Chemical Species/Chemical Interactions:
1. a.) Cu(s) Atomic
b.) H2O(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.
7. a.) CH4 Dispersion
b.) HF H-Bond
c.) H2O H-Bond
d.) CHCl3 Dipole-Dipole
9. a.) CH3CH2OH Dispersion, Dipole-Dipole, H-Bond
b.) CCl4 Dispersion
c.) CHF3 Dispersion, Dipole-Dipole
11. When a Hydrogen atom is bonded directly to a Nitrogen, Fluorine, or Oxygen atom.
13. CH4 , CH3CHO2 , HF
15. a.) CO Dispersion, Dipole-Dipole
b.) HBr Dispersion, Dipole-Dipole
c.) CCl4 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.) CH4
25. a.) I2 Dispersion
b.) F2 Dispersion
c.) SO2 Dipole-Dipole
d.) HCH3COO H-Bond
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 > CH3CH2OH > CHCl3 > Ar
31. At room temperature, the molecule with the stronger intermolecular force will be a liquid. CO2 only possesses dispersion forces, while CH3OH possesses hydrogen-bonding forces. Therefore, CH3OH 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.) NH4Cl *Remember: NH4+ and Cl- form an ionic bond*
37. c.) CH4
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. CH3CH2COH will have the higher boiling point because of the strong hydrogen-bonding forces present in the molecule.
53. b.) CH4
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