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Chemical Bonds: IONIC BONDING

Chemical Bonds: IONIC BONDING. electrostatic attraction between positive and negative ions. Ionic Bond. Na +. Cl -. salt crystal NaCl. cesium chloride. calcium fluoride. electrons are transferred from a metal atom to a nonmetal atom. Bond Formation:. e -. e -. opposite charges

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Chemical Bonds: IONIC BONDING

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  1. Chemical Bonds: IONIC BONDING

  2. electrostatic attraction between positive and negative ions Ionic Bond Na+ Cl- salt crystal NaCl cesium chloride calcium fluoride

  3. electrons are transferred from a metal atom to a nonmetal atom Bond Formation: e- e- opposite charges attract

  4. - Formation of Ions + Metals lose electrons to form a (+) charged ion called a cation This process is called oxidation Octet Rule: atoms gain or lose electrons in order to have the same number of electrons as a noble gas

  5. Group I A metals: Alkali metals (Li, Na, K….) sodium atom: Na has 11 p+ and 11 e- +11 -11 1s22s22p63s1 Na+ has 11 p+ and 10 e- sodium ion: +11 -10 1s22s22p6 Like Ne all alkali metals lose one electron to form an ion with a + 1 charge Rb+ Cs+ Na+ K+ Li+

  6. Group II A metals: Alkaline Earth metals ( Be, Mg,Ca..) calcium atom: ca has 20 p+ and 20 e- +20 -20 1s22s22p63s23p64s2 +20 -18 calcium ion: Ca2+ has 20 p+ and 18 e- 1s22s22p63s23p6 like Ar all group 2a metals lose 2 e- to form an ion with a +2 charge Mg2+ Ca2+ Ba2+ Ex:

  7. Group III A metals: Al, Ga, In….. All lose 3 e- to form an ion with a +3 charge Al3+ Ga3+ In3+ nonmetals gain electrons to form (-) charged ions called anions This process is called reduction

  8. Group VII A: Halogens F, Cl, Br, I fluorine atom: F has 9 p+ and 9 e- +9 -9 1s22s22p5 +9 -10 fluorine ion: F- has 9 p+ and 10 e- 1s22s22p6 Like Ne All group 7A elements gain 1 e- to form an ion with a -1 charge F- Cl- Br- I-

  9. Group VI A: O, S, Se….. +16 -16 sulfur atom: S has 16 p+ and 16 e- 1s22s22p63s23p4 sulfur ion: +16 -18 S2- has 16 p+ and 18 e- 1s22s22p63s23p6 like Ar allgroup 6A atoms gain 2 e- to form an ion with a -2 charge S2- Se2- O2-

  10. Group V A: N, P, As, Sb… All gain 3 e- to form an ion with a -3 charge N3- P3- As3- Transition metals: various oxidation numbers (charges) miscellaneous oxidation numbers Hydrogen is -1 when combined with a metal zinc is +2 , Zn2+ silver is +1, Ag+

  11. summary: memorize these No ions! +1 -1 +2 +3 -3 -2

  12. Formulas: Binary Ionic Compounds calciumfluoride sodium chloride Na+ Cl- NaCl Ca2+ F- CaF2 aluminum oxide zinc sulfide ZnS Al3+ O2- Al2O3 Zn2+ S2- not Zn2S2 ferric chloride tin (IV) oxide Fe3+ Cl- FeCl3 Sn4+ O2- SnO2 not Sn2O4

  13. 1. lead (II) iodide 2. potassium nitride PbI2 K3N Pb2+ I- K+ N3- 3. silver bromide 4. cadmium hydride Ag+ Br- AgBr CdH2 Cd2+ H- 5. Chromium (III) oxide 6. Copper (II) sulfide Cr2O3 Cr3+ O2- Cu2+ S2- CuS

