Domanda del libro di testo
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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TOC.tableOfContents
- 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 1: Properties and Electrophilic Additions158
- Ch. 9 - Alkenes 2: 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 1: Infrared Spectroscopy and Mass Spectrometry54
- Ch. 15 - Structural Identification 2: Nuclear Magnetic Resonance Spectroscopy93
- Ch. 16 - Metals in Organic Chemistry48
- Ch. 17 - Carbonyl Addition Reactions: Aldehydes and Ketones45
- Ch. 18 - Nucleophilic Acyl Substitution 1: Carboxylic Acids18
- Ch. 19 - Nucleophilic Acyl Substitution 2: Carboxylic Acid Derivatives39
- Ch. 20 - Enolates: Carbonyl Addition and Substitution13
- Ch. 21 - Conjugated Systems 1: Stability and Addition Reactions56
- Ch. 22 - Conjugated Systems 2: Pericyclic Reactions54
- Ch. 23 - Benzene 1: Aromatic Stability and Substitution Reactions64
- Ch. 24 - Benzene 2: 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: 9780137566471Non è quello che usi tu?Cambia libro di testo
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Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblema 30a
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblema 30aCapitolo 1, Problema 30a
Calculate the formal charge of the indicated atoms in the ions shown.
Guida verificata passo dopo passo1
Step 1: Recall the formula for calculating formal charge: Formal Charge = (Valence Electrons) - (Non-bonding Electrons) - (1/2 × Bonding Electrons). This formula helps determine the charge on an atom within a molecule or ion.
Step 2: Identify the atom whose formal charge needs to be calculated and determine the number of valence electrons it has based on its position in the periodic table. For example, carbon has 4 valence electrons, oxygen has 6, etc.
Step 3: Count the number of non-bonding electrons (lone pairs) around the atom. These are electrons that are not involved in bonding and are directly associated with the atom.
Step 4: Count the number of bonding electrons (shared electrons in bonds) around the atom. Since each bond consists of two electrons, divide the total bonding electrons by 2 to account for the atom's share.
Step 5: Substitute the values into the formal charge formula and simplify to determine the formal charge of the indicated atom. Repeat this process for each atom in the ion as needed.
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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 half the number of bonding electrons. It helps in determining the most stable structure of a molecule by minimizing the formal charges across the atoms. The formula is: Formal Charge = Valence Electrons - (Non-bonding Electrons + 1/2 Bonding Electrons).
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01:34
Calculating formal and net charge.
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 provide a visual way to understand the arrangement of electrons and the connectivity of atoms, which is essential for calculating formal charges. Drawing accurate Lewis structures is the first step in determining the formal charge of specific atoms.
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04:12Drawing the Lewis Structure for N2H4.
Ionic Species
Ionic species are atoms or molecules that have gained or lost electrons, resulting in a net charge. Understanding the nature of these ions is crucial when calculating formal charges, as the charge affects the distribution of electrons in the Lewis structure. Recognizing whether an ion is positively or negatively charged helps in applying the formal charge formula correctly to the indicated atoms.
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11:33Differences between ionic, polar and covalent bonds
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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.
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