1. Describe the difference betwwn polar andnon-polar molecules. can you provide
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Question
1. Describe the difference betwwn polar andnon-polar molecules. can you provide examples?2. Can you describe each of three IMF(intermolecular force) of attractions? 3. How do you distinguish between electrolyteand non-electrolytes? 4. Please expain how to balance an equation oneelement at a time 1. Describe the difference betwwn polar andnon-polar molecules. can you provide examples?
2. Can you describe each of three IMF(intermolecular force) of attractions? 3. How do you distinguish between electrolyteand non-electrolytes? 4. Please expain how to balance an equation oneelement at a time
Explanation / Answer
Polarity is measured on a scale ofelectronegativity (the electron disparity between two elements thatare combined in a compound). The more electrons you take from yourpartner element in the bonding process, the greater your negativecharge, and the greater your electronegativity.There are three terms to describe the polarity of a given molecularbond:
Ionic
Polar covalent
Non-polar covalent
Ionic is the most polar - essentially, one atomphysically takes electrons from another atom, creating a hugeelectron disparity between the two atoms. This tends to happen inmolecules where one atom has very few valence electrons and theother has a lot of valence electrons. Sodium chloride (NaCl) is agood example of an ionic bond.
Polar covalent is the mid-range - technicallycloser to ionic. This happens when one atom attempts to takeelectrons from its partner, but cannot quite attract them all toitself. The result is a covalent bond between the two atoms wherethe valence electrons are "shared," but the sharing is unequal. Oneatom pulls the "shared" electrons a little closer to itself. Polarcovalent bonds usually occur between very electronegative elements;hydrogen paired with elements like oxygen and fluorine almostalways creates polar covalent bonds. A good example of a polarcovalent bond is found in water (H2O).
Non-polar covalent is the least polar - in fact,it is not polar at all. This occurs when valence electrons areshared equally between two atoms. There is little or no tendencyfor either atom to pull any of the electrons toward itself.Non-polar covalent bonds can often be seen in molecules with twonon-metals. Methane (CH4) is an example of a non-polarcovalent bond.
First off, if the molecule is symmetrical, it is probablynon-polar. An example is CO2, CH4, or SeF5.
An idea of if it is polar, unequal sharing of electrons. H20. Theshape is actually a tetrahedral. The same structure at CH4. Thoughin the place of two H's, there are 4 e- . This makes the moleculenot symmetrical.
Think of H2O as this. The side where the H's are is slightly morepositive. The side where the two pairs of electrons are, themolecule is slightly negative. The molecule overall is a neutralcharge, but different portions of the molecule have slightvariations in charge.
In the molecule C2H2Cl2, there are three different structures. Onewith both Cl's on one carbon, one with both Cl's are either top andbottom, or both Cl's at diagonals. When they are at diagonals themolecule is non-polar. In both other cases it is polar.
3--- An electrolyte is a compound which conductselectricity when in solution. Any ionic compound which dissociatesinto ions in solution is an electrolyte. Ex > NaCl
Non electrolytes are just the opposite. They do not separate intoions in solution. Thus, they will not conduct electricity. Ex >C2H3O2 4- the main thing to think about when you balance equations arethe coefficients and subscripts on all the compounds and elements.You just want to make sure you have the same amount on both sidesfor the same elements or compounds.
1. H2 + O2 -> H2O
2H2 + O2 -> 2H2O
First I put a coefficient of 2 on the H2O to have 2H2O and have 2oxygens on both sides, but then you changed the hydrogen, so youbut another coefficient of 2 on the H2 to get 2H2 and then you have4 hydrogen on both sides and two oxygen on both sides and you'redone!
2. AlBr3+K2SO4-->KBr+Al2(SO4)3
2AlBr3 + 3K2SO4 ->6KBr + Al2(SO4)3
same process as above. Just work one element at a time andremember, in this case, that you balance SO4 as one element, as youwouldn C or H. Because SO4 has a charge on its own and exists thatway.
3. C3H8+O2-->CO2+H2O
C3H8+5O2-->3CO2+4H2O
4. FECl3 + NaOH -->Fe(OH)3 + NaCl
FECl3 + 3NaOH -->Fe(OH)3 + 3NaCl
do 3 and 4 and any balancing the same way
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