Intermolecular forces, electronegativity and bond properties
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Define electronegativity.
Electronegativity is the measure of the ability of an atom in a chemical compound to attract electrons in a covalent bond. The Pauling scale is commonly used, with fluorine being the most electronegative element.
Explain how electronegativity differences lead to bond polarity.
When there's a significant electronegativity difference between two bonded atoms, the more electronegative atom attracts electron density, resulting in a partial negative charge (δ-) and the other atom a partial positive charge (δ+). This creates a polar covalent bond.
What is a dipole moment?
A dipole moment is a measure of the polarity of a molecule. It arises when there is an uneven distribution of electron density, creating a separation of charge. It's a vector quantity with both magnitude and direction.
How can a molecule with polar bonds be nonpolar overall?
If the individual bond dipoles within a molecule cancel each other out due to the molecule's symmetry, the overall dipole moment is zero, and the molecule is nonpolar. CO₂ is an example, despite having polar C=O bonds.
List the relative strengths of ionic, covalent, metallic bonding, and intermolecular forces.
Ionic, covalent and metallic bonds are stronger than intermolecular forces. The relative order is generally: Ionic > Metallic > Covalent >> Intermolecular forces.
Give examples of compounds with each of the following: ionic, covalent, and metallic bonding.
Ionic: NaCl (sodium chloride). Covalent: CH₄ (methane). Metallic: Fe (iron).
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