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Bonding

Bonding. Chapter 13 (part 1) E-mail: benzene4president@gmail.com Web-site: http://clas.sa.ucsb.edu/staff/terri/. Bonding – ch 13. 1. Define electronegativity 2. Rank the following in order of electronegativity: a. Cl Br I b. Al Si P. Bonding – ch 13.

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Bonding

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  1. Bonding Chapter 13 (part 1) E-mail: benzene4president@gmail.com Web-site: http://clas.sa.ucsb.edu/staff/terri/

  2. Bonding – ch 13 1. Define electronegativity 2. Rank the following in order of electronegativity: a. Cl Br I b. Al Si P

  3. Bonding – ch 13 3. Consider the following bonds to determine the following: C-O C-Br C-S a. Most polar bond b. Most ionic character c. Longest bond

  4. Bonding – ch 13 4. Estimate the value of ΔH for the following reactions: a. CH4 + 2 Cl2 CCl4 + 4 HCl b. Formation of ammonia Ave Bond Energies (kJ/mol) ⇒H-H (432), C-H (413), Cl-Cl (239), H-Cl (427), C-Cl (339), N-H (391), N≡N (941)

  5. Bonding – ch 13 5. Fill in the following table:

  6. Bonding – ch 13 Lewis Structure Guidelines: 1. Determine the number of valence electrons (group number, add electrons for anions or subtract electrons for cations) 2. Determine the central atom(s) – least electronegative element (exception - hydrogen will not be the central atom) 3. Draw out structure with single bonds symmetrically 4. Subtract the bonding electrons from the valence electrons – place the remainder on the outer atoms before central atoms – H (wants 2e-), Be (wants 4e-), B and Al (wants 6 e-), all else (wants 8e-) 5. Once you’ve run out of electrons determine if all atoms have what they want – if yes you’re done – if not add a bond for every 2e- that’s missing – the bonding electrons come from the adjacent atoms non-bonded pair

  7. Bonding – ch 13 Formal Charge = Group number - #bonds - #nonbonded electrons

  8. Bonding – ch 13 6. Compare the relative stabilities of the resonance structures for SCN-

  9. Bonding – ch 13 7. Rank the following in order of relative carbon oxygen bond length: CO2 CO CO32-

  10. Bonding – ch 13 8. Use the following data to estimate the heat of formation for solid magnesium fluoride. Lattice energy -2913 kJ/mol First ionization energy of Mg 735 kJ/mol Second ionization energy of Mg 1445 kJ/mol Electron affinity of F -328 kJ/mol Bond energy of F2 154 kJ/mol Enthalpy of sublimation of Mg 150. kJ/mol

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