Molecular polarity arises from unequal sharing of electrons in a molecule, creating partial positive ($δ^+$) and partial negative ($δ^−$) charges. These polar molecules exhibit dipole-dipole interactions, which are attractive forces between the positive end of one polar molecule and the negative end of another. The strength of these interactions influences physical properties like boiling point and solubility. Understanding these concepts is crucial for predicting molecular behavior in chemical systems.
Match the term with its correct definition:
| Term | Definition |
|---|---|
| 1. Dipole Moment | A. Attractive forces between polar molecules |
| 2. Electronegativity | B. A molecule with an uneven distribution of charge |
| 3. Polar Molecule | C. The ability of an atom to attract electrons in a chemical bond |
| 4. Dipole-Dipole Interactions | D. A measure of the polarity of a molecule |
| 5. Nonpolar Molecule | E. A molecule with an even distribution of charge |
Match the correct term with the definition: 1-D, 2-C, 3-B, 4-A, 5-E
Complete the following paragraph using the words: Electronegativity, Dipole-Dipole, Polar, Nonpolar, Intermolecular.
A molecule is considered _______ if it has an uneven distribution of electron density. This uneven distribution results from differences in _______ between the atoms in the molecule. These molecules experience _______ forces, which are a type of _______ force. In contrast, _______ molecules have an even distribution of electron density.
Answer: Polar, Electronegativity, Dipole-Dipole, Intermolecular, Nonpolar
Explain how the strength of dipole-dipole interactions affects the boiling point of a liquid. Provide an example to illustrate your explanation.
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