Calculate the reduced mass for the following bonds.
(c) C―Cl

Verified step by step guidance

1. Identify the atomic masses of the elements involved in the bond. For carbon (C), the atomic mass is approximately 12 amu (atomic mass units), and for chlorine (Cl), it is approximately 35.5 amu.
2. Use the formula for reduced mass, which is given by: $\mu =\frac{m\mathrm{\_1}m\mathrm{\_2}}{m\mathrm{\_1}+m\mathrm{\_2}}$, where $m\mathrm{\_1}$ and $m\mathrm{\_2}$ are the atomic masses of the two atoms.
3. Substitute the atomic masses of carbon and chlorine into the reduced mass formula: $\mu =\frac{12\times 35.5}{12+35.5}$.
4. Simplify the expression in the numerator: $12\times 35.5$.
5. Add the atomic masses in the denominator: $12+35.5$.

Key Concepts

Reduced Mass

Reduced mass is a concept used in physics and chemistry to simplify the two-body problem, particularly in molecular vibrations and rotational motion. It is defined as μ = (m1 * m2) / (m1 + m2), where m1 and m2 are the masses of the two atoms involved in the bond. This value allows us to treat the two-body system as a single particle with mass μ, facilitating calculations in molecular dynamics.

Atomic Mass

Atomic mass is the mass of an atom, typically expressed in atomic mass units (amu). It is approximately equivalent to the number of protons and neutrons in the atom's nucleus. For calculating the reduced mass of a bond like C―Cl, the atomic masses of carbon (approximately 12 amu) and chlorine (approximately 35.5 amu) are used to determine the individual masses (m1 and m2) in the reduced mass formula.

Bond in Molecular Systems

In molecular systems, a bond represents the interaction between two atoms, which can be described by their shared electrons. Understanding the nature of the bond, such as C―Cl, is crucial for calculating properties like reduced mass, as it involves the specific atoms and their respective masses. This concept is fundamental in predicting molecular behavior, such as vibrational frequencies and rotational spectra.