Textbook Question
Draw the Lewis structure for the following ions. Be sure to calculate the formal charge of each atom to confirm that your structure is correct.
(c) BH4-
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Ch. 2 - General Chemistry Translated: Finding the Electrons
Mullins1st EditionOrganic Chemistry: A Learner Centered ApproachISBN: 9780137566471
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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
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Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 29d
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 29dChapter 1, Problem 29d
Draw the Lewis structure for the following ions. Be sure to calculate the formal charge of each atom to confirm that your structure is correct.
(d) AlCl4-
Verified step by step guidance1
Step 1: Identify the total number of valence electrons in the AlCl⁻₄ ion. Aluminum (Al) has 3 valence electrons, each chlorine (Cl) has 7 valence electrons, and the negative charge adds 1 extra electron. Calculate the total number of valence electrons: 3 + (7 × 4) + 1.
Step 2: Place Aluminum (Al) as the central atom since it is less electronegative than chlorine. Arrange the four chlorine atoms around the aluminum atom.
Step 3: Draw single bonds between the Aluminum atom and each of the four Chlorine atoms. Each single bond represents 2 electrons, so subtract these electrons from the total valence electron count.
Step 4: Distribute the remaining electrons as lone pairs around the chlorine atoms to satisfy the octet rule for each chlorine. Ensure that all chlorine atoms have 8 electrons (including bonding electrons).
Step 5: Calculate the formal charge for each atom using the formula: Formal charge = (Valence electrons) - (Non-bonding electrons) - (Bonding electrons ÷ 2). Verify that the sum of the formal charges equals the overall charge of the ion (-1).
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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 reactivity.
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Drawing the Lewis Structure for N2H4.
Formal Charge
Formal charge is a theoretical charge assigned to an atom in a molecule, calculated based on the number of valence electrons, the number of non-bonding electrons, and the number of bonds. It helps in assessing the stability of a Lewis structure; ideally, the formal charges should be minimized and should reflect the actual charge distribution in the molecule.
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Ionic Compounds
Ionic compounds are formed when atoms transfer electrons, resulting in the formation of charged ions. In the case of AlCl₄⁻, aluminum donates electrons to chlorine atoms, creating a negatively charged ion. Understanding the nature of ionic compounds is crucial for predicting their properties and behavior in chemical reactions.
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Related Practice
Textbook Question
Calculate the formal charge of the indicated atom in the following molecules or ions.
(f)
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Textbook Question
Draw the Lewis structure for the following ions. Be sure to calculate the formal charge of each atom to confirm that your structure is correct.
(b) H+
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Textbook Question
Calculate the formal charge on the non-hydrogen atoms in the molecules shown. Use the arrow-pushing formalism to 'move' an electron pair such that it is shared between two (formerly) charged atoms. Your arrow should account for the formation of the molecule on the right from the molecule on the left.
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Textbook Question
Calculate the formal charge of the indicated atoms in the ions shown.
2
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Textbook Question
You drew the Lewis structures of the following compounds and ion in Assessment 2.32. Predict their shapes around the central atom based on the Lewis structure.
(c) HCO2H
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