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Chapter 8: Problem 107

Distinguish between bond polarity and molecular polarity.

Short Answer

Expert verified
Bond polarity refers to the polarity in individual chemical bonds, which depends on the electronegativity difference between the bonded atoms. In contrast, molecular polarity depends on bond polarity and the arrangement of these bonds in the molecule, which refers to the overall charge distribution in the entire molecule. A molecule could have polar bonds but be a non-polar molecule if these polar bonds are symmetrically arranged.

Step by step solution

01

Definition of Bond Polarity

Bond polarity refers to the separation of charge in a chemical bond. This occurs when the atoms in the bond do not share the electrons equally. The atom with higher electronegativity pulls the shared electrons towards itself, creating a partial negative charge, and leaving the other atom with a partial positive charge. As a result, the bond is polar.
02

Definition of Molecular Polarity

Molecular polarity refers to the uneven distribution of molecular charge. The geometry of the molecule and its bond polarities determine the overall molecular polarity. If the polar bonds in a molecule are symmetrically distributed, they cancel out and the molecule is non-polar. If they are not, the molecule will be polar.
03

Distinguishing Between Bond Polarity and Molecular Polarity

Bond polarity and molecular polarity are intimately related, but they are not the same thing. Bond polarity refers to the polarity in individual bonds, a property dependent upon the difference in electronegativity between the two atoms in the bond. On the contrary, molecular polarity refers to the overall polarity of the entire molecule, which depends not only on bond polarity but also on the geometry of the molecule and how these polar bonds are arranged within it.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Molecular Polarity
In simple terms, molecular polarity is all about the overall charge distribution across a whole molecule. While bond polarity examines the charge difference between two atoms, molecular polarity goes one step further. It assesses how these individual polar bonds align with each other in space.
If polar bonds within a molecule are arranged symmetrically, their charges might cancel each other out. In this case, the molecule remains non-polar despite containing polar bonds. However, if the polar bonds are asymmetrical, the molecule ends up being polar.
  • A key aspect of determining molecular polarity is the molecular shape, often described by VSEPR theory (Valence Shell Electron Pair Repulsion theory).
  • Even a molecule with multiple identical polar bonds can be non-polar if those bonds are symmetrically arranged, as in carbon dioxide (CO鈧�).
  • A classic example of a polar molecule is water (H鈧侽), where the bent shape causes an uneven distribution of charge.
Electronegativity
Electronegativity is a chemical property that indicates how strongly an atom can attract a pair of bonded electrons. In other words, it's a measure of an atom's pull on shared electrons within a covalent bond.
  • The higher the electronegativity, the stronger the attraction for electrons.
  • Electronegativity values rise as you move from left to right across a period on the periodic table and decrease down a group.
  • Among the most electronegative elements are fluorine, oxygen, and nitrogen.
Differences in electronegativity between bonded atoms directly affect bond polarity. If the atoms have similar electronegativity, they share electrons more equally, resulting in a non-polar bond. Conversely, a significant electronegativity difference leads to one atom attracting the electron pair more strongly, forming a polar bond.
Chemical Bonding
Chemical bonding is all about how atoms combine to form molecules and compounds, and it encompasses various types of bonds. At the most basic level, we have ionic bonds and covalent bonds.
  • Ionic bonds: Formed when electrons are transferred from one atom to another, creating ions. This typically occurs between metals and nonmetals.
  • Covalent bonds: Occur when two atoms share electrons. These are more common in organic compounds and include both polar and non-polar covalent bonds.
  • Metallic bonding involves the pooling of free electrons among a lattice of metal atoms.
The type of bond鈥攊onic, covalent, or metallic鈥攄epends on the elements involved and factors like electronegativity and electron affinity. Understanding chemical bonding is crucial because it helps us predict molecular structure, behavior, and the properties of substances.

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Most popular questions from this chapter

Predict the shapes and give approximate bond angles for the following molecules. (a) OCS (c) FCN (e) \(\mathrm{PF}_{3}\) (g) \(\mathrm{NO}_{2}\) (b) FNO (d) \(\mathrm{HN}_{3}\) (f) \(\mathrm{SF}_{2}\)

Explain how nonbonding pairs of electrons influence molecular shape.

Which of the following compounds are likely to have covalent bonds? (a) \(\mathrm{HF}\) (c) \(\mathrm{NCl}_{3}\) (e) \(\mathrm{CF}_{4}\) (b) \(\mathrm{NaF}\) (d) \(\mathrm{MgBr}_{2}\)

Predict the bond angles in the following molecules. (a) \(\mathrm{NH}_{3}\) (c) \(\mathrm{HCl}\) (e) \(\mathrm{BF}_{3}\) (g) \(\mathrm{PCl}_{3}\) (b) \(\mathrm{H}_{2} \mathrm{O}\) (d) \(\mathrm{HCN}\) (f) \(\mathrm{H}_{2} \mathrm{CO}\)

Describe the difference between ionic and covalent bonding.
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