Draw a Lewis structure for each of the following: c. (CH 3 ) 2 CHCH(CH 3 )CH 2 C(CH 3 ) 3

All right. Hi, everyone. So this question is asking us to give the structure of the given. And here we have the condensed formula of 2235 tetra methyl hexane. Now, here we are given a condensed formula and our task is to convert this into a Lewis structure. Now recall that in a condensed formula, carbon, carbon and carbon, hydrogen bonds are not explicitly shown instead, atoms in a given compound are grouped together without necessarily showing their bonds. This means that carbon and hydrogen atoms are grouped together, which means that C three, for example, indicates that three hydrogens are connecting to that specific carbon and so on. Now, sometimes we come across groups that are written in parentheses, but the meaning of them depends on the context parentheses with no subscripts indicates that that is a substituent branching off of the parent chain. Parentheses with subscripts tell you there are multiple branches and repeating CH two units enclosed in parentheses with a subscript N indicates multiple repeating CH two units within a parent chain. Now a Lewis structure by contrast showcases all possible bonds and all atoms present within a compound loan pairs of electrons and formal charges are also shown. So in considering our given compound, we have 2235 tetra methyl hexane. So the first thing were going to do is go ahead and label the carbons in our parent chain. So we're going to start by drawing out all six carbon atoms connected to each other. Now, I made the bonds in between them quite long to make sure that I have enough space for my substituents. So let's go ahead and add substituents. We have two methyl groups. That's two ch three groups branching off of the second carbon in the parent chain. So that's two carbon atoms with three hydrogens bound to them. So now on the third carbon of the parent chain, we have another methyl group. So that's another ch three group. And lastly, we have one more methyl group on carbon five. So now that substituents have been added, let's go ahead and add the hydrogens on each of the remaining carbon atoms. Carbon one has three hydrogens associated to it. Carbon two has zero. Carbon three has only one. Carbon, four, has two, carbon, five, has one and carbon six has three. So now that all bonds have been added, loan pairs of electrons and formal charges are located and calculated if necessary. But recall that hydrogen can only share one electron, which means that it can only create one covalent bond carbon. On the other hand, is tetravalent, which means that it prefers to have four bonds in order to remain neutral. And what you'll notice is that all carbon atoms have four bonds and all hydrogen atoms have only one bond because all atoms are in line with their bonding preferences, their formal charges are going to be zero. But just for the record, lets go ahead and recall the formula of formal charge, formal charge or FC is equal to the number of valence electrons subtracted by the number of non bonding electrons that the lone pairs and also subtracted by the number of bonds. So this is the formula for formal charge. But because carbon or all carbon and hydrogen atoms are in line with their bonding preferences, then their formal charge is going to be zero and there you have it here is our complete Lewis structure. And so with that being said, thank you so very much for watching. And I hope you found this helpful.

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1. A Review of General Chemistry5h 5m
2. Molecular Representations1h 14m
3. Acids and Bases2h 46m
4. Alkanes and Cycloalkanes4h 17m
5. Chirality3h 39m
6. Thermodynamics and Kinetics1h 22m
7. Substitution Reactions1h 48m
8. Elimination Reactions2h 30m
9. Alkenes and Alkynes2h 9m
10. Addition Reactions3h 19m
11. Radical Reactions1h 58m
12. Alcohols, Ethers, Epoxides and Thiols2h 42m
13. Alcohols and Carbonyl Compounds2h 17m
14. Synthetic Techniques1h 26m
15. Analytical Techniques:IR, NMR, Mass Spect7h 3m
16. Conjugated Systems6h 13m
17. Ultraviolet Spectroscopy51m
18. Aromaticity2h 34m
19. Reactions of Aromatics: EAS and Beyond5h 1m
20. Phenols55m
21. Aldehydes and Ketones: Nucleophilic Addition4h 56m
22. Carboxylic Acid Derivatives: NAS2h 51m
23. The Chemistry of Thioesters, Phophate Ester and Phosphate Anhydrides1h 10m
24. Enolate Chemistry: Reactions at the Alpha-Carbon1h 53m
25. Condensation Chemistry2h 9m
26. Amines1h 43m
27. Heterocycles2h 0m
28. Carbohydrates5h 53m
29. Amino Acids4h 20m
30. Peptides and Proteins2h 42m
31. Catalysis in Organic Reactions1h 30m
32. Lipids 2h 50m
33. The Organic Chemistry of Metabolic Pathways2h 52m
34. Nucleic Acids1h 32m
35. Transition Metals6h 14m
36. Synthetic Polymers1h 49m

1. A Review of General Chemistry

Condensed Structural Formula

Organic Chemistry

1. A Review of General Chemistry

Condensed Structural Formula

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6:17 minutes

Problem 66c

Textbook Question

Draw a Lewis structure for each of the following:
c. (CH₃)₂CHCH(CH₃)CH₂C(CH₃)₃

Verified step by step guidance

Step 1: Identify the molecular formula and structure. The given compound is (CH3)2CHCH(CH3)CH2C(CH3)3. This is a branched alkane, and the structure can be broken down into groups: two methyl groups (CH3) attached to a CH group, followed by another CH group with a methyl group attached, then a CH2 group, and finally a carbon atom bonded to three methyl groups.

Step 2: Start with the main carbon chain. The main chain consists of six carbon atoms. Arrange these carbons in a linear fashion: C-C-C-C-C-C.

Step 3: Add substituents to the main chain. Attach the substituents (methyl groups) to the appropriate carbon atoms as indicated in the molecular formula. For example, two methyl groups are attached to the first CH group, one methyl group is attached to the second CH group, and three methyl groups are attached to the last carbon atom.

Step 4: Complete the valence of each carbon atom by adding hydrogen atoms. Each carbon atom should have a total of four bonds. For example, if a carbon atom is bonded to three other carbons, it will need one hydrogen atom to complete its valence.

Step 5: Verify the structure. Ensure that all carbon atoms have four bonds and that the total number of hydrogen atoms matches the molecular formula. The final structure should represent the correct connectivity and satisfy the octet rule for all atoms involved.

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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 electrons and lines to represent bonds, allowing chemists to visualize the arrangement of atoms and the distribution of electrons. Understanding how to draw Lewis structures is essential for predicting molecular geometry and reactivity.

Alkane Structure

Alkanes are saturated hydrocarbons consisting only of carbon and hydrogen atoms, connected by single bonds. The general formula for alkanes is CnH2n+2, where 'n' is the number of carbon atoms. Recognizing the structure of alkanes is crucial for drawing their Lewis structures, as it helps identify the number of hydrogen atoms attached to each carbon and the overall molecular shape.

Tertiary and Quaternary Carbons

In organic chemistry, carbon atoms can be classified based on the number of other carbon atoms they are bonded to. A tertiary carbon is bonded to three other carbons, while a quaternary carbon is bonded to four. Identifying these types of carbons is important when drawing Lewis structures, as it influences the connectivity and branching of the molecule, affecting its chemical properties.

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