4. Molecular Compounds

CIA Problem 4.2 Draw the Lewis dot structures for the molecules CO and NO. What is different about these structures compared with the general examples we have seen so far? How could these Lewis structures provide insight into the high chemical reactivity of these molecules?

How many covalent bonds are formed by each atom in the following molecules? Draw molecules using the electron-dot-symbols and lines to show the covalent bonds. a. PH₃ b. H₂Se c. HCl d. SiF₄

Write electron-dot symbols to show the number of covalent bonds and the lone pairs of electrons in the molecules that are formed by reactions between the atoms in Problem 4.34.

Distinguish between the following: c. A lone pair and a shared pair of elecctrons

Consider the following possible structural formulas for C₃H₆O₂ . If a structure is not reasonable, explain what changes could be made to convert it to a reasonable structure. a.

Expand the following condensed structures into the correct structural formulas. c. CH₃CH₂OCH₂Cl

The following formulas are unlikely to be correct. What is wrong with each? d. C₂OS

The phosphonium ion, PH⁺₄ is formed by reaction of phosphine, PH₃ , with an acid. d. Explain why the ion has a +1 charge.

State the number of valence electrons, bonding pairs, and lone pairs in each of the following Lewis structures: (6.6)c.

Draw the Lewis structure for each of the following: (6.6)b. H₂NOH N is the central atom)

Draw the Lewis structure for each of the following: (6.6)a. H₃COCH₃ (the atoms are in the order C O C)