Put the molecules in order of increasing bond polarity H-F, C-N, AND F-N.
Look up the electronegativities of each, subtract the two of each compound, and arrange in order of increasing difference.
To determine the order of increasing bond polarity between the given molecules (H-F, C-N, and F-N), we need to compare the electronegativity values of the atoms involved in each bond.
Electronegativity is a measure of an atom's ability to attract electrons towards itself in a chemical bond. The higher the electronegativity value of an atom, the stronger it attracts the shared electrons in a bond.
Here are the electronegativity values of the elements involved in the bonds you mentioned:
H (Hydrogen) - Electronegativity: 2.20
C (Carbon) - Electronegativity: 2.55
N (Nitrogen) - Electronegativity: 3.04
F (Fluorine) - Electronegativity: 3.98
Now let's compare the electronegativities of the atoms in each bond:
H-F: Hydrogen (2.20) and Fluorine (3.98)
C-N: Carbon (2.55) and Nitrogen (3.04)
F-N: Fluorine (3.98) and Nitrogen (3.04)
Since the electronegativity difference determines the bond polarity, we can order the molecules based on the largest difference in electronegativity.
In this case, the order of increasing bond polarity is as follows:
C-N < F-N < H-F
Explanation for the order:
1. C-N: The difference in electronegativity between Carbon and Nitrogen is 0.51 (3.04 - 2.55). This bond has the smallest electronegativity difference, making it the least polar among the given molecules.
2. F-N: The difference in electronegativity between Fluorine and Nitrogen is 0.94 (3.04 - 3.98). This bond has a larger electronegativity difference compared to C-N, making it more polar.
3. H-F: The difference in electronegativity between Hydrogen and Fluorine is 1.78 (3.98 - 2.20). This bond has the largest electronegativity difference among the given molecules, making it the most polar bond.
So, in summary, the order of increasing bond polarity for H-F, C-N, and F-N is C-N < F-N < H-F.