AP Chemistry Flashcards: Intramolecular Force and Potential Energy
Written by AP Content Team, Verified for 2026 AP Exams, Last updated: May 2026
Review key ideas with interactive flashcards. This set includes 10 cards to help you master important concepts.
How does the potential energy between two atoms change as they approach each other from a great distance to form a bond?
As the atoms approach, potential energy decreases until it reaches a minimum at the equilibrium bond length, after which it increases sharply due to internuclear repulsion.
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How does the potential energy between two atoms change as they approach each other from a great distance to form a bond?
As the atoms approach, potential energy decreases until it reaches a minimum at the equilibrium bond length, after which it increases sharply due to internuclear repulsion.
What does the potential energy minimum (the 'well') on a potential energy vs. internuclear distance graph represent?
The potential energy minimum represents the bond energy, which is the amount of energy required to separate the two bonded atoms.
What are the two primary factors that influence the length of a covalent bond?
The length of a covalent bond is influenced by the size of the atom cores and the bond order between the atoms.
On a potential energy versus internuclear distance graph, what is the equilibrium bond length?
The equilibrium bond length is the distance between atoms that corresponds to the minimum potential energy on the graph.
Which would have a higher bond energy: a C-C single bond or a C≡C triple bond? Why?
The C≡C triple bond would have a higher bond energy because its higher bond order results in a shorter, stronger bond.
What is bond energy?
Bond energy is the energy required to separate two bonded atoms from their equilibrium bond length to an infinite distance apart.
According to Coulomb's law, what two factors lead to a stronger ionic interaction?
A stronger ionic interaction is caused by larger ionic charges and smaller distances between the ions (smaller ionic radii).
Which ionic compound would have a stronger interaction: LiF or NaCl? Explain using the principles of Coulomb's law.
LiF would have a stronger interaction because Li+ and F- are smaller ions than Na+ and Cl-, resulting in a smaller distance between the charges.
How does a higher bond order affect the length and strength of a covalent bond?
A higher bond order results in a covalent bond that is both shorter and stronger, meaning it has a higher bond energy.
What law is used to explain the strength of an ionic interaction?
Coulomb's law is used to explain ionic interaction strength, relating it to the magnitude of the charges and the distance between the ions.