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Understanding Ionic Compounds: Formulas, Naming, and Properties

Explore the world of ionic compounds, from atoms vs. compounds to forming bonds, crystal lattice properties, and naming conventions. Learn about electrolytes, lattice energy, and how to write formulas for various compounds. Discover the Stock System for transition metals.

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Understanding Ionic Compounds: Formulas, Naming, and Properties

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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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