Textbook Question
Draw in all missing lone pairs for the following molecules.
(a)
2
views
Ch. 3 - Alkanes and Cycloalkanes: Properties and Conformational Analysis
Mullins1st EditionOrganic Chemistry: A Learner Centered ApproachISBN: 9780137566471
Not the one you use?Change textbookSelect a different textbook
Table of contents
- Ch. 2 - General Chemistry Translated: Finding the Electrons114
- Ch. 3 - Alkanes and Cycloalkanes: Properties and Conformational Analysis109
- Ch. 4 - Acids and Bases: Electron Flow144
- Ch. 5 - Chemical Reaction Analysis: Thermodynamics and Kinetics118
- Ch. 6 - Stereoisomerism: Arrangement of Atoms in Space112
- Ch. 7 - Principles of Green (Organic) Chemistry3
- Ch. 8 - Alkenes I: Properties and Electrophilic Additions158
- Ch. 9 - Alkenes II: Oxidation and Reduction150
- Ch. 10 - Alkynes: Electrophilic Addition and Redox Reactions101
- Ch. 11 - Properties and Synthesis of Alkyl Halides: Radical Reactions108
- Ch. 12 - Substitution and Elimination: Reactions of Haloalkanes172
- Ch. 13 - Alcohols, Ethers and Related Compounds: Substitution and Elimination239
- Ch. 14 - Structural Identification I: Infrared Spectroscopy and Mass Spectrometry54
- Ch. 15 - Structural Identification II: Nuclear Magnetic Resonance Spectroscopy93
- Ch. 16 - Metals in Organic Chemistry48
- Ch. 17 - Carbonyl Addition Reactions: Aldehydes and Ketones45
- Ch. 18 - Nucleophilic Acyl Substitution I: Carboxylic Acids18
- Ch. 19 - Nucleophilic Acyl Substitution II: Carboxylic Acid Derivatives39
- Ch. 20 - Enolates: Carbonyl Addition and Substitution13
- Ch. 21 - Conjugated Systems I: Stability and Addition Reactions56
- Ch. 22 - Conjugated Systems II: Pericyclic Reactions54
- Ch. 23 - Benzene I: Aromatic Stability and Substitution Reactions64
- Ch. 24 - Benzene II: Reactions Influenced by the Aromatic Ring62
- Ch. 25 - Amines: Structure, Reactions, and Synthesis27
- Ch. 26 - Amino Acids, Proteins, and Peptide Synthesis9
- Ch. 27 - Carbohydrates, Nucleic Acids, and Lipids54
Mullins1st EditionOrganic Chemistry: A Learner Centered ApproachISBN: 9780137566471Not the one you use?Change textbook
All textbooks
Mullins 1st EditionCh. 3 - Alkanes and Cycloalkanes: Properties and Conformational AnalysisProblem 49d
Mullins 1st EditionCh. 3 - Alkanes and Cycloalkanes: Properties and Conformational AnalysisProblem 49dChapter 2, Problem 49d
Draw in all missing lone pairs for the following molecules.
(d) 
Verified step by step guidance1
Step 1: Identify the atoms in the molecule that typically have lone pairs. In this structure, chlorine (Cl) is the atom that will have lone pairs because it is a halogen and typically has three lone pairs when bonded to one other atom.
Step 2: Recall that chlorine has seven valence electrons. When it forms a single bond, one electron is shared with the bonded atom, leaving six electrons to be arranged as three lone pairs.
Step 3: Draw the three lone pairs around the chlorine atom. These lone pairs should be evenly spaced to minimize electron repulsion, forming a tetrahedral-like arrangement with the bond.
Step 4: Examine the rest of the molecule. The positively charged carbon (indicated by the '+' sign) does not have lone pairs because it has lost an electron, resulting in a formal positive charge.
Step 5: Verify the structure to ensure that all atoms follow the octet rule where applicable, and that the formal charges are consistent with the given structure.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Was this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Lone Pairs
Lone pairs are pairs of valence electrons that are not involved in bonding and are localized on a single atom. They play a crucial role in determining the geometry and reactivity of molecules. Understanding how to identify and represent lone pairs is essential for accurately drawing molecular structures.
Recommended video:
Guided course
02:04
Heterocycles - Which lone pairs react?
Lewis Structures
Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons. They provide a visual way to understand the arrangement of electrons and the connectivity of atoms. Mastery of drawing Lewis structures is fundamental in organic chemistry for predicting molecular behavior and reactivity.
Recommended video:
Guided course
04:12Drawing the Lewis Structure for N2H4.
Valence Electrons
Valence electrons are the outermost electrons of an atom and are involved in forming bonds with other atoms. The number of valence electrons determines how an atom can bond and interact with others. Knowing how to count and distribute valence electrons is key to constructing accurate molecular representations.
Recommended video:
Guided course
03:40Valence Electrons of Transition Metals
Related Practice
Textbook Question
Given the first Newman projection and the direction and degree of rotation, fill in the resulting Newman projection. [One substituent has been labeled for you.]
(d)
2
views
Textbook Question
Given the first Newman projection and the direction and degree of rotation, fill in the resulting Newman projection. [One substituent has been labeled for you.]
(a)
2
views
Textbook Question
Draw in all missing lone pairs for the following molecules.
(c)
3
views
Textbook Question
Draw in all missing lone pairs for the following molecules.
(b)
1
views
Textbook Question
Given the first Newman projection and the direction and degree of rotation, fill in the resulting Newman projection. [One substituent has been labeled for you.]
(h)
2
views