Question 3 (9 points): Draw the \( \underline{M O} \) (molecular orbitals) of \( \mathrm{N}_{2}, \mathrm{~N}_{2}^{+} \)and \( \mathrm{N}_{2}{ }^{-} \)in the same way you learned in class. Calculate their respective bonding order. (Hint: You don't have to include inner orbitals, just start from \( 2 s \) and \( 2 p \) )
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Sketch the 1 s and $2 p$ orbitals. How do the $2 s$ and $3 p$ orbitals didfer from the 1 s and $2 p$ orbitals? MisSED THIS? Read Section 8.6 orbitals?
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Write the molecular orbital electron configuration and determine the bond order and number of unpaired electrons for the following ions. (a) $\mathrm{C}_{2}^{+}$ (b) $\mathrm{N}_{2}^{-}$ (c) $\mathrm{Be}_{2}^{-}$
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