The statement added is inherently wrong “Breaking bonds is an exergonic process” same with the opposite that you suggested for another card. I want you to think about the gibbs free energy formula G = H - TS. Enthalpy (H) is H = broken - formed. The broken is actually what takes energy and bonds formed is what releases energy. The Complication of the formulas does not make it as simple as broken = endergonic though. Always good to cite your sources to here is uworld biochem.
Uworld: in ATP hydrolysis (Figure 10.7), a phosphoanhydride bond and an O–H bond break, but another O–H bond forms (in the released inorganic phosphate) and a P–OH bond forms on the β-phosphate of ADP. The energy of the bonds formed outweighs that of the bonds broken, yielding an overall exothermic process (ie, a negative ΔH) and contributing to the favorability of the reaction. However, not all exothermic reactions are exergonic, and not all hydrolysis reactions are as exergonic as ATP hydrolysis. Exergonic reactions are considered energy releasing because their products have less free energy than their reactants.
This is what UWorld said about hydrolysis of macromolecules being a spontaneous reaction, so Negative Delta G, which is exergonic. What am I missing here
What you stated is an oversimplification. Notice how uworld never mentions bonds broken = exergonic. They say hydrolysis. That’s because in hydrolysis the formation of the molecule is what actually releases the energy and makes it exergonic. Not the breaking of the bonds. Breaking of the bonds is the activation energy and thus it requires energy.
Ah okay I see now, thanks for clarifying that. Man these topics get confusing sometimes