Which of the following statements is(are) true? Correct the...

Which of the following statements is(are) true? Correct the false statements. a. It is impossible to satisfy the octet rule for all atoms in $\mathrm{XeF}_{2}$. b. Because $\mathrm{SF}_{4}$ exists, $\mathrm{OF}_{4}$ should also exist because oxygen is in the same family as sulfur. c. The bond in $\mathrm{NO}^{+}$ should be stronger than the bond in $\mathrm{NO}^{-}$. d. As predicted from the two Lewis structures for ozone, one oxygen-oxygen bond is stronger than the other oxygenoxygen bond.

Which of the following statements is(are) true? Correct the false statements.
a. It is impossible to satisfy the octet rule for all atoms in $\mathrm{XeF}_{2}$.
b. Because $\mathrm{SF}_{4}$ exists, $\mathrm{OF}_{4}$ should also exist because oxygen is in the same family as sulfur.
c. The bond in $\mathrm{NO}^{+}$ should be stronger than the bond in $\mathrm{NO}^{-}$.
d. As predicted from the two Lewis structures for ozone, one oxygen-oxygen bond is stronger than the other oxygenoxygen bond.

Key Concepts

Resonance and Bond Equivalence

Resonance involves representing a molecule with multiple valid Lewis structures, with the true electronic structure being a hybrid of these forms. This distribution of electron density can lead to bonds that are equivalent even if individual Lewis structures suggest variability. Understanding resonance is key to comprehending how bond strengths can appear to differ in single structures but are actually averaged out in the real molecule.

Bond Order and Bond Strength

Bond order refers to the number of electron pairs shared between two atoms, and often a higher bond order results in a shorter, stronger bond. Variations in electron count, such as those found in charged species or different resonance contributors, affect the bond order. This relationship helps to rationalize why some bonds in cationic molecules are stronger than those in anionic ones.

Octet Rule and Expanded Octet

The octet rule is a guideline that atoms tend to complete eight electrons in their valence shell through bonding. However, elements from the third period onward can accommodate more than eight electrons using vacant d-orbitals, a phenomenon known as an expanded octet. This concept is essential for understanding compounds where central atoms exceed the octet, even though peripheral atoms (like fluorine) still obey the octet rule.

Periodic Trends and Chemical Reactivity

Periodic trends, such as the availability of d orbitals and differences in atomic size and electronegativity, play a critical role in the types of compounds that can form. These trends explain why some elements in the same group (for example, oxygen and sulfur) may behave very differently in their bonding capacities and reactivities, influencing the existence and stability of certain compounds.

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