Write the Lewis structure for each molecule. d. CH 3 SH (C and S central)

Hey everyone, we're being asked to draw the Lewis structure of the following compound and were told that our skeletal structure will look like this. So our skeletal structure is basically telling us how our atoms are going to be connected. So based on this, we know that our carbon and our phosphorus are going to be connected And we're going to have three hydrogen connected to our carbon. And looking at our phosphorus, we also have two Hydrogen surrounding it. Now counting our valence electrons per atom are hydrogen are going to be good since they all have one valence electron for our carbon. We have 123 and four, which is good since carbon is in our group. For a. Now for phosphorus phosphorus is in our group five a. So we should get five. So phosphorus has 123. Now in order to get our five failed electrons will need to add a lone pair around our phosphorus. So I hope this made sense. And let us know if you have any questions

Ch.10 - Chemical Bonding I: The Lewis Model

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Ch.10 - Chemical Bonding I: The Lewis Model

Problem 53d

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Chapter 10, Problem 53d

Write the Lewis structure for each molecule. d. CH₃SH (C and S central)

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Identify the total number of valence electrons in the molecule. Carbon (C) has 4 valence electrons, each hydrogen (H) has 1, and sulfur (S) has 6. Calculate the total valence electrons for CH_3SH.

Determine the central atoms. In this case, both carbon (C) and sulfur (S) are central atoms, with carbon bonded to three hydrogens and sulfur bonded to one hydrogen.

Draw a skeletal structure. Connect the carbon atom to three hydrogen atoms and the sulfur atom. Then, connect the sulfur atom to the remaining hydrogen atom.

Distribute the remaining valence electrons to satisfy the octet rule for each atom, starting with the outer atoms (hydrogens and sulfur) and then the central atoms (carbon and sulfur).

Check that all atoms have a complete valence shell: hydrogen should have 2 electrons, while carbon and sulfur should have 8 electrons. Adjust any lone pairs or bonds if necessary to ensure all atoms satisfy the octet rule.

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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 atom's reactivity and the types of bonds it can form. In the case of CH3SH, knowing the valence electrons of carbon, hydrogen, and sulfur helps in constructing the correct Lewis structure.

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 molecules, which can affect their physical and chemical properties.