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Naming Ionic Compounds

Sec. 2.2 Part A Science 10. Naming Ionic Compounds. How do atoms form ions? Why do they want to form ions? What are positively charged ions called? Negatively charged ions? What can occur once ions have been created? Why does this occur?. Review.

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Naming Ionic Compounds

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  1. Sec. 2.2 Part A Science 10 Naming Ionic Compounds

  2. How do atoms form ions? Why do they want to form ions? What are positively charged ions called? Negatively charged ions? What can occur once ions have been created? Why does this occur? Review

  3. explain why the IUPAC system of naming compounds is important describe the process of ionic bonding and give examples of ionic compounds give correct names and formulas for ionic compounds, using the periodic table, table of ions and IUPAC rules Objectives

  4. IUPAC – International Union of Pure and Applied Chemistry • Responsible for naming compounds • Allows consistent way of naming compounds • Why is this important? • Allows for clear and precise communication IUPAC and Compound Naming

  5. How do we form ionic compounds? • Transfer of electrons between atoms • Metal and non-metal • Transfer of electrons creates full outer energy levels • More stable • Attraction of ions called ionic bonding Ionic Compounds

  6. Practice: Give drawings and show electron transfer for the following atoms: • Sodium • Magnesium • Chlorine • Oxygen Ionic Compounds

  7. Two part name: cation and anion 1) name cation first with element’s name 2) name anion second with first part of name and change last part to “ide” Ex. Sodium chloride (sodium ion and chloride ion) IMPORTANT: always write names of elements as lower case (unless at beginning of sentence) Naming Ionic Compounds: The Rules

  8. Name the following compounds: • MgO • BaF2(s) • K3N(s) Practice

  9. Contains element symbols • Some have subscripts • Ex. BaF2(s) • What this means: • One barium ion for every two fluoride ions • Ionic compounds are neutral • Therefore, need to have enough of each atom to cancel the charges out Formulas for Ionic Compounds

  10. What are the charges for each ion in this compound? • Sodium chloride • How many of each ion do we need to cancel the charges out? • How about this one? • Magnesium chloride • How many do we need? • These make the subscripts! Formulas for Ionic Compounds

  11. Steps for Writing Formulas aluminium: Al3+ chloride: Cl- Al3+ : 3 Cl- : 1+1+1=3 1 to 3 AlCl3 If the ratio is 1:1, do not need to include subscripts The subscripts should be the simplest form What does this mean? Formula unit- name for ionic compound unit (NEUTRAL)

  12. When charges are not easy to balance: • i.e. calcium nitride • Ca2+ and N3- • Find the lowest common multiple to balance the charges • What is the lowest common multiple here? • Simplify!!! What do you end up with? Lowest Common Multiple

  13. Need to balance the charges i.e. one positive charge balances out one negative charge Why do we need to balance the charges? What happens to our compounds when we do this? Balancing Charges

  14. Write the formulas/names for the following compounds: • sodium bromide • calcium nitride • magnesium oxide • aluminium chloride • MgS • AlN • Li3P Practice

  15. Some metals have more than one stable ion • Ex. Iron has two stable ions: Fe2+ and Fe3+. • To indicate which ion it is, use Roman numerals in names • Example: iron (II) or iron (III) • Still use subscripts for compounds- be careful about which ion it is! • Ex. FeBr2 = iron (II) bromide • Ex. FeBr3 • Only use Roman numerals when more than one ion (ONLY for transition metals) Multivalent Elements

  16. Write formulas for following: • copper (I) nitride • lead (IV) chloride • nickel (III) oxide • Write the names for the following formulas: • AuN • CrO • TiBr4 Practice

  17. Sec A2.2 Part B Science 10 Naming Ionic and Molecular Compounds

  18. How does an ionic compound form? • What name would you give for the following? • MgCl2 • LiBr • K3N • FeCl3 Review

  19. predict formulas and write names for ionic compounds with polyatomic ions describe covalent bonding in molecular compounds identify diatomic/polyatomic molecular elements give correct names and formulas for molecular compounds with and without hydrogen using periodic table and IUPAC rules objectives

  20. Polyatomic ions- ions made of several non-metallic atoms Come as one “unit” (consider to be one unit when naming) List in periodic table of polyatomic ions with symbol and charge Ending usually “-ate” (more oxygen) or “-ite” (less oxygen) Polyatomic ions

  21. Cation + anion DO NOT change the ending of a polyatomic ion Practice: Au(NO3)3(s) (NH4)3PO4(s) K2Cr2O7(s) Naming with Polyatomic Ions

  22. Same method with exception: • Subscripts for polyatomic ions placed in brackets • Ex. Fe2(SO4)3 • Put 3 outside brackets because there are 3 SO42- for each Fe3+ • Practice: • barium hydroxide • iron (III) carbonate • copper (I) permanganate Writing Formulas

  23. Molecule: two or more non-metal atoms bonding Can be same or different atoms Fixed numbers of bonded atoms (unlike ionic compounds: formula unit= part of crystal lattice) Molecular Compounds

  24. How molecular compounds bond Atoms share electrons (no transfer) Pair of shared electrons makes one covalent bond Allows outer energy levels to be filled Can share more than one pair of electrons (double or triple bonds) http://www.youtube.com/watch?v=QqjcCvzWwww Covalent Bonds

  25. Elements that form own molecules (ex. O2) • Diatomic- molecule made of 2 of the same atom • H2, N2, O2, F2, Cl2, Br2, I2. • Polyatomic- More than two of the same atom • O3, P4, S8. • Only appear as these when by themselves • Should memorize these! Molecular Elements

  26. For binary compounds (two elements) • Use Greek prefixes: • What are they for numbers 1-10? • Indicates how many of each atom • Prefix + first element followed by prefix + second element ending in “-ide” • Ex. • N2O (dinitrogen monoxide) • PBr3 • CO • CS2 Naming Molecular Compounds without hydrogen

  27. Write the names or formulas for the following: CO2(g) N2O(g) PCl3(g) oxygen difluoride dinitrogentetrasulfide sulfur trioxide Practice

  28. Often given names Ex. “water” official IUPAC name for H2O Table A2.12 (Be familiar with this chart! Should know the important ones/ones you will see most often) Naming Molecular Compounds With Hydrogen

  29. Go through difference between ionic and molecular compounds • How do we know which is which and when to use what naming rules (dichotomous key) How do we tell the Difference?

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