Domanda del libro di testo
Which of the following substances would you expect to have
a nonzero dipole moment? Explain, and show the direction
of each.
(a) Cl2O
(b) XeF4
(c) Chloroethane, CH3CH2Cl
(d) BF3
858
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Ch.11 - Liquids & Phase Changes
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 11, Problema 85
Fluorine is more electronegative than chlorine, yet fluoromethane 1CH3F; m = 1.86 D2 has a smaller dipole moment than chloromethane 1CH3Cl; m = 1.90 D2. Explain.
Guida verificata passo dopo passo1
Step 1: Understand the concept of electronegativity. Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons. The higher the electronegativity, the greater the atom's strength to attract a pair of electrons.
Step 2: Understand the concept of dipole moment. The dipole moment of a molecule is the measure of its polarity. It depends on both the magnitude of the charge and the distance between the charges. It is calculated as the product of the charge and the distance between the charges.
Step 3: Consider the structure of fluoromethane (CH3F) and chloromethane (CH3Cl). Both molecules are tetrahedral in shape, with the hydrogen atoms and the halogen atom (F or Cl) surrounding the central carbon atom.
Step 4: Although fluorine is more electronegative than chlorine, the carbon-fluorine bond in fluoromethane is shorter than the carbon-chlorine bond in chloromethane due to the smaller size of the fluorine atom. This means that the separation of charges in fluoromethane is less than in chloromethane.
Step 5: Therefore, despite fluorine's higher electronegativity, the dipole moment of fluoromethane is smaller than that of chloromethane because the dipole moment depends on both the charge difference and the distance between the charges. In this case, the larger distance in chloromethane outweighs the larger charge difference in fluoromethane, resulting in a larger overall dipole moment for chloromethane.
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Electronegativity
Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. Fluorine is the most electronegative element, meaning it has a strong tendency to attract electrons compared to chlorine. This property influences the polarity of bonds formed with other atoms, affecting molecular dipole moments.
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Percorso guidato
02:10
Electronegativity Trends
Dipole Moment
The dipole moment is a vector quantity that measures the separation of positive and negative charges in a molecule. It is influenced by both the magnitude of the charge and the distance between the charges. A higher dipole moment indicates a greater polarity, which can be affected by molecular geometry and the arrangement of atoms within the molecule.
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Percorso guidato
01:25Dipole Moment
Molecular Geometry
Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule. The shape of a molecule can significantly influence its dipole moment, as the spatial distribution of polar bonds determines how the individual dipoles combine. In the case of fluoromethane and chloromethane, differences in geometry can lead to variations in their overall dipole moments despite the electronegativity differences.
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Percorso guidato
01:33Molecular Geometry with Two Electron Groups
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