Draw the Lewis structure for each compound. b. H 3 PO 3 (two OH bonds)

Hello everyone. So in this video we have to go ahead and draw the lewis structure for the H. N. 02 compound. First things first, let's go ahead and calculate the total number of electrons. All right so the compound is given to us right over here. So we have one hydrogen atom. Each gives us one valence electron for our nitrogen atom. Each will give us five vance electrons since it's in group 58. And lastly for oxygen, that gives us each six valence electrons in this compound, we have two atoms. So six times two is 12. Now adding 15 and 12. We get a total of 18 valence electrons for this compound now to see which will be our central atom. So first our hydrogen can only have one bond because of the duet role. So that leaves us with nitrogen and oxygen. So we compare the electro negativity. Nitrogen will have a lower electro negativity. So that's gonna be our central atom. So let's go ahead and draw that up. So again we have the nitrogen being our central atom, then it will be connected to an oxygen. And that one of those higher oxygen's can be connected to a hydrogen. So oxygen usually likes to have two bonds. So go ahead and do that for this one again. Out of all these atoms, these three will need to fulfill its octet. This one has already fulfilled its duet role by having this one bond. So let's see here for our nitrogen adam right now it has 123456 valence electrons. Let's go ahead and add one more or two more to fulfill its octet now has eight valence electrons surrounding this atom. It's happy. Let's look at this oxygen right here. So there's 1234. It needs four more. We'll go ahead and add two lone pairs. Now we count all the valence electrons being used. We have 123456789, 10, 11, 12, 13, 14, 15, 16, 17 and 18. Again, we have 18 valence electrons and we have used them all for this compound here. So then this right here will be our final Lewis structure for our HNO two. Thank you all so much for watching.

Ch.9 - Chemical Bonding I: The Lewis Model

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Tro 4th Edition

Ch.9 - Chemical Bonding I: The Lewis Model

Problem 107b

Chapter 9, Problem 107b

Draw the Lewis structure for each compound. b. H₃PO₃ (two OH bonds)

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Count the total number of valence electrons in the molecule. Phosphorus (P) has 5 valence electrons, each hydrogen (H) has 1, and each oxygen (O) has 6. Since there are three hydrogens and three oxygens, the total number of valence electrons is 5 (from P) + 3 (from H) + 18 (from O) = 26 valence electrons.

Place the least electronegative atom in the center, which is phosphorus in this case. Then, attach the oxygen and hydrogen atoms to the central phosphorus atom. Remember that two of the oxygens are bonded to hydrogen as OH groups.

Distribute the electrons around the atoms to complete the octets (or duet for hydrogen) while keeping in mind the total number of valence electrons. Each hydrogen will share two electrons, forming a single bond with oxygen. Each oxygen in the OH groups will form a single bond with hydrogen and a single bond with phosphorus.

Place any remaining electrons on the oxygen atoms to complete their octets. Oxygen typically needs 8 electrons to complete its octet, which includes shared and lone pairs.

Check the formal charges on each atom to ensure the most stable structure. The sum of the formal charges should equal the overall charge of the molecule, which is neutral in this case.

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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 an atom bonds with others. The number of valence electrons influences the atom's ability to form bonds, either by sharing electrons (covalent bonds) or transferring them (ionic bonds). For H3PO3, knowing the valence electrons of hydrogen, phosphorus, and oxygen is key to constructing its Lewis structure accurately.

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 reactivity and properties. In the case of H3PO3, understanding its geometry helps predict how it interacts with other molecules and its overall stability.