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Is acetone attracted to glass?

Acetone and water are polar molecules; water is more polar I think because it has hydrogen bonds and acetone has no hydrogen bonds. Water is attracted to glass, but is acetone attracted to glass?

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  • 3 months ago

    Both water and acetone (CH3COCH3) form upwardly concave meniscuses.  Water does exhibit hydrogen bonding as well as Keesom forces (dipole-dipole attraction), but acetone has no hydrogen bonds with itself (although it does form hydrogen bonds with water), and acetone is much more polar than water, therefore, acetone has stronger Keesom forces.  The net dipole moment of water is 1.85D and for acetone the net dipole moment is 2.91D.

    The facts that acetone can form hydrogen bonds with water and that it is more polar than water agree with the observation that acetone is highly miscible with water.

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Once a soluble ionic salt has dissolved, polar solvent water acts to ____ the free ions and keep them apart in?

precipitate

solvate

spectator ions

dissociate

net ionic equation

Once a soluble ionic salt has dissolved, polar solvent water acts to ____ the free ions and keep them apart in?

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  • Anonymous
    7 years ago
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    Dissociate

    Source(s): BSci in Chemistry
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  • bade
    Lv 4
    3 years ago

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Chemistry help? nonpolar and polar covalent bonds?

Discuss two ways that atoms share electrons using the terms nonpolar covalent bonds and polar covalent bonds.

Chemistry help? nonpolar and polar covalent bonds?

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  • 1 decade ago
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    I think what you're looking for here is that atoms in a covalent bond may share electrons either equally (non-polar covalent bond) or unequally (polar covalent bond). Whether a covalent bond will be polar or non-polar depends on the electronegativity of the atoms involved.

    Electronegativity is a measure of the ability of an atom to attract electrons. The Pauling scale gives each element an electronegativity score from 0 to 4. The closer an element's score is to 4, the better its atoms are at attracting and holding onto electrons.

    If two atoms with very different electronegativities react with each other, the result will not be a covalent bond at all, but rather an ionic bond. The bonding electron(s) will be transferred entirely to the more electronegative atom, as with sodium chloride.

    If two atoms with very similar electronegativities bond, the result is a non-polar covalent bond, as is the case with methane (CH4). Carbon and Hydrogen share the bonding electrons equally. If you could somehow lop off the atoms and just examine the bond, the bond would look the same no matter which way you turn it around.

    If two atoms in a bond have electronegativity values close enough together that the bond is still covalent, but far enough apart that the sharing of electrons is unequal, the result is a polar covalent bond. As another poster mentioned, water is a good example of a molecule that has polar covalent bonds. The electronegativity of Hydrogen is 2.20, and the electronegativity of Oxygen is 3.44. This means that Oxygen will have a greater portion of the bond's electron density near itself. The hydrogen ends of the bonds will have a lower electron density. This gives oxygen a partial negative charge, and the hydrogens a partial positive charge.

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  • 1 decade ago

    Water is a good example of a polar covalent material. The hydrogen atoms electrons are very attracted to the oxygen molecule at the center of the water molecule, which creates a slightly more positive charge towards the ends of the molecule and a slightly negative charge towards the center.

    Hope this helps! This is all i can remember!

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  • 4 years ago

    Almost right, H20, NH3 HF are all polar because the Electrons from the hydrogen spend more time around the othe atoms in the molecule, and because of the asymetry of the molecule. H2O is banana shaped, so the oxygen picks up a delta -ve and each hydrogen picks up a delta +ve Ammonia (NH3) I pyramidal with the hydrogens (delta +ve) at the base and the nitrogen (delta -ve) at the apex With HF, the Fluorine almost strips the electron from the hydrogen, and the resulting dipole, makes the HF molecule very soluble in water. In H2, Cl2 and N2, there is no polarity, because the electrons are shared equally, so the electrons can't be pulled one way or the other. The bonds in CH4 are more polar, but the dipole is cancelled by the symetry in CH3OH (Methanol) there is a polarity expressed around the oxygen atom as it tries to grab the hydrogen's electron, leading to a (delta +ve) around the Hydrogen, and a (delta -ve) around tthe oxygen Building models with the correct electron orbitals helps you to visualise the bond structures, and knowing the electronegativities, helps you to see where the polarising takes place. Correct bond structure can also help you to determine the physical properties ofthe substance

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For each covalently bonded compound will electron be shared evenly or unevenly?

water

ammonia

hydrogen iodide

iodine

lithium iodide

carbon dioxide

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For each covalently bonded compound will electron be shared evenly or unevenly?

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  • Anonymous
    1 decade ago
    Favorite Answer

    This question asks if the molecules are polar or nonpolar.

    Water is polar (oxygen is much more electronegative than hydrogen, so electrons are shared unevenly.

    Ammonia-polar, unevenly

    I think that you can figure out the rest.

    Good luck in chemistry.

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