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Chloramine has the chemical formula $NH _2 Cl$. Nitrogen has five valence electrons, each hydrogen has one valence electron, and chlorine has seven valence electrons. Complete the Lewis structure for this covalent compound.
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Answer (2)
Calculate the total valence electrons: 5 + 2 ( 1 ) + 7 = 14 .
Form single bonds between N and each H, and between N and Cl; this uses 6 electrons.
Add three lone pairs to Cl (6 electrons) and one lone pair to N (2 electrons) to complete octets.
The final Lewis structure contains only single bonds. Therefore, the answer is single bonds only. N H − Cl
Explanation
Determine the total number of valence electrons We are asked to complete the Lewis structure for chloramine ( N H 2 Cl ). We know that Nitrogen (N) has 5 valence electrons, Hydrogen (H) has 1 valence electron, and Chlorine (Cl) has 7 valence electrons. First, we need to calculate the total number of valence electrons in the molecule.
Calculate the total valence electrons The total number of valence electrons is calculated as follows:
1 Nitrogen atom: 1 × 5 = 5 valence electrons 2 Hydrogen atoms: 2 × 1 = 2 valence electrons 1 Chlorine atom: 1 × 7 = 7 valence electrons
Total valence electrons: 5 + 2 + 7 = 14 valence electrons
Determine the central atom and draw single bonds Nitrogen is the central atom because it is less electronegative than chlorine. We will connect the two hydrogen atoms and one chlorine atom to the nitrogen atom with single bonds. Each single bond represents two shared electrons.
Calculate remaining electrons We have formed 3 single bonds (N-H, N-H, and N-Cl), which accounts for 3 × 2 = 6 electrons. We started with 14 valence electrons, so we have 14 − 6 = 8 electrons remaining. These remaining electrons will be distributed as lone pairs around the atoms to satisfy the octet rule.
Add lone pairs to Chlorine Hydrogen atoms already have 2 electrons each (through the single bonds), so they do not need any more lone pairs. Chlorine needs 6 more electrons to complete its octet. We will add three lone pairs (6 electrons) to the chlorine atom. Now, we have 8 − 6 = 2 electrons remaining.
Add lone pair to Nitrogen The remaining 2 electrons will be added as a lone pair to the nitrogen atom. Now, the nitrogen atom has 3 single bonds (6 electrons) and 1 lone pair (2 electrons), giving it a total of 8 electrons, which satisfies the octet rule.
Final Lewis Structure The final Lewis structure has single bonds between N and each H, and a single bond between N and Cl. There are three lone pairs on Cl and one lone pair on N. Therefore, the correct connections are single bonds only.
Examples
Lewis structures are used to visualize the bonding between atoms in a molecule, helping chemists predict molecular properties and reactivity. For example, understanding the Lewis structure of chloramine helps in predicting its reactivity as a disinfectant in water treatment. By knowing how the atoms are connected and where the lone pairs are, we can understand how chloramine interacts with other molecules, which is crucial in designing effective chemical processes and ensuring safety in various applications.
To complete the Lewis structure for chloramine (NH₂Cl), we calculate a total of 14 valence electrons, with nitrogen as the central atom. We form single bonds between nitrogen and the two hydrogens, and nitrogen and chlorine, while distributing remaining electrons to satisfy the octet rule. The final structure displays nitrogen bonded to two hydrogens and one chlorine atom, with appropriate lone pairs on chlorines and nitrogen.
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