cide whether the Lewis structure proposed for each molecule is reasonable or not. molecule proposed Lewis structure 1Br BH₂ :: 1 Br :: :-: Br بت [R-B-] — B—H]* H :0: " SO :0-S 0: :0: 12- Is this a reasonable structure? If not, why not? O Yes, it's a reasonable structure. No, the total number of valence electrons is wrong. The correct number is: ☐ O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: O Yes, it's a reasonable structure. ☐ No, the total number of valence electrons is wrong. The correct number is: ☐ O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: ☐ O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. The correct number is: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: ☐ *If two or more atoms have the wrong number of valence electrons around them, just enter the chemical symbol for the atom as many times as necessary. For example, if two oxygen atoms have the wrong number of electrons around them, enter the symbol O twice. 00

Write Lewis structures for the following: (a) ClF3 (b) PCl5 (c) BF3 (d) PF6

A stable triatomic molecule can be formed that contains one atom each of nitrogen, sulfur, and fluorine. Three bonding structures are possible, depending on which is the central atom: NSF, SNF, and SFN. (a) Write a Lewis diagram for each of these molecules, indicating the formal charge on each atom. (b) Often, the structure with the least separation of formal charge is the most stable. Is this statement consistent with the observed structure for this molecule—namely, NSF, which has a central sulfur atom? (c) Does consideration of the electronegativities of N, S, and F from Figure 3.18 help rationalize this observed structure? Explain.

Fill in the blanks in each line of the following table that involves characteristics of various bonds between nonmetals. The first line is already completed as an example.

hat does it mean to say that a bond is polar? Give two examples of molecules with polar bonds. Indicate in your examples the direction of the polarity.

The percent ionic character of a bond can be approximated by the formula 16+3.52 , where is the magnitude of the difference in the electronegativities of the atoms (see Fig. 3.18). Calculate the percent ionic character of HF, HCl, HBr, HI, and CsF, and compare the results with those in Table 3.7.

7.47 Which of the species listed has a Lewis structure with only one lone pair of electrons? F2 , CO32 , CH4 , PH3

In the Lewis structure for chloromethane, the chlorine atom is sharing _____ electron pair and “owns” _____ of those electrons. Also, the chlorine atom possesses two electrons from each of _____ unshared pairs. The total number of electrons that belong to chlorine is 7 . Chlorine is a Group ____ element. The formal charge on chlorine in chloromethane is ____.

3. The skeleton of chloromethane is __________________ The central carbon atom is bonded to each of the other atoms by a shared electron pair (represented by a straight line, ___) giving Now, each hydrogen has two electrons and the carbon atom has eight. However, chlorine must be provided with unshared electrons (represented by pairs of dots, ) to complete its octet, thus

For three simple molecules of your own choice, apply the rules for writing Lewis structures. Write your discussion as if you are explaining the method to someone who is not familiar with Lewis structures.