What does polar, nonpolar, covalent, nonpolar covalent, polar covalent mean?
952034
polar refers to bonds and molecules where the electrons tend to be closer to one atom than another because of the "strength" with which the atoms "pull" the electrons.  This "strength" is usually measured by a number called "electronegativity".  There should be a chart or list of these numbers in your text book.\n\n"Covalent" is a type of chemical bond where the electrons are shared between atoms, rather than transferred (ionic bond).  Usually covalent bonds form between two non-metals.\n\nFrom your question it looks like the first two terms (polar and nonpolar) are referring to individual chemical bonds.  Find the two atoms attached to either end of the bond, look up their electronegativities and see if one atom "pulls" on the electrons stronger than the other.  This would produce a polar BOND.\n\nThe last two (nonpolar covalent; polar covalent) could refer to both a bond or a molecule.  For the molecule you need polar bonds,  and then you have to know the shape of the molecule since it is possible for the individual bond "pulls" to cancel each other - kind of like a tug of war.  Generally if a molecule is symmetrical (triangle, tetrahedron or linear triatomic) the "pulls" cancel.  Although the BONDS may be polar covalent, the entire MOLECULE would be nonpolar covalent.
451415
i think it is a polar covalent bond\nI used to remember why but I'm not in Chemistry anymore...\nHeres a website.. Look at Example #3\nhttp://users.rcn.com/jkimball.ma.ultranet/BiologyPages/E/Electronegativity.html#covalent_bond\nAnd another http://academic.brooklyn.cuny.edu/biology/bio4fv/page/polar_c.htm\nhope its not too late
716083
Its covalent.  When two atoms(or more) share one or more electrons, covalent bonds are formed.
1008726
Strong Love!\n\nIn other words, it's a covalent bond because sharing of electrons takes place in these elements when they combine with each other.
665955
it must be polar because the structure is tetrahedral with a lone pair at one corner of the tetrahedron and Cl atoms at the  rest three corners. so the individual As-Cl bond moments are not cancelled bcoz of the asymmetry of the molecule and the net polarity cant be zero.
273886
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.\n\nOther types of bonds include metallic bonds and hydrogen bonding. The attractive forces between molecules in a liquid can be characterized as van der Waals bonds.
12669
A covalent bond\nThe other is an Ionic Bond which is when one atom gives an electron to another atom.
1094405
A covalent bond is a bond in which the atoms making up the resulting molecule "share" the electrons in the form of covalent bonds.\nAn ionic bond is an extremely one sided "sharing" of electrons, so one sided, one atom is said to have completely stripped of an electron from another atom.\n\nWhat determines if the bond is covalent or ionic is the difference in the electronegativities of the two atoms bonding.  If the electronegativity difference is high enough, the bond is said to be ionic.  If the difference in electronagativities is significant, but not quite to the level of a full ionic bond, the bond is said to be polar (which may or may not mean that the resulting molecule is polar, this depends on several things).\n\nLooking at a chart of [Pauling] electronegativities,\nhttp://www.psigate.ac.uk/newsite/reference/plambeck/chem1/p01244a.htm\none can see that most elements are somewhere in the 1 to 2 range, with only a few elements getting much lower or higher than this value.  Unless the difference is high enough (usually a difference of about 1.5 is considered ionic), then the bond will just be polar, or less so.\n\nSo, all elements have the potential to theoretically bond ionically, but only in certain combinations with other elements.\nFor example, you will never see an ionic bond between Carbon and Hydrogen since the difference is just .4, but an ionic bond between Lithium and Fluorine is easy to make with a huge difference of 3.0.
789668
sugars are covalent \n\nif you are specifically talking about table sugar, or sucrose, you can find out all about it here\nhttp://en.wikipedia.org/wiki/Sucrose
953238
It is true for individual bonds, but not for molecules.\nThe dipole moment of the molecule will depend on the geometry of the polar covalent bonds. E.g. CF4 has 4 polar bonds but they arranged so that the sum of their dipole moments is zero and the molecule has actually no dipole moment.
872077
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.
675505
a molecule that carries a charge. Water is a very common polar molecule.  It sticks together when it streams because of the polar bonds between the molecules.  "Polarity results from the uneven partial charge distribution between the atoms in a compound."
799974
Covalent bond: are those which one or more pairs of electrons are shared by two atoms.\nCovalent chemical bonds involve the sharing of a pair of valence electrons by two atoms, in contrast to the transfer of electrons in ionic bonds. These bonds lead to stable molecules if they share electrons in such a way as to create a noble gas configuration for each atom. \n\nHydrogen gas forms the simplest covalent bond in the diatomic hydrogen molecule. The halogens such as chlorine also exist as diatomic gases by forming covalent bonds. The nitrogen and oxygen which makes up the bulk of the atmosphere also exhibits covalent bonding in forming diatomic molecules. \n\n\n\nIonic Bonds\nIn chemical bonds, atoms can either transfer or share their valence electrons. In the extreme case where one or more atoms lose electrons and other atoms gain them in order to produce a noble gas electron configuration, the bond is called an ionic bond. \n\nTypical of ionic bonds are those in the alkali halides such as sodium chloride, NaCl\n\n\nThe below reference has some diagrams which are helpful as well.
889275
Covalent bonding is a description 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 become filled. In contrast to electrostatic interactions labeled as "ionic bonds," the strength of covalent bond depends on the angular relation between atoms in polyatomic atoms. Covalent bonding is most important between atoms with similar electronegativities. Covalent bonding is often delocalized.
745688
To the first answer----WHAT? What does hydrogen bonds have to do with polarity? Ever heard of dipoles? Why do the need hydrogen bonds when the electronegativity is what is causing the polarity? Please, don't answer question you have no idea about. Anyone can look up stuff and copy and paste. NaCl  doesn't form hydrogen bonds but is VERY solube.\n\nNow, to answer the question. I think what you are eluding to by using "most," is the majority of them. What it boils down to is the molecule is too big. If you have like CH3-Cl, it is a small molecule and the polarity is spread of a small place, thus making it polar. Now, if you have something like C-C-C-C-C-C-C-C-C-C-Cl, the only part that is polar is the Cl part and the rest of the molecule is not, thus will not interact in water.
226109
It is lithium Chloride i.e. LiCl\nIt is an covalent compound rather than being an ionic compound. It is define by FAJAN's rule
863219
Electronegativity is a measure of the ability of an atom or molecule to attract electrons in the context of a chemical bond. The type of bond formed is largely determined by the difference in electronegativity between the atoms involved. Atoms with similar electronegativities will share an electron with each other and form a covalent bond. However, if the difference is too great, the electron will be permanently transferred to one atom and an ionic bond will form. Furthermore, in a covalent bond if one atom pulls slightly harder than the other a polar covalent bond will form.\n\nThe Pauling scale was devised in 1932 by Linus Pauling. On this scale, the most electronegative chemical element (fluorine) is given an electronegativity value of 3.98 (textbooks often state this value to be 4.0); the least electronegative element (francium) has a value of 0.7, and the remaining elements have values in between. On the Pauling scale, hydrogen is arbitrarily assigned a value of 2.1 or 2.2.\n\n'ΔEN' is the difference in electronegativity between two atoms or elements. Bonds between atoms with a large electronegativity difference (greater than or equal to 1.7) are usually considered to be ionic, while values between 1.7 and 0.4 are considered polar covalent. Values below 0.4 are considered non-polar covalent bonds, and electronegativity differences of 0 indicate a completely non-polar covalent bond.\n\nHope I helped!...\n