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Step 1:I'll solve this problem step by step, following the specified LaTeX formatting guidelines:
Step 2:: Determine the Molecular Geometry
- Electron geometry follows $$AX_{2}$$ molecular geometry type
- BeCl^2 has a linear molecular geometry - Central beryllium (Be) atom is bonded to two chlorine (Cl) atoms
Step 3:: Analyze Electronegativity Differences
- Electronegativity difference: $$3.16 - 1.57 = 1.59
- Beryllium (Be) electronegativity: 1.57 - Chlorine (Cl) electronegativity: 3.16 - This indicates polar bonds between Be and Cl
Step 4:: Examine Molecular Symmetry
- In a linear molecule, the two Be-Cl bonds are symmetrically opposite - The bond dipoles are equal in magnitude but point in opposite directions - These dipoles cancel each other out
Step 5:: Determine Polarity
- Despite polar bonds, the overall molecular symmetry results in zero net dipole moment - The bond dipoles completely cancel each other
Final Answer
BeCl^2 is a NONPOLAR molecule due to its linear symmetry and canceling bond dipoles.
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