Chemistry - metals and the reactivity series

List the reactivity series

Potassium

Sodium

Lithium

Calcium

Magnesium

Aluminum

Carbon

Zinc

Iron

Cobalt

Nickel

Tin

Lead

Hydrogen

Copper

Silver

Gold

Way to remember reactivity series

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What are ores

Metal compounds that contain a high enough percentage of the metal to make it worthwhile (economically) to extract.

Which metals are extracted by electrolysis?

Metals above carbon in the reactivity series: potassium, sodium, calcium, magnesium, aluminium

Which metals can be heated with carbon in a displacement reaction (oxygen is removed from the metal by carbon reduction in a blast furnace).

Metals below carbon in the reactivity series

What is reduction

The loss of oxygen (Opposite of oxidation where oxygen is gained)

Properties of metals

Hard, strong, dense, malleable, lustrous, good conductors of heat and electricity, ductile, sonorous.

Pure metals

The layers of atoms within the metal can slide over each other when a force is formed, meaning they are soft and malleable

Alloys

Mixtures of metals and some other elements. They are harder than pure metals. The layers of atoms can't slide over each other when after applying a force as the different sized atoms disrupt the regular arrangements of atoms.

What is effervescence?

Bubbling

Neutralisation

Metal + Acid ⇨ Salt + Hydrogen

When metals above hydrogen in the reactivity series react with hydrogen in an acid, the metals displace hydrogen from the acid, producing salt and hydrogen.

How is salt formed in an experiment named

The salt is named after the metal and the type of acid. For example, lithium reacts with hydrochloric acid to produce lithium chloride.

Salt formed with hydrochloric acid and lithium

Lithium chloride

Salt formed with sulphuric acid and lithium

lithium sulfate

Salt formed with nitric acid and lithium

Lithium nitrate

Displacement reaction

Metal + Salt ⇨ Salt + Metal

When a metal is added to a compound containing a metal less reactive than it in the reactivity series. The more reactive metal replaces the less reactive metal in the compound, resulting in a different compound produced, separating the less reactive one from the compound.

Metals reacting with water

Metal + Water ⇨ Metal hydroxide + Hydrogen

Very reactive metals will react with water, for example, alkali metals. Alkali metals are unusual metals because they are very soft and also very reactive. They are stored in oil as they react quickly with oxygen in the air forming compounds with oxygen almost instantly.

Universal indicator

Turns purple/blue/blue-green in an alkali.

Turns red/orange/yellowy in an acid.

Test for hydrogen

A lit splint makes a squeaky pop noise when it comes in contact with hydrogen gas.

What are group 1 metals on the periodic table?

Alkali metals

What groups are the transition metals?

3-12

What is group 0 on the periodic table?

noble gases

What is group 7 on the periodic table?

Halogens

What are all of the group 1 metals?

Lithium, Sodium, Potassium, Rubidium, Caesium, Francium

True of false - metal hydroxides are alkaline

true

Group 1 naming hydroxides

Group 1 metal hydroxides have the formula __OH, for example, Li OH (lithium hydroxide).

Group 2 naming hydroxides

Group 2 metal hydroxides have the formula __(OH)₂, for example, Ca(OH)₂ (calcium hydroxide).

Lithium reacting with water

Lithium fizzes, slowly travels and floats, slowly becoming smaller until it eventually disappears.

Sodium reacting with water

Sodium fizzes, travels quicker and dissolves into a molten ball that moves quickly on the water surface.

Potassium reacting with water

Potassium fizzes a lot, travels extremely quickly, disappears very quickly and a purple or pink flame is produced.

What must alkali metals be stored in and why?

Oil to prevent them from reacting with the air and producing metal oxide