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Ionic Compounds

Ionic Compounds. Ch.5. (5-1) Ions. Atom or group of atoms that has a charge b/c it has lost or gained e - Ex: [Na] = 1s 2 2s 2 2p 6 3s 1 [Na + ] = 1s 2 2s 2 2p 6. Types of Ions. Cation : + ion Lose e - Ex: K + Anion : - ion Gain e - Ex: Br -. Terms.

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Ionic Compounds

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  1. Ionic Compounds Ch.5

  2. (5-1) Ions • Atom or group of atoms that has a charge b/c it has lost or gained e- • Ex: [Na] = 1s22s22p63s1 [Na+] = 1s22s22p6

  3. Types of Ions • Cation: + ion • Lose e- • Ex: K+ • Anion: - ion • Gain e- • Ex: Br-

  4. Terms • Electroneutrality: having = #’s of + & - charges • Isoelectronic: having the same e- config. as another atom • [Na+] = 1s22s22p6 = [Ne]

  5. Octet Rule • Tendency of atoms to gain or lose e- so that their outer s & p orbitals are full w/ 8 e-

  6. Transition Metal Ions • Form cations • Some have multiple ions due to d orbitals • Ex: Fe2+ = Iron (II) Fe3+ = Iron (III)

  7. Ionic Compounds • Chemical cmpd composed of oppositely charged ions • Binary ionic cmpd: cation of 1 element & anion of another • Ex: ZnS, KBr

  8. Naming Binary Ionic Cmpds • Name of cation • Ca = calcium • Name of anion • S = sulfur • Drop anion suffix & add –ide • CaS = calcium sulfide

  9. Naming Practice • Al2S3 • Aluminum sulfide • Rb2O • Rubidium oxide • FeF2 • Iron (II) fluoride • CrI3 • Chromium (III) iodide Specify charge of transition metals

  10. Writing Formulas • Write the symbol & charges for the cation & anion • Aluminum oxide: Al3+O2- • Balance the charges by adding subscripts • Al2O3

  11. Formula Practice • Calcium oxide • CaO • Potassium nitride • K3N • Tin (II) oxide • SnO • Copper (I) bromide • CuBr

  12. (5-2) Ionic Bond • Force of attraction b/w ions of opposite charge

  13. Terms • Coulombic force: attraction or repulsion b/w 2 charged objects • Halide: salt w/ halogen anion • Ex: NaCl & KBr

  14. Crystal Lattice • Repetitive geometric arrangement of atoms • Unit cell: smallest repeating unit in a crystal NaCl

  15. Lattice Energy • E released when atoms, ions, or molecules come together to form a crystal

  16. Properties of Binary Ionic Cmpds • Hard & brittle • From crystal lattice • Melt & boil at high temps. • Need lots of E to break bonds • Solids generally don’t conduct electricity

  17. (5-3) Polyatomic Ion • Group of bonded atoms that functions as a single ion • Ex: NO2- = nitrite SO42- = sulfate

  18. Oxyanions • Neg. polyatomic ion containing oxygen • Suffix: • -ate, most common ion • sulfate: SO42- • -ite, anion w/ 1 less O • sulfite: SO32-

  19. Oxyanions (cont.) • Prefix: • Hypo-, anion w/ 1 less O than –ite • Per-, anion w/ 1 more O than -ate • Ex: hypochlorite = ClO-, chlorite = ClO2- chlorate = ClO3- perchlorate = ClO4-

  20. Naming • Name the cation • K+ • Name the anion • CO32- • Name the salt • K2CO3 = potassium carbonate

  21. Polyat. Ion Naming Practice • NaOH • Sodium hydroxide • LiClO2 • Lithium chlorite • H2O2 • Hydrogen peroxide • CaCO3 • Calcium carbonate

  22. Writing Formulas • Determine formula & charge of cation • Calcium = Ca2+ • Determine formula & charge of anion • Chlorite = ClO2- • Balance charges (keep polyat. ion in parentheses if necessary) • Calcium chlorite = Ca(ClO2)2

  23. Polyat. Ion Formula Practice • Iron (II) hydroxide • Fe(OH)2 • Potassium dichromate • K2Cr2O7 • Aluminum phosphate • AlPO4 • Ammonium nitrate • NH4NO3

  24. Oxidation #’s • # assigned to an atom in a polyatomic ion or molecular cmpd based on an assumption of complete transfer of e-

  25. Assigning Oxid. #’s • The sum of the oxid.#’s for all the atoms in a cmpd = 0 • The sum of oxid.#’s for all atoms in a polyatomic ion = charge on that ion

  26. Assigning Oxid. #’s (cont.) • Free (uncombined) elements = 0 • Na, O2 • Monatomic ion = charge of its ion • K+ = +1 • More EN element in binary cmpd = its charge if it were an ion • NaCl: Cl = -1

  27. Assigning Oxid. #’s (cont.) • H = +1 • w/ a metal it’s –1 • F = -1 • O = -2 • w/ F it’s +2 • in peroxides (H2O2) it’s –1 • In cmpds, Gr. 1 & 2 & Al are +1, +2, & +3, respectively

  28. Oxidation # Practice • Determine K in KOH • -2 +1 • K O H = 0 K = +1 • -2 +1 • Determine Cl in Ca(ClO3)2 • +2 -2 • Ca Cl2 O6 = 0 Cl = +10 = +5 • +2 -12 2

  29. Oxidation # Practice • Determine N in NO3- • -2 • N O3- = -1 N = +5 • -6 • Determine N in NH4+ • +1 • N H4+ = +1 N = -3 • +4

  30. Hydrate • Ionic cmpd that contains water molecules in its crystal lattice • Naming: use prefixes (See Table 5-8) • Na2CO3•10H2O = sodium carbonate decahydrate • Anhydrous: w/out water

  31. Mono - 1 Di - 2 Tri - 3 Tetra - 4 Penta - 5 Hexa - 6 Hepta - 7 Octa - 8 Nona - 9 Deca - 10 Hydrate Prefixes

  32. Naming Hydrates Practice • BaSO4•5H2O • Barium sulfate pentahydrate • MgSO4•7H2O • Magnesium sulfate heptahydrate • SrCl2•2H2O • Strontium chloride dihydrate

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