**Question:**Choose the bond below that is *least* polar.- ○ P-F- ○ C-Br- ○ C-F- ○ C-I- ○ C-Cl**Explanation:**When discussing the polarity of a bond, it is important to consider the difference in electronegativity between the two atoms involved. The greater the difference, the more polar the bond.1. **P-F (Phosphorus-Fluorine):** Fluorine is highly electronegative, making this bond quite polar.2. **C-Br (Carbon-Bromine):** Bromine has a moderate electronegativity that leads to a lesser degree of polarity.3. **C-F (Carbon-Fluorine):** Again, with fluorine’s high electronegativity, this bond is very polar.4. **C-I (Carbon-Iodine):** Iodine is less electronegative, leading to less polarity in this bond.5. **C-Cl (Carbon-Chlorine):** Chlorine has moderate electronegativity, though higher than bromine, making it more polar than C-Br.Among these options, **C-I** (Carbon-Iodine) is expected to be the least polar due to iodine’s relatively low electronegativity compared to other elements listed.Always refer to a periodic table of electronegativities when making these comparisons. **Question:** Choose the best Lewis structure for OCl₂.**Options:**1. Cl double bonded to O, single bonded to Cl, with lone pairs: •Cl═Ö─Cl•2. Cl single bonded to O, double bonded to Cl, with lone pairs: •Cl─Ö═Cl•3. Cl double bonded to O, double bonded to Cl, with lone pairs: •Cl═Ö═Cl•4. Cl single bonded to O, single bonded to Cl, with lone pairs: •Cl─O─Cl•5. Cl single bonded to O, single bonded to Cl, with lone pairs and different arrangement: •Cl─Ö─Cl•**Explanation:** Each option represents a different arrangement of atoms and bonds for the molecule OCl₂. The choices display variations in bonding (single or double bonds) between the oxygen and chlorine atoms, as well as the placement of lone pairs of electrons around each atom, which are indicated by dots.

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Answered: Choose the bond below that is least…

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Chemistry

Choose the bond below that is least polar. O P-F OC-Br OC-F O C-CI

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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- Complete the table. Number of electron groups Bond angle Outer atoms/Lone pairs 2 ? 2/0 3 4 ? ? bond angle in a two electron group molecule: bond angle in a three electron group molecule: bond angle in a four electron group molecule: 3/0 2/1 4/0 3/1 2/2 Shape ? trigonal planar (planar triangular) ? tetrahedral ? bent The shape of a two electron group molecule is The shape of a three electron group molecule with two outer atoms and one lone pair is The shape of a four electron group molecule with three outer atoms and one lone pair is