Identify the molecules with polar bonds and the po...

Question

Identify the molecules with polar bonds and the polar molecules.a. CCl4 b. CH3Clc. H2Od. CO2e. O2

Jules Bruno · Accepted Answer

a. CBr4Carbon (EN = 2.5) → carbon is the central atom. Chlorine (EN = 3.0)           Group           Valence ElectronsC         4A                   1 × 4 e– = 4 e–Cl        7A                   4 × 7 e– = 28 e–       Total:  32 valence e–Carbon prefers to form 4 bondsHalogens, when not the central atom, form only 1 bond. [readmore]The electronegativity difference between C and Cl is 0.5 so the C–Cl bond is polar. The Lewis structure is:Dipole arrows point at opposite directions so they cancel out.→ no net dipole in the molecule → nonpolar.b. CH3ClCarbon (EN = 2.5) → carbon is the central atom. Chlorine (EN = 3.0) Hydrogen → cannot be a central atom          Group           Valence ElectronsC         4A                   1 × 4 e– = 4 e–H         1A                   1 × 3 e– = 3 e–Cl        7A                   1 × 7 e– = 7 e–       Total: 14 valence e–Carbon → 4 bondsHalogens → when not the central atom → 1 bond.Hydrogen → 1 bondThe electronegativity difference between C and Cl is 0.5 so the C–Cl bond is polar. The Lewis structure is:Dipole arrows do not cancel out→ net dipole → polarc. H2OHydrogen → cannot be a central atom → oxygen is the central atom.           Group           Valence ElectronsH         1A                   1 × 2 e– = 2 e–O         6A                   1 × 6 e– = 6 e–        Total: 8 valence e–Oxygen → 2 bondsHydrogen → 1 bondThe electronegativity difference between O and H is 1.3 so the O–H bond is polar. The Lewis structure is:Dipole arrows do not cancel out→ net dipole → polard. CO2Carbon (EN = 2.5) → carbon is the central atom. Oxygen (EN = 3.5)           Group           Valence ElectronsC         4A                   1 × 4 e– = 4 e–O         6A                   2 × 6 e– = 12 e–        Total: 16 valence e–Oxygen → 2 bondsCarbon → 4 bondsThe electronegativity difference between C and O is 1.0 so the C–O bond is polar. The Lewis structure is:Dipole arrows point at opposite directions so they cancel out.→ no net dipole in the molecule → nonpolar.e. O2No central atom           Group           Valence ElectronsO         6A                   1 × 6 e– = 12 e–        Total: 12 valence e–Oxygen → 2 bondsThe electronegativity difference between O and O is 0 so the O–O bond is nonpolar. The Lewis structure is:Dipole arrows point at opposite directions so they cancel out.→ no net dipole in the molecule → nonpolar.The molecules with polar bonds and the polar molecules are b. CH3Cl, and c. H2O.

Problem: Identify the molecules with polar bonds and the polar molecules.a. CCl4 b. CH3Clc. H2Od. CO2e. O2

FREE Expert Solution

Problem Details

Problem: Identify the molecules with polar bonds and the polar molecules.a. CCl4 b. CH3Clc. H2Od. CO2e. O2

FREE Expert Solution

Problem Details

Sign up for free to watch this video!