Write down the Lewis structure of [1+1] i) N2O ii) HClO4

i) Lewis structure of $\mathrm{N}{}_2\mathrm{O}$

1. Total valence electrons:
   • N: 5 × 2 = 10
   • O: 6 × 1 = 6
   • Total = 16 electrons

2. Possible structures:

   • $\mathrm{N}-\mathrm{N}=\mathrm{O}$ (linear) or $\mathrm{N}=\mathrm{N}=\mathrm{O}$ (linear).
   • The correct structure is $\mathrm{N}=\mathrm{N}=\mathrm{O}$ (nitrogen oxide), where the central N is bonded to the terminal N and O via triple and double bonds, respectively.

3. Electron distribution:

   • Triple bond (N≡N) uses 6 electrons.
   • Double bond (N=O) uses 4 electrons.
   • Remaining 6 electrons form lone pairs on the terminal N and O.

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ii) Lewis structure of $\mathrm{HClO}{}_4$

1. Total valence electrons:

   • H: 1
   • Cl: 7
   • O: 6 × 4 = 24
   • Total = 32 electrons

2. Structure:

   • Cl is the central atom bonded to 4 O atoms (one via a single bond and three via double bonds).
   • One O is bonded to H, forming $-\mathrm{O}-\mathrm{H}$.

3. Electron distribution:

   • Single bond (Cl–O–H) uses 2 electrons.
   • Three double bonds (Cl=O) use 12 electrons.
   • Remaining 18 electrons form lone pairs on O and Cl.

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