In the following molecule, indicate the hybridization and shape of the indicated atoms. CH3 N CH3 HÖ: H3C CI: ::

Describe the shapes of C2H6 and C2H4. In doing so, explain why one molecule is planar and why the other molecule cannot be planar.

• explain how hybridization reconciles observed molecular shapes with the orbital overlap model.

Give the shape that describes each hybrid orbital set: (a) sp2 (b) sp3d (c) sp (d) sp3d2

What hybrid orbitals would be expected for the central atom in each of the following molecules or ions?

• explain the formation of multiple bonds in terms of the overlap of a combination of hybridized and unhybridized atomic orbitals.

7.96 Consider the hydrocarbons whose structures are shown below. Which of these molecules would be planar, meaning that all of the atoms must lie in the same plane? Explain your answer in terms of orbital hybridizations.

Strike-anywhere matches contain a layer of KClO3 and a layer of P4S3. The heat produced by the friction of striking the match causes these two compounds to react vigorously, which sets fire to the wooden stem of the match. KCIO3 contains the ClO3 ion. P4S3 is an unusual molecule with the skeletal structure. (a) Write Lewis structures for P4S3 and the ClO3 ion. (b) Describe the geometry about the P atoms, the S atom, and the Cl atom in these species. (c) Assign a hybridization to the P atoms, the S atom, and the Cl atom in these species. (d) Determine the oxidation states and formal charge of the atoms in P4S3 and the ClO3 ion.

A molecule with the formula AB3 could have one of four different shapes. Give the shape and the hybridization of the central A atom for each.

Draw three contributing structures of the following compound (called guanidine) and state the hybridization of the four highlighted atoms. In which orbitals do the three lone pairs drawn reside?