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IONIC COMPOUNDS

IONIC COMPOUNDS. STABILITY. Relates to nobility Every element’s dream They’ll do what they can to look like a noble gas… pseudo-noble gas configuration Duet Rule Octet Rule Potential Energy. Bond Energy. The energy required to break a bond

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IONIC COMPOUNDS

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  1. IONIC COMPOUNDS

  2. STABILITY • Relates to nobility • Every element’s dream • They’ll do what they can to look like a noble gas…pseudo-noble gas configuration • Duet Rule • Octet Rule • Potential Energy

  3. Bond Energy • The energy required to break a bond • The energy is absorbed when the bond is broken, thus…released when formed • Stronger bonds are more stable • Require more energy to break them • i.e. ionic bonds • Weaker bonds are less stable • Require less energy to break them • i.e. molecular or covalent bonds

  4. Achieving Stability • Ionic bonds made by transferring electrons • Metals will do what? • Nonmetals will do what? • Once electrons are transferred, the atoms are converted to ions. lose electron(s) gain electron(s)

  5. Ions • Positively charged ions are called? • Negatively charged ions are called? • Bond to make an ionic compound or salt cations anions

  6. Salts • Made of metals and nonmetals or polyatomic ions • Solid • Ordered arrangement called crystal lattice • Brittle • High melting point • Electrical conductors in aqueous and molten phases

  7. More About Ions • Written as a symbol with superscript to the right indicating the charge • Charge is written as a number followed by a + or – sign • Monatomic ions—”one-atomed” ions • Polyatomic ions—”many-atomed” ions

  8. Monatomic Ions • Use periodic table to determine charges of representative elements • Group 1…1+…element name + ion • Group 2…2+…element name + ion • Group 13…3+…element name + ion • Group 14…skip • Group 15…3-…ide ending + ion • Group 16…2-…ide ending + ion • Group 17…1-…ide ending + ion

  9. Monatomic Ions • For the transition metals, you must memorize the possible charges of the common ions

  10. Monatomic Ions

  11. Monatomic Ions

  12. Polyatomic Ions • Refer to handout • Know the formula (that means elements, subscripts, and charge) of each listed

  13. Making Ionic Compounds • A cation and an anion will bond in order to bring the charge of the compound to zero. • A “criss-cross” method is used to determine the number of each ion necessary to balance the charges • Always reduce subscripts.

  14. Na1+ Mg2+ Al3+ Cl1- Cl1- Cl1- 1 1 1 1 2 3 Making Ionic Compounds = NaCl = MgCl2 = AlCl3

  15. Making Ionic Compounds NaCl sodium chloride MgCl2 magnesium chloride AlCl3 aluminum chloride

  16. Na1+ Mg2+ Ca2+ S 2- O 2- P 3- 2 2 3 1 2 2 Making Ionic Compounds = Na2S = MgO = Ca3P2

  17. Making Ionic Compounds Na2S sodium sulfide MgO magnesium oxide Ca3P2 calcium phosphide

  18. Pb4+ O 2- 2 4 Ag1+ I 1- 1 1 Making Ionic Compounds = PbO2 = AgI = Fe2O3 Fe3+ O 2- 2 3

  19. Making Ionic Compounds PbO2 Lead (IV) oxide or plumbic oxide AgI silver iodide iron (III) oxide or ferric oxide Fe2O3

  20. Making Ionic Compounds Pb4+ = Pb(OH)4 (OH)1- 1 4 Mg2+ (SO4)2- = MgSO4 2 2 = Al2(C2O4)3 Al3+ (C2O4)2- 2 3

  21. Making Ionic Compounds Pb(OH)4 lead (IV) hydroxide or plumbic hydroxide MgSO4 magnesium sulfate Al2(C2O4)3 aluminum oxalate

  22. Crystal Lattice • 3-dimensional arrangement of atoms or ions in a solid • Simplest part is called a unit cell • There are six types of crystal systems • We will focus on the cubic unit cell

  23. Cubic Unit Cells • Three types: • Simple • Body-centered • Face-centered

  24. Simple Cubic Unit Cell P

  25. Face-centered Cubic Unit Cell NaCl Cl- ions Na+ ions

  26. Body-centered Cubic Unit Cell CsCl Cs+ ion Cl- ion

  27. Now… • PRACTICE • PRACTICE • PRACTICE

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