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Bonding

Bonding. p. 97-106. chemical bond : interaction between atoms or ions decreases the potential energy of an atom; makes it more stable only the valence electrons are involved!. Three Types of Bonds. Bond type depends on electronegativity (electron affinity)

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Bonding

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  1. Bonding p. 97-106

  2. chemical bond: interaction between atoms or ions • decreases the potential energy of an atom; makes it more stable • only the valence electrons are involved!

  3. Three Types of Bonds • Bond type depends on electronegativity (electron affinity) • IONIC：verydifferent electronegativities • one metal, one non-metal • COVALENT: both very high • two non-metals • METALLIC: both low • one or more metals

  4. Review of Ionisation +1 +2 -3 -2 -1 Anions Cations Non-metals Metals

  5. What kind of bond? • Na and Cl • O and F • K and Br • Au and Ag • H and O • Mg and F • S and Cl • Ni and Cu • Ionic • Covalent • Ionic • Metallic • Covalent • Ionic • Covalent • Metallic

  6. Ionic Bonds • metal (low electroneg., cation) + non-metal (high electroneg., anion) • Array of positively and negatively charged ions • held together by electrostatic attraction

  7. metal loses e- = cation • group 1 (+1) and group 2 (+2) • transition metals (+2 most common) • non-metal gains e- = anion • groups 17, 16, 15… • List, p. 100

  8. Cl sodium and chlorine • sodium transfers its electron to chlorine Na

  9. Crystal Lattice (Array) • structure of an ionic bond • each anion is surrounded by cations and vice versa

  10. Writing Formulae for Ionic Compounds

  11. chemical formula: shorthand for elements, ions and compounds • Ratio of the number of atoms of each element • MgCl2 • C6H12O6

  12. Ions of opposite charges are attracted to one another. • Mg2+ Cl- • MgCl2 • Ions bond because they are electrically attracted to one another • “Opposites attract”

  13. Polyatomic ions: most covalently bonded, but have an overall electronic charge • Hand out list: memorize it.

  14. Ionic or Covalent? • NaCl • NO2 • N2Br • NaI • CaS

  15. Ionic or Covalent? • KNO3 • Fe(CrO4)2 • Cu(OH)2 • BaI • F2

  16. Ionic or Covalent? • O2 • AgCl • AgNO3

  17. Ionic or Covalent? • NO2 • CO2 • PCl5 • P2S4 • NO3

  18. Writing Formulae forIonic Compounds • Write the symbols and their charges • “Cross” the charges to the other side • Use the charges, without + or – as subscripts

  19. Polyatomic Ions to Memorize • Ammonium • Nitrite • Nitrate • Sulfite • Sulfate • Hydroxide • Phosphite • phosphate • Carbonate • Chlorite • Chlorate • Chromate

  20. Naming Ionic Compounds

  21. Naming Cations • Same as the element!!

  22. Naming Anions • Ending changes to “ide” • O oxygen oxide • F fluorine fluoride • S sulfur sulfide • Cl chlorine chloride • Br bromine bromide • I iodine iodide

  23. Chlorine • Iodine • Oxygen • Sulfur • Bromine • Fluorine • Chloride • Iodide • Oxide • Sulfide • Bromide • Fluoride

  24. Naming Ionic Compounds • Cation + Anion (“ide” ending) • NaCl sodium chloride • KBr potassium bromide

  25. Naming Ionic Compounds – Type I • One positively charged ion and one negatively charged ion. • NaCl • Sodium chloride • SrF2 • Strontium fluoride

  26. cesium bromide • magnesium oxide • potassium fluoride • aluminum chloride • lithium hydride • CaI2 • Rb2S • CsBr • MgO • KF • AlCl3 • LiH • calcium iodide • rubidium sulfide

  27. LiI • CaS • AgBr • ZnCl2 • Na2S • barium fluoride • silver oxide • lithium iodide • calcium sulfide • silver bromide • zinc chloride • sodium sulfide • BaF2 • Ag2O

  28. Stock system • Some elements make ions with different charges (p. 100) • “oxidation states” • Fe2+ Fe3+ • iron(II) iron(III) • Roman numerals

  29. Elements that use theStock System • These elements have more than one “oxidation state” • Fe (2+, 3+) Cr (2+, 3+) • Cu (1+, 2+) Mn (2+, 3+) • Co (2+, 3+) Pb (2+, 4+) • Sn (2+, 4+) • Hg2+ (mercury II), Hg22+ (mercury I) • Zumdahl, p. 65

  30. Ions to memorize • Al3+ • Zn2+ • Ag+ • Cd2+

  31. copper (I) chloride • tin (II) oxide • iron (III) oxide • manganese (IV) oxide • lead (II) chloride • Cu2O3 • VF4 • CuCl • SnO • Fe2O3 • MnO2 • PbCl2 • copper (III) oxide • vanadium (IV) fluoride

  32. CoBr2 • CrCl3 • CaCl2 • Al2O3 • SnBr4 • Cu2S • iron (II) fluoride • tin (II) oxide • cobalt (II) bromide • chromium (III) chloride • calcium chloride • aluminum oxide • tin (IV) bromide • copper (I) sulfide • FeF2 • SnO

  33. Fe(NO3)3 • Iron(III) nitrate • Fe2(SO4)3 • iron(III) sulfate Polyatomic Ion

  34. Ionic Compounds with Polyatomic Ions • NH4+ • ammonium • NO3- • nitrate

  35. Na2SO4 • KH2PO4 • Fe(NO3)3 • Mn(OH)2 • Na2SO3 • Rb2CO3 • Mg(HCO3)2 • sodium sulfate • potassium dihydrogen phosphate • iron (III) nitrate • manganese (II) hydroxide • sodium sulfite • rubidium carbonate • magnesium bicarbonate

  36. Name Ionic Compounds • potassium nitrate • magnesium hydroxide • lithium chromate • iron (III) hydroxide • cobalt nitrate • Manganese (II) posphite • KNO3 • Mg(OH)2 • LiCrO4 • Fe(OH)3 • Co(NO3)2 • Mn3(PO3)2

  37. Homework FeBr2 cobalt (II) iodide SnO2 ammonium nitrate Ag2S • CaO • lithium sulfide • CrCO3 • silver iodide • Cu2SO3 • calcium phosphate • SrI2 • iron (III) bromide

  38. Covalent Bonding

  39. Covalent Bonding • two or more non-metals • atoms share some valence electrons (not transfer) • single covalent bond: shares one pair of electrons • double: 2 pairs of e- • triple: 3 pairs of e-

  40. F • usually each atom donates (shares) one of each pair of electrons • dative covalent bond: sometimes one atom donates both electrons Electron Pair Shared by both atoms Each e- donate by each atom F

  41. number of bonds formed depends on the number of e- required to fill the valence shell • noble gases = full valence, rarely form compounds • octet rule: usually, atoms want 8 valence e- (H, He need 2)

  42. Ex: C has 4 valence e- • needs 4 more to form a full octet • C forms 4 bonds • Ex: F has 7 valence e- • needs 1 more to form a full octet • F makes one bond • Nitrogen?

  43. Bonding between C and F F F C F F F F C F F C F F F F structural hybrid Lewis formula diagram diagram =e- pair F e- C e- =covalent bond

  44. Double Bond • sharing two pairs of electrons • bonds more strongly than a single bond • structural hybrid Lewis O C O O C O O C O

  45. Triple Bond • Strongest N N N N N N

  46. Length and Strength of Bonds single doubletriple longestshortest lowestenergyhighest energy

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