Question

Find if Polar or Non Polar?

Answer 1

No specific option to choose as it is a list of molecules and their properties.

Answer 2

To determine if a molecule is polar or nonpolar, we need to consider two main factors:

1. Bond polarity: Whether the individual bonds within the molecule are polar due to a difference in electronegativity between the bonded atoms.
2. Molecular geometry: Whether the arrangement of these polar bonds and any lone pairs on the central atom results in a net dipole moment for the entire molecule. Symmetrical molecules often have their bond dipoles cancel out, leading to a nonpolar molecule, even if individual bonds are polar. Asymmetrical molecules, or those with lone pairs on the central atom, are typically polar.

Let's analyze each molecule:

① HCl:

• Bond: H-Cl bond is polar (Cl is more electronegative).
• Geometry: Linear.
• Net dipole: Yes, the dipole points towards Cl.
• Polar (P)

② HF:

• Bond: H-F bond is highly polar (F is much more electronegative).
• Geometry: Linear.
• Net dipole: Yes, the dipole points towards F.
• Polar (P)

③ H₂:

• Bond: H-H bond is nonpolar (no electronegativity difference).
• Geometry: Linear.
• Net dipole: Zero.
• Nonpolar (NP)

④ O₃ (Ozone):

• Structure: Bent (V-shaped) with resonance. The central oxygen atom has one lone pair.
• Net dipole: Due to its bent geometry and the presence of formal charges/resonance, it has a net dipole moment.
• Polar (P)

⑤ CO₂:

• Structure: Linear (C=O bonds).
• Net dipole: C=O bonds are polar, but their dipoles are equal and opposite, canceling each other out in the linear geometry.
• Nonpolar (NP)

⑥ AlCl₃:

• Structure: Trigonal planar. No lone pairs on central Al.
• Net dipole: Al-Cl bonds are polar, but the symmetrical trigonal planar arrangement causes the dipoles to cancel.
• Nonpolar (NP)

⑦ BrCl₃:

• Structure: T-shaped (central Br has two lone pairs).
• Net dipole: Br-Cl bonds are polar. The T-shaped geometry is asymmetrical, and the lone pairs contribute to a net dipole moment.
• Polar (P)

⑧ PCl₅:

• Structure: Trigonal bipyramidal. No lone pairs on central P.
• Net dipole: P-Cl bonds are polar, but the symmetrical trigonal bipyramidal arrangement causes the dipoles to cancel.
• Nonpolar (NP)

⑨ SF₆:

• Structure: Octahedral. No lone pairs on central S.
• Net dipole: S-F bonds are polar, but the highly symmetrical octahedral arrangement causes the dipoles to cancel.
• Nonpolar (NP)

⑩ CH₄:

• Structure: Tetrahedral. No lone pairs on central C.
• Net dipole: C-H bonds are slightly polar, but the symmetrical tetrahedral arrangement causes the dipoles to cancel.
• Nonpolar (NP)

⑪ IF₇:

• Structure: Pentagonal bipyramidal. No lone pairs on central I.
• Net dipole: I-F bonds are polar, but the highly symmetrical pentagonal bipyramidal arrangement causes the dipoles to cancel.
• Nonpolar (NP)

⑫ CH₂Cl₂:

• Structure: Tetrahedral.
• Net dipole: C-H and C-Cl bonds are polar. The molecule is asymmetrical due to different types of atoms (H and Cl) attached to the central carbon, leading to a net dipole moment.
• Polar (P)

⑬ CH₂Cl₂: (Duplicate of ⑫)

• Polar (P)

⑭ PFCl₃:

• Structure: Tetrahedral (central P, 1 F, 3 Cl).
• Net dipole: P-F and P-Cl bonds are polar and have different magnitudes. The molecule is asymmetrical, so the bond dipoles do not cancel.
• Polar (P)

⑮ BHCl₂:

• Structure: Trigonal planar (central B, 1 H, 2 Cl).
• Net dipole: B-H and B-Cl bonds are polar. The molecule is asymmetrical due to different atoms, leading to a net dipole moment.
• Polar (P)

⑯ PBrCl₂:

