Sketch the Lewis structure of an ethylenediamine molecule and upload the image.
The Correct Answer and Explanation is:
Here is the correct Lewis structure for an ethylenediamine molecule, followed by a detailed explanation.
Explanation of the Lewis Structure for Ethylenediamine
The construction of a Lewis structure for any molecule, such as ethylenediamine, follows a systematic process to accurately represent the bonding and electron distribution.
First, the molecular formula and the total number of valence electrons must be determined. Ethylenediamine (systematically named 1,2-ethanediamine) has the chemical formula C₂H₈N₂. The number of valence electrons is calculated by summing the contributions from each atom:
- Carbon (C): 2 atoms × 4 valence electrons/atom = 8 electrons
- Nitrogen (N): 2 atoms × 5 valence electrons/atom = 10 electrons
- Hydrogen (H): 8 atoms × 1 valence electron/atom = 8 electrons
- Total Valence Electrons: 8 + 10 + 8 = 26 electrons
Next, the skeletal structure is established. In ethylenediamine, the two carbon atoms form a central backbone, connected by a single bond. An amine group (–NH₂) is attached to each of these carbon atoms. Hydrogen atoms are always terminal, so they are placed around the carbon and nitrogen atoms. The resulting skeleton is H₂N–CH₂–CH₂–NH₂.
Single bonds are then drawn to connect all the atoms in the skeletal structure. This includes one C–C bond, two C–N bonds, four N–H bonds, and four C–H bonds, for a total of 11 single bonds. Each bond represents two electrons, so 22 electrons (11 × 2) are used for bonding.
The remaining electrons are distributed as lone pairs to satisfy the octet rule. With 26 total valence electrons and 22 used in bonds, 4 electrons remain (26 – 22 = 4). These are placed on the most electronegative atoms that do not yet have an octet. In this case, each nitrogen atom has three bonds (6 electrons), so each receives one lone pair (2 electrons) to complete its octet.
Finally, the structure is verified. Each hydrogen atom satisfies the duet rule with one single bond (2 electrons). Each carbon atom has four single bonds, fulfilling the octet rule (8 electrons). Each nitrogen atom has three single bonds and one lone pair, also fulfilling the octet rule (8 electrons). The final structure correctly uses all 26 valence electrons and satisfies the octet/duet rules for all atoms.thumb_upthumb_down
