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IONIC BONDS

IONIC BONDS. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. e -. 1. Bonds formed by transferring electrons between atoms

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IONIC BONDS

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  1. IONIC BONDS e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- 1. Bonds formed by transferring electrons between atoms 2. Metal + Nonmetal 3. Metal loses e- Nonmetal gains e- ION - charged atom 1. Cation (+ charge); metal Na+1 Ca+2 Al+3 Sodium Ion Calcium Ion Aluminum Ion 2. Anion (- charge); nonmetal I-1 S-2 P-3 Iodide Ion Sulfide Ion Phosphide Ion 3. Results in Noble Gas electron configuration for each atom K: 1s22s2p63s2p64s1 19 p+ 19 e- Cl: 1s22s2p63s2p5 17 p+ 17 e-

  2. e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- 19 p+ 18 e- K+1:1s22s2p63s2p6 17 p+ 18 e- Cl-1:1s22s2p63s2p6 Now, both exhibit Noble Gas e- configuration “8 valence electrons” complete filled s & p orbitals Ionic compounds are composed of “ions”

  3. IONIZATION ENERGY E required to remove e- from atom in its gaseous state Na + E ----------> Na+1+ e- Mg + E -----------> Mg+2+ 2e- Trend: increases L2R across row decreases down column ELECTRON AFFINITY E released when gaining an e- to an atom in its gaseous state O + 2e- ---------> O-2+ E Br + e- --------> Br-1+ E The Z=5, 6, 7, group 4A, & group 7A elements not easily gain or lose e- Tend to form Covalent Bonds

  4. OXIDATION - REDUCTION “REDOX” Reduction: gain electron Oxidation: lose electron H2(g) + O2(g) --------> H2O(g) Both H2 & O2 are diatomics: charge on each 0 In the cmpd. H is +1 & O is -2 H: from 0 to +1 charge, loses e-, oxidized (reducing agent) O: from 0 to -2 charge, gain e-, reduced (oxidizing agent)

  5. REDOX – Reduction/Oxidation LEO the lion says GER-r-r-r-r-r-r-r- Lose Electron Oxidize Gain Electron Reduce

  6. REDOX – Reduction/Oxidation OIL RIG Reduce Is Gain Oxidize Is Lose

  7. IA + VIIIA COMPOUNDS Combine in 1:1 ratio High melting point >5000C) NAMING IONIC COMPOUNDS BINARY REGULAR METAL (1 charge) 1st: Name of element 2nd: Name changed to -ide ending SrI2 Strontium Iodide IRREGULAR METAL (2+ charges) 1st: Name of element common name w/ roman numeral or “derived name” 2nd: Name changed to -ide ending Pb3P2 Lead II Phosphide Plumbous Phosphide

  8. POLYATOMICS radicals, polyatomic ions Group of 2+ elements combined together to make a group with an overall charge SO3-2 SO4-2 NO2-1 NO3-1 PO3-3 PO4-3 Sulfite Sulfate Nitrite Nitrate Phosphite Phosphate OH-1 CO3-2 HCO3-1 Hydroxide Carbonate Hydrogen Carbonate or Bicarbonate NH3: Ammonia NH4+1: Ammonium Ion Complete Molecule Itself Polyatomic Ion; needs Anion to complete cmpd. NH4Cl NH4C2H3O2 (NH4)2SiO3 Ammonium Ammonium Ammonium Chloride Acetate Silicate

  9. REGULAR METAL Na2C2O4 MgCr2O7 Sodium Oxalate Magnesium Dichromate IRREGULAR METAL FeSO4 Fe2(SO3)3 Iron II Sulfate Iron III Sulfite Ferrous Sulfate Ferric Sulfite

  10. ACIDS -- BASES Acid: 1st element, cation, is “H+1” Base: Metal + OH Anion, OH-1 Ca(OH)2 LiOH CuOH Calcium Hydroxide Lithium Hydroxide Copper I Hydroxide Cuprous Hydroxide OxidesIAPeroxides Li2O Lithium Li2O2 Na2O Sodium Na2O2 K2O Potassium K2O2 Oxide Peroxide O-2 O-1---> O2-2 NH4OH Ammonium Hydroxide MnO4-1: Permanganate MnO4-2: Manganate Mercury I or II Hg+2 Hg+1--Hg+1 Hg2+1

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