Draw Lewis structures for the following compounds. e. dimethylamine, CH 3 NHCH 3 f. diethyl ether, CH 3 CH 2 OCH 2 CH 3 g. 1-chloropropane,CH 3 CH 2 CH 2 Cl

Welcome back, everyone draw the Louis structures. We're given three compounds and we're going to begin with the first one. According to the problem, we want to draw the structure of the ethyl amine. And because we're not given any parentheses in the given condensed formula, we have to recognize that this is a condensed formula. We can simply begin by drawing our parent chain excluding all of the hydrogens. So we have carbon, carbon, nitrogen, carbon and another carbon. So we can just draw carbon bonded to carbon bonded to nitrogen. So let's include letter M followed by two carbons. Now, what we're going to do from here is simply add the missing hydrogens. So we know that we can read a condensed formula from left to right. If we look at the left, we have CH three, which means that carbon is bonded to three hydrogens. So we're just going to add them, every carbon must have four bonds, right? So we are done with CH three followed by CH two. We simply want to add two hydrogens, followed by NH we want to add hydrogen bonded to nitrogen and we want to recall that nitrogen must have three bonds and a long pair of electrons based on the octet rule. So we have also added a long pair and then we have ch two, so two more hydrogens in siege three, three more hydrogens. This is how we get our first one and we can move on to the second one. Once again, we are given a condensed formula of the muscle ether. There are no brain c so we can just draw a parent chain coc excluding all of the hydrogens. That'll be coc. Now, let's add three hydrogens to each carbon because we are given siege, we which is a methyl group and another c another siege three on the other side of oxygen. And from here, we once again have to recall that similarly, it's not and oxygen will have two lone pairs and two bonds based on the octet rule. So we have our Louis structure and we can move on to the final one. The final one is one bromo ethane. And if we exclude hydrogens, we have carbon carbon bromine. So we are just going to draw carbon bond it to carbon, wanted to bromine. And let's simply add three hydrogens to the first carbon because it's ch three and two Hagens. The second one because it's siege two. So each carbon has four bonds. What about bromine? It's a halogen. So it will have one bond and three lo pairs based on the octet rule. Well, then, so we have our le structures, let's label them as our final answers. That would be it for today. And thank you for watching.

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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
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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
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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

Lewis Structure

Organic Chemistry

1. A Review of General Chemistry

Lewis Structure

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3:41 minutes

Problem 2e,f,g

Textbook Question

Draw Lewis structures for the following compounds.
e. dimethylamine, CH₃NHCH₃
f. diethyl ether, CH₃CH₂OCH₂CH₃
g. 1-chloropropane,CH₃CH₂CH₂Cl

Verified step by step guidance

To draw the Lewis structure for dimethylamine (CH3NHCH3), start by identifying the central atom, which is nitrogen (N). Connect the nitrogen atom to two methyl groups (CH3) and one hydrogen atom (H). Ensure that nitrogen has a lone pair of electrons to complete its octet.

For diethyl ether (CH3CH2OCH2CH3), identify the central atom as oxygen (O). Connect the oxygen atom to two ethyl groups (CH3CH2). Each carbon atom in the ethyl groups should form four bonds, and the oxygen should have two lone pairs to complete its octet.

In the case of 1-chloropropane (CH3CH2CH2Cl), start by drawing a three-carbon chain. Attach a chlorine atom (Cl) to the terminal carbon atom. Ensure that each carbon atom forms four bonds, and the chlorine atom has three lone pairs to complete its octet.

For each compound, ensure that all hydrogen atoms are connected to carbon atoms, and each carbon atom forms four bonds, either with hydrogen, carbon, or other atoms like nitrogen, oxygen, or chlorine.

Check that all atoms satisfy the octet rule (except hydrogen, which follows the duet rule) and that the total number of valence electrons used in the structure matches the sum of valence electrons for each atom in the compound.

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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 of a molecule and the lone pairs of electrons that may exist. They are essential for visualizing the arrangement of atoms, the distribution of electrons, and the types of bonds (single, double, or triple) in a molecule. Understanding how to draw Lewis structures helps in predicting the geometry, reactivity, and properties of the compound.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial in forming chemical bonds. In drawing Lewis structures, it is important to account for all valence electrons to ensure that each atom achieves a stable electron configuration, often resembling the nearest noble gas. This involves distributing electrons to satisfy the octet rule for most atoms, except for hydrogen, which follows the duet rule.

Functional Groups

Functional groups are specific groups of atoms within molecules that have characteristic properties and reactivity. In organic chemistry, recognizing functional groups like amines, ethers, and halides is essential for understanding the behavior of molecules. For example, dimethylamine contains an amine group, diethyl ether contains an ether group, and 1-chloropropane contains a halide group, each influencing the molecule's chemical properties and interactions.

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