Let's solve for structure **h** as an example. The same process can be followed for the rest. --- ## Step-by-Step Solution for Structure h ### Step 1: Redraw the Structure with All Atoms and Electrons Structure **h**: It's a vinylic cation: ``` + | CH2=CH-CH=CH2 ``` Draw all hydrogen atoms: - Leftmost carbon (C1, with the positive charge) is CH₂⁺ (missing one bond). - Second carbon (C2) is attached to C1 and has a double bond with C3. - C3 has a double bond with C2 and a single bond with C4. - C4 is a CH₂ group. So, the expanded structure is: ``` H2C⁺-CH=CH-CH2 ``` ### Step 2: Draw Resonance Structures with Arrows #### Structure 1 (Starting Structure) ``` H2C⁺-CH=CH-CH2 ``` - Positive charge on C1. #### Structure 2 Move the pi electrons from the C2=C3 double bond **toward** the C1-C2 single bond: Curved arrow: from the double bond (C2=C3) to between C1 and C2. Result: ``` H2C=CH-CH⁺-CH2 ``` - Now, the positive charge is on C3. #### Structure 3 Move the pi electrons from the C3-C4 single bond (now C3 is positive) to form a new double bond: Curved arrow: from the two electrons in the C3-C4 bond, move to between C3 and C4. Result: ``` H2C=CH-CH=CH2⁺ ``` - Now, the positive charge is on C4. ### Step 3: Assign Formal Charges In all three structures, the positive charge is always on a carbon atom. ### Step 4: Circle the Most Contributing Structure The **most contributing resonance structure** is usually the one that: - Has the positive charge on the most substituted carbon (most stable carbocation). - Has the least separation of charges (here, all are carbocations). For this system, the most stable is the one where the positive charge is on the carbon that is allylic or more substituted. In this case, the most stable is the one with the positive charge on the internal carbon, **Structure 2**: ``` H2C=CH-CH⁺-CH2 ``` --- ## Summary Table | Structure | Resonance Form | Formal Charge Location | |-----------|------------------------------------------|-----------------------| | 1 | H2C⁺-CH=CH-CH2 | Leftmost C | | 2 | H2C=CH-CH⁺-CH2 | Internal C (C3) | | 3 | H2C=CH-CH=CH2⁺ | Rightmost C | **Most contributing structure (circle this):** **H2C=CH-CH⁺-CH2** --- ## **Repeat for i, j, k** Follow the same steps: 1. Draw all hydrogens and lone pairs. 2. Use arrows to show electron movement for resonance. 3. Assign formal charges. 4. Circle the most stable resonance contributor. If you'd like, I can show the step-by-step for another specific molecule (i, j, or k). Let me know which you'd like next!