QQuestionChemistry
QuestionChemistry
"The central atom in which of the following does not violate the octet rule?
A. SF₄
B. ICl₄⁻
C. XeF₄
D. CF₄
E. KrF₂"
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Answer
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Step 1:
The octet rule states that atoms tend to have eight electrons in their valence shell to achieve a stable electronic configuration. Let's analyze each option to determine which one does not violate the octet rule.
Step 2:
A. SF₄: Sulfur has six electrons in its outer shell. By sharing four electrons with four fluorine atoms, sulfur achieves a stable octet. However, each fluorine atom needs one more electron to complete its octet, so this compound does not satisfy the octet rule for all atoms.
Step 3:
B. ICl₄⁻: Iodine has seven electrons in its outer shell. By sharing an electron with each of the four chlorine atoms, iodine achieves a stable octet. Additionally, the negative charge is distributed among the four iodine-chlorine bonds, so each chlorine atom also has an octet.
Step 4:
C. XeF₄: Xenon has eight electrons in its outer shell. By sharing four electrons with four fluorine atoms, xenon maintains its stable octet. Each fluorine atom needs one more electron to complete its octet, so this compound does not satisfy the octet rule for all atoms.
Step 5:
D. CF₄: Carbon has four electrons in its outer shell. By sharing four electrons with four fluorine atoms, carbon achieves a stable octet. Each fluorine atom needs one more electron to complete its octet, so this compound does not satisfy the octet rule for all atoms.
Step 6:
E. KrF₂: Krypton has eight electrons in its outer shell. By sharing two electrons with two fluorine atoms, krypton maintains its stable octet. Each fluorine atom needs one more electron to complete its octet, so this compound does not satisfy the octet rule for all atoms.
Step 7:
From our analysis, we can see that option B, ICl₄⁻, is the only molecule where all atoms have an octet. Therefore, ICl₄⁻ is the answer that does not violate the octet rule.
Final Answer
The central atom in option B, ICl₄⁻, does not violate the octet rule.
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