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Understanding Ionic Compounds and Stability in Chemistry

Learn about ionic compounds and stability in chemistry, including the Duet Rule, Octet Rule, and bond energy. Discover how to achieve stability through ionic bonds and understand the properties of ions and salts. Practice making ionic compounds using the criss-cross method and explore crystal lattice structures in a simple, body-centered, and face-centered cubic unit cell.

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Understanding Ionic Compounds and Stability in Chemistry

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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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