Question about the trends of acids **Understanding the Effect of Electron-Withdrawing Oxygens on Acid Strength in Oxoacids**When discussing oxoacids, which are acids that contain oxygen, it's important to understand how the number of electron-withdrawing oxygens impacts their acid strength. Below are several explanations regarding this relationship:1. **Increase in Polarity** - **Statement**: "It makes H's more polar in the molecule." - **Explanation**: This suggests that the presence of oxygens affects the distribution of electrons, potentially making the hydrogen atoms more polar, though not the most critical factor in determining acid strength.2. **Effect on Hydrogen Release** - **Statement**: "As the number of oxygens increases, it makes the hydrogen's harder to lose. Oxygen's are electronegative, drawing the electron density towards themselves this makes the bonds to hydrogen stronger making the hydrogens less likely to fall off, resulting in weaker acids." - **Explanation**: This statement articulates that the increase in the number of electron-withdrawing oxygens can make the hydrogen atoms harder to dissociate due to stronger bonds. While it acknowledges the increased bond strength due to electron withdrawal, it inaccurately describes weaker acids, as stronger acids are linked to easier hydrogen ion release.3. **Threshold for Strong Acid** - **Statement**: "If the number of oxygens - number of ionizable H's is greater than or equal to 2, the acid is strong." - **Explanation**: This provides a more quantitative approach, indicating that an oxoacid with a surplus of oxygens relative to hydrogen ions by at least two is considered strong. However, this statement lacks detailed chemical reasoning.4. **Stabilization of Conjugate Base** - **Statement**: "The more electron withdrawing groups, the more stabilized the conjugate base, the more polar the ionizable H is in the molecule, and the more likely the molecule is to lose H ions into solution." - **Explanation**: This is the most comprehensive and accurate statement, explaining that electron-withdrawing groups indeed stabilize the conjugate base. This stabilization makes the hydrogen ion in the molecule more polar and more readily dissociated, leading to higher acid strength.In summary, the most accurate and detailed explanation acknowledges that electron-withdrawing oxygens stabilize the conjugate base, making the hydrogen ions more likely to dissociate and thereby increasing the acid strength of oxoacids. ### Acid Strength Trend in a Column**Question:**What is the trend in acid strength going down a column, and what is the trend based on?**Answer Options:**1. **Option A:** Acid strength increases down a column with the trend being differences in electronegativity. The greater the electronegativity differences the more polar the H atom is in the molecule, the more likely it is to fall off as an H+ ion in solution. 2. **Option B:** Acid strength increases down a column, with the trend being based on atomic size. Larger atoms have longer bonds, longer bonds are weaker bonds, weaker bonds break easier releasing more H+ ions into solution.3. **Option C:** Acid strength decreases down a column with the trend being differences in electronegativity. The greater the electronegativity differences the more polar the H atom is in the molecule, the more likely it is to fall off as an H+ ion in solution. 4. **Option D:** Acid strength decreases down a column, with the trend being based on atomic size. Smaller atoms have shorter bonds, shorter bonds are weaker bonds, weaker bonds are harder to break, releasing fewer H+ ions into solution.**Correct Answer:**- **Option B:** Acid strength increases down a column, with the trend being based on atomic size. Larger atoms have longer bonds, longer bonds are weaker bonds, weaker bonds break easier releasing more H+ ions into solution.### Explanation:As you proceed down a group in the periodic table, the atomic size increases. This causes the bond between hydrogen and the other atom (e.g., halogens in the case of hydrogen halides) to become longer and weaker. Weak bonds are more easily broken, resulting in the increased release of H+ ions into the solution, thereby increasing the acid strength.

Option A is correct. The strength of oxyacids is measured as its ability to dissociate and form H+…

Answered: In oxoacids, the number of electron…

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...