Chapter 3: Problem 3
Which of the following type(s) of bonds are nonpolar?
a.
Short Answer
Expert verified
The nonpolar bonds among the given options are and , so the correct answer is 'e', which is both 'a' and 'c'.
Step by step solution
01
Identify the electronegativities of Carbon, Hydrogen and Oxygen
As a first step, let's find the electronegativities of Carbon (C), Hydrogen (H) and Oxygen (O). From periodic table, it is known that Carbon (C) has an electronegativity of 2.5, Hydrogen (H) has an electronegativity of 2.1 and Oxygen (O) has a high electronegativity of 3.5.
02
Analyze bond type
The bond is formed between two Carbon atoms. Since both atoms have the same electronegativity (2.5), the difference of electronegativity is zero, which classifies the bond as nonpolar.
03
Analyze bond type
The bond is formed between Carbon and Oxygen. The electronegativity of Oxygen (3.5) is significantly higher than that of Carbon (2.5), which means there is a considerable electronegativity difference. Therefore, this bond is polar.
04
Analyze bond type
The bond is between Carbon and Hydrogen. The electronegativity difference is 2.5 (C) - 2.1 (H) = 0.4, which is small enough that the bond can be considered as slightly polar, but generally treated as nonpolar in many contexts.
05
Conclusion
So, comparing the above examination, the bonds that can be treated as nonpolar are and . Option 'e' which states both 'a' and 'c' therefore seems to be the most appropriate answer.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Electronegativity
Electronegativity is a key concept in understanding chemical bonding. It measures an atom's ability to attract and hold onto electrons in a chemical bond. Each element has a different electronegativity value, which can be found on the periodic table. Generally, the higher the electronegativity value, the stronger an atom's pull on electrons.
For instance, oxygen, with an electronegativity of 3.5, is highly electronegative. This means it has a strong tendency to attract electrons towards itself in a bond. On the other hand, elements like carbon and hydrogen have lower electronegativity values of 2.5 and 2.1, respectively.
For instance, oxygen, with an electronegativity of 3.5, is highly electronegative. This means it has a strong tendency to attract electrons towards itself in a bond. On the other hand, elements like carbon and hydrogen have lower electronegativity values of 2.5 and 2.1, respectively.
- Differences in electronegativity between atoms help us determine the nature of the bond they form.
- A higher difference usually indicates a polar bond, while a near-zero difference suggests a nonpolar bond.
Polar and Nonpolar Bonds
Understanding the difference between polar and nonpolar bonds is fundamental in predicting the behavior of molecules. A nonpolar bond occurs when two atoms share electrons equally, meaning the electronegativity difference is negligible or zero. This typically happens between atoms of the same element, like in a
C-C bond.
In contrast, polar bonds arise when there's a significant difference in electronegativity between the bonding atoms. For example, the C-O bond in carbon dioxide is polar because oxygen is more electronegative than carbon and pulls the shared electrons closer.
In contrast, polar bonds arise when there's a significant difference in electronegativity between the bonding atoms. For example, the C-O bond in carbon dioxide is polar because oxygen is more electronegative than carbon and pulls the shared electrons closer.
- The C-H bond is special: the slight difference in electronegativity is so small that it's often treated as nonpolar in many contexts, despite being slightly polar.
- Always check electronegativity differences to determine bond polarity.
Chemical Bonding
Chemical bonding is the glue that holds atoms together in substances. Bonds form when atoms share or transfer electrons to achieve a stable electron arrangement. Depending on the method of electron interaction, these bonds can be broadly categorized into ionic, covalent, and metallic. Our focus here is on covalent bonds, where atoms share electrons.
Within covalent bonds, electrons can be shared equally or unequally, leading to the formation of nonpolar and polar bonds, respectively.
Within covalent bonds, electrons can be shared equally or unequally, leading to the formation of nonpolar and polar bonds, respectively.
- Nonpolar covalent bonds involve equal sharing of electrons because the involved atoms have identical or similar electronegativity.
- Polar covalent bonds feature unequal sharing due to differing electronegativities, causing partial charges on the atoms.