*What is:

1. A metal…

2. A non metal…

3. Molecular compound…

4. Ionic compound…

5. Group…

6. Period…

7. Charge…

HH2(g)2(g) hydrogenhydrogen NN2(g)2(g) nitrogennitrogen OO2(g)2(g) oxygenoxygen

FF2(g)2(g) fluorinefluorine ClCl2(g)2(g) chlorinechlorine BrBr2(2(ll)) brominebromine

II2(g)2(g) iodineiodine SS8(s)8(s) sulfursulfur PP4(s)4(s) phosphorusphosphorus

Are now found in the data booklet!!!!

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: P4O3(g) =

4 atoms

tetraphosphorus trioxidetetraphosphorus trioxide

3 atoms3 atoms

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: CaCl2 - calcium chloride

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 Mg2+ and P3–

Mg3 P2

Mg3P2 (s)

***all ionic compounds are solids at room temperature.

* 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 SO42–

Put the two together grouping the complex ion: Na+ (SO4

2–)Now cross the charges: Na2(SO4)1

Since 1’s are not necessary: Na2SO4 (s)

Example: calcium nitrate - Ca2+ and NO3–

Ca2+(NO3–) Ca(NO3)2 (s)

Example: sodium hydroxide - Na+ and OH–

Na+(OH–) NaOH (s)

*use the first ion listed as the most common. For example, Cu2+ is more common than Cu+, so Cu2+ would be used if no choice is given.

When naming these compounds containing When naming these compounds containing elements with more than one charge:elements with more than one charge:

• use Roman numerals to indicate the charge of the ion used.

Example: CuCl is copper (I) chloride

Example: CuCl2 is copper (II) chloride

*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: CuSO4 6H2O is: copper (II) sulfate hexahydrate

Example: aluminum chloride trihydrate is:

AlCl3 3H2O

* Formation of a precipitate

* Formation of a gas

* Colour change

* Energy change

Simple Compositionelement + element compound2 Na(s) + Br2(g)

Simple Decompositioncompound element + element + element2CaCO3(s)

Single Replacementelement + compound element + compoundMg(s) + 2 NaOH(aq)

Double Replacementcompound + compound compound + compound3 HCl(aq) + Al(OH)3(aq)

Hydrocarbon Combustionhydrocarbon + oxygen carbon dioxide + water vapourC3H8(g) + 5O2(g)

Oxidation Metal + oxygen Compound2Fe(s) + O2(g)

2 NaBr(s)2 NaBr(s)

2Ca(s) + 2C(s) + 3O2(g)2Ca(s) + 2C(s) + 3O2(g)

2 Na(s) + Mg(OH)2(aq)2 Na(s) + Mg(OH)2(aq)

AlCl3(s) + 3 HOH(AlCl3(s) + 3 HOH(ll))

FeO (s)FeO (s)

3CO3CO22(s) + 4 HOH((s) + 4 HOH(g)g)

Examples:

NaOH(aq) Na+(aq) + OH–(aq)

Al2(SO4)3(aq) 2 Al3+(aq) + 3 SO42–(aq)

Ionic compounds Molecular compounds

may be soluble (turn into aq)

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

Example: A silver nitrate solution reacts with a solution of barium chloride.

AgNO3(aq) + BaCl2(aq) Ba(NO3)2(aq) + AgCl(s) (unbalanced)

Nonionic Equation: (regular balanced equation)

2 AgNO3(aq) + BaCl2(aq) Ba(NO3)2(aq) + 2 AgCl(s)

Total Ionic Equation: (list dissociations for electrolytes only)2 Ag+(aq) + 2 NO3–(aq) + Ba2+(aq) + 2 Cl–(aq) Ba2+(aq) + 2 NO3–(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 Do page 2 of your

workbookworkbook

*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

*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.

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.

Example:Example: If 200 mL of 0.100 mol/L silver nitrate If 200 mL of 0.100 mol/L silver nitrate solution reacts with a piece of copper, determine the mass solution reacts with a piece of copper, determine the mass of metal reacted.of metal reacted.

2 AgNO2 AgNO3 (aq)3 (aq) + + Cu Cu(s)(s) 2 Ag 2 Ag(s)(s)

+ Cu(NO + Cu(NO33))2(aq)2(aq)

v = 0.200 Lv = 0.200 L m = ?m = ?

C = 0.100 mol/LC = 0.100 mol/L

nnAgNO3AgNO3 = Cv = Cv

nnAgNO3AgNO3= (0.200 mol/L)(0.100 L)= (0.200 mol/L)(0.100 L)

nnAgNO3AgNO3 = =

nnCuCu = 0.0200 mol x ½ = = 0.0200 mol x ½ =

mmCuCu = nM = nM

mmCuCu = (0.0100 mol)(63.55 g/mol) = (0.0100 mol)(63.55 g/mol)

mmCuCu = =

0.636 g0.636 g

0.0100 mol0.0100 mol

0.0200 mol0.0200 mol

Do page 3 of workbook!!