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A. Chemical Formula

1 oxygen atom. 2 hydrogen atoms. A. Chemical Formula. Shows: 1) elements in the compound 2) ratio of their atoms. H 2 O. B. Chemical Bond. Strong attractive force between atoms or ions in a molecule or compound. Formed by: transferring e - (losing or gaining) sharing e -. Ne.

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A. Chemical Formula

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  1. 1 oxygen atom 2 hydrogen atoms A. Chemical Formula • Shows: 1) elements in the compound 2) ratio of their atoms H2O

  2. B. Chemical Bond • Strong attractive force between atoms or ions in a molecule or compound. • Formed by: • transferring e- (losing or gaining) • sharing e-

  3. Ne C. Stability • Octet Rule • most atoms form bonds in order to have 8 valence e- • full outer energy level • like the Noble Gases! • Stability is the driving force behind bond formation!

  4. C. Stability • Transferring e- • Sharing e-

  5. Ch. 22 - Chemical Bonds II. Kinds of Chemical Bonds Ionic Bond Covalent Bond Comparison Chart

  6. A. Ionic Bond • Attraction between 2 oppositely charged ions • Ions - charged atoms • formed by transferring e-from a metal to a nonmetal

  7. NaCl A. Ionic Bond • ions form a 3-D crystal lattice

  8. B. Covalent Bond • Attraction between neutral atoms • formed by sharing e- between two nonmetals

  9. Cl2 H2O NH3 B. Covalent Bond • covalent bonds result in discrete molecules

  10. B. Covalent Bond • Nonpolar Covalent Bond • e- are shared equally • usually identical atoms

  11. - + B. Covalent Bond • Polar Covalent Bond • e- are shared unequally between 2 different atoms • results in partial opposite charges

  12. B. Covalent Bond • Nonpolar • Polar • Ionic View Bonding Animations.

  13. C. Comparison Chart COVALENT IONIC transferred from metal to nonmetal shared between nonmetals Electrons Melting Point high low Soluble in Water yes usually not yes (solution or liquid) Conduct Electricity no molecules, odorous liquids & gases crystal lattice of ions, crystalline solids Other Properties

  14. Ch. 22 - Chemical Bonds III. Naming Molecular Compounds Molecular Names Molecular Formulas

  15. A. Molecular Names • Write the names of both elements. • Change the final ending to -ide. • Add prefixes to indicate subscripts. • Only use mono- prefix with oxide.

  16. PREFIX mono- di- tri- tetra- penta- hexa- SUBSCRIPT 1 2 3 4 5 6 A. Molecular Names

  17. A. Molecular Names • CCl4 • N2O • SF6 • carbon tetrachloride • dinitrogen monoxide • sulfur hexafluoride

  18. B. Molecular Formulas • Write the more metallic element first. • Add subscripts according to prefixes.

  19. B. Molecular Formulas • phosphorus trichloride • dinitrogen pentoxide • dihydrogen monoxide • PCl3 • N2O5 • H2O

  20. B. Molecular Formulas • The Seven Diatomic Elements Br2 I2 N2 Cl2 H2 O2 F2

  21. Ch. 22 - Chemical Bonds IV. Naming Ionic Compounds Oxidation Number Ionic Names Ionic Formulas

  22. A. Oxidation Number • The charge on an ion. • Indicates the # of e- gained/lost to become stable. 1+ 0 2+ 3+ 4+ 3- 2- 1-

  23. B. Ionic Names • Write the names of both elements, cation first. • Change the anion’s ending to -ide. • Write the names of polyatomic ions. • For ions with variable oxidation #’s, write the ox. # in parentheses using Roman numerals. Overall charge = 0.

  24. B. Ionic Names • NaBr • Na2CO3 • FeCl3 • sodium bromide • sodium carbonate • iron(III) chloride

  25. C. Ionic Formulas • Write each ion. Put the cation first. • Overall charge must equal zero. • If charges cancel, just write the symbols. • If not, crisscross the charges to find subscripts. • Use parentheses when more than one polyatomic ion is needed. • Roman numerals indicate the oxidation #.

  26. C. Ionic Formulas • potassium chloride • magnesium nitrate • copper(II) chloride • K+ Cl- KCl • Mg2+ NO3-  Mg(NO3)2 • Cu2+ Cl- CuCl2

  27. C. Ionic Formulas • calcium oxide • aluminum chlorate • iron(III) oxide • Ca2+ O2- CaO • Al3+ ClO3-  Al(ClO3)3 • Fe3+ O2- Fe2O3

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