Question

predict the products of this organic reaction:

ch₂=c(ch₃)-c(=ch₂)-ch=ch₂ + 3 h₂ → (pd catalyst) ?

specifically, in the drawing area below draw the condensed structure of each pr you like.

if there is no reaction, check the no reaction box under the drawing area.

Explanation:

Step1: Identify the reaction type

The reaction is a hydrogenation reaction (addition of \(H_2\)) in the presence of a palladium (\(Pd\)) catalyst. This is a catalytic hydrogenation, which reduces carbon - carbon double bonds (\(C = C\)) to carbon - carbon single bonds (\(C - C\)) by adding \(H_2\) across the double bond.

Step2: Count the number of double bonds

The given organic compound \(\ce{CH2 = C(CH3)-C(=CH2)-CH = CH2}\) has three carbon - carbon double bonds (one at the left: \(\ce{CH2 = C}\), one in the middle: \(\ce{C = CH2}\), and one at the right: \(\ce{CH = CH2}\)).

Step3: Perform the hydrogenation

For each carbon - carbon double bond, we add two hydrogen atoms (from \(H_2\)). Since there are 3 moles of \(H_2\) (and each \(H_2\) molecule can reduce one \(C = C\) bond), all three double bonds will be reduced.

The original structure:
- The left double bond \(\ce{CH2 = C(CH3)}\) will become \(\ce{CH3 - CH(CH3)}\) after adding \(H_2\) (the \(C = C\) becomes \(C - C\) with \(H\) atoms added: \(\ce{CH2}\) adds one \(H\) to become \(\ce{CH3}\), and the \(\ce{C(CH3)}\) adds one \(H\) to become \(\ce{CH(CH3)}\)? Wait, no, more accurately, for a double bond \(\ce{C = C}\), each carbon gets one \(H\) from \(H_2\). So \(\ce{CH2 = C(CH3)-}\) becomes \(\ce{CH3 - CH(CH3)-}\) (the \(\ce{CH2}\) (with double bond) becomes \(\ce{CH3}\) (single bond, two \(H\) atoms: one from the original and one from \(H_2\)? Wait, the general reaction for catalytic hydrogenation of an alkene \(\ce{R - CH = CH - R' + H2\xrightarrow{Pd} R - CH2 - CH2 - R'}\).

So for the middle double bond \(\ce{-C(=CH2)-}\), it is \(\ce{-C(CH2)=}\) (wait, the structure is \(\ce{CH2 = C(CH3)-C(=CH2)-CH = CH2}\), so the middle carbon has a double bond to \(\ce{CH2}\), so \(\ce{-C(=CH2)-}\) becomes \(\ce{-CH2 - CH2 -}\) after adding \(H_2\) (the \(C = C\) (between \(C\) and \(CH_2\)) becomes \(C - C\), with each carbon getting one \(H\) from \(H_2\)).

For the right double bond \(\ce{-CH = CH2}\), it becomes \(\ce{-CH2 - CH3}\) after adding \(H_2\).

Putting it all together, after hydrogenating all three double bonds, the structure becomes \(\ce{CH3 - CH(CH3)-CH2 - CH2 - CH2 - CH3}\)? Wait, let's re - examine the original structure:

Original structure: \(\ce{CH2 = C(CH3)-C(=CH2)-CH = CH2}\)

Let's number the carbons:

Carbon 1: \(\ce{CH2}\) (double bonded to C2)

Carbon 2: \(\ce{C(CH3)}\) (double bonded to C1 and single bonded to C3)

Carbon 3: \(\ce{C}\) (double bonded to \(\ce{CH2}\) (C4) and single bonded to C2)

Carbon 4: \(\ce{CH2}\) (double bonded to C3)

Carbon 5: \(\ce{CH}\) (double bonded to C6)

Carbon 6: \(\ce{CH2}\) (double bonded to C5)

After hydrogenation (adding \(H_2\) across each \(C = C\) bond):

