All Flashcards
Define intramolecular forces.
Forces that hold atoms together within a molecule.
Define intermolecular forces.
Forces that exist between molecules.
Define equilibrium bond length.
The distance between atoms where potential energy is at its lowest; the most stable distance.
Define bond energy.
The energy required to break a bond; the difference in potential energy between separated atoms and atoms at their equilibrium bond length.
Define bond order.
The number of chemical bonds between a pair of atoms.
Define Coulomb's Law (in context of ionic bonds).
The principle that the strength of attraction between ions is directly proportional to the magnitude of the charges and inversely proportional to the distance between them.
What is the effect of increased charge magnitude on ionic bond strength (Coulomb's Law)?
Stronger ionic interactions/attraction.
What is the effect of increased distance between ions on ionic bond strength (Coulomb's Law)?
Weaker ionic interactions/attraction.
What is the effect of electron-electron repulsion when atoms are too close?
Increases potential energy, making the bond unstable.
What is the effect of atoms being too far apart to form a bond?
No bond forms, and potential energy is near zero.
What is the effect of higher bond energy on bond strength?
Stronger, more stable bond.
What is the effect of lower potential energy on bond stability?
More stable bond.
Compare and contrast intramolecular and intermolecular forces.
Intramolecular: Forces within a molecule, stronger, determine chemical properties. Intermolecular: Forces between molecules, weaker, determine physical properties like boiling point.
Compare single, double, and triple covalent bonds in terms of bond length.
Single: Longest | Double: Intermediate | Triple: Shortest
Compare single, double, and triple covalent bonds in terms of bond energy.
Single: Smallest | Double: Intermediate | Triple: Largest
Compare single, double, and triple covalent bonds in terms of stability.
Single: Least Stable | Double: Medium Stability | Triple: Most Stable
How does the potential energy curve differ for two atoms with a strong bond versus a weak bond?
Strong bond: Deeper potential energy well (higher bond energy) | Weak bond: Shallower potential energy well (lower bond energy)