Question

The bond energy for a \(\mathrm{C}-\mathrm{H}\) bond is about \(413 \mathrm{kJ} / \mathrm{mol}\) in \(\mathrm{CH}_{4}\) but \(380 \mathrm{kJ} / \mathrm{mol}\) in \(\mathrm{CHBr}_{3}\). Although these values are relatively close in magnitude, they are different. Explain why they are different. Does the fact that the bond energy is lower in CHBr \(_{3}\) make any sense? Why?

Short answer

The difference in bond energy between the C-H bond in CH4 and CHBr3 can be attributed to the molecular environment and the influence of surrounding electronegative atoms on electron density. In CH4, all neighboring atoms are hydrogen, resulting in a uniform distribution of electron density. In CHBr3, the presence of more electronegative Br atoms affects the electron density around the C-H bond, ultimately affecting the bond strength. This explains the lower bond energy observed in CHBr3 (380 kJ/mol) compared to CH4 (413 kJ/mol).

Step-by-step solution

Understanding bond energy

Bond energy is the energy required to break a bond in a molecule. It is an indicator of bond strength, with higher bond energies suggesting stronger bonds.

Comparison of molecules

In this exercise, we are comparing the bond energies of a C-H bond in two different molecules: CH4 and CHBr3. In CH4, all the bonds are C-H bonds, whereas in CHBr3, there are three C-Br bonds and one C-H bond.

Factors affecting bond energy

Bond energy can be affected by various factors, such as the types of atoms involved, the electronegativity difference between the bonded atoms, and the molecular environment surrounding the bond. In our case, the primary factor we should consider is the molecular environment surrounding the C-H bond in both molecules.

Influence of molecular environment

Different atoms surrounding the C-H bond can influence the bond energy. In CH4, all the neighboring atoms are hydrogen, so the molecule has a symmetrical and uniform distribution of electron density. In CHBr3, the C-H bond is surrounded by three more electronegative bromine atoms, leading to a different distribution of electron density in the molecule.

Electronegativity and bond energy

The difference in electronegativity between carbon and hydrogen is relatively small, resulting in a mostly nonpolar C-H bond. When the C-H bond is surrounded by more electronegative atoms like bromine, the electron density around the C-H bond might be slightly influenced by the electronegative Br atoms. This can cause a change in bond strength, resulting in differences in bond energy between CH4 and CHBr3.

Explanation for lower bond energy in CHBr3

The C-H bond in CHBr3 has a lower bond energy (380 kJ/mol) compared to that in CH4 (413 kJ/mol). This difference can be attributed to the molecular environment, as the presence of more electronegative Br atoms in CHBr3 can influence the electron density around the C-H bond, ultimately affecting the bond strength. So yes, the lower bond energy in CHBr3 makes sense based on the factors discussed above. In conclusion, the difference in bond energy between the C-H bond in CH4 and CHBr3 can be attributed to the molecular environment and the influence of surrounding electronegative atoms on electron density. The lower bond energy in CHBr3 is reasonable considering these factors.

Key concepts

Molecular Environment

The molecular environment refers to the surroundings or context in which a bond exists within a molecule. It includes the types of atoms bonded to each other, as well as nearby atoms that can influence bond characteristics.

• In CH₄ (methane), the molecule's environment is simple: one carbon atom is bonded to four hydrogen atoms. The symmetry and uniform electron density around the C-H bonds contribute to consistent bond energies.
• In CHBr₃ (bromoform), the situation is more complex. The carbon is bonded to one hydrogen and three bromine atoms which are larger and more electronegative. This affects the distribution of electrons around the carbon atom.

Compared to methane, the unequal electronegativity in bromoform causes an uneven electron cloud distribution. This environment reduces the bond energy of the C-H bond in CHBr₃ compared to CH₄. The distinct surroundings directly impact the bond energy, illustrating how different molecular environments can cause variations in bond energy.

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold electrons. It plays a crucial role in bond formation and strength.

• Carbon and hydrogen have similar electronegativities, resulting in a fairly even sharing of electrons in C-H bonds, making them primarily covalent and nonpolar.
• Bromine is much more electronegative than both carbon and hydrogen. When bromine is bonded to carbon, it attracts electrons more strongly, slightly altering electron distribution in adjacent bonds such as the C-H bond in CHBr₃.

This influencing power of bromine creates a slight dipole, modifying the electron density around the C-H bond. Consequently, this affects the bond's strength and energy. The lower bond energy in CHBr₃'s C-H bond, compared to CH₄, illustrates the impact of surrounding electronegative atoms. It helps explain why the molecular environment, including the presence of more electronegative atoms, alters the apparent bond energy.

C-H Bond

The C-H bond, or carbon-hydrogen bond, is a common and important covalent bond in organic chemistry. Understanding its properties in different environments helps explain variations in bond energy. The C-H bond is generally strong and nonpolar due to the small difference in electronegativity between carbon and hydrogen. However, this typical bond energy can vary based on the molecule it is part of. In CH₄ each C-H bond experiences the same environment, with no nearby electronegative atoms affecting the distribution of electrons. This leads to relatively consistent and high bond energy. In contrast, the C-H bond in CHBr₃ exists alongside three C-Br bonds. These bonds involve more electronegative bromine atoms which have a subtle but significant influence.

• Bromine’s electronegativity pulls electron density away, modifying the C-H bond's electron density.
• This affects the bond's strength, generally decreasing the bond energy as seen in CHBr₃.

Understanding the environmental and electronic influences helps clarify why bond energies differ and why the C-H bond in CHBr₃ is weaker than in CH₄. This showcases the crucial interaction between molecular structure and bond energy.