Chemical bonding question!
The partial Lewis structure that follows (Figure 1) is for a hydrocarbon molecule. In the full Lewis structure, each carbon atom satisfies the octet rule, and there are no unshared electron pairs in the molecule. The carbon-carbon bonds are labeled 1, 2, and 3 in order from left to right.
C=C-C(triple bond)C
Rank the carbon-carbon bonds in order of decreasing bond enthalpy.
Rank carbon-carbon bonds from highest bond enthalpy to lowest. To rank bonds as equivalent, overlap them.
To rank the carbon-carbon bonds in order of decreasing bond enthalpy, we need to consider the strength of the bonds. The strength of a bond is typically determined by the amount of energy required to break the bond.
In this case, we have three carbon-carbon bonds labeled 1, 2, and 3. The bond enthalpy increases with the number of bonds between the carbon atoms. So, we can expect that the triple bond (bond 3) will have the highest bond enthalpy, followed by the double bond (bond 2), and then the single bond (bond 1).
To confirm this, we can look at the periodic trends of bond enthalpy. Carbon-carbon bonds involve the sharing of electrons, and the energy required to break these bonds depends on the strength of the bond and the stability of the resulting fragments. Generally, double and triple bonds are stronger and have higher bond enthalpies compared to single bonds.
To get the exact bond enthalpies, we can refer to the Experimental Standard Bond Enthalpy Table. This table provides the average bond enthalpy values for various types of bonds. By looking up the bond enthalpies for the carbon-carbon single, double, and triple bonds, we can determine the exact values and rank them accordingly.
It's important to note that bond enthalpy values can vary due to factors such as molecular environment and the presence of functional groups. However, in a general hydrocarbon molecule like the one given, the trend of triple bond > double bond > single bond in terms of bond enthalpy holds.
To rank the carbon-carbon bonds in order of decreasing bond enthalpy, we need to consider the strength of the different types of bonds between the carbon atoms.
In the given hydrocarbon molecule (C=C-C≡C), there are three carbon-carbon bonds labeled as 1, 2, and 3 in order from left to right.
Bond 1: C=C
Bond 2: C-C
Bond 3: C≡C
Now, let's analyze the bond strengths:
1. Bond 3 (C≡C) - Triple Bond: Triple bonds consist of one sigma bond and two pi bonds. Pi bonds are generally weaker than sigma bonds, so a triple bond will be stronger than a double bond.
2. Bond 1 (C=C) - Double Bond: Double bonds consist of one sigma bond and one pi bond. Pi bonds are relatively weaker than sigma bonds.
3. Bond 2 (C-C) - Single Bond: Single bonds consist of only one sigma bond. Sigma bonds are generally stronger than pi bonds.
Based on this analysis, we can rank the carbon-carbon bonds in order of decreasing bond enthalpy:
Bond 3 (C≡C) > Bond 1 (C=C) > Bond 2 (C-C)
Therefore, ranked from highest bond enthalpy to lowest, the bonds are:
1. Bond 3 (C≡C)
2. Bond 1 (C=C)
3. Bond 2 (C-C)