Answer :
Final Answer:
Nitrogen has a formal charge of -1 due to an excess of electrons, oxygen has a formal charge of +1 due to a deficiency of electrons, and chlorine has a formal charge of 0, as it has the appropriate number of valence electrons in the proposed Lewis structure. Therefore, the correct answer is c) Nitrogen: -1, Oxygen: +1, Chlorine: 0.
Explanation:
In assigning formal charges to atoms in a Lewis structure, we follow the rule that the sum of the formal charges should equal the overall charge of the molecule, which in this case is 0 because ONCl is a neutral molecule.
Here's how the formal charges are assigned:
- Nitrogen (N) has 5 valence electrons. In the proposed structure, it is bonded to one oxygen atom (sharing 2 electrons) and one chlorine atom (sharing 2 electrons), and it has one lone pair of electrons. To calculate its formal charge: Valence electrons (5) - 1/2(bonded electrons) (2) - lone pair electrons (2) = -1. So, Nitrogen has a formal charge of -1.
- Oxygen (O) has 6 valence electrons. In the proposed structure, it is bonded to one nitrogen atom (sharing 2 electrons) and one chlorine atom (sharing 2 electrons), and it has two lone pairs of electrons. To calculate its formal charge: Valence electrons (6) - 1/2(bonded electrons) (2) - lone pair electrons (4) = +1. So, Oxygen has a formal charge of +1.
- Chlorine (Cl) has 7 valence electrons. In the proposed structure, it is bonded to one nitrogen atom (sharing 2 electrons) and one oxygen atom (sharing 2 electrons). To calculate its formal charge: Valence electrons (7) - 1/2(bonded electrons) (2) = 0. So, Chlorine has a formal charge of 0.
Therefore, the correct assignment of formal charges for the ONCl molecule is:
- Nitrogen: -1
- Oxygen: +1
- Chlorine: 0, which corresponds to option c).
Therefore, the correct answer is c) Nitrogen: -1, Oxygen: +1, Chlorine: 0.
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