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Chemistry Inorganic Nomenclature Binary Ionic Compounds

Chemistry Inorganic Nomenclature Binary Ionic Compounds. Do Now: What are the common charges for atoms by group in the s and p block? CALCULATORS NOT REQUIRED PERIODIC TABLES REQUIRED. Ionic Compounds.

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Chemistry Inorganic Nomenclature Binary Ionic Compounds

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  1. ChemistryInorganic NomenclatureBinary Ionic Compounds Do Now: What are the common charges for atoms by group in the s and p block? CALCULATORS NOT REQUIRED PERIODIC TABLES REQUIRED

  2. Ionic Compounds • Formed from attractions between positive and negative ions, usually between a metal and a nonmetal. • Example: sodium (Na+) and chlorine (Cl-)

  3. Naming Cations • The names of positive ions do not change. • Alkali metals (IA): +1 ions • Li+, Na+, K+ • Lithium, sodium, potassium • Alkaline earth metals (IIA): +2 ions • Mg2+, Ca2+ • Magnesium, calcium • Boron group (IIIA): +3 ions • Al3+, Ga3+ • Aluminum, gallium • Carbon group (IVA): +4 • C4+ • carbon

  4. Naming Anions • The endings of negative ions change to -ide. • Carbon group (IVA): -4 ions • C4- • carbide • Nitrogen group (VA): -3 ions • N3-, P3- • Nitride, phosphide • Chalcogens (VIA): -2 ions • O2-, S2- • Oxide, sulfide • Halogens (VIIA): -1 ions • F-, Cl- • Fluoride, chloride

  5. Formulas of Ionic Compounds • Cations will combine with anions to form binary ionic compounds. • Binary = two-element • Ionic compounds are electrically neutral, so the charges must cancel each other out. • Ex: sodium oxide • Sodium: Na+ • Oxide: O2- • Need 2 sodiums to cancel out the oxide’s -2 charge. • Na2O

  6. The Cheesy Trick • When you want the correct formula given two ions, flip-flop the charges and make them subscripts. • If, when you do this, the subscripts are not the lowest whole-number ratio, reduce the subscripts. • NEVER, NEVER, NEVER, NEVER leave the charges on the atoms in a formula. The compound is neutral. • Ex: NaCl, NOTNa+Cl- • If I ever have to see this again, I will be very sad.

  7. Naming Ionic Compounds • The cation comes before the anion. • NaCl • Cation: sodium (Na+) • Anion: chloride (Cl-) • Name: sodium chloride • BeF2 • Beryllium fluoride

  8. Practice • Give the formulas for the following: • Sodium oxide • Potassium phosphide • Gallium nitride • Calcium carbide

  9. Practice • Give the names of the following: • Rb2S • CaO • AlCl3 • Mg3N2

  10. Polyatomic Ions • Some ions are made up of multiple atoms, these are called polyatomic ions. • These ions are covalently bonded together, but form ionic bonds with other elements. • Examples: • Nitrate (NO3-) • Sulfate (SO42-) • Phosphate (PO43-)

  11. Names & Formulas With Polyatomics • Sodium acetate • Procedure is the same – balance charges with ions • Sodium: Na+ • Acetate: C2H3O2- • NaC2H3O2

  12. Names & Formulas With Polyatomics • Magnesium nitrate • Magnesium: Mg+2 • Nitrate: NO3- • If you need multiple polyatomic ions, enclose the polyatomic ion in parentheses before you add the new subscript. • Mg(NO3)2

  13. Practice • Give the names of the following: • Na2SO4 • (NH4)3P • Al(NO3)3 • Give the formulas for the following: • Potassium chromate • Calcium carbonate • Aluminum chlorate

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