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Chemical Bonding

Chemical Bonding. Chapter 6. Sample Problem One. Use Electronegativity Differences and Figure 6.2 to classify bonding between S and the following elements: H, Cs, Cl. In each pair, which atom will be more negative?. Sample Problem One.

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Chemical Bonding

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  1. Chemical Bonding Chapter 6

  2. Sample Problem One • Use Electronegativity Differences and Figure 6.2 to classify bonding between S and the following elements: H, Cs, Cl. In each pair, which atom will be more negative?

  3. Sample Problem One • From figure 5-20 on page 151 we can find their electonegativties. • S = 2.5 • H = 2.1 • Cs = .7 • Cl = 3.0 • In each pair, the atom with the larger electronegatity will be more negative atom.

  4. Solution Sample Problem

  5. When differences are 1.7 or greater, the bond is usually ionic. Less than 1.7, the bond is usually covalent, and unless the difference is less than 0.5 the bond has some degree of polarity.

  6. Differences of less than 0.5 are considered to be nonpolar.

  7. Diatomic molecules- are two atom molecules • A. 5 gases are diatomic molecules-H2 , O2, N2, Cl2, F2 • B. diatomic liquid is Br2 • C. Diatomic solid is I2

  8. Empirical formula- indicates the simplest whole number ratio in which the atoms of the elements are present in the compound • Molecular formula- shows the number of atoms of each element in one molecule of the substance • Structural formula- shows the way in which atoms are joined together in a molecule

  9. H--Br 141 366 Br-Br 228 193 H--I 161 298 I--I 267 151 C--C 154 348 C--C 154 348 C=C 134 614 C--N 147 308 CºC 120 839 C--O 143 360 C--S 182 272 O--O 148 145 C--F 135 488 O=O 121 498 C--Cl 177 330 C--Br 194 288 N--N 145 170 C--I 214 216 NºN 110 945

  10. Bond Lengths and Bond Energies I • Bond Bond length(pm) Bond Energy • (kj/mol) • H--H 74 436 • H--C 109 413 • C--C 154 348 • H--N 101 391 • N--N 145 170

  11. Bond Lengths and Bond Energies II • Bonds Bond Length Bond energy • (pm) (kj/mol) • H--O 96 366 • O—O 148 145 • H--F 92 568

  12. Bond Lengths and Bond Energies III Bond and Bond Length(pm) Bond Energies(kj/mol) 581 432 243 366 193 298 151 • F--F 142 • H--Cl 127 • Cl-Cl 199 • H--Br 141 • Br-Br 228 • H--I 161 • I--I 267

  13. Bond Lengths and Bond Energies IV Bonds and bond Lengths(pm) Bond energies(kj/mol) 348 614 308 839 360 • C--C 154 • C=C 134 • C--N 147 • CºC 120 • C--O 143 • C--S 182 272 • O--O 148 145 • C--F 135 488

  14. Bond Lengths and Bond Energies V Bonds and Bond Length(pm) Bond Energy (kJ/mol) 498 330 288 170 216 945 • O=O 121 • C--Cl 177 • C--Br 194 • N--N 145 • C--I 214 • NºN 110

  15. Electrons are placed around the symbol in a counterclockwise fashion. •   6th • 2nd •   3rd • Symbol • 5th • 7th • 1st •   4th • 8th

  16. Multiple Bonds Formula Structure • H-C= C- H

  17. Resonance Structures • Resonance

  18. Metallic Bonds

  19. Molecular Geometry • VSEPR • Molecular Geometry

  20. Vocabulary I • Chemical Bond • Covalent bonding • Ionic bonding • Nonpolar-covalent bond • Polar • Polar-covalent bond • Bond energy • Bond length • Chemical formula • Diatomic molecule • Double bond • Electron dot notation • Lewis Structure • Lone pair • Molecular compound • Molecular formula • Molecule

  21. Vocabulary II • Multiple bond • Octet Rule • Resonance • Single bond • Structural formula • Triple bond • Unshared pair • Formula Unit • Ionic Compound • Lattice energy • Polyatomic Ion • Ductility • Malleability • Metallic bonding • Dipole • Dipole-Dipole force • Hybrid Orbital • Hybridization

  22. Vocabulary III • Hydrogen Bonding • Intermolecular force • London dispersion force • Molecular polarity • VSEPR theory

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