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An overview of electronegativity, its relationship with electron affinity and bond character, and how it impacts the formation of polar and nonpolar covalent bonds. The document also discusses intramolecular and intermolecular forces, including dispersion forces, dipole-dipole interactions, and hydrogen bonds, and their relative strengths.
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Increases across a period Decreases down a group This is why your halogens create anions – they have high electron affinities!
Increases across a period Decreases down a group Most electronegative = F
Electronegativity Difference Bond Character
1.7 Mostly Ionic 0.4 – 1.7 Polar Covalent < 0.4 Mostly Covalent 0 Nonpolar Covalent
Nonpolar covalent bond - nuclei of atoms pull on electrons equally; bonding electrons are shared
Polarity of a molecule depends on the individual bonds and the shape of the overall molecule. If the polar bonds are symmetrical, the polarity cancels out and the overall molecule is nonpolar. If the polar bonds are asymmetric, the polarity persists in the molecule.
Inter – between
Dispersion Forces – weak forces that result from temporary shifts in the density of electrons in electron clouds Larger molecules experience larger dispersion forces Dipole-dipole – attractions between oppositely charged regions of polar molecules Hydrogen Bonds – dipole-dipole attraction between molecules with a H bonded to a small, electronegative atom that has one lone electron pair H bonded to a F, O, or N From weakest to strongest: Dispersion Dipole-dipole Hydrogen Bonds
Stronger the force, the more energy is needed to break the bond Energy needed to break a metallic or an ionic bond will be much higher than the energy needed to break a covalent bond Separating NaCl will require more energy than separating CO 2 Energy needed to overcome intermolecular forces will increase with an increase in force strength Boiling H 2 O will require more energy than boiling H 2 S because H 2 O experiences hydrogen bonding and H 2 S experiences only a slight dipole-dipole