Question

Which is a valid statement about bond formation?
A) potential energy decreases
B) Potential energy increases
C) Exothermic
D) Endothermic

Answer 1

Hint: A chemical bond is a long-term attraction between atoms, ions, or molecules that allows chemical compounds to form. Ionic bonds are formed by the electrostatic force of attraction between oppositely charged ions, whereas covalent bonds are formed by the sharing of electrons.

Complete answer:
The amount of energy contained in a bond between atoms in a molecule is described by bond enthalpy (also known as bond-dissociation enthalpy, average bond energy, or bond strength). In the gas phase, it's the energy that must be supplied for the homolytic or symmetrical cleavage of a bond. When a homolytic or symmetrical bond is broken, each of the original participants in the bond receives one electron and becomes a radical, rather than an ion.
Chemical bonds develop when the thermodynamics are favourable, and breaking them necessitates the addition of energy. As a result, bond enthalpy values are always positive, and they are generally expressed in kJ/mol units. The higher the enthalpy of a bond, the more energy is required to break it and the stronger the bond. We just make the bond's enthalpy value negative to calculate how much energy will be released when we establish a new bond rather than breaking it.
A bond can only exist if breaking it requires energy, therefore the bond dissociation energy is always positive. The creation of bonds is always an exothermic activity, while the breakdown of bonds is always an endothermic process. The system loses energy and gains stability as bonds are created. Because there is a loss of energy, the lost energy is released as heat energy, making this an exothermic process.
Hence option A and C are correct.

Note:
Because bond enthalpy values are so helpful, reference tables with average bond enthalpies for common bond types are widely available. While the exact energy shift while establishing and breaking bonds is dependent on adjacent atoms in a given molecule, the average values in the tables can still be used as a rough guide.