QQuestionChemistry
QuestionChemistry
"Of these molecules, the bond in ____ is most polar:
A. HBr
B. HI
C. HCl
D. HF
E. H₂"
12 months agoReport content
Answer
Full Solution Locked
Sign in to view the complete step-by-step solution and unlock all study resources.
Step 1:: To determine the polarity of a bond, we need to look at the difference in electronegativity between the two atoms in the bond.
A larger difference in electronegativity results in a more polar bond.
Step 2:: Let's look up the electronegativity values for the atoms in each of these molecules.
We can use the Pauling scale, which assigns a value to each element. The values are as follows: - Hydrogen (H): 2.20 - Fluorine (F): 4.00 - Chlorine (Cl): 3.16 - Bromine (Br): 2.96 - Iodine (I): 2.66
Step 3:: Now, let's calculate the difference in electronegativity for each bond:
A. HBr: |2.20 - 2.96| = 0.76 B. HI: |2.20 - 2.66| = 0.46 C. HCl: |2.20 - 3.16| = 0.96 D. HF: |2.20 - 4.00| = 1.80 E. H₂: This is a homonuclear diatomic molecule, so the bond is nonpolar.
Step 4:: Based on the calculations, we can rank the bonds from most polar to least polar:
D. HF: 1.80 C. HCl: 0.96 A. HBr: 0.76 B. HI: 0.46 E. H₂: Not polar
Final Answer
The bond in molecule D, HF, is the most polar.
Need Help with Homework?
Stuck on a difficult problem? We've got you covered:
- Post your question or upload an image
- Get instant step-by-step solutions
- Learn from our AI and community of students