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Do endothermic reactions make stronger bonds?

Posted on August 28, 2022 by Author

Do endothermic reactions make stronger bonds?

In endothermic reactions, the reactants have higher bond energy (stronger bonds) than the products.

What happens to bonds in an endothermic reaction?

Chemical reactions that absorb (or use) energy overall are called endothermic. In endothermic reactions, more energy is absorbed when the bonds in the reactants are broken than is released when new bonds are formed in the products.

Does an exothermic reaction break stronger bonds to form weaker ones?

Usually an exothermic reaction corresponds to the breaking of weak bonds (with small bond enthalpies) and the making of strong bonds (with large bond enthalpies).

Are endothermic products more stable than reactants?

In the case of an endothermic reaction, the reactants are at a lower energy level compared to the products—as shown in the energy diagram below. In other words, the products are more stable than the reactants.

Are the bonds formed in the products stronger or weaker than the bonds broken in the reactants?

-The bonds formed in the products are stronger than the bonds broken the reactants. The bond dissociation energy is the energy needed to break a covalent bond by equally diving the electrons between the two atoms in the bond. -The higher the bond dissociation energy, the stronger the bond.

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Why are product bonds stronger in exothermic?

When the energy absorbed from the breaking of old bonds is less than the energy released from making new bonds, the excess energy from making new bonds is released as heat, forming an exothermic reaction. These new bonds are stronger, because they released more energy than the bonds in the reactants.

When the bonds in the products are stronger than the bonds in the reactants the reaction is?

When the bonds in product molecules are stronger than those in reactant molecules, the reaction is endothermic.

Why are exothermic reactions more common than endothermic?

Exothermic reactions represent energetically favorable transformations and are more spontaneous than endothermic reactions, so it stands to reason that there are “more exothermic reactions.” From the second law of thermodynamics we know that the entropy of the universe will increase for all spontaneous processes.

Which reaction is more stable endothermic or exothermic?

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You are correct. Exothermic reactions where things that go to a lower energy state are generally more stable. Endothermic is vice versa. If elements go to a higher energy state, they are generally less stable.

Are endothermic or exothermic bonds stronger?

Endothermic reactions will form weaker bonds compared to its reactants, while exothermic reactions will form stronger bonds.

Are bonds formed or broken stronger?

Are bonds formed stronger than bonds broken?

What is an endothermic reaction?

Endothermic reaction means energy is absorbed in the process. Whenever a bond is formed , energy is always released. This in turn implies that when a bond is broken , energy needs to be supplied.

What happens when bonds are broken in exothermic reactions?

This in turn implies that when a bond is broken , energy needs to be supplied. If the bonds in product are stronger than those in reactants , more energy is released from the product compared to the energy absorbed to break the bonds in reactants . So overall, energy is released making it exothermic.

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Why is the ΔH° value negative in exothermic reactions?

When the released energy during the formation of bonds in the molecules of the products is higher than the absorbed energy during the breaking of bonds in the molecules of the reactants , So , The reaction will be exothermic and its ΔH° value will have a negative sign .

What happens when the bonds in reactants are weaker than products?

Vice versa , if the bonds in the product are weaker than the bonds in reactants, the formation of product releases less energy compared to the energy required to break the reactants bonds. Overall, there is a deficiency in energy and hence the required amount of energy needs to be supplied for the reaction to occur.

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