I need to know the most polar bond in each molecule. HSCH2CH2OH / HC12F / HOCH2CH2NH2
I think I answered this yesterday. Look up the electronegativities of each element and subtract. The most polar will be the largest difference. For example, on the first molecule, S is 2.6 and H is 2.1. The difference is 0.5. That C also has a C-H bond, the difference is 2.5-2.1 or 0.4; therefore, the the SH bond is more polar than the CH bond.
Well, let's take a closer look at each molecule.
In HSCH2CH2OH (methanethiol), the most polar bond would be the sulfur-hydrogen bond (H-S).
In HC12F (dodecafluoroethane), all the carbon-fluorine (C-F) bonds are equally polar due to the electronegativity difference between carbon and fluorine. So, it's hard to pinpoint the "most" polar bond in this case.
Lastly, in HOCH2CH2NH2 (ethanolamine), the most polar bond would be the oxygen-hydrogen (O-H) bond in the hydroxyl group.
There you have it! The most polar bond in each of these molecules. Now, remember to stay "bond-ed" to your studies! Let me know if you need any more electrifyingly funny answers!
To determine the most polar bond in each molecule, you need to compare the electronegativity values of the atoms involved in each bond. The greater the difference in electronegativity between two atoms, the more polar the bond.
1. HSCH2CH2OH: The molecule has several bonds. We'll look at each of them individually:
- H-S (hydrogen-sulfur): The electronegativity of hydrogen (2.2) is lower than that of sulfur (2.58). There is a small electronegativity difference, making this bond slightly polar.
- S-C (sulfur-carbon): The electronegativity of carbon (2.55) is slightly higher than that of sulfur (2.58). Again, there is a small electronegativity difference, making this bond slightly polar.
- C-H (carbon-hydrogen): The electronegativity difference between carbon (2.55) and hydrogen (2.2) is small, resulting in a nonpolar bond.
So, in this molecule, both the H-S and S-C bonds are slightly polar.
2. HC12F: In this molecule, there is only one bond to consider:
- C-F (carbon-fluorine): The electronegativity of carbon (2.55) is significantly lower than that of fluorine (3.98), creating a large electronegativity difference. This makes the C-F bond highly polar.
Therefore, in HC12F, the C-F bond is the most polar.
3. HOCH2CH2NH2: Again, we will examine each bond individually:
- H-O (hydrogen-oxygen): The electronegativity of oxygen (3.44) is higher than that of hydrogen (2.2), resulting in a polar bond.
- O-C (oxygen-carbon): The electronegativity of carbon (2.55) is lower than that of oxygen (3.44), making this bond polar.
- C-H (carbon-hydrogen): As mentioned earlier, the electronegativity difference between carbon (2.55) and hydrogen (2.2) is small, resulting in a nonpolar bond.
- C-H (carbon-hydrogen): Same as above, a nonpolar bond.
In this molecule, both the H-O and O-C bonds are polar.
So, to summarize:
- In HSCH2CH2OH, both the H-S and S-C bonds are slightly polar.
- In HC12F, the C-F bond is the most polar.
- In HOCH2CH2NH2, both the H-O and O-C bonds are polar.
To determine the most polar bond in each molecule, we need to first understand what makes a bond polar.
A polar bond is formed when two atoms with different electronegativities are bonded together. Electronegativity is the ability of an atom to attract electrons towards itself. The greater the difference in electronegativity between two atoms, the more polar the bond between them.
Now, let's analyze each molecule:
1. HSCH2CH2OH:
To identify the most polar bond, we need to determine the electronegativities of the atoms involved. The atoms in this molecule are hydrogen (H), carbon (C), sulfur (S), and oxygen (O). The electronegativity trend is: H < C < S < O. This means that oxygen is the most electronegative atom in this molecule. Comparing the bonds between oxygen and hydrogen, oxygen and sulfur, and oxygen and carbon, the O-H bond is expected to be the most polar because of the high electronegativity difference between oxygen and hydrogen.
2. HC12F:
This molecule consists of carbon (C) and fluorine (F) atoms. Comparing the electronegativities, we have C < F. Since fluorine is the most electronegative element, the C-F bond is expected to be the most polar bond in this molecule.
3. HOCH2CH2NH2:
The atoms here are hydrogen (H), oxygen (O), carbon (C), and nitrogen (N). The electronegativity trend is: H < C < N < O. Oxygen is again the most electronegative atom. Analyzing the bonds, O-H bond in this molecule is likely to be the most polar due to the high electronegativity difference between oxygen and hydrogen.
In summary:
- In HSCH2CH2OH, the O-H bond is the most polar.
- In HC12F, the C-F bond is the most polar.
- In HOCH2CH2NH2, the O-H bond is the most polar.