If you calculated the bond enthalpies, wouldn't you be in a better position to tell us the trend, rather than us telling you?ReidMerrill said:Need to find a trend in predicting the bond enthalpy of several atom-hydrogen bonds I calculated using gaussian.
I just wondered if there was supposed to be a trend since they don't appear to follow any pattern.TeethWhitener said:If you calculated the bond enthalpies, wouldn't you be in a better position to tell us the trend, rather than us telling you?
Bond enthalpy, also known as bond energy, is the amount of energy required to break a chemical bond between two atoms in a molecule.
Bond enthalpy is typically measured in units of kilojoules per mole (kJ/mol) and is determined experimentally using calorimetry or spectroscopy techniques.
The periodic trend for bond enthalpy is that it generally increases as you move across a period from left to right, and decreases as you move down a group on the periodic table. This is due to the increasing electronegativity and decreasing atomic size of elements across a period.
A higher bond enthalpy indicates a stronger bond, which results in a more stable molecule. This is because it requires more energy to break the bond, making it less likely for the molecule to undergo chemical reactions.
While bond enthalpy can give an indication of the strength of a chemical bond, it is not the only factor that affects bond strength. Other factors such as bond length, bond angle, and molecular geometry also play a role in determining the overall strength of a bond.