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Science 10 Chapter 4.2 Names and Formulas of Ionic Compounds

Science 10 Chapter 4.2 Names and Formulas of Ionic Compounds. Ionic Compounds (metal + non-metal {+,-}) Hydrates (water attached) Covalent Compounds (non-metal + non-metal {-,-}) Acids (H + something). Ionic Compounds. Made up of ions (+ & -) Compounds are NEUTRAL

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Science 10 Chapter 4.2 Names and Formulas of Ionic Compounds

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  1. Science 10 Chapter 4.2Names and Formulas of Ionic Compounds • Ionic Compounds (metal + non-metal {+,-}) • Hydrates (water attached) • Covalent Compounds (non-metal + non-metal {-,-}) • Acids (H + something)

  2. Ionic Compounds • Made up of ions (+ & -) • Compounds are NEUTRAL • The sum of (+) ion charges must equal the (-) ion charges • Opposites attract • Form crystals from insideout Salt, NaCl

  3. Ionic Compounds3 rules for chemical formula, given name • Write formula for (+) ion first, then (-) ion second • Criss-cross the charge numbers on the ions • Tidy up the formula • Divide evenly by 2 or 3 • Omit superscript charges • Omit subscripts of 1 • Put brackets around polyatomic ions (PAIs) if there’s more than 1 *Table of PAI’s pg. 66 of wb

  4. Ionic Compounds - Construct formula given name Sodium Iodide Na+1 I-1NaI Calcium Oxide Ca+2 O-2CaO Calcium Phosphate Ca+2 PO4-3Ca3(PO4)2 Copper (I) Oxide Cu+1 O-2 Cu2O

  5. Ionic Compounds - Construct name given formula • Write metal name first, then non-metal ending with “ide” • E.g., CaCl2 calcium chloride

  6. Ionic Compounds - Construct name given formula • For PAIs, don’t change their ending • E.g., CaCrO4  calcium chromate

  7. Ionic Compounds: Construct name given formula • For multivalent metals reverse criss-cross subscripts to find charges • Always check charge of non-metal (2nd ion) • If not, multiply both sides by the same # to correct • Write metal’s charge in roman numerals after name (I, II, III, IV, V, VI, VII) *On periodic table, most common ion is listed on top

  8. Ionic Compounds - Construct name given formula • CuO • Cu can either be 1+ or 2+ • Reverse criss-cross = 1+ • Check: can oxygen be 1-? • Multiply • Name: copper (II) oxide

  9. Hydrates • Molecules that include water in their crystal structures Naming • Find name before water is attached • Add water using a prefix with the word “hydrate” CoCl2 cobalt (II) chloride hexahydrate CoCl2·6H2O

  10. Prefixes for Hydrates =

  11. Name a hydrate!

  12. Name a hydrate Cr(NO3)3·9H2O chromium (III) nitrate nonahydrate

  13. Science 10 Quiz Feb 12, 2014 • Identify the hydrate(s) in the list below a) Al(NO3)3 b) H2O2c) Al(NO3)3·9H2O d) CaCrO4 2. The least/most common ion charge is written above the other ion charges

  14. Science 10 Quiz Feb 12, 2014 • Identify the hydrate(s) in the list below a) Al(NO3)3 b) H2O2c) Al(NO3)3·9H2O d) CaCrO4 2. The least/most common ion charge is written above the other ion charges

  15. Covalent compounds (aka molecules) • Share electrons • No order in formation (clump as (s), (l), or (g) • Use the same prefixes (mono, di, tri, …) • Made of 2 or more non-metals • Subscripts show actual number of atoms in molecule • examples: carbon monoxide, carbon dioxide CO CO2

  16. Naming binary covalent compounds • Binary = 2 elements Steps: • Write the most metallic (left) element first • Second element gets “ide” ending ***Subscripts must be named*** e.g., nitrogen dioxide, dinitrogen dioxide NO2 N2O2

  17. TRAPS • NH4+ = ammonium • NH3 = ammonia • H2O = water

  18. 1. H + Non Metal (found on right side of Periodic table {Halogen}) start with “HYDRO add non metal change ending to IC most times {RIC} add word “acid” Example: HF = hydrofluoric acid HB = HCl = Some Common Acids naming scheme: {H + something} Three Acids:

  19. 2. H + Poly atomic ion with a ATE ending • name P.A.I. • change ending to “RIC” • add word “acid” Example: H2SO4 = sulphuric acid H3PO4 = H2CrO4 =

  20. 3. H + Poly atomic ion with a ITE ending • name P.A.I • change ending to “ROUS” • add word “acid” • Examples: HNO2 = nitrous acid • H2SO3 = • H3PO3 =

  21. Silver chloride__________ 2. Sulphur dioxide__________ 3. Lead (II) acetate decahydrate_______________ Silver dichromate__________ Silicon tetraflouride__________ 6. Ammonium phosphate __________ 7. Copper (I) iodide__________ 8. Iron (II) fluoride nonahydrate_____________ 9. Zinc hydrogen sulphite______________ 10. Manganese (IV) monohydrogen phosphate trihydrate ________________ Try Some Name into Formula

  22. Try Some Formula into Name 1. NI3 _______________________________ 2. Ca(OH)2 _______________________________ 3. Fe2(SO4)3.H2O _______________________________ 4. (NH4)2C2O4 _______________________________ 5. Co3(PO4)2.8H2O_______________________________ 6. H3PO4 _______________________________ 7. HClO2 _______________________________ 8. N3O _______________________________ 9. HI _______________________________ 10. Mg3P2 _______________________________

  23. Science 10 Chapter 4.2Names and Formulas of Ionic Compounds 4 types of compounds • CO2 • HNO3 • CoO • Cr(NO3)3·9H2O • workbook pages 71, 73 due tomorrow

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