QQuestionChemistry
QuestionChemistry
A valid Lewis structure of ________ cannot be drawn without violating the octet rule.
A. ClF₃
B. CO₂
C. CCl₄
D. PCl₃
E. SO₃
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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 of this rule occur when an atom cannot achieve eight electrons through normal bonding.
Step 3:: Analyze the Valence Electrons for Each Molecule
Let's count the valence electrons for each molecule: A. ClF₃: - Cl: 7 valence electrons - F: 7 × 3 = 21 valence electrons - Total: 28 valence electrons B. CO₂: - C: 4 valence electrons - O: 6 × 2 = 12 valence electrons - Total: 16 valence electrons C. CCl₄: - C: 4 valence electrons - Cl: 7 × 4 = 28 valence electrons - Total: 32 valence electrons D. PCl₃: - P: 5 valence electrons - Cl: 7 × 3 = 21 valence electrons - Total: 26 valence electrons E. SO₃: - S: 6 valence electrons - O: 6 × 3 = 18 valence electrons - Total: 24 valence electrons
Step 4:: Draw Lewis Structures and Check Octet Rule
After carefully drawing Lewis structures for each molecule, we find: A. ClF₃: Cl has 10 electrons (expanded octet) B. CO₂: Follows octet rule C. CCl₄: Follows octet rule D. PCl₃: Follows octet rule E. SO₃: S has 12 electrons (expanded octet)
Step 5:: Identify the Molecule that Cannot Be Drawn Without Violating the Octet Rule
The key is to find a molecule that CANNOT satisfy the octet rule through normal bonding.
Final Answer
ClF₃ Explanation: In ClF₃, the central chlorine atom would need to have 10 electrons to bond with three fluorine atoms, which violates the standard octet rule. This makes ClF₃ the molecule that cannot be drawn with a standard Lewis structure without expanding the octet.
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