Domanda del libro di testo
(b) An AB4 molecule has two lone pairs of electrons on the A atom (in addition to the four B atoms). What is the electron-domain geometry around the A atom?
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Ch.9 - Molecular Geometry and Bonding Theories
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 9, Problema 20
Would you expect the nonbonding electron-pair domain in NH3 to be greater or less in size than the corresponding one in PH3?
Guida verificata passo dopo passo1
Identify the central atoms in NH3 and PH3, which are nitrogen (N) and phosphorus (P), respectively.
Recall that nonbonding electron pairs, also known as lone pairs, occupy more space than bonding pairs due to their higher electron density and lack of shared attraction to another nucleus.
Consider the position of nitrogen and phosphorus in the periodic table. Nitrogen is in the second period, while phosphorus is in the third period.
Understand that atoms in higher periods have larger atomic radii and more diffuse electron clouds, which can affect the size of the electron-pair domains.
Conclude that the nonbonding electron-pair domain in NH3 is expected to be smaller than in PH3 because nitrogen's lone pairs are closer to the nucleus and more compact compared to the more diffuse lone pairs in phosphorus.
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VSEPR Theory
Valence Shell Electron Pair Repulsion (VSEPR) Theory is used to predict the geometry of molecules based on the repulsion between electron pairs. Nonbonding electron pairs, or lone pairs, occupy more space than bonding pairs, influencing the overall shape of the molecule. In NH3 and PH3, the presence of lone pairs affects the bond angles and molecular geometry.
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02:13
Molecular Shapes and VSEPR
Atomic Size and Electronegativity
Atomic size generally increases down a group in the periodic table due to the addition of electron shells. In NH3, nitrogen is smaller and more electronegative than phosphorus in PH3, which affects the size of the nonbonding electron-pair domain. The greater size of the phosphorus atom leads to a larger nonbonding electron-pair domain compared to nitrogen.
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02:10Electronegativity Trends
Hybridization
Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate bonding and lone pairs. In NH3, nitrogen undergoes sp3 hybridization, resulting in a tetrahedral arrangement with one lone pair, while PH3 has less effective hybridization, leading to a different spatial arrangement. This difference in hybridization affects the size and spatial distribution of the nonbonding electron-pair domain.
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00:51Hybridization
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Domanda del libro di testo
b. The NH3 molecule is trigonal pyramidal, while BF3 is trigonal planar. Which of these molecules is flat?
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Domanda del libro di testo
Describe the bond angles to be found in each of the following molecular structures: (a) trigonal planar, (b) tetrahedral, (c) octahedral, (d) linear.
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Domanda del libro di testo
In which of the following molecules can you confidently predict the bond angles about the central atom, and for which would you be a bit uncertain? Explain in each case. (a) H2S, (b) BCl3, (c) CH3I, (d) CBr4, (e) TeBr4.
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