made only of non-metals and thus covalently bonded.
840267
The word molecule tells you that it is a covalent compound (if it were ionic, it would be called a unit cell). Covalent compounds are USUALLY between nonmetals but in some cases can be between a metal and a non-metal. It all boils down to electronegativity difference (how much harder one atom is pulling on the electrons in question than the other atom). I hope this helps!
426762
you know its ionic because Na is a metal while Cl isnt. a metal and nonmetal almost always from an ionic bond. to draw a lewis digram, determine how many valence electons are in each and draw the diagram.. its kinda hard to explain without actually drawing it.. consult a chem bk.
950410
Mainly H-bonding (intermolecular forces)
7695
The monomers are linked by covalent chemical bonds.
194668
Cl2 has a single bond.\n\nO2 has a double bond.\n\nN2 has a triple bond.\n\nAs the number of bonds increas, the attraction increases and so the bond length decreases.\n\nAs much the bondlength decreases bond energy increases.
817547
yes, they always covalently bond with each other under any normal type conditions\n\neven if you were to conveniently have an oxygen cation and anion that you combined, they would lose their ionic nature and bind in a covalent fashion
706732
Maleable and formatable\nand\ngood insulators. They both are properties of metals, which are bonded.\n\nStiff,viscous, and brittle are descriptions of an ionic bond like, for example NaCl, salt.
1160360
by molecular bonds.  covalent and ionic.
1101405
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.
548540
Ionic bonds are comprised of a metal and a non-metal.\nCovalent bonds are comprised of two bonded non-metals.
260316
An ionic compound.\nA covalent compound.
549677
This is a chemistry question, the anomaly is due to Hydrogen bonding.
376102
The Halogens are very, very reactive chemicals, and tend to hook up and form salts with the other elements rather than hanging around in a pure elemental form.  They tend to pick up extra charge very well which makes them prime candidates for bonding.
226731
sand could be considered covalently bonded material.  which in very simple terms...when added to water it will not dissolve. Salt on the other hand is ionic allowing it dissolve in water.  Sand is often made of a silicon crystal lattice, where a common table salt is sodium chloride.
715766
It is not a reaction because the bond formed is ionic, not covalent.  Extraction is a better term for the process you are describing.
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.