Metals

$FeO$

$Fe_2O_3$

$Fe_3O_4$

$Fe(OH)_2$

Shared pairs of electrons between atoms

Transfer of electrons from metal to non-metal

Attraction between positive ions and a 'sea' of delocalized electrons

Attraction between oppositely charged ions in a lattice

$1-$

$1+$

$2+$

$2-$

It is highly reactive

It is dull and brittle

It is resistant to corrosion

It has a low melting point

Potassium

Aluminum

Lead

Calcium

It is a transition metal.

It reacts quickly with acids in food.

It forms a stable, non-porous oxide layer that prevents further corrosion.

It is magnetic and can be easily sorted for recycling.

To act as a fuel to provide heat and to produce the reducing agent carbon monoxide.

To react with the limestone to form slag.

To lower the melting point of the iron ore.

To provide a source of oxygen for the combustion.

Roasting in air to form $ZnO$, then reduction with carbon.

Electrolysis of molten $ZnS$.

Reduction of $ZnS$ directly with hydrogen gas.

Dissolving $ZnS$ in acid followed by displacement with copper.

It is a Group 2 metal.

It has a high density.

It has variable oxidation states.

It is very reactive.

Black: Carbon; White: Magnesium Oxide

Black: Magnesium; White: Carbon Dioxide

Black: Iron Oxide; White: Magnesium Carbonate

Black: Carbon; White: Magnesium Carbonate

Alloys are always cheaper than any pure metal

Alloys can be designed to have specific properties like increased hardness

Pure metals are always gases at room temperature

Alloys are more reactive than pure metals

Lead

Tin

Zinc

Copper

It can be easily sterilized and does not corrode

It is very magnetic

It has a very low melting point

It is a good insulator of heat

It is very soft

It is extremely hard and holds a sharp edge

It is transparent

It is a liquid

Brass is a significantly better conductor of electricity than pure copper.

Brass has a lower density, making the electrical plug much lighter.

Brass is harder and more resistant to wear than pure copper.

Brass is more reactive, allowing it to form a protective coating faster.

Copper used in electrical wires

Aluminum hammered into thin sheets for foil

Iron used as a catalyst

Tungsten used in light bulb filaments

As a catalyst in the Contact process

For the casing of dry-cell batteries

As the main component of aircraft wings

For the production of jewelry like rings

Pure copper has a higher electrical conductivity than brass.

Brass is too difficult to etch with chemicals like iron(III) chloride.

Copper is harder than brass and supports the components better.

Brass would react with the solder, causing the components to fall off.

As a liquid medicine to treat nickel deficiency.

As a stent that can be inserted into an artery and then expanded to its original shape by body heat.

As a coating for X-ray machines to block radiation.

As a material for disposable syringes.

Nickel is cheaper than steel.

Nickel-based alloys have superior resistance to corrosion by strong acids compared to iron-based alloys.

Nickel is a better thermal insulator than steel.

Nickel reacts with the acid to form a protective layer of hydrogen gas.

Gas

Liquid

Solid

Plasma

It is extremely hard and tough

It is very soft and flexible

It dissolves in rain

It is a liquid metal

Bronze

Steel

Copper

Solder

It is very soft

It is magnetic

It is resistant to wear and corrosion

It is lighter than water

Pure metals are too expensive to use in large quantities

Alloys provide a better combination of strength, toughness, and corrosion resistance

Alloys are easier to dissolve in water for recycling

Pure metals are too heavy to stay upright

Nickel

Sodium

Lead

Zinc

The density is always exactly the average of the constituent metals

The density is usually close to the weighted average of its constituents

The density of an alloy is always much lower than any of its constituents

Alloys have no measurable density

They lack a long-range crystalline order, resulting in high strength and unique magnetic properties.

They are made entirely of glass and contain no metal atoms.

They are liquid at room temperature but look like solid steel.

They are extremely soft and can be molded like play-dough at room temperature.

It floats on top of the molten iron, protecting it from being re-oxidized by the air.

It acts as a catalyst to speed up the reduction of hematite.

It is the main source of carbon for the steelmaking process.

It is a highly explosive byproduct that must be handled with extreme care.

Galvanization is a surface coating of Zinc, whereas an alloy is a uniform mixture of elements throughout the bulk.

