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definition of polar and non polar

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non-polar molecule Dictionary definition of non-polar molecule...

Definition of non-polar molecule Our online dictionary has non-polar molecule information from A Dictionary of Zoology dictionary.

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Question:Guys, I need help. I'm studying for my test which is on Monday 3rd, 2007. Question 1 How do I determine how a Molecule is Polar/Non-Polar using the Lewis Structure/Molecular Geometry??? Question 2 How do I know when a Molecule has a double/triple bond when I'm using the Lewis Structure? I know how to do Lewis Structure but I don't know when it calls for a Double/Triple Bond. Question 3 Intermolecular Forces. Ok, my book is stupid they just give me the definition of the forces but they don't tell me how to distinguish which Molecule is which InterMolecular Forces. Can somone give me information on how to distinguish Molecules for Hydrogen Bonding, London Dispersion, and Dipole-Dipole? Please explain to the simplest form please. I'm a little slow :S. I really appreciate everyones help :). Thank You..

Answers:1) You can tell the polarity of the molecule through the lewis structure, by examining it's symetry. Tetrahedrals will always be symettrical, therefore, are non - polar. On the other hand, something like water, which is not symettrical, is polar. 2) you will know when u need a double / triple bond when either you dont not get the correct amount of electrons you came in with, or if the formal charges are obscure. Ozone for example. O3 has 18 electrons. 2 Oxygens bonded to a centrally bonded Oxygen If you put on oxygen in the middle, and single bond both of the other oxygens you have 6 electrons (dots) around one O, 6 dots around another, and 4 around the other. This is 16. Add the two bonds (2 electrons a piece = 4) and you have a total of 20 electrons - not the 18 you started with. You need to double bond one of the Oxygens to the central atom Oxygen. Then you have one Oxygen with 6 electrons (dots) around it, another with 4, and the Central oxygen with 2. 6 + 2 + 4 = 12 Now you have one single bond (2 electrons) and one double bond (4 electrons) 12 lone pair electrons + 6 bonded electrons = 18 electrons, the correct amount of electrons that you came into the problem with. Dont forget "resonance" structions. The double bond on one oxygen is shared between both of the outer oxygens. 3) London Dispersion are for non-polar molecules - It is a slight pull of electrons towards the more electronegative element. This type of intermolecular force is found in almost every molecule. Dipole - Dipole is when you have a mixture of polar molecules that all have a significant negative charge and positive charge. The positive charge of one molecule will allign itself with the negative charge of another molecule, and this process will go on and on for every molecule in the substance. Hydrogen bonding takes place in covelant bonds, when a HYDROGEN is bonded to a ELECTRONEGATIVE element with LONE PAIRS. Water, H20 O is electronegative with two lone pairs, and bonded to hydrogen. The lone pairs on anotoher water molecule are attracted to the hydrogens rich positive charge, as all of its negative charge was pulled away to the electronegative atom, in this case, oxygen. Hydrogen bonding is the strongest intermolecular force.

Question:I've researched and found that Acetone is highly polar. But while doing my Beet Membrane Lab, where Acetone was mixed with a piece of a Beet causing damage to the Beet Cells, it says that the Acetone is capable of dissolving hydrophobic phospholipids? How can this supposed Polar Solvent dissolve non-polar Phospholipids??

Answers:It is polar. That is part of the reason it mixes with water. It is also soluble with nonpolar substances like hydrocarbons because of the two methyl side groups.

Question:Is isopropyl alcohol (C3H7OH) polar or non polar? Why? Is acetone (C3H60) polar or non polar? Why? I really can't tell the difference between polar and non polar bonds.. Please help!

Answers:Polarity occurs to a greater or lesser extent depending on the atoms involved. In teh cases you cite the double bond in acetone (the carbonyl group) is polar due to the electronegativity of oxygen compared to carbon. The same is true in the single C-O bond in isopropanol (the alcohol group) for the same reason.

Question:You preform an experiment to determine whether various substances are polar, non-polar, or amphipathic (having both polar and non-polar character). Based on the results in the table below, determine the solubility of three unknown substances in each other the three solvents: water, oil, and ethyl alcohol. Decided whether each unknown should be classified as polar, non-polar, or amphipathic. Write the correct letter in the space given besides each unknown below using the following code. P = Polar , NP = Non-polar, A = Amphipathic 1.(Water) insoluble, (Oil) highly soluble, (Ethanol) slightly soluble 1._____________ 2. (Water) highly soluble, (Oil) insoluble, (Ethanol) slightly soluble 2. ______________ 3. (Water) slightly soluble, (Oil) slightly soluble, (Ethanol) highly soluble 3.____________

Answers:1. non polar (soluble in oil) 2. polar (soluble in water) 3. amphipathic (both soluble in water and oil)

From Youtube

Polar and Non-Polar Molecules :Tells how to decide if a molecule is polar or non-polar

Dosely - Non Polar Solvent :a dubstep and ambient inspired track w/ MilkDrop visuals