QQuestionChemistry
QuestionChemistry
BCl^3 is a non-polar molecule, but why does it form polar bonds?
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Answer
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Step 1:I'll solve this problem step by step, explaining the molecular structure and bonding of BCl^3.
Step 2:: Understand the Molecular Structure
- BCl^3 is a trigonal planar molecule with boron (B) at the center - Boron has 3 valence electrons, and chlorine has 7 valence electrons - Each B-Cl bond is formed by sharing electrons
Step 3:: Analyze the Electronegativity Difference
- Electronegativity difference: $$3.16 - 2.04 = 1.12
- Boron (B) electronegativity: 2.04 - Chlorine (Cl) electronegativity: 3.16 - This significant difference creates polar covalent bonds
Step 4:: Explain Polar Bonds
- And a partial positive charge ($$\delta^{+}$$) on boron
- The electronegativity difference causes unequal electron sharing - Chlorine pulls electron density more strongly toward itself
Step 5:: Understand Molecular Polarity
- Despite polar B-Cl bonds, the trigonal planar geometry - Symmetrical arrangement of three identical Cl atoms - Dipole moments cancel out, resulting in a non-polar molecule
Final Answer
BCl^3 forms polar bonds due to the significant electronegativity difference between boron and chlorine, but its symmetrical molecular geometry results in a non-polar molecule overall.
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