Sulfur hexafluoride SF6 is the most potent greenhouse gas to date. It is 22,800 times more effective at trapping heat than carbon dioxide (CO2), and lasts in the atmosphere for thousands of years. Please refer to the molecule diagrams below to answer the following questions:                 a. Explain why SF6 has more asymmetrical vibrations than CO2 b. Explain why asymmetrical vibrations in SF6 bonds are stronger than asymmetrical vibrations in CO2 bonds  c. Explain the relationship between strength and quantity of asymmetrical vibrations and greenhouse gas potency

Methane, CH4, has the ideal tetrahedral angle (109.5°) and is a nonpolar molecule, while NH3 and H₂O show a deviation from the ideal bond angle. Explain the cause and why water has a greater deviation than ammonia.

Explain the trend that bond formation does to atomic order by selecting all those that apply. Larger molecules have higher entropies than smaller molecules. Larger molecules have larger entropies on a per atom basis. Larger molecules have lower entropies than smaller molecules. Larger molecules have smaller entropies on a per atom basis.

11. What is the electron-domain geometry of water molecule (H2O)? a. bent b. tetrahedral c. trigonal planar d. linear 12. Write the correct Lewis dot structure for O2. Which statement correctly describes the structure of the whole molecule? a. There is a double bond and four lone pairs. b. There is a double bond and six lone pairs. c. There is a single bond and six lone pairs. d. There is a single bond, a double bond, and six lone pairs. 13. If there are four (4) electron pairs around the central atom of a molecule, these electron pairs are in a/n a. trigonal planar b. trigonal pyramidal arrangement. C. octahedral d. tetrahedral 14 The molecular geometry of the molecule NF3 is a. linear b. trigonal pyramidal c. tetrahedral d. trigonal planar 15 Which of the following species will exhibit tetrahedral molecular geometry? d. PCI5 a. CCI4 b. CO2 C. O3

What information does the molecular representation provide? (more than one option)1. The number and type of atoms2. Two-dimensional structure of molecules3. The type of link4. How Atoms Bond5. The intermolecular force6. Three-dimensional structure of molecules7. Polarity8. More realistic representation of molecules

16. For the molecule BrF5, what is its molecular geometry? Group of answer choices A. Square pyramid B. Octahedral C. trigonal pyramid D. tetrahedral

56. Use bond enthalpies to calculate AH° for the reaction of methane with rxn chlorine and fluorine to form CF₂Cl₂ (Freon–12). CH4(g) + 2 Cl₂(g) + 2 F₂(g) → CF₂Cl₂(g) + 2 HF(g) + 2 HCl(g)

Compound ∆Hf (kJ/mole) ∆S (J/mole K) C2H4 52.4 219.3 C2H6 –84.68 229.2 SiO2 –910.7 41.5   HF –273.3 173.8 SiF4 –1615.0 282.8 NH3 –45.9 192.9 O2 1.88 2.43 NO 91.3 210.8 H2O(g) –241.8 188.8 For the following reactions, using the provided ∆H and ∆S data, determine whether each one would be spontaneous or nonspontaneous at 25°C. C2H4(g) + H2(g) --------à                                  C2H6(g)                 SiO2 + 4 HF(g) ------------->             SiF4 (g) + 2 H2O(g)               4 NH3(g)  +  5 O (g)  ---------> 4 NO(g) + 6 H2O(g)

Consider how bond strength affects the speed of particles. Describe what happens to the kinetic energy of particles after a single bond is broken compared to a stronger double bond. You can answer this question with words, pictures, or graphs.

What are the angles a and b in the actual molecule of which this is a Lewis structure? H H H C H a a = C b = ⁰ C H Note for advanced students: give the ideal angles, and don't worry about small differences from the ideal that might be caused by the fact that different electron groups may have slightly different sizes. H X