(a) Construct a Lewis structure for hydrogen peroxide, H 2 O 2 , in which each atom achieves an octet of electrons.

Hello Everyone in this video we're trying to draw the lewiS structure for arsenic acid and we have to keep in mind the octet rule. So first things first, let's go ahead and count the valence electrons. So from hydrogen we have three items of hydrogen. Each hydrogen atom will contribute one fans electron. So three times one is equal to three. Now let's do the same thing for arsenic. So we have one item of arsenic. Each atom will contribute five valence electrons. So one times five is five. Now for oxygen we have three items of oxygen. Each will contribute six vans electrons. Three times six is 18. Now we take the sum of all these fans electrons to get a total of fans electrons in our arsenic um acid molecule. Alright, so oxygen prefers to have two bonds and arsenic prefers to have three bonds. So with that in mind we can have arsenic as our central atom connected to three oxygen atoms. And because hydrogen can only be a terminal item since it can only hold two electrons, it will be at the end of our oxygen's. And of course we need to fill in the lone pairs to give it its octet rule and one more long pair on an arsenic to fulfill its octet. So this right here is going to be our final lewis structure for our arsenic acid molecule. Thank you all so much for watching

Ch.8 - Basic Concepts of Chemical Bonding

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Brown 14th Edition

Ch.8 - Basic Concepts of Chemical Bonding

Problem 36a

Chapter 8, Problem 36a

(a) Construct a Lewis structure for hydrogen peroxide, H₂O₂, in which each atom achieves an octet of electrons.

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Identify the total number of valence electrons in the molecule. Hydrogen (H) has 1 valence electron and Oxygen (O) has 6 valence electrons. Therefore, for H2O2, calculate the total valence electrons as: 2(1) + 2(6) = 14 valence electrons.

Arrange the atoms with the least electronegative atom in the center. In H2O2, the structure is linear with the two oxygen atoms in the center: H-O-O-H.

Connect the atoms with single bonds initially. Each single bond represents 2 electrons. So, connect H-O, O-O, and O-H with single bonds, using 8 electrons in total (4 bonds x 2 electrons each).

Distribute the remaining valence electrons to satisfy the octet rule for each atom. Start by placing the remaining electrons around the oxygen atoms to complete their octets. Each oxygen should have 8 electrons around it, including those in bonds.

Check that all atoms have achieved a full valence shell. Hydrogen atoms should have 2 electrons (1 bond), and each oxygen should have 8 electrons (including shared electrons in bonds). Adjust if necessary to ensure all atoms satisfy their respective electron requirements.

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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. Constructing a Lewis structure involves determining the total number of valence electrons, arranging atoms, and ensuring that each atom achieves a stable electron configuration, typically an octet for main group elements.

Octet Rule

The octet rule is a chemical principle that states that atoms tend to bond in such a way that they each have eight electrons in their valence shell, achieving a stable electronic configuration similar to that of noble gases. This rule is particularly applicable to main group elements and guides the formation of covalent bonds, where atoms share electrons to fulfill this requirement.

Valence Electrons

Valence electrons are the electrons in the outermost shell of an atom that are involved in forming bonds with other atoms. The number of valence electrons determines an element's chemical properties and its ability to bond with other elements. In the case of hydrogen peroxide (H2O2), understanding the valence electrons of hydrogen and oxygen is crucial for constructing its Lewis structure and ensuring that all atoms achieve an octet where applicable.