Metals

A salt and oxygen gas

A salt and hydrogen gas

A metal oxide and water

A metal hydroxide and carbon dioxide

Iron

Calcium

Silver

Lead

Sodium

Potassium

Lithium

Calcium

Iron

Lead

Magnesium

Calcium

Lead

Tin

Zinc

Copper

The iron ore is oxidized to iron metal

Coke is used as both a fuel and a source of the reducing agent

The temperature at the top of the furnace is higher than at the bottom

Molten iron floats on top of the molten slag

Yellow

Red

Lilac

Blue

The Zinc atoms are smaller and fill the gaps between Copper atoms.

The Zinc atoms are larger than Copper atoms and disrupt the regular arrangement, making it harder for layers to slide.

Zinc reacts with Copper to form covalent bonds that lock the atoms in place.

Zinc increases the number of electrons in the sea, which increases the electrostatic attraction.

It increases as the number of valence electrons increases.

It decreases as electronegativity increases and the ability to lose electrons decreases.

It remains constant because all elements in Period 3 are metals.

It increases because the atomic radius decreases, strengthening the metallic bond.

12

8

6

4

Zinc

Magnesium

Iron

Copper

Aluminum oxide and iron

Aluminum sulfide and iron

Aluminum carbonate and iron

Aluminum hydroxide and iron

Sodium

Calcium

Magnesium

Zinc

To act as a catalyst

To increase the reactivity of aluminum

To lower the melting point of the electrolyte

To prevent the anodes from burning

Thermal stability increases.

Thermal stability decreases.

Thermal stability remains constant.

There is no predictable trend.

Calcium

Sodium

Zinc

Copper

$Zn$

$Ag^{+}$

$Zn^{2+}$

$Ag$

Magnesium and Zinc

Iron and Copper

Sodium and Potassium

Zinc and Aluminum

Hydroxides of very reactive metals like $K$ and $Na$ decompose easily on heating.

Hydroxides of moderately reactive metals like $Mg$ and $Ca$ decompose to form oxides.

Transition metal hydroxides are the most thermally stable.

All metal hydroxides decompose to give the metal and water.

$A + B^{n+} \rightarrow A^{n+} + B$

$B + A^{n+} \rightarrow B^{n+} + A$

$A^{n+} + B^{n+} \rightarrow AB$

$A + B \rightarrow AB$

It uses more energy than extraction from ore

It is much cheaper and saves energy

It produces more carbon dioxide than extraction

It requires the use of cryolite

Carbon dioxide

Limestone

Iron(III) oxide

Calcium silicate

Because aluminum gains oxygen

Because aluminum ions gain electrons

Because the volume of the ore is reduced

Because the temperature is reduced

A pure form of iron used in jewelry

The impure iron directly from the blast furnace

Iron that has been mixed with aluminum

A type of iron ore found in farms

Proximity to a limestone quarry

Proximity to a source of cheap, abundant electricity

Availability of large amounts of coke

A dry climate to prevent the ore from getting wet

It is recycled back into the electrolyte

It reacts with the molten aluminum to form alumina

It is released into the atmosphere as a waste gas

It is used to cool the graphite electrodes

To decrease the surface area for a slower reaction

To increase the surface area for a faster reaction

To prevent the coke from burning too quickly

To ensure the limestone does not decompose

To separate insoluble iron(III) oxide and silicates from the soluble sodium aluminate solution

To recover the sodium hydroxide for reuse in the electrolytic cell

To remove the water from the aluminum hydroxide precipitate

To neutralize the acidity of the bauxite ore before it enters the kiln

$Al^{3+}$ ions move toward the cathode and $O^{2-}$ ions move toward the anode

$Al^{3+}$ ions move toward the anode and $O^{2-}$ ions move toward the cathode

$Na^+$ ions are reduced at the cathode while $F^-$ ions are oxidized at the anode

$O^{2-}$ ions are reduced at the cathode while $Al^{3+}$ ions are oxidized at the anode

$3.75\text{ mol}$

$3.00\text{ mol}$

$4.00\text{ mol}$

$1.50\text{ mol}$

Zinc covers the iron so no air reaches it

Zinc is more reactive and corrodes instead of the iron

Zinc turns the iron into steel

Iron reacts with the zinc to form a new metal

It always stays the same

It often decreases compared to the pure metals

It always doubles

It becomes absolute zero

Tungsten

Zinc

Platinum

Iron

Building bridges

Fire sprinkler systems (fuses)

Making car engines

Constructing aircraft

It is the most abundant metal

It is highly resistant to oxidation and is an excellent conductor

It is a very strong magnetic material

It has a very low density

They are highly magnetic

They are non-sparking

They are very heavy

They are transparent

Zinc

Platinum

Aluminum

Lead

It is too expensive compared to gold.

It is highly toxic and causes environmental damage and 'itai-itai' disease.

It reacts violently with oxygen in the air.

It makes the steel bolts too weak to hold structures.

Impurities like arsenic or iron significantly increase the electrical resistance by scattering electrons.

Impure copper is a liquid at room temperature.

Impure copper is highly toxic to the touch.

The electricity would react with the impurities to produce explosive gases.

It is used as a fuel to heat the furnace.

It acts as a deoxidizer and desulfurizer, removing impurities from the molten steel.

It is used to line the inside of the furnace to prevent it from melting.

It turns the steel into a liquid state.