Reactivity Series

What is the reactivity series

An order of how reactive a group of metals are with water, steam, oxygen and each ther (displacement reactions)

Order of reactivity series

1. Potassium,

2. sodium,

3. calcium,

4. magnesium ,

5. aluminium,

6. zinc ,

7. iron ,

8. copper

List of all diatomic elements

+state of substance

Iodine I - = solid

Hydrogen Have -Gas

Nitrogen No - Gas

Bromine Bright - liquid

Oxygen Or -gas

Chlorine Clever - gas

Fluroine Friends -gas

What determines how reactive a metal is

1. the tendency of the metal to lose electron(s) and form a positive ion/ more reactive metals lose electrons more easily e.g potassium and sodium lose electrons easily and from ions while copper does not lose electroms easily therefore is very unreactive

metal + oxygen →

metal + oxygen → metal oxide

reaction with air

potassium reaction when heated in air

• burns with a lilac flame

• Forms a white solid

• 4K + 0_{2 ^→} 2k₂0

sodium reaction when heated in air

• burns with a yellow flame

• forming a white soli

• 4Na + 0_{2 ^→} 2Na₂0

calcium reaction when heated in air

• Burns with a red flame

• forming a white solid

• 2Ca+ 0_{2 ^→} 2Ca0

Magnesium reaction when heated in air

• Burns with a bright white light

• Forming a white solid

• 2Mg + 0_{2 ^→} 2Mg0 _{( magnesium oxide)}

Aluminium reaction when heated in air

• Burns only when a fine powder

• Forming white solid

  • 4Al + 30_{2 ^→} 2Al₂0₃

zinc reaction when heated in air

• burns in air

• forming yellow solid which changes to white on cooling

• 2Zn + 0_{2 ^→} 2Zn0

Iron reaction when heated in air

• Iron fillings burn with orange sparks

• Forming black solid

• 3Fe + 20_{2 ^→} Fe₃0₄

copper reaction when heated in air

• does not burn but becomes covered in black layer

  • 2Cu + 0_{2 ^→} 2Cu0

Ionic compounds are all white

metal + water →

metal + water → metal hydroxide + hydrogen

lithium observations with water

• equation

• floats and moves on the surface

• fizzes gas is given off

• eventually disappears

• heat given out

• colourless solution is formed

• 2Li+2H₂0 ^_→ 2LiOH+H₂

sodium observations with water + equation

• FFEHC

• melts into a silvery ball

• burns with a yellow flame

• 2Na+2H₂0 ^_→ 2NaOH+H₂

potassium observations with water

• FFEHC

• burns with a lilac flame

• 2Li+2H₂0 ^_→ 2LiOH+H₂

group 2 less reactive metals with water

Calcium Reaction with water

• Fizzing

• Sinks then rises

• Heat released

• Calcium disappears

• Cloudy solution is formed

• Ca+2H₂0 ^_→ Ca(OH)₂+H₂

magnesium reaction with water

• Slow reaction

• Few bubbles

• Mg+2H₂0 ^_→ Mg(OH)₂+H₂

How do you test did hydrogen gas

lit splint into test tube of hydrogen then hear squeaky pop

metal + steam →

metal + steam → metal oxide + hyrdogen

Magnesium reaction with steam

• Bright white light

• White solid forms

• Heat given out

aluminium reaction with steam

• powdered aluminium reacts to form a white solid. Heat given out

• no reaction in foil form- aluminium only reacts when the protective layer of aluminium oxide is removed

zinc reaction with steam

• glows to form a yellow powder which changes to white on cooling. Heat given out

iron reaction with steam

• powdered iron flows to form a black solid

What is a displacement reaction

A more reactive metal takes the place (displaces) of a less reactive metal in a component

Magnesium + copper (4) sulfate →

• observations and how to carry out

a solid metal reacting with a solution of a metal ion

• magnesium powder is added to blue copper sulphate solution

• Blue solution fades to colourless

• Magnesium disappears

• Black specks at bottom

• Heat given off

• equation

Aluminium + iron (III) oxide →

Solid metal reacting with a solid metal ion

• THERMIT REACTION

• Produces sparks

• Very exothermic

• Molten iron produced

SAM CID

Same - Control

Alter - Indepentend

Measure - Dependent

what is an ore

an ore is a rock that contains a metal colour d from which the metal can be extracted

what metals are reduced from it’s ore by electrolysis

• Potassium

• sodium

• Calcium

• Magnesium

• Aluminium