3.  IUPAC (The International Union of Pure and Applied Chemistry) is the organization responsible for the naming of chemical compounds.  Using IUPAC guidelines ensures the use of a consistent, practical way of naming that allows all scientists to communicate clearly and precisely.

4.  Ionic compounds form when electrons transfer from one atom to another.  Binary ionic compounds consist of a cation and an anion  NaCl  Na has 1 valence electron, and Cl has 7 valence electrons. When they combine the 1 Na electron transfers to the Cl atom. The result, both have full outer energy levels.  the positive sodium ions are attracted to the negative chloride ions.  This is called ionic bonding, when bonds are formed between ions of metals (+) and non-metals (-).

5. + - Na Cl Illustrating the bonding of Sodium and Chlorine

6. 11P 12N Sodium Na = 2,8,1 Sodium is soft and very reactive metal It has only 1 electron in its outside shell

7. 17P 18N Chlorine = 2,8,7 Chlorine is a highly poisonous green gas. It has 7 electrons in the outside shell and is not stable.

8. 11P 12N Na 17P 18N Cl

9. 11P 12N 17P 18N NaCl

10. 17P 18N 11P 12N NaCl

11. 17P 18N 11P 12N Na + 2,8 Cl- 2,8,8

12. 17P 18N 11P 12N Strong forces of attraction exist between Na+ and Cl- and hold the bond together Na+ 2,8 Cl- 2,8,8

13. The Octet rule is simply a rule which helps us to understand bonding Atoms bond together so that each atom attains an electron arrangement of 8 electrons in its outermost shell. The Octet Rule :

14.  Na lost 1 electron  Na changed from electron configuration of 2,8,1 to 2,8  Na changed from a neutral Na atom to a positively charged Na ion (Na + )  Cl gained 1 electron  Cl changed from electron configuration of 2,8,7 to 2,8,8  Cl changed from a neutral Cl atom to a negatively charged Cl ion (Cl - )

15. 1. Name the metal first by using the element’s name. 2. Than name the non-metal using the suffix “ide”.  NaCl (Na + and Cl - ), sodium chloride.  BaF (Ba 2+ and F - ), barium fluoride.

16. 1. Identify the ions and their charges.  Aluminum ion: Al 3+  Chloride ion: Cl - 2. Determine the total charges needed to balance. All ionic compounds must have an equal number of positive and negative charge.  total charge of anions = total charge of cations  Al 3+ : 3  Cl - : 1+1+1=3 3. Note the ratio of cations to anions.  1 to 3 4. Use subscripts to write the formula, if needed. Always use the smallest whole number ratio.  AlCl 3

17. Write the formulas for the following ionic compounds. a)magnesium chloride b)sodium sulfide c)calcium phosphide

18. a) magnesium chloride  magnesium ion: Mg 2+ chloride ion: Cl -  Mg 2+ :2 Cl - : 1+1=2  1:2  MgCl 2 b) sodium sulfide  sodium ion: Na + sulfide ion: S 2-  Na + : 1+1=2 S 2- : 2  2:1  Na 2 S c) calcium phosphide  calcium ion: Ca 2+ phosphide ion: P 3-  Ca 2+ : 2+2+2=6P 3- : 3+3=6  3:2  Ca 3 P 2

19. Elements with more than one ion are called multivalent elements.  Iron has two stable ions: Fe 2+ and Fe 3+  Ionic compounds containing multivalent elements must have Roman numeral in their names to indicate which ion is forming that compound.  FeCl 3 -> iron (III) chloride

20. 1. Identify the ions that form the compound. 2. Use the charge of the known ion and the rule that the total positive and negative charge in the formula unit must equal to determine the unknown charge of the multivalent element. 3. Write the name of the compound. Remember the Roman numeral must be in brackets.

