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Understanding Polarity: The Tug-of-War for Electrons in Chemical Bonds

This section explores the concept of polarity in molecules, highlighting how electrons are shared unequally in covalent bonds. Through examples like HCl, we examine electronegativity and its role in determining a molecule's polarity. Essential criteria for polarity include the presence of at least one polar bond or lone pair and their spatial arrangement. We analyze various molecules such as CO2, NH3, and SF4 to see how their structures affect molecular polarity. Visual representations of electron density maps and dipole moments are also covered.

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Understanding Polarity: The Tug-of-War for Electrons in Chemical Bonds

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  1. Week 4, Section Bonds: Tug of war for electrons 9/30/05

  2. H2 H-H Do both atoms contribute equally to the bond?

  3. HCl Do both atoms contribute equally to the bond? Are the electrons in the bond shared equally by both atoms?

  4. Polarity • Polarity is an unequal sharing of electrons • What causes polarity in HCl?

  5. Electronegativity the ability of an atom in a covalent bond to attract shared electrons to itself

  6. Is the molecule polar? • CO2 • NH3 • SF4 In order to determine polarity, you must visualize the tug-of-war going on in the molecule for the electrons.

  7. For a molecule to be polar it must: 1. have at least 1 polar bond or 1 lone pair 2. and polar bonds or lone pairs must be arranged in space so that the dipoles do not cancel out

  8. Are they polar? • C2H2 • XeF2 • BF3 • SF6 • CHCl3 • XeF4 • ICl3 • BrF5 Report back: #Valence electrons Lewis structure Molecular structure Dipole (if any)

  9. Polarity of molecules • Electron density maps (color) • Plus-arrows CHCl3 BrF5 SCN- SO2 or H2O?

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