hot2moli said:Calculate the approximate frequency of the C-H bond, with the force constant of k = 500 N/m.
Use:
Frequency = (1/2pi) Sqrt(k/((m1m2)/(m1 m2)))
BUTT WHAT DO I USE FOR MY MASS VALUES??
I tried, 12.011g/mol and 1.01g/mol and that is incorrect.
hot2moli said:Yes I understand but since its 1:1 you can just multiply it by 1mol correct? Then it's 12.01g and 1.01g?? Which is my method of solving but evidently incorrect... therefore how do you find the masses?
The formula for calculating the approximate frequency of the C-H bond is given by the equation: ν = (1/2π) √(k/μ), where ν is the frequency, k is the force constant, and μ is the reduced mass of the bond.
The force constant for the C-H bond can be determined experimentally using spectroscopic techniques, such as infrared spectroscopy. It can also be calculated using computational methods, such as molecular orbital theory.
The reduced mass of the C-H bond is the effective mass of the bond, which takes into account the masses of the carbon and hydrogen atoms. It is given by the equation: μ = (mC mH) / (mC + mH), where mC and mH are the masses of the carbon and hydrogen atoms, respectively.
The approximate frequency calculation for the C-H bond is typically accurate to within a few percent of the actual frequency. However, the accuracy may vary depending on the specific method used for calculation and the accuracy of the input parameters.
No, the approximate frequency of the C-H bond cannot be used to determine the strength of the bond. The frequency is only a measure of the bond's vibration, and does not take into account other factors that contribute to bond strength, such as bond length and electronegativity.