High School

Give the formal charge for each atom (except hydrogen) in [tex]H_2C=NN[/tex]. The end nitrogen has 2 electron pairs. Be sure to include the charge (+1, -1, etc.).

Formal charges:
- C (central)
- N (end)

Answer :

Final answer:

The formal charge for each atom (except hydrogen) in H2C=NN is: Carbon (C): 0, Central Nitrogen (N): 0, End Nitrogen (N): +1.

Explanation:

To calculate the formal charge for each atom (except hydrogen) in the molecule H2C=NN, we need to follow these steps:

  1. Determine the number of valence electrons for each atom. Carbon (C) has 4 valence electrons, and nitrogen (N) has 5 valence electrons.
  2. Count the number of lone pair electrons and bonding electrons around each atom. In this molecule, the central carbon atom is bonded to two hydrogen atoms and one nitrogen atom. The end nitrogen atom has 2 electron pairs.
  3. Calculate the formal charge for each atom using the formula: Formal Charge = Valence Electrons - Lone Pair Electrons - 1/2 * Bonding Electrons.

Let's calculate the formal charges:

  • Carbon (C): Formal Charge = 4 - 0 - 1/2 * 4 = 0
  • Central Nitrogen (N): Formal Charge = 5 - 2 - 1/2 * 4 = 0
  • End Nitrogen (N): Formal Charge = 5 - 2 - 1/2 * 4 = +1

Therefore, the formal charge for each atom (except hydrogen) in H2C=NN is:

  • Carbon (C): 0
  • Central Nitrogen (N): 0
  • End Nitrogen (N): +1

Learn more about formal charges in a molecule here:

https://brainly.com/question/34481427

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