4. Using Lewis theory, show and explain why nitrogen gas exists as a diatomic molecule. 5. For each molecule or ion complete the following: (a) Determine the total number of valence electrons available for bonding / electron-pairs available for bonding. (b) Draw the Lewis structure. (c) Determine whether the molecule exists as a resonance hybrid If it does, draw the resonance structures. If it does not, write "NA" for not applicable. ● ● (d) State the name of the molecular geometry (e) Draw the VSEPR representation of the molecular geometry using wedges and dashed lines where appropriate Include the bond angles. ●

Consider the following ion: BrO3−. a)  Show the full electron configuration for Br.  b)  Draw the most correct Lewis structure for BrO3− and briefly explain why your Lewis structure is correct. c)  If the structure is stabilised by resonance, draw at least one of the possible resonance forms. If it is not stabilised by resonance, briefly explain why.  d)  What is the electronic geometry of BrO3−? What is its molecular shape?  e)  Does BrO3− have a dipole moment? Briefly justify your answer. f)  On average, would you expect IO3− to have longer or shorter bonds than BrO3−? Briefly explain your answer.  g)  Which of the following molecules would you expect to have the lowest vapour pressure? Briefly explain your choice. (IMAGE WITH POSSIBILITIES) h)  What is the molecular formula for Compound C? What is the empirical formula for Compound C?

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For a molecule of XeCl3H a) Draw the Lewis structure then predict the shape of the compound and draw the shape of the compound b) Determine if the molecule is polar or nonpolar and explain how you made that determination. If there is a dipole moment, draw it.