Galvanized steel is made by a nuclear reaction, whereas alloys are made by melting.

Galvanized steel contains only one metal, while alloys contain at least five.

Zinc and Iron cannot form an alloy together under any circumstances.

Aluminum is less reactive than carbon

Aluminum is more reactive than carbon

Carbon is too expensive

The reaction would be too slow

Loss of oxygen

Gain of oxygen

Loss of electrons

Addition of water

Iron

Magnesium

Copper

Lead

Silver dissolves

Zinc is deposited on the silver

No reaction occurs

The solution turns silver

Copper(II) carbonate

Iron(II) hydroxide

Copper(II) hydroxide

Magnesium hydroxide

Zinc atoms

Copper(II) ions

Oxygen ions

Zinc ions

Lead

Sodium

Aluminum

Gold

Aluminum

Sodium

Iron

Calcium

Copper

Magnesium

Iron

Zinc

They have been oxidized to $Fe^{2+}$ ions.

They have been reduced to $Fe^{2-}$ ions.

They have acted as the oxidizing agent.

They have gained electrons from the $Cu^{2+}$ ions.

It contains fat

It was traditionally cast into molds that looked like piglets

It is pink in color

It is only used to make farm equipment

Flux

Reducing agent

Ganga (Impurity)

Fuel

Limestone

Coke (via carbon monoxide)

Sand

Hot air

It reacts with iron to form iron nitride

It reacts with coke to form cyanides

It leaves the furnace unchanged as a waste gas

It is converted into liquid nitrogen at the bottom

Stage 1: Solid compound; Stage 2: Molten compound; Stage 3: Molten metal

Stage 1: Solid metal; Stage 2: Solid metal; Stage 3: Molten metal

Stage 1: Solid compound; Stage 2: Solid metal; Stage 3: Molten metal

Stage 1: Solid compound; Stage 2: Solid compound; Stage 3: Solid metal

They are completely non-toxic

They contain nitrogen which was not involved in the reactions

They consist only of pure oxygen

They are used to create the limestone charge

To react with impurities

To withstand extreme temperatures and prevent heat loss

To provide a source of calcium oxide

To filter the waste gases

It is oxidized to $P_{4}O_{10}$ and leaves as a gas.

It is reduced to Phosphorus and dissolves almost entirely into the molten iron.

It reacts with $CaO$ and is completely removed in the slag.

It remains as a phosphate mineral in the unreacted ore.

To oxidize the iron ore directly.

To oxidize the coke to provide heat and produce $CO_{2}$ for further reaction.

To react with the limestone to produce lime.

To keep the iron in a liquid state by preventing its reduction.

Ore reacts with $CO$ gas at $500^{\circ}C$.

Molten $FeO$ reacts with solid coke.

Steam reacts with iron to form $H_{2}$.

Nitrogen reacts with coke to form cyanides.

The gain of electrons

The loss of electrons

The gain of protons

The loss of neutrons

It is evaporated

It is siphoned or tapped off from the bottom

It is filtered through paper

It is skimmed off the top surface

A protective layer of aluminum oxide forms on its surface

It is kept under oil permanently

It is naturally unreactive like gold

It is coated in a layer of plastic

It is a physical change only

Electrons flow through the electrolyte

Ions carry the charge through the electrolyte

The process produces carbon and oxygen ions at the cathode

To melt the aluminum oxide

To convert aluminum hydroxide into aluminum oxide by heating

To dissolve bauxite in sodium hydroxide

To remove the carbon dioxide from the anodes

It is more reactive than aluminum

It conducts electricity when molten

It is a solid at $1000^\circ C$

It is insoluble in water

It stays constant due to cryolite

It decreases because more aluminum is produced

It increases due to the heating effect of the current

It drops to zero because the resistance disappears

It acts as a filter for oxygen bubbles

It acts as the liquid cathode surface where reduction occurs

It provides thermal energy to keep the cryolite molten

It prevents the carbon lining from touching the electrolyte

Carbon monoxide

Carbon dioxide

Tetrafluoromethane ($CF_{4}$)

Oxygen

Both the anode and cathode are inert throughout the process

The cathode is consumed while the anode remains intact

The anode is consumed while the cathode remains relatively intact

Both electrodes react with the electrolyte and must be replaced daily