Two hydrogen atoms interact to form a hydrogen molecule. Classify the following statements that describe the stages of bond formation in a hydrogen molecule according to the predominant force existing between the two hydrogen atoms.1. The two hydrogen atoms are very far apart. 2. The internuclear distance between the two hydrogen atoms is less than the bond length. 3. The potential energy of the system is at a minimum. 4. The potential energy of the system is positive.5. The two hydrogen atoms approach each other to form a bond. 6. The two hydrogen atoms form a stable hydrogen molecule. 7. The two hydrogen atoms start to combine to form a hydrogen molecule.8. The attractive force is predominant between the two atoms9. Repulsive force is predominant between the two atoms10. Attractive and repulsive forces balance each other11. There is no interaction between the two atoms

Attractive force is predominant between the two atoms

The two hydrogen atoms approach each other to form a bondThe two hydrogen atoms start to combine to form a hydrogen molecule

Repulsive force is predominant between the two atoms

The potential energy of the system is positiveThe internuclear distance between the two hydrogen atoms is less than the bond length

Attractive and repulsive forces balance each other

The two hydrogen atoms form a stable hydrogen moleculeThe potential energy of the system is at minimum

There is no interaction between the two atoms

The hydrogen atoms are very far apart

Explanations:

increase in potential energy causes repulsion between the atoms, whereas decrease in potential energy causes attraction between the atomsin order for the bonding to occur, the attractive forces must be greater than the repulsion forces.The potential energy is positive when the repulsion forces is greater. This is because the distance between the two atoms is smaller than the bond lengthThe potential energy of the system is at its minimum because the attractive and repulsive forces balance out each other.

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