QQuestionChemistry
QuestionChemistry
Is BeCl^2 polar or nonpolar in terms of its bonds and molecule?
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Answer
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Step 1:I'll solve this step by step using proper chemical bonding and molecular geometry analysis:
Step 2:: Determine the Lewis Structure
- Total valence electrons: $$2 + (2 \times 7) = 16$$ electrons
- Beryllium (Be) is the central atom - Chlorine (Cl) atoms are terminal - Be has 2 valence electrons, each Cl has 7 valence electrons
Step 3:: Analyze Bond Polarity
- Electronegativity difference: $$3.16 - 1.57 = 1.59
- Electronegativity of Be: 1.57 - Electronegativity of Cl: 3.16 - This difference indicates polar covalent bonds - Chlorine will have partial negative charge - Beryllium will have partial positive charge
Step 4:: Determine Molecular Geometry
- BeCl^2 has linear geometry - Two identical polar bonds pointing in opposite directions - Bond dipoles cancel each other out
Step 5:: Molecular Polarity Conclusion
- Despite polar bonds, the linear symmetry results in a nonpolar molecule - Net dipole moment is zero
Final Answer
BeCl^2 is a nonpolar molecule with polar bonds.
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