Which of the compounds below will have the shortest C-N bond? [HINT: Assess all electronic effects.] NO NO₂ O₂N O₂N HO NC H₂C- -NO₂ HO- A NO₂ NO₂ O₂N O₂N B D E NO₂

The bond energy of a C—C single bond averages 347 kJ mol-1; that of a CC triple bond averages 839 kJ mol-1. Explain why the triple bond is not three times as strong as a single bond.

Which compound contains a bond with no ionic character? a.CO b.CaO c.K2O d.Na2O

Which set shows the correct resonance structures for SeO2? O O O - :: O SeO2 does not have a resonance structure. O = Se 0:0 - Se = = 0: = Se - 0:0 :: Se = : 0: 0-Se-00 = Se = 0 :0 = Se= 0: O= Se- 0 :: 0 -Se= 0:

Which of these three is most stable? Explain (justify)

Q/ Three resonance structures of the highly unstable CSN – ion are shown below. a) Label any and all atomic formal charges that are present in each structure. b) Which of the structures is the major resonance structure? Why?

Identify the formal charge in the case below by indicating the magnitude, sign, and location of the charge. 2.. 1 :N 3 4 5 Magnitude and sign of formal charge Location of formal charge (atom number):

Resonance, hybridization, Lewis structures: Draw the lowest energy alternative resonance structure for acetamide Part A Draw the lowest energy alternative resonance structure for this compound. Interactive 3D display mode NN H₂C Draw the structure on the canvas by choosing buttons from the Tools (for bonds), Atoms, and Advanced Template toolbars. The single bond is active by default. [1] A NH,₂ H 12D EXP.¹ CONT ● L Marvin JS by ChemAxon H C N O S CI Br I P F

Which of the following central atoms would be expected to accommodate more than four electron pairs in some of its compounds?Simply explain your answer in a seperate sheet as well. F Br O N

Identify the formal charge in the case below by indicating the magnitude, sign, and location of the charge. :0: Magnitude and sign of formal charge Location of formal charge (atom number):