1. Sec. 2.2 Part A Science 10

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?

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

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

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

6.  Practice: Give drawings and show electron transfer for the following atoms:  Sodium  Magnesium  Chlorine  Oxygen

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)

8.  Name the following compounds:  MgO  BaF 2 (s)  K 3 N(s)

9.  Contains element symbols  Some have subscripts  Ex. BaF 2 (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

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!

11. StepsExample Sodium chlorideAluminium chloride Identify ions and chargessodium: Na+ chloride: Cl- Determine total charges needed to balance Na+ : 1 Cl- : 1 Note the ratio of cations to anions 1 to 1 Use subscripts to write formulaNaCl 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) aluminium: Al 3+ chloride: Cl - Al 3+ : 3 Cl - : 1+1+1=3 1 to 3 AlCl 3

12.  When charges are not easy to balance:  i.e. calcium nitride  Ca 2+ and N 3-  Find the lowest common multiple to balance the charges  What is the lowest common multiple here?  Simplify!!! What do you end up with?

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?

14.  Write the formulas/names for the following compounds:  sodium bromide  calcium nitride  magnesium oxide  aluminium chloride  MgS  AlN  Li 3 P

15.  Some metals have more than one stable ion  Ex. Iron has two stable ions: Fe 2+ and Fe 3+.  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. FeBr 2 = iron (II) bromide  Ex. FeBr 3  Only use Roman numerals when more than one ion (ONLY for transition metals)

16.  Write formulas for following:  copper (I) nitride  lead (IV) chloride  nickel (III) oxide  Write the names for the following formulas:  AuN  CrO  TiBr 4

17. Sec A2.2 Part B Science 10

18.  How does an ionic compound form?  What name would you give for the following?  MgCl 2  LiBr K3NK3N  FeCl 3

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

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)

21.  Cation + anion  DO NOT change the ending of a polyatomic ion  Practice:  Au(NO 3 ) 3(s)  (NH 4 ) 3 PO 4(s)  K 2 Cr 2 O 7(s)

22.  Same method with exception:  Subscripts for polyatomic ions placed in brackets  Ex. Fe 2 (SO 4 ) 3  Put 3 outside brackets because there are 3 SO 4 2- for each Fe 3+  Practice:  barium hydroxide  iron (III) carbonate  copper (I) permanganate

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)

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

25.  Elements that form own molecules (ex. O 2 )  Diatomic- molecule made of 2 of the same atom  H 2, N 2, O 2, F 2, Cl 2, Br 2, I 2.  Polyatomic- More than two of the same atom  O 3, P 4, S 8.  Only appear as these when by themselves  Should memorize these!

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.  N 2 O (dinitrogen monoxide)  PBr 3  CO  CS 2

27.  Write the names or formulas for the following:  CO 2(g)  N 2 O (g)  PCl 3(g)  oxygen difluoride  dinitrogen tetrasulfide  sulfur trioxide

28.  Often given names  Ex. “water” official IUPAC name for H 2 O  Table A2.12 (Be familiar with this chart! Should know the important ones/ones you will see most often)

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)