posted by .

How does the 3D structure of SP3 bonds of Carbon, Oxygen and Nitrogen cause them to form polar molecules?
How does the three dimensional structure
of SP3 bonds of Carbon, Oxygen and Nitrogen
cause them to form polar or non-polar

The answer must include a 3d
diagram of the molecules, and a discussion of the
effect of their electron configurations for bonds to
H; and how their filled or bonded orbitals
contributes to the polar nature of the molecule.


Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    what are 4 chemical properties of organic compounds?

    I am refreshing on bonding and structure before starting an organic chem class. I am a bit rusty on hybrid orbitals in bonding. Take Methane, CH4, I understand each carbon has an sp3 orbital that overlaps an s orbital on the H to form …
  3. Chem URGENT!!

    Which bond is most polar? F-Cl O-P O-S F-F Si-O Which species has the shortest carbon/oxygen bond?
  4. Chemistry

    Consider the Lewis structure for the major resonance form of PCS–. (Note that carbon is the central atom.) The structure shows: a. A phosphorus-carbon triple bond and a carbon-sulfur single bond. b. A phosphorus-carbon double bond …
  5. chemistry

    Which of the following statements is true regarding the Lewis structure for methylamine, CH3NH2?
  6. chemistry

    How does Carbon hybridize it's S and P orbitals and what effect does this have on the 3D structure and chemical behavior?
  7. Chemistry(Please check)

    What is the hybridization of each carbon in the molecule of ethanol. CH3 = sp3 CH2OH = sp3 I think that the carbons are all sp3 because there are only single bonds in this molecule. Is this correct?
  8. chemistry

    The structure of graphite is shown below. What kind of hybridization exists for each carbon in the lattice?
  9. Chemistry

    B. Could non-polar nitrogen molecules and polar water molecules form bonds with one another?
  10. Chemistry pretty urgent!!!!!!!

    Chemical bonding question! The partial Lewis structure that follows (Figure 1) is for a hydrocarbon molecule. In the full Lewis structure, each carbon atom satisfies the octet rule, and there are no unshared electron pairs in the molecule. …

More Similar Questions