A. Increasing halogen atom size.
B. Decreasing acid strength.
C. Shortening of the C-C bond.
D. Increasing electronegativity.
E. Higher dipole values going from F to Cl to Br.
cant paste the spartan stuff... whats the answer?!?!?
What's the question?
For fluoracetic acid the highest Boltzmann distribution is when the dihedral angle is at 0 degrees. However, going from chloro- to bromoacetic acid, an increasing dip in the Boltzmann distribution occurs at 0 degrees. What is responsible for this "dip?" (HINT: look at how the structure of the molecule changes as the halogen atom rotates around toward the hydrogen atom attached to the oxygen atom.)
I can tell you its NOT
decreasing acid strength
and its NOT
Increasing electronegativity..
your guess is as good as mine.. : //
its increasing halogen atom size...i just answered it and thankfully got it right
Yes, it is increasing halogen atom size
It is increasing halogen atom size...
For those who care, look at the plots in Spartan and you can automatically rule out Increasing Electronegativity and higher dipole values.
To determine the answer based on the given options (A, B, C, D, and E), we need to consider the effect of each factor on the observed trend.
A. Increasing halogen atom size: As the size of the halogen atom increases, the strength of the halogen-halogen bond generally decreases. This would result in a weaker intermolecular force, leading to a decrease in boiling point.
B. Decreasing acid strength: The acidity of a compound is influenced by various factors, such as the stability of the conjugate base. If the acid strength is decreasing, it indicates that the stability of the conjugate base is increasing. This could be due to factors like electron-withdrawing effects or resonance stabilization.
C. Shortening of the C-C bond: The length of the carbon-carbon bond typically affects the strength of intermolecular forces. A shorter bond tends to create a stronger intermolecular force, leading to a higher boiling point.
D. Increasing electronegativity: Electronegativity is the ability of an atom to attract electrons in a chemical bond. Increasing electronegativity generally leads to stronger intermolecular forces due to an increase in dipole-dipole interactions. This results in higher boiling points.
E. Higher dipole values going from F to Cl to Br: A higher dipole value indicates a greater difference in electronegativity between the atoms in a compound. As mentioned earlier, a higher electronegativity leads to stronger intermolecular forces and higher boiling points.
Now, we need to compare the boiling points of the halogens (F, Cl, and Br) to determine the correct answer. The trend in the boiling points of the halogens indicates that as we move from F to Cl to Br, the boiling points generally increase. This suggests that the factor affecting the boiling point trend is related to increasing intermolecular forces.
Comparing the options, we can see that option D, Increasing electronegativity, best explains the trend. As we move from F to Cl to Br, the electronegativity increases, leading to stronger intermolecular forces and higher boiling points. Therefore, the answer is D. Increasing electronegativity.