covalent bonds in water
119684
It would largely depend on the polarity of the bond.\n\nEver hear of the "like dissolves like" rule?\nWater, being a polar molecule, will dissolve other polar molecules as well as ionic compounds.  If the colvalently bonded molecule you are trying to dissolve is polar, you have a good chance at dissolving it in water (actual solubility values will varry).  However, if the molecule is non-polar, the molecule is not going to be soluble.\n\nExample,\nWater will easily dissolve "Salt" (NaCl) since it is an ioic compound.\nWater will dissolve alcohol since alcohol has an OH group, making it polar.\nWater will not dissolve gassoline for example since it is a non-polar hydrocarbon (that is why you cant mix oil and water).
438177
Water has (relatively) high cohesion, due to the polar covalent bonding of the water molecule. Soap destroys this covalency by adhering to water molecules with its ionic end. This is why soap is used as a cleanser. Soap itself doesn't clean, it disperses water molecules, thus increasing water's absorption properties. Without water's cohesive ability, items that float on the surface of water now sink.
383608
the shape of the molecule of the water is non linear because of the two lone pairs in C atom, therefore the shape of the molecule is non-symmterical. In a non symmetrical molecule, bond dipoles do not cancel out (although bond is polar) so overall, it's polar...\n\nin the case of water, the shape of its molecule is linear with double bonds. There are no lone pairs that will repel the other element, therefore the shape of the molecule is symmetrical. Dipole bond cancel out in the symmetrical molecule so the it does not become polar overall.\n\nsorry i don't know the answer to your second query...
508336
I would say CH2O2 (I'm assuming you mean formic acid, not dioxirane), CH3CO2H, and water.  \n\n"Important" is a tough word here, as all of these compounds can participate in h-bonding to varying degreees, with water being the strongest and CH2F2 being the weakest.  That said, strong hydrogen bonding gives rise to many of the nifty properties of water and in all three cases the h-bonding is powerful enough to raise the boiling points to be significantly higher than what you would expect based on molecular weight.
650484
Able to be dissolved by water.
322809
methane wouldnt really dissolve in water.  KCl would ionize in water to become K+ and Cl-.  Helium wouldn't dissolve in water.  MgSO4 would also ionize in water.  Sucrose would dissolve in water to a significant extent, because of hydrogen bonding.  Sucrose has lost of hydroxyl groups in its structure and allow it to hydrogen bond in water, therefore dissolving.  Sodium bicarb would also just ionize.
394714
Halogens, in their elemental state, are covalent. In their elemental state, they are not compounds, because they are not combined with other elements. But F2, Cl2, Br2, I2, and At2 are covalently bonded.
297399
http://www.chemguide.co.uk/atoms/bonding/vdw.html
329064
Most liquids dilate when heated and therfore the density increases with temperature. Water is an exception below 4 degrees Celsius. The reason are hydrogen bonds.\n\nIn the H20 molecule the hydrogen atoms share their electrons with the oxygen atom in socalled covalent bonds. But the oxygen atom attracts the electrons very strongly and takes more than its share.\n\nAs a consequence the hydrogen atoms form bonds with the oxygen atoms of other water molecules. These hydrogen bonds are weaker than the covalent bonds.\n\nThe result of the existence of hydrogen bonds is that ice is organised in a hexagonal structure which is less dense than water. These structures form already in liquid water too, but to a lesser degree.\n\nThe end result is a tug-of-war between the effect of the hydrogen bonds and the normal dilation of water. With a maximum density at 4 degree C as a consequence.
458466
Firstly, I would like to indicate that the bonds that chlorine forms with hydrogen are not hydrogen bonds at all. Hydrogen bonds are only present in compounds of hydrogen with the three most electronegative elements, i.e, fluorine, oxygen and nitrogen. Hence, hydrogen bonds may be found in water and ammonia, but not in hydrochloric acid.\n\nAlso you need to remember that the hydrogen bonds are intermolecular forces or attraction, that is the attraction between the hydrogen of one molecule of - taking the example of water - to the oxygen of another molecule of water. The bond within the molecule H - O - H is predominantly covalent, as it is formed by the sharing of electrons. The molecule might have an ionic tendency, how much depends on the electronegativity difference between the two elements sharing the electron.\n\nHence the bonds between the hydrogen and chlorine atoms sharing the electrons are predominantly covalent, with a slightly ionic tendency. Henceforth, water is very much an important factor in ionising an acid, and increase the hydrogen ion concentration in an acid.\n\nI hope this would be of good help to you.
276342
ice has less density than water.  the H2O bonds in ice are in a crystal lattice structure and there are small bits of air trapped between them.
162198
Sounds like you've got too much time on your hands to me!  The ions in solution keep the water molecules farther apart from eachother on average than they would be in pure water.  Therefore the hydrogen bonds are weaker and the water will boil at a lower energy level.  At least that's what I'd guess.
215108
POLAR bonds and hydrogen bonds are found in Water.\n\n"As a stable, polar molecule prevalent in the atmosphere" (Wikipedia).
85868
polar...water molecules "stick" to each other so to speak...
585713
Of course ice and water are chemically identical consisting of H2O.  The two hydrogen atoms attach to the oxygen atom other than in a straight line (not like beads on a string).  The electron field surrounding the water molecule is uneven providing it with a "polarity" that makes it much easier to pack many molecules together in a given (rather than arbitrary) arrangement.  When water is a vapor (or steam) there is so much vibrational energy that the molecules bounce off each other maintaining a "pressure" depending on their energy (temperature).  When the molecules are a liquid, they are very closely packed and are nearly incompressible (even seven miles below the surface of the ocean!).  The bulk water expands and contracts only a little with temperature changes.  When heat is removed from the water (in a freezer?) the molecules are attracted to each other in a preferred array due to polarity and form long chains of molecules that use up space far less efficiently.  The "ice" is less dense and floats on water because the space between chains is filled with a vacuum or gases that weigh very little.  When the water is allowed to freeze in open space (a cloud?) the polarity is free to align water molecules in the most preferred orientation; a six sided snow flake.  When hoar frost forms on a cold window pane the ice forms in dendrites, like growing Christmas trees.  Hope that helps a little.
58409
There are 3 types of bond in sugars :\n\n1) -C-H (Covalent)\n2) -C-0H (Partially ionic)\n3) -C-O-C- (Covalent)\nand vander-waals force of attraction.
611919
"what element(s) and what bond(s) make water a universal solvent?"