Domanda del libro di testo
Explain why the properties of boron differ so markedly from the properties of the other group 3A elements.
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Ch.22 - The Main Group Elements
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Capitolo 22, Problema 22.113
Compare and contrast the properties of ammonia and phosphine.
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Identify the chemical formulas for ammonia and phosphine: Ammonia is NH₃ and phosphine is PH₃.
Compare the molecular geometry: Both ammonia and phosphine have a trigonal pyramidal shape due to the presence of a lone pair on the nitrogen and phosphorus atoms, respectively.
Discuss the polarity: Ammonia is polar due to the difference in electronegativity between nitrogen and hydrogen, while phosphine is less polar because the electronegativity difference between phosphorus and hydrogen is smaller.
Examine the hydrogen bonding: Ammonia can form hydrogen bonds due to the presence of highly electronegative nitrogen, whereas phosphine cannot form hydrogen bonds as effectively because phosphorus is less electronegative.
Compare the boiling points: Ammonia has a higher boiling point than phosphine due to the presence of hydrogen bonding, which requires more energy to break compared to the weaker van der Waals forces in phosphine.
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Molecular Structure and Polarity
Ammonia (NH3) and phosphine (PH3) have distinct molecular structures that influence their properties. Ammonia has a trigonal pyramidal shape due to the presence of a lone pair on nitrogen, making it polar and capable of hydrogen bonding. In contrast, phosphine has a similar structure but is less polar due to phosphorus's larger size and lower electronegativity, resulting in weaker intermolecular forces.
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Percorso guidato
02:38
Molecular Polarity
Boiling Points and Volatility
The boiling points of ammonia and phosphine differ significantly due to their molecular interactions. Ammonia has a higher boiling point (−33.34 °C) because of strong hydrogen bonds, while phosphine has a lower boiling point (−87.7 °C) due to weaker van der Waals forces. This difference in boiling points reflects their volatility and stability as gases at room temperature.
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03:05Boiling Point Elevation
Reactivity and Chemical Behavior
Ammonia and phosphine exhibit different reactivities due to their molecular characteristics. Ammonia is a strong base and can readily donate a proton, participating in various acid-base reactions. Phosphine, on the other hand, is less basic and more stable, making it less reactive under similar conditions. This difference affects their roles in chemical reactions and their applications in various fields.
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03:31Chemical Properties
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