Textbook Question
Classify each species as either a Lewis acid or a Lewis base. a. Fe3+ b. BH3 c. NH3 d. F-
Ch.17 - Acids and Bases
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving90
- Ch.2 - Atoms & Elements94
- Ch.3 - Molecules and Compounds103
- Ch.4 - Chemical Reactions and Chemical Quantities46
- Ch.5 - Introduction to Solutions and Aqueous Solutions65
- Ch.6 - Gases100
- Ch.7 - Thermochemistry85
- Ch.8 - The Quantum-Mechanical Model of the Atom51
- Ch.9 - Periodic Properties of the Elements79
- Ch.10 - Chemical Bonding I: The Lewis Model70
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory68
- Ch.12 - Liquids, Solids & Intermolecular Forces44
- Ch.13 - Solids & Modern Materials42
- Ch.14 - Solutions77
- Ch.15 - Chemical Kinetics88
- Ch.16 - Chemical Equilibrium57
- Ch.17 - Acids and Bases121
- Ch.18 - Aqueous Ionic Equilibrium126
- Ch.19 - Free Energy & Thermodynamics80
- Ch.20 - Electrochemistry87
- Ch.21 - Radioactivity & Nuclear Chemistry61
- Ch.22 - Organic Chemistry114
Chapter 17, Problem 126
Which is a stronger base, PO4^3- or AsO4^3-? Explain.
Verified step by step guidance1
Consider the periodic trend of electronegativity: Electronegativity generally decreases as you move down a group in the periodic table.
Identify the position of phosphorus (P) and arsenic (As) in the periodic table: Phosphorus is above arsenic in Group 15.
Compare the electronegativity of phosphorus and arsenic: Phosphorus is more electronegative than arsenic.
Relate electronegativity to base strength: A more electronegative central atom will hold onto its electrons more tightly, making the conjugate base weaker.
Conclude which is the stronger base: Since arsenic is less electronegative than phosphorus, AsO4^3- is a stronger base than PO4^3-.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Acid-Base Theory
Acid-base theory explains the behavior of acids and bases in chemical reactions. According to the Brønsted-Lowry theory, an acid is a proton donor, while a base is a proton acceptor. The strength of a base is determined by its ability to accept protons, which is influenced by its structure and the stability of its conjugate acid.
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Bronsted-Lowry Acid-Base Theory
Conjugate Acid Stability
The stability of a conjugate acid plays a crucial role in determining the strength of a base. A more stable conjugate acid indicates a stronger base, as it is less likely to donate protons back to the solution. Factors affecting stability include electronegativity, resonance, and the overall charge distribution within the molecule.
Comparative Basicity of Anions
When comparing the basicity of anions like PO4^3- and AsO4^3-, one must consider the central atom's electronegativity and size. Phosphorus (P) is less electronegative than arsenic (As), which can lead to a stronger basic character for PO4^3- due to its ability to stabilize the negative charge more effectively than AsO4^3-.
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