Chemical Species/Chemical Interactions: 1. a.) Cu (s) Atomic b.) H 2 O (s) Molecular c.) NaCl (s) Ionic d.) Fe (s) Atomic 3. This mixture would be miscible because both molecules are polar. 5. A solution that mixes completely, without any particles left unmixed. Homogenous mixtures are most commonly thought of as a mixture behaving as a single substance. Intermolecular Forces: 7. a.) CH 4 Dispersion b.) HF H-Bond c.) H 2 O H-Bond d.) CHCl 3 Dipole-Dipole 9. a.) CH 3 CH 2 OH Dispersion, Dipole-Dipole, H-Bond b.) CCl 4 Dispersion c.) CHF 3 Dispersion, Dipole-Dipole 11. When a Hydrogen atom is bonded directly to a Nitrogen, Fluorine, or Oxygen atom. 13. CH 4 , CH 3 CHO 2 , HF 15. a.) CO Dispersion, Dipole-Dipole b.) HBr Dispersion, Dipole-Dipole c.) CCl 4 Dispersion d.) KCl ion-ion 17. c.) H-Bond 19. a.) ammonia H-Bond b.) silicon dioxide Dispersion c.) ethanol H-Bond d.) acetic acid H-Bond 21. b.) Dipole-Dipole 23. a.) CH 4 25. a.) I 2 Dispersion b.) F 2 Dispersion c.) SO 2 Dipole-Dipole d.) HCH 3 COO H-Bond Boiling/Melting Point: 27. The molecule with the higher boiling point will be the molecule with the strongest intermolecular force. If they all have the same intermolecular force, then you will need to determine which molecule is the longest. 29. *remember: Ionic bonding is stronger than Hydrogen bonding!* NaCl > CH 3 CH 2 OH > CHCl 3 > Ar 31. At room temperature, the molecule with the stronger intermolecular force will be a liquid. CO 2 only possesses dispersion forces, while CH 3 OH possesses hydrogen-bonding forces. Therefore, CH 3 OH will be a liquid at room temperature. 33. NaCl will have the higher melting point because ionic bonding between sodium and chlorine is stronger than the dispersion forces in methane. 35. a.) NH 4 Cl *Remember: NH 4 + and Cl - form an ionic bond* 37. c.) CH 4 39. b.) HCl 41. HI > HBr > HCl 43. Octane > Hexane > Butane 45. No, ethanol and propane will not have the same boiling point because we have to put the intermolecular forces into account when deciding boiling points—not just their molar mass. Because ethanol has hydrogen-bonding forces, ethanol will have the higher boiling point. 47. a.) propanol and methanol b.) methane and pentane c.) dihydrogen monoxide and dihydrogen monosulfide 49. Acetic acid would most likely be a liquid at room temperature because of the strong hydrogen-bonding forces. 51. CH 3 CH 2 COH will have the higher boiling point because of the strong hydrogen-bonding forces present in the molecule. 53. b.) CH 4 Cumulative/Challenge Problems: 55. No, a hydrogen-bond would not be able to form by connecting two acetone molecules together because the hydrogen atom would not be covalently bonded to the oxygen atom in the structure. For a hydrogen-bond to form, the hydrogen atom must be covalently bonded to either Nitrogen, Fluorine, or Oxygen atoms. 57. b.) vinegar 59. a.) acetone Dipole-Dipole b.) butane Dispersion c.) iso-butane Dispersion