You will not turn in a formal write-up for this experiment. Turn in the completed Lewis dot structures for all molecules and answer the questions found in the supplemental exercises. А. For each molecule, or ion, write the name, then draw the Lewis structure. 1. H2 I2 CH4 13. СНь 14. СНа 15. *CH:CH:Cl Clo 2. 3. HF 16. 17. CN 4. 5. H2O BF3 NH3 NH, *NH; CHCI3 6. 18. NC13 7. 19. 20. *CH;OH 21. CH;O (make the C atom central) OH 8. 9. 10. 22. 11. 12. CO2 N2 23. 24. SF6 ICI: SbCls

ll X b My Questions | bartleby Login | bartleby 101 Chem101 ぐ app.101edu.co Question 1 Draw a resonance structure that shifts a pi bond to a new position. Don't increase the number of atoms with formal charges. Include all hydrogen atoms in your structure. H. Atoms, Bonds an Drawing CHa :CHs: %3. 3D CH2 CH2 MacBook 0:0 3D 3D

E D To answer the questions, interpret the following Lewis structure for NH4+. + H-N-H 1 H H 1 $ 4 Submit Answer R 1. For the central nitrogen atom: The number of lone pairs = The number of single bonds = The number of double bonds= F 2. The central nitrogen atom 5 Retry Entire Group F6 T G Cengage Learning Cengage Technical Support A 6 8 r F6 MacBook Air H obeys the octet rule has an incomplete octet has an expanded octet & 7 F7 U J * 00 8 DII F8 Laht Values if needed for this q - ( 9 K F9 O ) 0 L F10 P Previous available 11 + Email Instructor Save = Nex 11 F12

1. Write Lewis structures for the following. Show ALL resonance structures whereapplicable. For a, the central atom is carbon: a. SCN- b. N3- 2. Benzene (C6H6) consists of a six membered ring of carbon atoms with one hydrogen bonded to each carbon. Write Lewis structures for benzene, including resonance structures.

1. SiHA 2. CHO; 3. NO+ 4. S2,2- 5. NOCI Draw the following: 1. Lewis structure 2. Assign formal charges (for elements with non-zero formal charges only). 3. Draw resonance forms (if applicable), pick the most plausible structure (if possible) on the basis of formal charge and electronegativity.

Values if needec Draw (on paper) a Lewis structure for XeOF4 and answer the following questions based on your drawing. 1. For the central xenon atom: The number of lone pairs The number of single bonds = The number of double bonds = 2. The central xenon atom A. obeys the octet rule. B. has an incomplete octet. C. has an expanded octet. Submit Answer 5 question attempts remaining

Fill in the lone pairs on each atom to give every main group element except hydrogen an octet.

Bonding Electron Valence Shell Nonbonding Electron Approx. Bond Molecule or Lewis Electron VSEPR Geometric Molecular Ion Structure Pairs Pairs Pairs Formula Angle Shape 1. CH4 4 4 AX4 109.5° tetrahedral H:C:H H 2. Complete the table (as outlined above) for the following molecules/molecular ions, none of which obey the Lewis octet rule. Complete those that are assigned by your laboratory instructor. b. PCl,F3 с. BrF;

1. Draw the Lewis structure to the following compounds. For each compound, state whether the bonding is covalent, ionic, or a mixture of covalent and ionic. Be sure to indicate any charge on the correct atom. a) C3Hg b) HCIO c) NaCIO d) CH,OH e) NaOH f) CaCl, 8.

Instead of drawing the Electron dot structure, can you please draw the Lewis Structure. And count the Stigmas.