Click to Chat
1800-1023-196
+91-120-4616500
CART 0
Use Coupon: CART20 and get 20% off on all online Study Material
Welcome User
OR
LOGIN
Complete Your Registration (Step 2 of 2 )
Hi Experts , Plz explain .....Why are OH, NH, and FH bonds so polar?
Hi Experts ,
Plz explain .....Why are OH, NH, and FH bonds so polar?
Hi , Hydrogen atoms are very small (with an atomic radius of about 37 pm, they're smaller than any other atom but helium). So when a bonded electronegative atom pulls electrons away from the hydrogen atom, the positive charge that results is tightly concentrated. The small size of the hydrogen atom is one factor responsible for the unusual strength of the dipole-dipole interaction we call "hydrogen bonding". When gauging the strength of intermolecular attractions, considering the magnitude of partial charges isn't enough; you also must look at how spread out the charges are. The atomic radius trends you've learned are often very helpful here.
Hi ,
Hydrogen atoms are very small (with an atomic radius of about 37 pm, they're smaller than any other atom but helium). So when a bonded electronegative atom pulls electrons away from the hydrogen atom, the positive charge that results is tightly concentrated. The small size of the hydrogen atom is one factor responsible for the unusual strength of the dipole-dipole interaction we call "hydrogen bonding". When gauging the strength of intermolecular attractions, considering the magnitude of partial charges isn't enough; you also must look at how spread out the charges are. The atomic radius trends you've learned are often very helpful here.
When gauging the strength of intermolecular attractions, considering the magnitude of partial charges isn't enough; you also must look at how spread out the charges are. The atomic radius trends you've learned are often very helpful here.
Find solution of question on doubt solving app Instasolv
Post Question
Dear , Preparing for entrance exams? Register yourself for the free demo class from askiitians.
points won -