- C1 - C2 double bond: C1 (\(\ce{CH2}\)) becomes \(\ce{CH3}\) (adds one \(H\)), C2 (\(\ce{C(CH3)}\)) becomes \(\ce{CH(CH3)}\) (adds one \(H\))? No, the correct way is that each \(C = C\) bond takes one \(H_2\) molecule (\(H - H\)) and becomes \(C - C\) with each \(C\) getting one \(H\). So for \(\ce{CH2 = C(CH3)-}\) (C1 - C2), it becomes \(\ce{CH3 - CH(CH3)-}\) (C1: \(\ce{CH2}\) + \(H\) → \(\ce{CH3}\); C2: \(\ce{C(CH3)}\) + \(H\) → \(\ce{CH(CH3)}\))? Wait, no, the formula for the number of \(H_2\) required: each \(C = C\) bond needs 1 \(H_2\) to become \(C - C\). The given compound has three \(C = C\) bonds, so 3 \(H_2\) are used.

The product after hydrogenation will have all \(C = C\) bonds converted to \(C - C\) bonds. So the condensed structure is \(\ce{CH3 - CH(CH3)-CH2 - CH2 - CH2 - CH3}\)? Wait, let's count the carbons. The original compound has 6 carbons (C1: \(\ce{CH2}\), C2: \(\ce{C(CH3)}\), C3: \(\ce{C}\), C4: \(\ce{CH2}\), C5: \(\ce{CH}\), C6: \(\ce{CH2}\)). After hydrogenation, each \(C = C\) (C1 - C2, C3 - C4, C5 - C6) is converted to \(C - C\). So:

- C1 - C2: \(\ce{CH2 = C(CH3)}\) → \(\ce{CH3 - CH(CH3)}\)

- C3 - C4: \(\ce{C = CH2}\) → \(\ce{CH2 - CH2}\)

- C5 - C6: \(\ce{CH = CH2}\) → \(\ce{CH2 - CH3}\)

Putting it together: \(\ce{CH3 - CH(CH3)-CH2 - CH2 - CH2 - CH3}\) (2 - methylhexane? Wait, let's check the carbon chain. The longest chain is 6 carbons. Carbon 2 has a methyl group. So the condensed structure is \(\ce{CH3CH(CH3)CH2CH2CH2CH3}\) (or \(\ce{(CH3)2CHCH2CH2CH2CH3}\) but no, wait, the original structure:

Wait, the original structure is \(\ce{CH2 = C(CH3)-C(=CH2)-CH = CH2}\). Let's write it with proper bonding:

\(\ce{H2C = C(CH3)-C(=CH2)-CH = CH2}\)

So the carbon atoms:

1: \(\ce{H2C}\) (double bond to C2)

2: \(\ce{C(CH3)}\) (double bond to C1, single bond to C3)

3: \(\ce{C}\) (double bond to \(\ce{CH2}\) (C4), single bond to C2)

4: \(\ce{CH2}\) (double bond to C3)

5: \(\ce{CH}\) (double bond to C6)

6: \(\ce{CH2}\) (double bond to C5)

After hydrogenation:

- C1 - C2: \(\ce{H2C = C(CH3)}\) → \(\ce{H3C - CH(CH3)}\) (add \(H\) to C1 and C2)

- C3 - C4: \(\ce{C = CH2}\) → \(\ce{CH2 - CH2}\) (add \(H\) to C3 and C4)

- C5 - C6: \(\ce{CH = CH2}\) → \(\ce{CH2 - CH3}\) (add \(H\) to C5 and C6)

So the structure is \(\ce{CH3 - CH(CH3)-CH2 - CH2 - CH2 - CH3}\) (the carbon chain is 6 carbons, with a methyl group on carbon 2).

Answer:

The product of the catalytic hydrogenation reaction is \(\boldsymbol{\ce{CH3CH(CH3)CH2CH2CH2CH3}}\) (or 2 - methylhexane in IUPAC nomenclature, with the condensed structure as shown).