Is breaking bonds endothermic or exothermic?
Question
Is breaking bonds endothermic or exothermic?
Solution
Breaking bonds is an endothermic process. This means it requires energy to break the bonds in the reactant molecules. This energy is usually in the form of heat, which is absorbed from the surroundings. This is why the term 'endothermic' is used, as it comes from the Greek words 'endo' meaning 'inside' and 'therm' meaning 'heat'. So, in an endothermic reaction, heat is taken in from the environment.
Here are the steps to understand this:
- Consider a molecule, which is made up of atoms bonded together.
- To break these bonds and separate the atoms, energy is required.
- This energy is absorbed from the surroundings, making the process endothermic.
- The absorbed energy is used to overcome the forces holding the atoms together, thus breaking the bonds.
So, breaking bonds is an endothermic process because it requires the absorption of energy.
Similar Questions
In an exothermic reaction, which is greater: the energy released from forming new bonds, or the energy needed to break existing bonds?
Which of the following statements is true?Breaking bonds is endothermic, making bonds is exothermicBreaking bonds and making bonds are both exothermicBreaking bonds and making bonds are both endothermicBreaking bonds is exothermic, making bonds is endothermic
Which of the following statements is true?Breaking bonds and making bonds are both endothermicBreaking bonds is endothermic, making bonds is exothermicBreaking bonds is exothermic, making bonds is endothermicBreaking bonds and making bonds are both exothermic2When calculating energy changes from bond energies, what is the first thing you should do?Calculate the bond energies of the reactantsSubtract the bond energies of the products from those of the reactantsBalance the equationCalculate the bond energies of the products3If a reaction requires more energy to break the bonds in the reactants than the amount of energy released when new bonds are formed, what does this tell us?It is exothermicThe product is a gasIt is endothermicThe reactant is a solid4Calculate the energy required to break the bonds in propane (C3H8) given the following bond energies: C-C = 347 kJ/mol; C-H = 413 kJ/mol.1520 kJ/mol3998 kJ/mol4345 kJ/mol760 kJ/mol
exothermic and endothermic
What are the differences between endothermic and exothermic reactions?
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