How to draw the molecular bonding structure of diazene (N2H2)

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Welcome to our exploration of diazene, also known as N2H2. Diazene is a fascinating nitrogen-hydrogen compound featuring two nitrogen atoms connected by a double bond. Each nitrogen atom is also bonded to one hydrogen atom and possesses a lone pair of electrons. This unique structure allows diazene to exist in two different geometric forms called cis and trans isomers. The first step in drawing the Lewis structure is to count the total valence electrons. Nitrogen is in Group 15, so each nitrogen atom contributes 5 valence electrons. Hydrogen is in Group 1, contributing 1 valence electron each. With 2 nitrogen atoms and 2 hydrogen atoms, we have 2 times 5 plus 2 times 1, giving us a total of 12 valence electrons to work with. Step 2 involves drawing the skeletal structure by connecting atoms with single bonds. We place the two nitrogen atoms in the center and connect each to a hydrogen atom, forming the initial structure H-N-N-H. This skeletal structure uses 3 single bonds, with each bond containing 2 electrons, so we've used 6 electrons. This leaves us with 6 remaining electrons from our total of 12. In step 3, we check octets and form multiple bonds as needed. After placing lone pairs on the nitrogen atoms, we find that one nitrogen doesn't have a complete octet. To solve this, we form a double bond between the two nitrogen atoms by moving a lone pair to create a second bond. This gives us the final structure H-N=N-H, where both nitrogen atoms now have complete octets with 8 electrons each.