Chemical Reactions Ch 5.1, 5.2, 5.3 starting at page 141 Chemical Reactions wiki Questions 1-14 page 147 Chemical Equations - Part A Youtube 10 mins Chemical equations – Part B Youtube 9 mins

Ch 5.1 page 142 – What is a Chemical Equation? Chemical equation: a short-hand notation that scientists use to communicate what happens during a chemical reaction Word equation: involves replacing the reactants and products with their chemical names.

Formula equation – uses the chemical formulas for the reactants and products. Copy the formula

Showing states of matter

Balanced chemical equations pg 143 Copy this section including the definition and description below

Read the instructions but copy the equations and working. P 143

Read the instructions but copy the equations and working. P 143

Draw simple stick models. P 144

Read the instructions but copy the equations and working. P 144

Chemical equations – Part B Youtube 9 mins Read each instruction/thinking process, then write the equation as directed on page 145. Then do the interactive – Balancing Equations Review Q’s 1-14 page 147

5.2 page 149 Classifying chemical reactions Decomposition reactions Combination reactions Precipitation reactions Oxidation and Reduction reactions Extraction of Metals As you finish the notes – go on with the Unit Review questions on page 158 – answer in full sentences where appropriate. Q 1-21 (leave out Q 16)

Copy all of the above + the reaction to the right

Copy the definition above + the blue reactions to the right

Copy the definition above.

Copy these notes in total.

Page 152

We are not doing the section on predicting precipitates on page 152

Naming Ionic Compounds page152 To name Ionic compounds simply place the cation first and the anion second Ammonium, hydrogen carbonate, carbonate, nitrate and phosphate are poly-atomic ions – they are treated as a single entity with a set of brackets around the ion.

Crossover rule – Balanced ionic compounds Cross-over rule youtube - 5 mins The superscript eg 3+ represents the ionic charge. The subscript number represents the number of atoms of each ion in the neutral compound. A number in front is call a coefficient that multiplies all atoms in the molecule.

Write balanced ionic formulae for the following ion compounds (page 152 or your notes) Hydrogen fluoride Sodium hydrogen carbonate Calcium nitride Potassium oxide Magnesium sulfate Potassium iodide Ammonium bromide Iron (III) oxide Barium hydroxide

Oxidation and reduction reactions page 153 Oxidation: when a substance gains oxygen atoms or loses electrons Reduction: when a substance loses oxygen atoms or gains electrons Redox: an abbreviation for oxidation and reduction pairs of reactions

Oxidation – combustion page 153 Combustion reaction: any chemical reaction where a substance burns in oxygen to produce heat and light. Read the explanation below and copy the equations.

Oxidation – Corrosion page 154 Corrosion is a natural process, which converts refined metal to their more stable oxide. It is the gradual destruction of materials (usually metals) by chemical reaction with their environment. In the most common use of the word, this means electrochemical oxidation of metal (rusting) in reaction with an oxidant such as oxygen.

Read the explanation and copy the equations.

Reduction reactions page 154 Copy the definition, then read the explanation and copy the equations.

Read the explanation and copy the blue definitions.

Metal displacement (redox) reactions page 154 Read the explanation and copy the equations.

For replacement reactions to occur, the solid metal (Zn) must be higher on the reactivity scale than the ionic solution ion (Cu) for this REDOX reaction to occur. Zn transfers electrons to Cu++ ions, therefore Zn has been oxidized to Zn+ (OILRIG). Cu++ ions have been reduced as it has gained electrons to become Copper metal crystals (OILRIG).

Extraction of metals Activity series plays a large role in the extraction of metals. Highly reactive metals such as K, Na and Mg are usually found in compounds or as ions – therefore must be extracted by electrolysis – electrons are forced into the ions, reducing them to their pure element. The least reactive metals such as Ag and Au rarely form compounds and are regularly found as pure elements in nature – froth floatation can be used for these P 156. Zn, Fe, Pb, Sn, Cu can all be extracted by carbon reduction (heat and carbon)

Copy the definition below, then read the explanation and copy the equations.

Electrolysis page 157 Reduction Oxidation REDOX

Ch 5.3 Rates of Chemical reactions Reaction rates can be affected by the following factors. Increasing the following will increase reaction rates by increasing the likelihood of particles interacting with one another. Temperature Concentration Surface area Agitation Catalysts such as enzymes increase the rate but are not consumed by the reaction.