Write the Lewis structure for each molecule. a. CH 2 O b. C 2 Cl 4 c. CH 3 NH 2 d. CFCl 3 (C central)

Hey everyone, we're asked to draw an appropriate lewis dot structure for each of the following compounds first. Let's go ahead and start off with a carbon tetra chloride. We want to calculate the total number of valence electrons and we know that carbon is in our group four A And since we have one of carbon, this will give us four valence electrons and chlorine is in our group seven A. And since we have four of chlorine, we're going to multiply seven times four And this will get us to a total of 28 valence electrons. When we add these two values up, we get a total of 32 valence electrons. Now let's go ahead and draw out our lewis. Now carbon is going to be our central atom and this is because it is less electro negative than our chlorine And it is going to be connected to four chlorine. And to complete our 32 valence electrons and chlorine states will have to add three lone pairs onto each chlorine. And this will be our final lewis dot structure. Now moving on to be we have water which is H or a total number of valence electrons. We have two of hydrogen. So we're going to multiply one times two which will get us two valence electrons and oxygen is in our group six A. So this will give us six valence electrons in total, we will have eight valence electrons to draw out to draw our lewis structure, even though hydrogen is less electro negative than oxygen, it cannot be our central atom. So oxygen has to be our central atom and we're going to connect to hydrogen is to our oxygen. And to complete those eight valence electrons and oxygen will add two lone pairs onto our oxygen. Next moving on to see we have two of carbon. So we're going to multiply two times four valence electrons since carbon is in our group four A and this will get us to eight valence electrons looking at hydrogen, We're going to multiply six times one since we have six of hydrogen and we're going to get a total of six valence electrons. When we add these two values up, we have to draw out a total of 14 valence electrons. Now our two carbons are going to be connected to one another. And to complete our structure, each carbon will hold three hydrogen and this is going to be our final lewis dot structure. Now for our last compound, we know that carbon is going to give us four valence electrons, oxygen is going to give us six. And since we have four of hydrogen, we're going to multiply one times four and this will get us to four valence electrons drawing this out. We end up with a total of 14 valence electrons. Now our central atoms here are going to be our carbon and our oxygen which are going to be connected to one another with a single bond. Our carbon is going to hold three hydrogen and oxygen is going to hold one hydrogen to complete our 14 valence electrons and oxygen octet will add two lone pairs onto our oxygen. So this is going to be our final lewis dot structures for our compounds. Now, I hope that made sense and let us know if you have any questions.

Ch.10 - Chemical Bonding I: The Lewis Model

Tro - Chemistry: A Molecular Approach 6th Edition

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Ch.10 - Chemical Bonding I: The Lewis Model

Problem 58

Chapter 10, Problem 58

Write the Lewis structure for each molecule. a. CH₂O b. C₂Cl₄ c. CH₃NH₂ d. CFCl₃ (C central)

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1. Identify the total number of valence electrons for each molecule. For example, in CH2O, Carbon has 4 valence electrons, Hydrogen has 1 each (total 2 for 2 Hydrogen atoms), and Oxygen has 6. So, the total number of valence electrons is 4+2+6=12.

2. Draw a skeleton structure of the molecule, placing the least electronegative atom in the center (usually Carbon). Hydrogen and Fluorine are usually terminal atoms. For example, in CH2O, the skeleton would be H-C-O-H.

3. Distribute the valence electrons among the atoms, starting with the outer atoms first. Each bond counts as 2 electrons. Make sure each atom (except Hydrogen) has an octet (8 electrons). For example, in CH2O, after forming single bonds between C-H, C-O, and O-H, we have 4 electrons left. We place these on the Oxygen atom to complete its octet.

4. If there are not enough electrons to give every atom an octet, try multiple bonds (like double or triple bonds). For example, in CH2O, we can form a double bond between Carbon and Oxygen to satisfy the octet rule for Carbon.

5. Repeat these steps for each molecule: C2Cl4, CH3NH2, and CFCl3.

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Key Concepts

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

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They use 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 atoms bond with each other. The number of valence electrons influences the molecule's reactivity and stability. In Lewis structures, it is important to account for all valence electrons to ensure that the structure accurately represents the molecule's electron configuration.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is influenced by the number of bonds and lone pairs around the central atom, which can affect the molecule's physical and chemical properties. Understanding molecular geometry is vital for predicting the behavior of molecules in reactions and their interactions with other substances.