Question

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ᴅᴇғɪɴᴇ ʙᴏɴᴅ ᴇɴᴛʜᴀʟᴘʏ?¿

sᴏʀʀʏ(〒﹏〒)​(〒﹏〒)​

Answer 1

Answer:

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• Bond Enthalpy, also known as bond energy, is a quantity that offers insight into the strength of a chemical bond and, by extension, its stability. The bond enthalpy of a chemical bond can be defined as the total amount of energy required to break 1 mole of that chemical bond. For example, the bond enthalpy of the oxygen-hydrogen single bond is equal to 463 kJ/mol. This implies that a total of 463 kilojoules of energy is required to break 1 mole of hydrogen-oxygen single bonds.

• It is important to note that the breaking of a chemical bond is always an endothermic process (because energy must be supplied to the molecule in order to break the chemical bonds that constitute it). Thus, the enthalpy change associated with the breaking of a chemical bond is always positive (ΔH > 0). On the other hand, the formation of a chemical bond is almost always an endothermic process. In such cases, the enthalpy change will have a negative value (ΔH < 0).

Answer 2

Explanation:

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In chemistry, bond energy, also called the mean bond enthalpy or average bond enthalpy is the measure of bond strength in a chemical bond. IUPAC defines bond energy as the average value of the gas-phase bond-dissociation energy for all bonds of the same type within the same chemical species