7. Consider xenon thiodichloride, XeSCI2 (a) Write the Lewis structure (b) What is the electron pair and molecular geometry about the xenon central atom? (c) What is the hybridization of the internal xenon atom in XeOF2?

Predict the electron pair geometry and the molecular structure of each of the following molecules or ions:(a) SF6(b) PCl5(c) BeH2(d) CH3+

. Assume that the third-period element phosphorus forms a diatomic molecule, P2, in an analogous way as nitrogen does to form N2. (a) Write the electronic configuration for P2. Use [Ne2] to represent the electron configuration for the first two periods. (b) Calculate its bond order. (c) What are its magnetic properties (diamagnetic or paramagnetic)?

What are the electron-pair geometry and the molecular structure of each of the following molecules or ions?(a) ClF5(b) ClO2−(c) TeCl42−(d) PCl3(e) SeF4(f) PH2−

The sulfate ion can be represented with four S-O bonds or with two S-O and two So=O bonds.(a) Which representation is better from the standpoint of formal charges?(b) What is the shape of the sulfate ion, and what hybrid orbitals of S are postulated for the σ bonding?(c) In view of the answer to part (b), what orbitals of S must be used for the π bonds? What orbitals of O?(d) Draw a diagram to show how one atomic orbital from S and one from O overlap to form a π bond.

Consider the reaction BF3 + NH3 -> F3B-NH3 (a) Describe the changes in hybridization of the B and N atoms as a result of this reaction. (b) Describe the shapes of all the reactant molecules with their bond angles. (c) Draw the overall shape of the product molecule and identify the bond angles around B and N atoms. (d) What is the name of the bond between B and N. (e)Describe the bonding orbitals that make the B and F, B and N & N and H bonds in the product molecule.

In addition to Al₂Cl₆, aluminum forms other specieswith bridging halide ions to two aluminum atoms. One suchspecies is the ion Al₂Cl₇. The ion is symmetrical, with a 180° Al−Cl−Al bond angle.(a) What orbitals does Al use to bond with the Cl atoms?(b) What is the shape around each Al?(c) What is the hybridization of the central Cl?(d) What do the shape and hybridization suggest about the pres-ence of lone pairs of electrons on the central Cl?

(a) Why do stable xenon fluorides have an even number of F atoms? (b) Why do the ionic species XeF₃⁺ and XeF₇⁻ have odd numbers of F atoms? (c) Predict the shape of XeF₃⁺ .

The structure of caffeine is shown below. (a) Complete the Lewis structure. (b) How many pi bonds are present in caffeine? How many sigma bonds? (c) Identify the hybridization of the carbon atoms. (d) What is the value of the O-C-N angle?

Borane (BH3) is unstable under normal conditions, but it has been detected at lowpressure.(a) Draw the Lewis structure for borane.(b) Draw a diagram of the bonding in BH3, and label the hybridization of each orbital.(c) Predict the H¬B¬H bond angle