Figure 3 shows the reaction between ethene and chlorine and is similar to the reaction between ethene and bromine. The more energy levels (shells) of electrons an atom has, the weaker the covalent bonds that it forms.”Use the above statement to predict and explain how the overall energy change for the reaction of ethene with chlorine will differ from the overall energy change for the reaction of ethene with bromine. – 6168

One thought on “Figure 3 shows the reaction between ethene and chlorine and is similar to the reaction between ethene and bromine. The more energy levels (shells) of electrons an atom has, the weaker the covalent bonds that it forms.”Use the above statement to predict and explain how the overall energy change for the reaction of ethene with chlorine will differ from the overall energy change for the reaction of ethene with bromine. – 6168”

1. Chlorine atoms are smaller because they have fewer electron shells than bromine. This means chlorine can form stronger bonds.

   The Cl–Cl bond is stronger than Br–Br, and the C–Cl bond is also stronger than the C–Br bond.

   Because of this, it takes more energy to break bonds with chlorine. But also, more energy is released when forming new bonds with chlorine.

   So overall, the energy change depends on how much energy is needed to break and how much is released when bonds form.

   Conclusion:
   If the C–Cl bond increases more in strength, the reaction will be more exothermic.

   If the Cl–Cl bond gets harder to break, then it could be less exothermic.

   We can’t tell for sure how much the total energy change will be, unless we know which bond energy changes more.

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