To draw the Lewis structure of CH₂N₂ (dimethyl hydrazine), we first need to determine the total number of valence electrons available. Carbon (C) has 4 valence electrons, hydrogen (H) has 1, and nitrogen (N) has 5 valence electrons.
In CH₂N₂, we have:
- 2 Carbon atoms: 2 × 4 = 8 valence electrons
- 4 Hydrogen atoms: 4 × 1 = 4 valence electrons
- 2 Nitrogen atoms: 2 × 5 = 10 valence electrons
This gives us a total of 8 + 4 + 10 = 22 valence electrons.
Next, we will sketch the structure. Start by placing the carbon atoms in the center, connected to each other. Attach two hydrogen atoms to each carbon atom. The nitrogen atoms will be placed to the side, connected to one of the carbon atoms.
Now, we will focus on fulfilling the octet rule:
- Each carbon can form four bonds, while each hydrogen can form only one.
- Each nitrogen atom can form three bonds, so we can connect each nitrogen to a carbon and include a lone pair of electrons on them.
After making sure that each atom has the required number of bonds, we can count and ensure that all 22 valence electrons are accounted for, including any lone pairs. The final Lewis structure will show the bonds clearly, indicating a double bond between the carbons and a single bond between nitrogen and carbon.
This representation offers a visual insight into the bonding and structure, showcasing the sigma bonds interconnecting the atoms. Drawing it carefully aids in the understanding of the molecular geometry and electron distribution within the compound.