Question

Which of the following best describes an important property of bond energy? A. Bond energy increases with increasing bond length. B. The more shared electron pairs comprising a bond, the higher the energy of that bond. C. Single bonds are more difficult to break than double bonds. D. Bond energy and bond length are unrelated.

Short answer

B. The more shared electron pairs comprising a bond, the higher the energy of that bond.

Step-by-step solution

Identify the Key Concept

The question is about bond energy and key properties related to it.

Analyze Option A

Bond energy does not increase with increasing bond length. In fact, bond length and bond energy are inversely related. So, Option A is incorrect.

Analyze Option B

The more shared electron pairs comprising a bond, such as in double or triple bonds, generally results in higher bond energy. This statement accurately describes an important property of bond energy. Option B is likely correct.

Analyze Option C

Single bonds are typically easier to break than double bonds because single bonds have less bond energy than double bonds. Therefore, Option C is incorrect.

Analyze Option D

Bond energy and bond length are related; as bond length increases, bond energy typically decreases. Therefore, Option D is incorrect.

Conclusion

Based on the analysis, the description that accurately captures an important property of bond energy is Option B.

Key concepts

bond length

Bond length refers to the average distance between the nuclei of two bonded atoms. It plays a crucial role in understanding the properties of chemical bonds. Typically measured in picometers (pm) or angstroms (Å), bond length can tell us a lot about the stability and strength of a bond.
For example:

• Shorter bonds are usually stronger and have higher bond energy
• Longer bonds tend to be weaker and have lower bond energy

When comparing single, double, and triple bonds, the trend generally is:

• Triple bonds are the shortest
• Double bonds are intermediate in length
• Single bonds are the longest

shared electron pairs

Shared electron pairs are pairs of electrons that are shared between two atoms in a molecule. This sharing of electrons is what forms a covalent bond, the kind of bond found in many organic and inorganic molecules. The number of shared electron pairs affects the properties of the bond.
Here are some points to understand shared electron pairs better:

• Single bonds involve one shared pair of electrons
• Double bonds involve two shared pairs of electrons
• Triple bonds involve three shared pairs of electrons

The more shared electron pairs, the stronger and shorter the bond will be. For instance, a triple bond is generally stronger and shorter than a double bond, which itself is stronger and shorter than a single bond.

types of chemical bonds

Chemistry identifies various types of chemical bonds based on how atoms share or exchange electrons. The three primary types of chemical bonds are:

• Ionic Bonds: Formed when one atom donates an electron to another, resulting in attraction between positively and negatively charged ions. Example: Sodium chloride (NaCl)
• Covalent Bonds: Formed when atoms share electron pairs. These can be single, double, or triple bonds depending on the number of shared pairs. Example: Water (H₂O)
• Metallic Bonds: Found in metals, where electrons flow freely through a lattice of metal cations. Contributes to conductivity and malleability in metals. Example: Copper (Cu)

Understanding the type of bond helps predict properties like solubility, melting point, and electrical conductivity.

bond strength

Bond strength refers to the energy required to break a bond between two atoms. Higher bond energy means a stronger bond, which is more difficult to break. Several factors influence bond strength:

• Bond length: Shorter bonds are typically stronger
• Shared electron pairs: More shared electron pairs (e.g., double and triple bonds) generally mean stronger bonds
• Electronegativity: Large differences in electronegativity between bonded atoms can lead to stronger bonds due to greater attraction

Knowing bond strength helps chemists understand reaction mechanisms and predict the stability of compounds.