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Ionic bonds-crystalline structure

Ionic bonds-crystalline structure. Sodium Chloride Green spheres are Chloride ions. Blue spheres are Sodium ions. Lewis dot structure (Covalent Bonds).

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Ionic bonds-crystalline structure

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  1. Ionic bonds-crystalline structure Sodium Chloride Green spheres are Chloride ions. Blue spheres are Sodium ions.

  2. Lewis dot structure (Covalent Bonds) • Determine the number of valence electrons. Draw the first dots around the symbol (see 3Li to 6C). Draw the remaining dots (see 7N to 10Ne).

  3. Lewis dot structure (Covalent Bonds) Draw Lewis structures for the following: Determine the number of valence electrons to be in the structure. Be sure there are 2e- ’s around each hydrogen (Duet rule) and 8e- ’s around the other atoms (Octet rule). • CH4 2. NH4+ 3. O2 4. N2 5. C2H2 6. NCO- 7. CO2 8. N2H2 9. CH4O 10. NF3 11. CH2O 12. N2H4 13. CH2O2

  4. Lewis dot structure (Covalent Bonds) Use formal charges (FC = #valance e- - ½# bonding e- - # lone pair e- ) to determine the most likely correct formula. See also Tro Page 381. A. The sum of all formal charges equals the charge on the structure. [(0) for molecules and (-1 for NO2- ) or (+1 for NH4+)]. B. Lewis structures with formal charges of 0 are most likely to exist. Lewis structures with formal charges of -1 or +1 ( -1 on the most electronegative element) probably exist. Lewis structures with formal charges -2 , -3, etc. or +2, +3, etc. probably do not exist and should be rejected.

  5. Lewis dot structure (Covalent Bonds) Write the Lewis dot structure for: 1. 16S 2. 16S2- 3. 34Se 4. 55Cs 5. 8O 6. 7N7.19K 8. 19K+ 9. 32Ge 10. 36Kr Write at least 2 Lewis structures for the following: Consider the duet rule, octet rule, and multiple bonds. Use formal charges to decide the most likely correct Lewis structure. Draw the line bond formula for the most likely correct Lewis structure. [Formal charges = #valance e- - ½# bonding e-- # lone pair e-] 1. CH4 2. NH4+ 3. C2H2 4. C2H4 5*. NCO- 6. HCN 7. NO3-8. NO2-9. CO210. HNO3 11. N2H2 12. CH4O 13. C2H2F2 14. CH2O 15. C2H6O 16. N2H4 17. NF3 18. ClO2- 19. C2H6O220. C3H8O21. C2H4O2 *22. Actually both NCO- (cyanate) and CNO‑ (fulminate) exist. Which is least stable?

  6. Lewis dot structure (Covalent Bonds)Electronegativity

  7. Lewis dot structure (Covalent Bonds) Octet rule exceptions: H2 H is stable with 2 e-(duet rule);Be is stable with 4 e- ;B is stable with 6 e- Write the Lewis structure and line bond formulas for: 1 . H2 2. BeF23. BF6 Octet rule exceptions: Elements containing d orbitals may (or may not) use them for bonding and, therefore, may (or may not) be surrounded 8 or more electrons. Write the Lewis structure and line bond formula for: 4. BrF5 5. XeF2 6. SF4 *7. SO42- 8. BrF3 9. PF5 10. I3- *Use formal charges(FC = #valance e- - ½# bonding e-- # lone pair e- ) to decide on the best structure.

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