For each pair, circle the most polar bond
- C—F O—F


- O—Cl S—Br
- C—S B—F
- C—P N—F
- N—O C—O
- By referring only to the periodic table, select most electronegative element in each pair
- Al or Si
- F or N
- Ga or P
- Na or K
- Br or Pb
- Write Lewis structures that obey the octet rule for each of the following, and assign formal charges to each atom
- CF4
- BrO3–
Write Lewis structures for the following
H2CO (both H atoms are bonded to C) NF3
AsO33- C2H2
O3 NO
BF3 XeF4
- Write the Lewis Structures for the following molecules. Based on Lewis structures, predict which molecule will have the longest N—O bond lengths: NO+, NO2–, and NO3–.
- OCS, has three possible Lewis structures. (a) Draw these three structures and assign formal charges in each. (b) Which Lewis structure is dominant? Treat C as the central atom in each of the three Lewis structures
O C S O C S O C S
- Using Table 8.4, estimate DH for the following reactions and indicate whether they are exothermic or endothermic
