Decide whether each of the molecules in the table below is stable, in the exact form in which it is drawn, at pH = 11. 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.) HO 40 OH Ostable O unstable .OH HO stable O unstable X Ostable Ounstable HO OH Ostable O unstable

16522631&OpenVellumHMAC=250253b32e9565151f3a112a4880967e#10001 I Review Constants Periodic Table ving reactions. Part A | 1. CH3O 2. HCI CH;CH2CH2 OCH3 Draw the molecule on the canvas by choosing buttons from the Tools (for bonds), Atoms, and Advanced Template toolbars. The single bond is active by default. CONT. 12D H | +) X) EXP H. C N.

Rank the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest boiling point, choose 2 next to the substance with the next highest boiling point, and so on. substance A B C D H chemical symbol, chemical formula or Lewis structure H :0: 44 - C- C-H H - H 1 C I Ar H H | | - C - | 1 H H H Ag H CIO : 0: H boiling point ✓ (Choose one) 1 (highest) 2 3 4 (lowest) (Choose one) ✓ (Choose one) ✓

Bonds Bond Energy (kJ/mol) C-H 411 C-Br 285 H-Br 362 Br-Br 190 Determine ΔH for the reaction:    CH4 + 2Br2 ----> CH2Br2 + 2HBr

CO, CO₂, CH3OH, and CO32- all contain carbon-oxygen bonds. Draw Lewis structures for these molecules and ions. Given that double bonds are stronger than single bonds and triple bonds are stronger than double bonds, rank the four species in order of increasing CO bond strength. Weakest: Strongest:

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.

1. Draw Lewis structures for ozone and for dioxygen. Using the data given below, qualitatively compare the bond enthalpies, bond orders, and bond lengths of these two compounds. O₂ (g) 20 (g) AH" = +498 kJ O(g) + O₂(g) →O, (g) AH-105 kJ

Rank the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest boiling point, choose 2 next to the substance with the next highest boiling point, and so on. substance A B U D chemical symbol, chemical formula or Lewis structure H H 1 | H-C C 1 I I H H H Ar H I Ag : 0: C-O-H :0: ||| H-C-C-C-H 44 boiling point ✓ (Choose one) 1 (highest) 2 W N 3 4 (lowest) (Choose one) ↑ (Choose one) (Choose one) ↑

The picture below shows a model of a chemical reaction. The magnitude of energy associated with each of the bonds indicated in the figure is: Bond X: 4 eV Bond Y: 5 eV Bond A: 6 eV Bond B: 7 eV If the reaction proceeds in the direction indicated, what will be the change in chemical energy? O -2 ev O +11 ev +4 eV -11 eV +2 eV

Please do question 6 and 7 and please very short answers