Although CO2 molecule has polar covalent bonds, it is a non-polar compound. Why?
540597
dont cheat ur a bad person
316023
intermolecular polarity and the fact that fluids dont compress the way gases do?
744495
Carbon Tetrachloride is a non-polar molecule, thus it is capable of dissolving similar non-polar molecules.
554160
A molecule is polar when it has a dipole moment that does not cancel out. For example, consider the molecule CH4 (methane) which is nonpolar. It has a carbon atom bonded to 4 hydrogen atoms. Bonding is the overlap of the electron density. So you have an electron from a hydrogen and an electron from the carbon forming each of the bonds. Carbon is just very slightly more electronegative (tendency of pulling electrons closer to itself) than hydrogen. This means that the electrons are pulled by carbon away from hydrogen, but not by much (the difference is very very small). This shifting of electron density allows for the carbon to be slightly more negatively charged and hydrogen slightly electron deficient. This makes the C-H bond just slightly polar. However, because there are 4 hydrogen atoms that are bonded to the carbon, this bond polarity cancels each other out...meaning that the bonds are slightly polar, but the overall molecule is nonpolar. \n\nTo determine if the bonds are polar you just have to know the electronegativity differences. To know if a molecule is polar, you must know the correct geometry. Since electrons are negatively charged and repel each other, they want to be as far away from each other as possible. If you have a carbon bonded to 4 hydrogens, you will have a tetrahedral geometry with the hydrogens 109.5 degrees apart from each other creating the best possible arrangement. Also, if you have a lone pair of electrons, then the molecule will always be polar because of that charge separation.
825775
With respect to covalent bonds, polarity refers to the tendency of electrons to move towards one of the atoms.  Polarity in covalent bonds arises from differences in electronegativity between the participating elements.  For example, the covalent bond in a molecule of water, H2O, is polar.  Oxygen is more electronegative than hydrogen, so the end of the molecule containing the oxygen atom has a partial negative charge.
47652
Because of its valence shell carbon atoms always have 4 bonds. In addition to this carbon atoms are unique in thier ability to form strong covalent bonds to each other while at the same time bonding atoms of other nonmetals strongly.
20674
The simple answer is probably: covalent bond\n\nI quote: "Covalent bonding is an intramolecular form of chemical bonding characterized by the sharing of one or more pairs of electrons between two species, producing a mutual attraction that holds the resultant molecule together. Atoms tend to share electrons in such a way that their outer electron shells are filled. Such bonds are always stronger than the intermolecular hydrogen bond and similar in strength to or stronger than the ionic bond."
1027607
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   +
980851
C, having both positive and negative charges on one molecule.
701742
I do not have a reference, but can tell you that Ethanote (Acetate) ion has the negative charge delocalised over 2 oxygen atoms.  This means that the bond energy is between that of a carbon-oxygen single bond and that of a carbon-oxygen double bond.\n\nThe bond energy for the carbon-oxygen (double) bond in CO2 is 799 kJ/mol while a single bond C-O is about 358 kJ/mol, so the answer is between these.  It is probably in the ball park of 580 kJ/mol.\n\nThe true or more accurate answer is a very complexed Physical Chemistry calculation.
702197
1) Coordinate covalent bond is a covalent bond that both electrons are donated by the same atom. In the case of CO, C has 4 valence electrons and needs another 4 to reach 8. For O, it has 6 valence electrons and needs another 2. In order to make both atom happy (which both have to have 8 electrons), the only way is to have the following structure\n\n. .\nO\n:::\nC\n. .\n\nIn this case, both C and O has one lone pair. In between them, there are three bond pairs, however, one of this bond pair is made up using both electrons from O. You can easily count the number of electrons for C and O to see this.\n\n\n2) Water molecules can form hydrogen bond because every H atom can have a small attraction towards the O atom from another water molecule and vice versa. This H-bond in water increases the attraction between adjacent water molecules, and make it harder to break them, thus, leads to a higher water tension (think of it all the water molecules are sort of connecting between each other, and is not easy to break it). \n\nWhen water turns to ice, this H-bond force the water molecule to freeze at a position that every water molecule are connected to the adjacent molecule through H-bonding structure. If you draw out this V-shape water molecule and start connecting them with the another water molecule, you can see how the water molecules are bonded when they are in ice form. This structure is not a very good way to pack molecules, and leads to lots of open space in between molecules. As a result, for the same amount of water, when it turns to ice, it takes up more space. As a result, leads to a lower density, so ice floats on water.
327842
I am pretty sure that it is due to polarity.  Since sulfur forms nonpolar S8 molecules, they are nonpolar, where water has a + end and a -end, making it polar (has a dipole moment).  The general rule is like dissolves like.  Molecules that a alike can interact on  the molecular level and form solutions, unlike molecules can not.
122909
A polar charge occurs when there is a difference in charge between the different parts of a molecule.  In the water molecule, H2O has a positive charge at the two Hs and a negative charge at the O because the shape is "bent".  These charges are called dipoles.  In a strait molecule, the + and - charges cancel each other out (called a nonpolar molecule).  Polar and Nonpolar molecules cannot mix because they are virtually insoluble in each other.
983019
Carbon monoxide has a triple bond between the two elements, and has a LINEAR electron geometry.  Although, there IS a fairly large electronegativity difference between the carbon and oxygen, lone-pair distribution makes up for it.  Therefore, a carbon monoxide molecule is still a little polar.  It does have a small dipole moment.
942952
Water itself is a polar molecule, with a partial negative charge on the oxygen atom and a partial positive on the hydrogens. It allows water to hydrogen bond with other molecules.
136157
Mostly because of its sp3 hybridization - that is, the fact that 4 atoms or molecules can bond with great stability to the carbon atom. For example, methane (CH4) is the simplest of the carbon compounds. But now, replace any of those H's with almost any other kind of molecule and you get the meat & potatoes of what organic chemistry is all about.
633870
this is because water is made up of hydrogen and oxygen. oxygen is significantly more electronegative than hydrogen (basically it is better at attracting electrons) and this means that in water oxygen has a small - charge (because electrons are negative) and hydrogen has a slight + charge. now we know why the bonds are polar the reason that the molecule is polar is because water is a bent molecule and therefore the bond polarities do not cancel each other out leading to a polar molecule.