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Chapter 5: Problem 114

Which molecule has bonds that are the most polar covalent? (a) \(\mathrm{H}_{2}\) (b) \(\mathrm{CO}\) (c) \(\mathrm{H}_{2} \mathrm{~S}\) (d) \(\mathrm{H}_{2} \mathrm{O}\)

Short Answer

Expert verified
The molecule with the most polar covalent bond is (d) \(\mathrm{H}_{2}\mathrm{O}\), as it has the highest electronegativity difference between its bonded atoms (1.4).

Step by step solution

01

Find the electronegativity values

To compare the bonds, we first need the electronegativity values of hydrogen, carbon, oxygen, and sulfur. These values can be found in an electronegativity chart or a periodic table with electronegativity values. Hydrogen (H): 2.1 Carbon (C): 2.5 Oxygen (O): 3.5 Sulfur (S): 2.6
02

Calculate the electronegativity difference for each bond

Now that we have the electronegativity values, we can calculate the difference in electronegativity for each bond: (a) H-H bond in \(\mathrm{H}_{2}\): Difference: |2.1 - 2.1| = 0 (b) C-O bond in \(\mathrm{CO}\): Difference: |2.5 - 3.5| = 1.0 (c) H-S bond in \(\mathrm{H}_{2}\mathrm{S}\): Difference: |2.1 - 2.6| = 0.5 (d) H-O bond in \(\mathrm{H}_{2}\mathrm{O}\): Difference: |2.1 - 3.5| = 1.4
03

Compare the electronegativity differences and find the most polar covalent bond

Comparing the electronegativity differences, we can see that the H-O bond in \(\mathrm{H}_{2}\mathrm{O}\) has the highest difference of 1.4. This indicates that the H-O bond in \(\mathrm{H}_{2}\mathrm{O}\) is the most polar covalent bond among the options given. The answer is (d) \(\mathrm{H}_{2}\mathrm{O}\).

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Most popular questions from this chapter

Using only the periodic table, arrange these sets of atoms in order of increasing electronegativity: (a) \(\mathrm{Li}, \mathrm{Be}, \mathrm{K}\) (b) \(\mathrm{O}, \mathrm{Si}, \mathrm{S}\) (c) \(\mathrm{Br}_{t} \mathrm{I}, \mathrm{Te}\)

Suppose one of the electrons from the covalent bond in \(\mathrm{H}_{2}\) suddenly vanished. Why would the bond between the atoms weaken?

What is a binary compound? Is atmospheric oxygen an example of a binary compound?

Arrange the following sets of bonds in order of increasing ionic character. Use the symbols \(\delta+\) and \(\delta-\) to indicate partial charges, if any, in the bonds: \(\mathrm{O}-\mathrm{Cl}, \mathrm{C}-\mathrm{F}, \mathrm{N}-\mathrm{Cl}, \mathrm{O}-\mathrm{H}, \mathrm{S}-\mathrm{O}\)

Which of the following represents the correct resonance forms for \(\mathrm{SO}_{2} ?\) Explain what is wrong with the sets you did not choose.
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