21. Write the name of the following compounds: a) PbO 2 (s) b) Ni 2 S 3 (s) c) CuF 2 (s)

22. Write the name of the following compounds: a) PbO 2 (s)  lead (IV) oxide b) Ni 2 S 3 (s)  nickel (III) sulfide c) CuF 2 (s)  copper (II) fluoride

23. Polyatomic Ions are ions made up of several non-metallic atoms joined together.  hydroxide ion (OH - ), when in a compound such as NaOH, Na has a charge of 1+, O and H together form the polyatomic hydroxide ion, with a charge of 1-.

24. Two common suffixes used in naming polyatomic ions are "-ate" and "-ite”  "-ate" means more atoms are a part of the ion  "-ite" means less atoms are a part of the ion  The suffixes do not tell you how many atoms are in the formula.  "-ate" and "-ite" are used when similar ions exist.  sulfate (SO 4 2- ) and sulfite (SO 3 2- ), sulfate has one more oxygen atom than sulfite. If more than 2 variation exist, then other naming strategies are used.

25. More than two types of atoms indicates there is a polyatomic ion Look at the formula, name the cation, followed by the anion. You do not need to change the ending of the polyatomic ion.

26.  Au(NO 3 ) 3 (s)  (NH 4 ) 3 PO 4 (s)  K 2 Cr 2 O 7 (s)

27.  Au(NO 3 ) 3 (s) gold nitrate  (NH 4 ) 3 PO 4 (s) ammonium phosphate  K 2 Cr 2 O 7 (s) potassium dichromate

28. Rules are similar to writing ionic compounds, except: When more than one polyatomic ion is required you must use brackets to indicate multiples of the group of atoms i.e. Ca(OH) 2 (s) The formula unit for an ionic compound always consists of positive and negative ions in the smallest whole-number ratio that results in a neutral unit. i.e. NH 4 + and HCO 3 - results in NH 4 HCO 3 (s)

29. Rules for writing:  Identify the ions and their charges.  iron (III) sulfate  iron (III): Fe 3+  sulfate: SO 4 2-  Determine the total charges needed to balance  Fe 3+ : 3 + 3 = 6  SO 4 2- : 2 +2 + 2 = 6

30.  Note the ratio of cations to anions  Ratio 2:3  Use brackets and subscripts if needed to write the formula. This is not required when it is a 1:1 ratio.  Fe 2 (SO 4 ) 3

31. Write the formulas of the following ionic compounds:  barium hydroxide  iron(III) carbonate  copper(I) permaganate

32.  barium hydroxide  Ba 2+ OH -  21 + 1 =2  Ratio 1:2  Ba(OH) 2  iron(III) carbonate  Fe 3+ CO 2 3- 3333  Ratio 1:1  FeCO 2

33.  copper(I) permaganate  Cu 1+ MnO 4 1- 1111  Ratio 1:1  CuMnO 4

34. These are elements that form molecules from only one type of atom. There are 3 kinds of molecular elements.  Monatomic - elements that can exist on there own. Ex. Carbon, noble gasses, and all metals.  Diatomic - elements from the in pairs of itself. Ex. H 2, O 2, N 2, F 2, Cl 2, Br 2, I 2 (seven that make a 7) *memorize*  Polyatomic - molecules that can exist with more than one pair of itself. Eg. O 3, P 4, S 8

35.  Bonding between two non metals  Name the first non-metal element.  Name the 2 nd element with "ide" at the end.  Add Greek prefixes indicating the number of atoms  N 2 O -> dinitrogen monoxide  PBr 3 ->phosphorous tribromide  Note that the prefix "mono" is not usually used when an element is single Greek Prefixes 1-mono6-hexa 2-di7-hepta 3-tri8-octa 4-tetra9-nona 5-penta10-deca

36. Write the name or formula of these molecular compounds:  CO 2(g)  PCl 3(g)  oxygen difluoride  dinitrogen tetrasulfide

37.  CO 2 (g)  carbon dioxide  PCl 3 (g)  phosphorus trichloride  oxygen difluoride  OF 2  dinitrogen tetrasulfide N2S4N2S4 Homework: Read Science 10 p. 40-50 Check and Reflect # 1-12, due the next day.