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Chapter 8

Chapter 8. Ionic Compounds. Atoms vs Compounds. Atom-smallest piece of matter that retains a material’s properties Molecule- atoms covalently bonded, bonded by the sharing of electrons

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Chapter 8

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  1. Chapter 8 Ionic Compounds

  2. Atoms vs Compounds • Atom-smallest piece of matter that retains a material’s properties • Molecule- atoms covalently bonded, bonded by the sharing of electrons • Diatomic molecules- elements that exist as two atoms covalently bonded (H2, N2, O2, F2, Cl2, Br2, I2) • Ionic compounds- ions bonded by their oppositely charged forces

  3. 8.1/ 8.2 Forming Ionic bonds • Ionic bonds- formed by the donation of an electron from a (+) ion to a (-) ion EX: K+1 + F – 1 → KF (neutral) • Cations and anions arrange into a crystal lattice: • Cation- donates e- to achieve octet • K: 1s22s22p63s23p64s1 • Anion- accepts e-to achieve octet • F: 1s22s22p5

  4. Ionic Crystal Lattice

  5. Properties of Ionic Compounds • Solid • Crystalline • Brittle • High melting point • High boiling point • Conducts electricity when dissolved in water

  6. 8.2 Vocubulary • Electrolyte- an ionic compound whose aqueous solution conducts electric current • Lattice energy- energy required to separate one mole of the ions of an ionic compound

  7. 8.3 Formulas for Ionic Compounds • Formula unit- simplest ratio of the ions represented in an ionic compound EX: NaCl, MgCl2, AlCl3 • Monatomic ion- a one-atom ion, EX: Mg2+, Br – • Oxidation number- the charge of a monatomic ion • Polyatomic ion- ions made up of more than one atom EX: NH4+, SO42-

  8. Ionic Formulas • Ex: sodium oxide • Identify charge on metal and nonmetal ions- (Ex: Na+, O2-) • Criss-cross superscripts to balance charges (Ex: Na2O) • Check if total formula has 0 charge • Write answer with subscripts (Ex: Na2O) • Note: Polyatomic (many atom) ions are same except parenthesis put around them before subscripts are added

  9. Practice Writing Formulas • Lithium chloride • Potassium sulfide • Magnesium bromide • Calcium oxide • Sodium nitrate • Sodium sulfate • Calcium chlorate

  10. Naming Ionic Compounds • NO PREFIXES • If last ion is polyatomic, name normally • (Ex: CaSO4 = calcium sulfate) • If last ion is monatomic, add –ide at end • (Ex: CaCl2 = calcium chloride)

  11. Practice Naming Ionic Compounds • CaO • Na2SO4 • Ca3(PO4)2 • MgSO3

  12. Transition Metals- The Stock System • Some metals can exist in several forms • Ex: Cu1+, Cu2+ • Chemical formula used to decide which ion is present • (Ex: CuCl2 – must be Cu2+ • Name puts metal ion charge in parenthesis • Ex: copper (II) chloride ***only done for some transition metals

  13. Practice the Stock System • Tin (II) oxide • Iron (III) sulfide • Copper (I) sulfate • PbO • PbO2 • Fe2(SO4)3

  14. 8.4 Metallic Bonds • Electron Sea Model for delocalized electrons • All atoms contribute their electrons to the community

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