• Structure: Trigonal pyramidal (central P has one lone pair).
• Net dipole: P-Br and P-Cl bonds are polar. The lone pair and the asymmetrical arrangement of different atoms lead to a net dipole moment.
• Polar (P)

⑰ XeO₃F₂:

• Structure: Trigonal bipyramidal (central Xe, 3 O, 2 F). No lone pairs on central Xe.
• Net dipole: Xe-O and Xe-F bonds are polar. Even with F in axial and O in equatorial positions, the different bond types and their arrangement make the molecule asymmetrical, resulting in a net dipole moment.
• Polar (P)

⑱ XeO₂F₂:

• Structure: See-saw (central Xe has one lone pair).
• Net dipole: Xe-O and Xe-F bonds are polar. The see-saw geometry is asymmetrical, and the lone pair contributes to a net dipole moment.
• Polar (P)

⑲ SO₂Cl₂:

• Structure: Tetrahedral (central S, 2 O, 2 Cl).
• Net dipole: S=O and S-Cl bonds are polar. The molecule is asymmetrical due to different atoms, leading to a net dipole moment.
• Polar (P)

⑳ NH₃:

• Structure: Trigonal pyramidal (central N has one lone pair).
• Net dipole: N-H bonds are polar. The lone pair on N and the trigonal pyramidal geometry result in a net dipole moment.
• Polar (P)

⑳ ClO₂⁻: (Assuming this is a separate entry)

• Structure: Bent (V-shaped) (central Cl has two lone pairs).
• Net dipole: Cl-O bonds are polar. The lone pairs and bent geometry lead to a net dipole moment.
• Polar (P)

㉒ NF₃:

• Structure: Trigonal pyramidal (central N has one lone pair).
• Net dipole: N-F bonds are polar. The lone pair on N and the trigonal pyramidal geometry result in a net dipole moment.
• Polar (P)

㉓ XeF₄:

• Structure: Square planar (central Xe has two lone pairs in axial positions).
• Net dipole: Xe-F bonds are polar, but the symmetrical square planar arrangement and cancellation of lone pair dipoles result in no net dipole moment.
• Nonpolar (NP)

㉔ XeF₂:

• Structure: Linear (central Xe has three lone pairs in equatorial positions).
• Net dipole: Xe-F bonds are polar, but the symmetrical linear arrangement and cancellation of lone pair dipoles result in no net dipole moment.
• Nonpolar (NP)

㉕ ICl₂⁻:

• Structure: Linear (central I has three lone pairs in equatorial positions).
• Net dipole: I-Cl bonds are polar, but the symmetrical linear arrangement and cancellation of lone pair dipoles result in no net dipole moment.
• Nonpolar (NP)

㉖ H₂O:

• Structure: Bent (V-shaped) (central O has two lone pairs).
• Net dipole: O-H bonds are polar. The lone pairs and bent geometry lead to a net dipole moment.
• Polar (P)

㉗ SO₄²⁻:

• Structure: Tetrahedral (all S-O bonds equivalent by resonance).
• Net dipole: S-O bonds are polar, but the symmetrical tetrahedral arrangement causes the dipoles to cancel.
• Nonpolar (NP)

㉘ CO₃²⁻:

• Structure: Trigonal planar (all C-O bonds equivalent by resonance).
• Net dipole: C-O bonds are polar, but the symmetrical trigonal planar arrangement causes the dipoles to cancel.
• Nonpolar (NP)

㉙ SO₃²⁻:

• Structure: Trigonal pyramidal (central S has one lone pair).
• Net dipole: S-O bonds are polar. The lone pair on S and the trigonal pyramidal geometry result in a net dipole moment.
• Polar (P)

㉚ CH₄: (Duplicate of ⑩)

• Nonpolar (NP)

㉛ C₂H₄ (Ethene):

• Structure: Planar.
• Net dipole: C-H bonds are slightly polar, but the overall symmetrical planar structure causes the dipoles to cancel.
• Nonpolar (NP)

The question asks to "Find if Polar or Non Polar?". It implies providing the correct classification. The provided list in the image has several incorrect classifications.