Question

In V.B.T., the idea of hybridization was required to explain which of the following facts
The equivalence of the bonds in most of the compounds
The reactivity of the molecules
The better overlapping of the orbitals
none of these​

Answer 1

Explanation:

However, the application of VSEPR theory can be expanded to complicated molecules such as

   H H         H   O

   | |         |  //

 H-C-C=C=C-C=C-C-C

   |           |  \

   H           N   O-H

              / \

             H   H

By applying the VSEPR theory, one deduces the following results:

H−C−C  bond angle = 109o

H−C=C  bond angle = 120o, geometry around  C  trigonal planar

C=C=C  bond angle = 180o, in other words linear

H−N−C  bond angle = 109o, tetrahedral around  N  

C−O−H  bond angle = 105 or 109o, 2 lone electron pairs around  O  

Confidence Building Questions

In terms of valence bond theory, how is a chemical bond formed?

Hint: A chemical bond is due to the overlap of atomic orbitals.

Discussion -

Molecular orbital theory considers the energy states of the molecule.

When one s and two p atomic orbitals are used to generate hybrid orbitals, how many hybrid orbitals will be generated?

Hint: Using three atomic orbitals generates three hybrid orbitals.

Discussion -

Number of orbitals does not change in hybridization of atomic orbitals.

In the structures of  SO2  and  NO2 , what are the values of the bond angles?

Hint: The bond angles are expected to be less than 120 degrees.

Discussion -

Since the lone electron pair in  :SO2  and lone electron in  ⋅NO2  take up more space, we expect the structure to distort leaving a smaller angle than 120 between the bonds.

What is the geometrical shape of the molecule  CH4 , methane?

Hint: Methane molecules are tetrahedral.

Discussion -

The 4  H  atoms form a tetrahedron, and methane has a tetrahedral shape.

What do you expect the bond angles to be in the  NH+4  ion?

Hint: All bond angles are 109.5 degrees, the ideal value for a symmetric tetrahedral structure.

Discussion -

The structure of this ion is very similar to that of  CH4 .

What hybrid orbitals does the  C  atom use in the compound  H−C≡C−H , in which the molecule is linear?

Hint: The sp hybrid orbitals are used by the  C  atom.

Discussion -

Sigma (s) bonds are due to sp hybrid orbitals, and 2 p orbitals are used for pi (p) bonds. The two sigma bonds for each  C  are due to overlap of sp hybrid orbitals of each  C  atom.