Decide whether each of the molecules in the table below is stable, in the exact form in which it is drawn, at pH = 1. If you decide at least one molecule is not stable, then redraw one of the unstable molecules in its stable form below the table. (If more than one molecule is unstable, you can pick any of them to redraw.) OH O stable O unstable OH X 5 O stable O unstable O stable O stable O unstable OH O unstable OH

Consider the acid-base reaction between iodoethane (CH3CH2I) and hydroxide (-OH). CH3CH2I + OH- --> CH3CH2OH + l- Use the table of bond energies to estimate the change in enthalpy (∆H in kJ/mol) for this reaction. Think about the bonds that are broken and that are formed.  This reaction is endothermic, exothermic or energy neutral   Using your calculation, what can you say about the strengths of the bonds?  -The bonds before the reaction are stronger than the bonds after the reaction. -The bonds after the reaction are stronger than the bonds before the reaction.  or -The bonds before and after the reaction are equivalent in strength.

8) Label the energy states in the diagram below (options are 1s4d, 1s3d, 1s3s). You will need to think about which energy gap is the largest, which energy gap is the smallest. This is an idealized energy diagram (shape is simplified, focus on distance from nucleus) 1s2p

CO₂H -OH -OH heat 1. SOCI 2, A 2. NaO,CCH2CH3 ?

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)

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     4 NH3 + 5 O2 -> 4 NO + 6 H2O

Energy in the reaction center comes from bond energy. red light. absorbed photons. green light. potential energy. перов d OO d a b U

Which of these three is most stable? Explain (justify)

7. Estimate the enthalpy of reaction (in kJ/mol) for the combustion of methane. Be sure to show a lewis structure for each molecule. CH, (g) + 20, (g) ·CO, (g) + H,O (g) Bond Bond Enthalpy (kJ/mol) C-O 351 C=0 799 CEO 1070 O-O 142 O=0 498 C-H 414 O-H 460

parts b and c please