Intramolecular and Interparticle Force - AP Chemistry

1. Which has a higher boiling point: $\text{CH}_3\text{OH}$ or $\text{CH}_4$?

   $\text{CH}_3\text{OH}$. Methanol has hydrogen bonding unlike nonpolar methane.

2. Which has stronger intermolecular forces: $\text{H}_2\text{O}$ or $\text{CO}_2$?

   $\text{H}_2\text{O}$. Water has hydrogen bonding vs. CO₂'s weak dispersion forces.

3. Which intermolecular force is present in $\text{CO}_2$?

   London dispersion forces. Nonpolar CO₂ only has weak temporary dipole attractions.

4. Which force is primarily responsible for the high boiling point of water?

   Hydrogen bonding. H-O bonds create strong intermolecular attractions.

5. Which is stronger: hydrogen bond or van der Waals forces?

   Hydrogen bond. Hydrogen bonds are stronger than dispersion forces.

6. Identify the type of bond in diatomic oxygen ($\text{O}_2$).

   Double covalent bond. Two pairs of electrons are shared between oxygen atoms.

7. What is the predominant intermolecular force in $\text{NH}_3$?

   Hydrogen bonding. N-H bonds enable strong hydrogen bonding interactions.

8. What type of interaction occurs between polar molecules?

   Dipole-dipole interactions. Permanent dipoles align positive to negative ends.

9. What is the term for the energy required to break one mole of bonds in gaseous molecules?

   Bond enthalpy. Energy needed to completely separate bonded atoms.

10. Which has stronger intermolecular forces: $\text{H}_2\text{O}$ or $\text{CO}_2$?

    $\text{H}_2\text{O}$. Water has hydrogen bonding vs. CO₂'s weak dispersion forces.

11. What is the molecular geometry of $\text{CO}_2$?

    Linear. Two bonding groups with no lone pairs on carbon.

12. Which interaction can occur between a polar molecule and an ion?

    Ion-dipole interaction. Charge attracts to opposite partial charge on molecule.

13. What is the VSEPR shape of $\text{BF}_3$?

    Trigonal planar. Three bonding groups arrange in flat triangle.

14. Which has stronger intermolecular forces: $\text{H}_2\text{O}$ or $\text{CO}_2$?

    $\text{H}_2\text{O}$. Water has hydrogen bonding vs. CO₂'s weak dispersion forces.

15. Which force is stronger: dipole-dipole or London dispersion?

    Dipole-dipole. Permanent dipoles are stronger than temporary ones.

16. What is the bond type in a molecule with a large difference in electronegativity?

    Ionic bond. Electronegativity difference > 1.7 typically results in electron transfer.

17. Which bond is stronger: single, double, or triple covalent bond?

    Triple covalent bond. More shared electrons create stronger, shorter bonds.

18. State the type of bond formed by the sharing of electron pairs.

    Covalent bond. Electrons are shared between atoms in overlapping orbitals.

19. What is the molecular geometry of $\text{H}_2\text{O}$?

    Bent. Two bonds plus two lone pairs create angular shape.

20. What type of bond forms between $\text{H}$ and $\text{Cl}$ in $\text{HCl}$?

    Polar covalent bond. Chlorine is more electronegative, creating unequal sharing.

21. Which type of bond involves the transfer of electrons?

    Ionic bond. Complete electron transfer from metal to nonmetal occurs.

22. What is the primary intermolecular force in $\text{CH}_4$?

    London dispersion forces. Nonpolar methane only exhibits weak temporary dipole forces.

23. What is the VSEPR shape of $\text{BF}_3$?

    Trigonal planar. Three bonding groups arrange in flat triangle.

24. What type of bond is present in $\text{H}_2\text{O}$?

    Polar covalent bond. O is more electronegative than H, creating unequal sharing.

25. Identify the strongest type of interparticle force present in water.

    Hydrogen bonding. H bonded to O creates strong dipole-dipole interactions.

26. What is the term for the energy change when a bond is formed?

    Bond formation enthalpy. Energy released when atoms combine to form bonds.

27. What is the bond angle in a molecule with trigonal planar shape?

    120 degrees. Three electron groups spread equally around central atom.

28. Identify the type of force that holds $\text{Na}^+$ and $\text{Cl}^-$ together.

    Ionic bond. Electrostatic attraction between oppositely charged ions.

29. What is the VSEPR shape of $\text{BF}_3$?

    Trigonal planar. Three bonding groups arrange in flat triangle.

30. What type of bond is present in $\text{H}_2\text{O}$?

    Polar covalent bond. O is more electronegative than H, creating unequal sharing.

31. What is the molecular geometry of $\text{NH}_3$?

    Trigonal pyramidal. Three bonds plus one lone pair create pyramid shape.

32. What type of interaction occurs between nonpolar molecules?

    London dispersion forces. Temporary dipoles induce attractions in all molecules.

33. Which has stronger intermolecular forces: $\text{HCl}$ or $\text{Ar}$?

    $\text{HCl}$. HCl has dipole-dipole forces vs. Ar's dispersion only.

34. What is the typical bond angle in a tetrahedral molecule?

    109.5 degrees. Four electron groups arrange to minimize repulsion.

35. What is the strongest type of intramolecular force?

    Covalent bond. Shared electrons create the strongest molecular attractions.

36. Name the type of bond formed between metals and nonmetals.

    Ionic bond. Metal cations and nonmetal anions attract electrostatically.

37. Which molecule has a higher boiling point: $\text{H}_2\text{O}$ or $\text{H}_2\text{S}$?

    $\text{H}_2\text{O}$. Hydrogen bonding in water vs. weaker forces in H₂S.

38. Identify the weakest type of intermolecular force.

    London dispersion forces. Temporary induced dipoles provide minimal attraction.

39. What type of bonding is predominant in metallic substances?

    Metallic bonding. Sea of delocalized electrons holds metal atoms together.

40. What is the term for the attraction between molecules of the same substance?

    Cohesion. Intermolecular forces between identical molecules.

41. What type of bond is present in $\text{H}_2\text{O}$?

    Polar covalent bond. O is more electronegative than H, creating unequal sharing.

42. What is the term for the attraction between different substances?

    Adhesion. Forces between molecules of different substances.

43. Name the type of intermolecular force that exists between ions and polar molecules.

    Ion-dipole interactions. Charges attract polar molecule's partial charges.

44. Identify the main type of intermolecular force in $\text{CCl}_4$.

    London dispersion forces. Large, polarizable molecule exhibits strong dispersion forces.

45. What is the VSEPR shape of $\text{CH}_4$?

    Tetrahedral. Four bonding groups around carbon minimize repulsion.

46. What is the primary intermolecular force in $\text{C}_2\text{H}_5\text{OH}$?

    Hydrogen bonding. O-H bond enables hydrogen bonding with other molecules.

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