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Draw the resonance structure indicated by the arrows.

Draw the resonance structure indicated by the arrows. 1). 2). 3). Label each atom with the correct hybridization. 4). sp 3. sp 3. sp 3. sp 3. sp 3. sp 3. 5). sp 3. sp 2. sp 2. sp 3. sp 2. 6). sp 2. sp. sp. sp 3. 7) Draw H 2 NCH 2 + in its second best resonance structure.

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Draw the resonance structure indicated by the arrows.

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  1. Draw the resonance structure indicated by the arrows. 1) 2)

  2. 3) Label each atom with the correct hybridization. 4) sp3 sp3 sp3 sp3 sp3 sp3

  3. 5) sp3 sp2 sp2 sp3 sp2 6) sp2 sp sp sp3

  4. 7) Draw H2NCH2+ in its second best resonance structure. 8) Draw the best Lewis structure for CH3CHO, a neutral molecule

  5. 9) Draw the Lewis structure for CH3COOH, a neutral molecule. 10) Draw the Lewis structure for N2H2, a neutral molecule.

  6. 11) Draw in the electron flow arrows in on the left hand structure that lead to the resonance structure on the right. 12) In the empty box, draw the best resonance structure of the left-hand compound, and draw one or more electron-flow arrows on the preexisting structure that lead to the new structure.

  7. 13) 14)

  8. Label each of the following as an ionic or covalently bonded compound. • NaF • BrCl • NaOCHe ionic covalent ionic Calculate the formal charge of nitrogen in each of the following compounds. a) b) FC = 5 – (4 + (1/2(4))) = -1 FC = 5 – (2 + (1/2(6))) = 0 FC = 5 – (0 + (1/2(8))) = +1

  9. Draw the Lewis structure. • (CH3(OH2))+ • CH3NO2 Draw all possible isomers of C2H4O.

  10. Are each of the following pairs isomers or resonance structures? a) b) Neither, different formulas Isomers, same formula but different arrangement of atoms.

  11. Draw a resonance structure of each, and identify which is the major contributor. a) b)

  12. Draw all possible resonance structures of the compound below and it’s resonance hybrid.

  13. Predict the geometry around each indicated atom. a) b) tetrahderal Trigonal planar

  14. Draw the three dimensional structure of the following. a) CH3OH b) (CH3)2NH

  15. Convert each molecule into a skeletal structure. a) (CH3)2CHCH2CH2CH(CH3)2 b)

  16. Convert into Lewis structures. a) (CH3)3COH b) CH3COCH2Br

  17. What is the hybridizatio of th eindicated atom. a) b) sp3 sp2 sp2 sp

  18. Which is the weakest of the indicated bonds? A is the weakest bond due to it being composed of a sp3 and sp2 hybridized orbital, thus having the least amount of S character B is the weakest, b/c bond strength increases across a row in the periodic table and N is to the left of O.

  19. Draw the products and label each part. A B CA CB CB CA B A

  20. Draw the products and determine if the reaction occurs. pka=0.2 pka=16 Products favored pka=-7 pka=5 reactants favored

  21. Which is the strongest base? HBr, HCl or HF HF, b/c it is the weakest acid. Identify the most acidic hydrogen. C is the most acidic hydrogen b/c it’s bonded to an sp hybridized carbon.

  22. Draw the products of each reaction and label the starting materials as a Lewis acid and base. LB LA LB LA

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