Draw Lewis structures for the following: (d) H 2 SO 4 (H is bonded to O)

Well everybody. So in this video we have to go ahead and draw the Lewis structure for formaldehyde. The molecular form has given to us in the problem as CH 20. So first let's go ahead and calculate for the total number of vans electrons. So for a carbon it's in group 48 will have four valence electrons. For hydrogen is in group one A. So there's going to be one vance electron in our formula we have two atoms. So multiply that number by two and one times two is two. Last year we have our oxygen atom that's in group 68. So I have six valence electrons Adding those three numbers up we get a total of 12 advanced electrons in this molecule. Then we go ahead and start drawing out our lower structure. So out of the three different atoms that we have, our hydrogen atom can only have one bond due to its duet role. Now comparing the carbon and the oxygen atom the carbon is a lot more electro negative or a lot less electro negative. So it can be our central atom. So again we have our carbon Connected to two hydrogen and one oxygen. So oxygen usually likes to have a double bond. So go ahead and do that. So are hydrogen atoms are happy because of the duet rule. They only have one bond. Our carbon needs to fulfill its octet rule and it does have eight valence electrons surrounding it. But for auction adam it needs to long pairs because it only has four Vance electrons because of the double bond. So now we have used all 12 electrons, as we have calculated to the left. And this is going to be my final structure for formaldehyde. 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 47d

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Chapter 8, Problem 47d

Draw Lewis structures for the following: (d) H₂SO₄ (H is bonded to O)

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Identify the total number of valence electrons in the molecule. For H<sub>2</sub>SO<sub>4</sub>, hydrogen (H) has 1 valence electron, sulfur (S) has 6, and oxygen (O) has 6. Since there are 2 hydrogens and 4 oxygens, the total number of valence electrons is 2(1) + 6 + 4(6) = 32 electrons.

Place sulfur (S) in the center as it is the least electronegative element (excluding hydrogen which generally forms only one bond). Arrange the oxygen atoms around sulfur and place the hydrogen atoms bonded to two of the oxygen atoms.

Form single bonds between sulfur and each oxygen, and between hydrogen and oxygen. Each single bond uses 2 electrons. After forming these bonds, subtract the used electrons from the total valence electrons.

Complete the octets of the oxygen atoms by adding lone pairs. Each oxygen should have a total of 8 electrons around it, including the bonding electrons.

Check the formal charges and adjust the structure if necessary to minimize charges, keeping in mind that sulfur can have an expanded octet (more than 8 electrons around it).

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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 H2SO4, knowing the valence electrons of hydrogen, sulfur, and oxygen helps in accurately constructing its Lewis structure.

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 important for predicting the shape of H2SO4 and how it interacts with other substances.

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Textbook Question

Which one of these statements about formal charge is true? (a) Formal charge is the same as oxidation number. (b) To draw the best Lewis structure, you should minimize formal charge. (c) Formal charge takes into account the different electronegativities of the atoms in a molecule. (d) Formal charge is most useful for ionic compounds. (e) Formal charge is used in calculating the dipole moment of a diatomic molecule.

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Draw Lewis structures for the following: (d) H2SO4 (H is bonded to O)

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Key Concepts

Lewis Structures

Valence Electrons

Molecular Geometry

Draw Lewis structures for the following: (d) H₂SO₄ (H is bonded to O)