Week 5/6: Metal Reactivity

Emerging	Foundation	Core	Beyond Core	Accomplished
Can investigate and then determine which everyday metals easily corrode	Can observe and describe single displacement reactions involving metals	Can observe and describe reasons for the reactivity series in metals	Can describe why certain periodic table group elements are more reactivity than other groups and predict the reactivity series down a column	Can describe different crystal structures in metals and how they affect its physical properties

Week 5/6 TASKSHEET


LEO GER


Loss of Electrons = Oxidation     


eg. Al_(s) --> Al³⁺ _(aq)  + 3 e^-


Gain of Electrons = Reduction

eg. O_{2 (g)} + 2e^-  --->    O^2-

DISPLACEMENT REACTIONS (precipitation)







The difference between the SINGLE and DOUBLE displacement reactions is shown below in this image.......

A, B, C & D all represent atoms of elements.....

SINGLE displacement reactions are the first image - A&B are chemically joined to form a compound and C is all on its own. When they react together, B swaps to become chemically joined to C to form a compound and A ends up all on its own.

Example:    HCl  +  Zn -->   H2    + ZnCl

                

DOUBLE displacement reactions are what we were doing last week - where both compounds swap partners.

Example:      CaBr    +    KOH   -->  CaOH   +   KBr

VISUAL: To explain how the reactivity series is used