Consider these molecules: H2 O, NH3, CO2, CIF, CCl4 (a) In which compound are the bonds most pol

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Consider these molecules: H2 O, NH3, CO2, CIF, CCl4 (a) In...

Consider these molecules: $\mathrm{H}_{2} \mathrm{O}, \mathrm{NH}_{3}, \mathrm{CO}_{2}, \mathrm{CIF}, \mathrm{CCl}_{4}$
(a) In which compound are the bonds most polar?
(b) Which compounds in the list are not polar?
(c) Which atom in CIF has a partial negative charge?

Key Concepts

Molecular Polarity

Molecular polarity is the net dipole moment of a molecule, which is determined by both the polarities of its individual bonds and its geometric shape. Even if a molecule contains polar bonds, the overall molecule can be non-polar if its shape allows the dipole moments to cancel each other out.

Electronegativity

Electronegativity refers to the ability of an atom to attract electrons in a chemical bond. Differences in electronegativity between bonded atoms lead to an uneven distribution of electron density, which is the fundamental basis for understanding bond polarity and the resulting partial charges on atoms.

Bond Polarity

Bond polarity arises when two atoms in a bond have different electronegativities, causing electrons to be unequally shared. This creates a dipole with a partial positive charge on the less electronegative atom and a partial negative charge on the more electronegative atom; the magnitude of which depends on the electronegativity difference.

Molecular Geometry

Molecular geometry is the three-dimensional arrangement of atoms within a molecule and plays a crucial role in determining how individual bond dipoles interact. Depending on the molecular symmetry, these bond dipoles can either cancel out, resulting in a non-polar molecule, or add together to produce an overall molecular dipole.

Partial Charges

Partial charges occur when electrons are unequally shared in a bond due to differences in electronegativity. This results in one end of the bond acquiring a slight negative charge and the other a slight positive charge, which is essential for understanding the distribution of charge within molecules and their interactions.

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