  14. 7. sodium oxide Na+ O2- Na2O 8. aluminum fluoride AlF3 Al3+ F- 9. iron (II) phosphide Fe2+ P3- Fe3P2 10. zinc chloride ZnCl2 Zn2+ Cl-

  15. Naming Binary IonicCompounds Rule: Name the metal, then the nonmetal; change ending to –ide; if the metal has more than one oxidation number, use Roman numerals KI potassium iodide Ca3N2 calcium nitride sodium hydride BaCl2 barium chloride NaH HgCl2 Hg2+ Cl- mercury (II) chloride

  16. iron (III) oxide Fe2O3 Fe3+ O2- PbO2 Pb4+ lead (IV) oxide O2- 1. AlBr3 aluminum bromide 2. AgF silver fluoride 3. CaS calcium sulfide

  17. 4. FeCl2 iron (II) chloride zinc phosphide 5. Zn3P2 magnesium oxide 6. MgO cobalt (III) bromide 7. CoBr3 copper (II) sulfide 8. CuS 9. BaI2 Barium iodide

  18. Ternary Ionic Compounds o o N All contain a polyatomic ion o nitrate carbonate nitrite bicarbonate hypochlorite sulfate chlorite sulfite phosphate chlorate phosphite perchlorate

  19. cyanide chromate dichromate hydroxide permanganate ammonium acetate writing formulas: magnesium sulfate Mg2+ SO42- MgSO4

  20. sodium acetate NaC2H3O2 Na+ C2H3O2- potassium carbonate CO32- K+ K2CO3 ammonium nitrite NH4+ NO2- NH4NO2 iron (III) nitrate Fe3+ NO3- Fe NO3 3

  21. ammonium dichromate NH4+ NH4 Cr2O72- Cr2O7 2 copper (II) sulfate Cu2+ SO42- CuSO4 1. Lead (II) chlorite Pb (ClO2)2 Pb2+ ClO2- 2. calcium hydroxide Ca OH 2 Ca2+ OH-

  22. 3. silver sulfite Ag2SO3 Ag+ SO32- 4. potassium permanganate KMnO4 K+ MnO4- 5. ammonium perchlorate NH4+ ClO4- NH4ClO4 3. mercury (II) phosphate Hg3(PO4)2 Hg2+ PO43-

  23. 4. aluminum acetate Al(C2H3O2)3 Al3+ C2H3O2- 5. lithium chromate Li2CrO4 Li+ CrO42- 6. zinc bicarbonate Zn(HCO3)2 Zn2+ HCO3- 7. tin (IV) sulfate Sn(SO4)2 Sn4+ SO42-

  24. Naming Ternary Compounds Rule: Name cation then the anion; use Roman numerals for metals with multiple oxidation numbers Al(NO3)3 aluminum nitrate sodium chlorate NaClO3 ammonium hydroxide NH4OH barium cyanide Ba(CN)2

  25. CuSO4 copper (II) sulfate lead (II) chromate PbCrO4 iron (II) nitrite Fe (NO2)2 Sn3 (PO4)4 tin (IV) phosphate Sn Sn Sn PO4 3-PO43- PO43- PO43- +12 -12

  26. 1. CaCO3 calcium carbonate 2. KNO2 potassium nitrite 3. Zn(C2H3O2)2 zinc acetate chromium (III) nitrate 4. Cr(NO3)3 5. AgCN silver cyanide aluminum hypochlorite 6. Al(ClO)3

  27. 7. BaSO4 barium sulfate 8. FePO4 iron (III) phosphate 9. Li 2Cr2O7 lithium dichromate 10. Pb (OH)3 lead (III) hydroxide

  28. Properties of Ionic Compounds (Salts) made up of metal w/ nonmetal solid, crystalline structure high melting point

  29. soluble in water hard or brittle (not malleable) conduct electricity when melted or dissolved nonconductor as solid

  30. bonding in plain metals metals are malleable, ductile, shiny and good conductors because of the: metallic bond metal ions In a “sea of electrons”

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