2. * What is: 1. A metal… 2. A non metal… 3. Molecular compound… 4. Ionic compound… 5. Group… 6. Period… 7. Charge…

3. H 2(g) hydrogen N 2(g) nitrogen O 2(g) oxygen F 2(g) fluorine Cl 2(g) chlorine Br 2(l) bromine I 2(g) iodine S 8(s) sulfur P 4(s) phosphorus

4. Are now found in the data booklet!!!!

5. 1. write the first name as given on the periodic table of elements. 2. write the last name using an “ide” ending. 3. place the appropriate prefix in front the first and last name to describe the number of atoms there are of each element. 4. where the first element has only one atom, “mono” is not necessary. Example: P 4 O 3 (g) = 4 atoms tetraphosphorus trioxide 3 atoms

6. 1. Combining elements of the periodic table that come from the metals and nonmetals (left and right side of the “staircase” only) forms an ionic compound. 2. When naming ionic compounds: 3. write the first name as given on the periodic table of elements. 4. write the last name using an “ide” ending. 5. use no prefixes. Example: CaCl 2 - calcium chloride

7. 1. Using the crossover method: 1. put down the metallic element first. 2. put down the nonmetallic element last. 3. cross the elements’ ionic charge to become the subscript for each other element. 4. numerically simplify the subscripts. Example: magnesium phosphide Mg 2+ and P 3– Mg 3 P 2 Mg 3 P 2 (s) ***all ionic compounds are solids at room temperature.

8. * use the same format as above but whenever a complex ion is named, use brackets to keep that complex ion as a group. Example:sodium sulfate - Na + and SO 4 2– Put the two together grouping the complex ion:Na+ (SO 4 2– ) Now cross the charges: Na 2 (SO 4 ) 1 Since 1’s are not necessary: Na 2 SO 4 (s) Example:calcium nitrate - Ca 2+ and NO 3– Ca 2+ (NO 3– ) Ca(NO 3 ) 2 (s) Example: sodium hydroxide - Na + and OH – Na + (OH – ) NaOH (s)

9. * use the first ion listed as the most common. For example, Cu 2+ is more common than Cu +, so Cu 2+ would be used if no choice is given. When naming these compounds containing elements with more than one charge: use Roman numerals to indicate the charge of the ion used. Example:CuCl is copper (I) chloride Example:CuCl 2 is copper (II) chloride

10. * Follow ionic rules: * Then use a dot along with the number of water molecules required. * When naming hydrated compounds, follow all ionic rules described above. * Then use a prefix in front of the word “hydrate”. Example:CuSO 4  6H 2 O is: copper (II) sulfate hexahydrate Example:aluminum chloride trihydrate is: AlCl 3  3H 2 O

11. * Formation of a precipitate * Formation of a gas * Colour change * Energy change

12. Simple Composition element + element  compound 2 Na(s) + Br 2 (g)  Simple Decomposition compound  element + element + element 2CaCO 3 (s)  Single Replacement element + compound  element + compound Mg(s) + 2 NaOH(aq)  Double Replacement compound + compound  compound + compound 3 HCl(aq) + Al(OH) 3 (aq)  Hydrocarbon Combustion hydrocarbon + oxygen  carbon dioxide + water vapour C 3 H 8 (g) + 5O 2 (g)  Oxidation Metal + oxygen  Compound 2Fe(s) + O 2 (g)  2 NaBr(s) 2Ca(s) + 2C(s) + 3O2(g) 2 Na(s) + Mg(OH)2(aq) AlCl3(s) + 3 HOH(l) FeO (s) 3CO 2 (s) + 4 HOH(g)

13. Examples: NaOH(aq)  Na + (aq) + OH – (aq) Al 2 (SO 4 ) 3 (aq)  2 Al 3+ (aq) + 3 SO 4 2– (aq) Ionic compoundsMolecular compounds may be soluble (turn into aq) DO form ions (individual charged elements in water) do not form ions (individual charged elements in water) Are electrolytes (because ions are electrolytes Are not electrolytes

14. Example:A silver nitrate solution reacts with a solution of barium chloride. AgNO 3 (aq) + BaCl 2 (aq)  Ba(NO 3 ) 2 (aq) + AgCl(s) (unbalanced) Nonionic Equation: (regular balanced equation) 2 AgNO 3 (aq) + BaCl 2 (aq)  Ba(NO 3 ) 2 (aq) + 2 AgCl(s) Total Ionic Equation: (list dissociations for electrolytes only) 2 Ag + (aq) + 2 NO 3– (aq) + Ba 2+ (aq) + 2 Cl – (aq)  Ba 2+ (aq) + 2 NO 3– (aq) + 2 AgCl(s) (do not write dissociations for solids, liquids or gases) Net Ionic Equation: (list only what reacts or changes) 2 Ag + (aq) + 2 Cl – (aq)  2 AgCl(s) or, simplified: Ag + (aq) + Cl – (aq)  AgCl(s) Do page 2 of your workbook

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17. * All numbers listed are significant except zeros before or after a decimal that must be used as placeholders. Example:100.0010 - 7 significant digits 0.001010 - 4 significant digits

18. * Multiplication or Division Rules: * Count the number of digits in each number being multiplied or divided. * Perform the multiplication or division. * Round off to the least number of digits found in each of the individual numbers being multiplied.

19. 1. Determine the balanced chemical equation. 2. Determine information given. 3. Determine your wanted. 4. Determine the number of moles of what is given. 5. Use a wanted over given to determine the number of moles of the unknown. 6. Solve for the answer.

20. Example:If 200 mL of 0.100 mol/L silver nitrate solution reacts with a piece of copper, determine the mass of metal reacted. 2 AgNO 3 (aq) + Cu (s)  2 Ag (s) + Cu(NO 3 ) 2(aq) v = 0.200 Lm = ? C = 0.100 mol/L n AgNO3 = Cv n AgNO3 = (0.200 mol/L)(0.100 L) n AgNO3 = n Cu = 0.0200 mol x ½ = m Cu = nM m Cu = (0.0100 mol)(63.55 g/mol) m Cu = 0.636 g 0.0100 mol 0.0200 mol Do page 3 of workbook!!