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Learn about polar and nonpolar covalent bonds, how electronegativity affects polarity, and how to determine if a molecule is polar or nonpolar based on its shape and bond polarities. Explore examples and the concept of dipole moments.
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Molecular Compounds Polarity
Molecular Compounds • Polarity– is the difference between the electronegativity values for the two atoms sharing a pair of electrons. • The greater the difference, the more polar the bond is.
Molecular Compounds • Nonpolar Covalent Bonds– this occurs when the two atoms sharing the electrons have the same electronegativity. • H2 Cl2 Br2 N2 • The electron pair is shared equally between the two atoms.
Molecular Compounds • Polar Bonds - this occurs when the two atoms sharing the electrons have different electronegativity values. H-C N-O C-Cl • The electron pair is shared unequally between the two atoms. • This unequal sharing is shown by drawing an arrow towards the more electronegative atom
Molecular Compounds Examples: d+ d- d+ d- C O C Cl d+ is a partial positive charge caused by the e- moving away from the atom d- is a partial negative charge caused by the e- moving toward the atom
Molecular Compounds • A molecule can have polar bonds, yet still not be a polar molecule. • You must evaluate the bonds as they appear in the 3-D shape of the molecule.
Molecular Compounds Example: CO2 O=C=O AX2 linear 180o Therefore, the pull of one bond cancels out the pull of the other bond. (tug-of-war; the middle doesn’t move) Each bond is polar, but the overall affect results in a nonpolar molecule
Molecular Compounds • Example: CH4 H H - C - H H AX4 tetrahedral 109.5o Again, each bond is polar, yet overall, the effects cancel each other out. The molecule is nonpolar
Molecular Compounds • Example: NH3 H ;; H - N - H AX3E trigonal pyramidal 109.5o Each bond is polar. In this case, the molecule is polar As the electrons are being drawn towards one end of the molecule. d- d+
Molecular Compounds • It is the uneven distribution of electrons in a molecule that results in a dipole moment. • Example: • Compare the dipole moment in H2S to that of H2O
Molecular Compounds H2SAX2E2 bent 109.5 H2O AX2E2 bent 109.5 • Because the H-S bond is less polar than the H-O bond, the dipole moment in H2S is weaker than the dipole moment in H2O