Draw the Lewis structure for each of the following molecules: d. ClNO 2 (N is the central atom)

Hello. In this problem, we are asked to show the best age structure for Nitrol fluoride. And to note that nitrogen here is the central atom. Let's make use of the need available share method which we'll denote as N A S. So need is based on most things trying to acquire an Octa nitrogen. Oxygen and fluorine are not exceptions to the Octa rule. So all three are trying to acquire eight valence electrons. So that's a total of 24 electrons that we need available comes from the number of valence electrons. Nitrogen is in group five A. So it has five valence electrons. Oxygen is in group six A. So it has six valence electrons and fluorine is in group seven A. So it has seven valence electrons. That's a total of 18 electrons that are available. We will then share the difference between what we need, which is 24 electrons and what is available, which is 18. So we will share six electrons, we will put nitrogen in the center of our skeletal structure and then we will share six electrons. So we will form a double bond between the nitrogen and oxygen and a single bond between the nitrogen and the fluorine. So now we have a sharing of 246 electrons, we put a single bond between the nitrogen and fluorine because fluorine will only form a single bond, we then need to account for all 18 electrons. And so we've accounted for six in forming the bonds. So we have 12 electrons left over to account for, we will then fulfill octets for the outer electrons first or elements first and then the central element. So oxygen has four around it with the double bond. So we need four more. So two pairs of electrons fluorine has a single bond. So it needs six more electrons. So three more pairs. So that gives us a total of 2468, 10 electrons that we've accounted for the remaining two, then go on nitrogen to fulfill its octet the Lewis dot Structure. Then is that provided in answer D thanks for watching. Hope this helps.

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4. Molecular Compounds

Lewis Dot Structures: Multiple Bonds

GOB Chemistry

4. Molecular Compounds

Lewis Dot Structures: Multiple Bonds

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Problem 59d

Textbook Question

Draw the Lewis structure for each of the following molecules:
d. ClNO₂ (N is the central atom)

Verified step by step guidance

Step 1: Count the total number of valence electrons in the molecule. Chlorine (Cl) has 7 valence electrons, nitrogen (N) has 5 valence electrons, and each oxygen (O) has 6 valence electrons. Add these together to determine the total number of valence electrons available for the Lewis structure.

Step 2: Identify the central atom. In this case, nitrogen (N) is the central atom because it is less electronegative than oxygen and chlorine. Place nitrogen in the center and arrange chlorine and the two oxygen atoms around it.

Step 3: Connect the central atom (N) to the surrounding atoms (Cl and O) using single bonds. Each single bond represents 2 electrons. Subtract the electrons used in these bonds from the total valence electrons calculated in Step 1.

Step 4: Distribute the remaining electrons as lone pairs around the outer atoms (Cl and O) to satisfy the octet rule for each atom, starting with the most electronegative atoms (oxygen). Ensure that each oxygen atom has 8 electrons (including bonding and lone pairs).

Step 5: Place any remaining electrons on the central atom (N). If the central atom does not have a full octet, consider forming double bonds between nitrogen and one or more oxygen atoms to satisfy the octet rule for all atoms. Verify that the total number of electrons matches the total valence electrons calculated in Step 1.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Lewis Structure

A Lewis structure is a diagram that represents the bonding between atoms in a molecule and the lone pairs of electrons that may exist. It uses dots to represent valence electrons and lines to represent bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting the behavior of molecules in chemical reactions.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial in determining how an atom bonds with others. The number of valence electrons influences the molecule's reactivity and stability. For ClNO₂, knowing the valence electrons of chlorine, nitrogen, and oxygen helps in accurately constructing the Lewis structure and ensuring that all atoms achieve a stable electron configuration.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is influenced by the number of bonding pairs and lone pairs of electrons around the central atom. Understanding molecular geometry is important for predicting the shape and polarity of the molecule, which can affect its physical and chemical properties, such as reactivity and interaction with other molecules.

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