QQuestionChemistry
QuestionChemistry
A valid Lewis structure of __________ cannot be drawn without violating the octet rule.
A. NI^3
B. SiF^4
C. SO^2
D. CO^2
E. ICl^5
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Answer
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Step 1:Let's solve this step by step:
Step 2:: Understand the Octet Rule
The octet rule states that atoms tend to combine in such a way that they each have eight electrons in their valence shell. Violations occur when an atom cannot achieve eight electrons through normal bonding.
Step 3:: Analyze the Valence Electrons for Each Molecule
7 + (7 \times 5) = 42$$ total valence electrons
Let's count valence electrons for each molecule: A. NI^3: - N: 5 valence electrons - I: 7 valence electrons × 3 B. SiF^4: - Si: 4 valence electrons - F: 7 valence electrons × 4 C. SO^2: - S: 6 valence electrons - O: 6 valence electrons × 2 D. CO^2: - C: 4 valence electrons - O: 6 valence electrons × 2 E. ICl^5: - I: 7 valence electrons - Cl: 7 valence electrons × 5
Step 4:: Determine Octet Rule Violations
- NI^3: Nitrogen cannot achieve an octet - SiF^4: All atoms can achieve an octet - SO^2: Can achieve an octet - CO^2: Can achieve an octet - ICl^5: Iodine will exceed an octet
Step 5:: Identify the Molecule that Cannot Draw a Valid Lewis Structure
NI^3 cannot be drawn without violating the octet rule because nitrogen lacks sufficient electrons to form a stable octet with three iodine atoms.
Final Answer
NI^3
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