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Metals
Mahum Mujeeb 8A
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Aluminum (Al)
Discovered:
Discoverer: Hans Christian
Oersted
Discovery Location: Copenhagen,
Denmark Discovery
Year: 1825
Properties:
Aluminum has a melting point of 660.37°C, boiling
point of 2467°C, specific gravity of 2.6989 (20°C),
and valence of 3. Pure aluminum is a silvery-white
metal. It is soft, light, relatively nontoxic, with a high
thermal conductivity, and high corrosion resistance.
It can be easily formed, machined, or cast.
Aluminum is nonmagnetic and nonspeaking. It is
second among metals in terms of malleability and
sixth in ductility. Aluminum coatings are highly
reflective of both visible and radiant heat. The
coatings form a thin layer of protective oxide and
do not deteriorate like silver coatings.
Uses:
Ancient Greeks and Romans used alum as an
astringent, for medicinal purposes, and as a mordant in
dyeing. It is used in kitchen utensils, exterior
decorations, and thousands of industrial applications.
Although the electrical conductivity of aluminum is only
about 60% that of copper per area of cross section,
aluminum is used in electrical transmission lines
because of its light weight. The alloys of aluminum are
used in the construction of aircraft and rockets.
Reflective aluminum coatings are used for telescope
mirrors, making decorative paper, packaging, and
many other uses. Alumina is used in glassmaking and
refractoriness. Synthetic ruby and sapphire have
applications in producing coherent light for lasers.
Extraction:
The alumina must be molten for electrolysis
to work,
Unfortunately, alumina has a high melting
point (2040 °C)
and it is not practical to do electrolysis at
such a high temperature.
A solution of alumina in cryolite melts at
about 900 °C
and electrolysis is done at about 950 °C.
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Aluminum
On the right are some pictures of
Aluminum and where they can
be used.
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Calcium (Ca)
Discovered:
Discoverer: Sir Humphy Davy
Discovery Location: London
Year: 1808
Properties:
Uses:
Calcium is essential for human nutrition. Animals
skeletons get their rigidity primarily from calcium
phosphate. The eggs of birds and shells of mollusks
are comprised of calcium carbonate. Calcium is
also necessary for plant growth. Calcium is used as
a reducing agent when preparing metals from their
halogen and oxygen compounds; as a reagent in
purification of inert gases; to fix atmospheric
nitrogen; as a scavenger and decarbonizes in
metallurgy; and for making alloys. Calcium
compounds are used in making lime, bricks,
cement, glass, paint, paper, sugar, glazes, as well as
for many other uses.
Extraction:
1.
The melting point of calcium is 839 +/- 2°C, boiling
point is 1484°C, specific gravity is 1.55 (20°C), with
a valence of 2. Calcium is a silvery white, soft
alkaline earth metal. Although none of the alkaline
earths occur free in nature, calcium compounds are
abundant.
Grinding, crushing , wet milling and screening, particle size
fractionation. The calcium carbonate so obtained is normally
delivered to the consumer (such as paper mills for paper
coating, wet end filler for the production of neutral or alkaline
sized papers) in slurry form. The solids content of the slurry is
high, near to 65 - 70%, various deflocculates are used to
maintain a very low viscosity even with the high solids.
2. 2. The limestone is fired in a furnace to convert the calcium
carbonate to calcium oxide. The CaO is delivered to the
customer as a bulk powder where it is made into a Ca(OH)2
slurry with water. Carbon dioxide is then added to the slurry to
reform Calcium Carbonate, This latter process yields a
carbonate with controlled characteristics such as particle size
and particle size distribution. This method is used for calcium
carbonate used in the pharmaceutical industry as a vey pure
carbonate is obtained.
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Calcium
On the right are some pictures of
Calcium and where they can be
used.
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Iron (Fe)
Discovered:
Unfortunately, no one knows who was the first
person to discover iron. Iron has been used since
prehistory. The Ancient Egyptians and Sumerians
began using iron on the tips of spears and in some
ornaments around 4000 BC. They obtained the iron
from meteorites that hit the earth. Sometime
between 2000 and 1200 BC the smelting of iron
(that is, obtaining iron metal from iron ore) began
in either India, Anatolia or Caucasus. We don’t
know who was the first to invent this process as
artifacts containing iron are found throughout the
history of these civilizations
Properties:
The melting point of iron is 1535°C, boiling point is
2750°C, specific gravity is 7.874 (20°C), with a
valence of 2, 3, 4, or 6. Pure iron is chemically
reactive and corrodes rapidly, especially in moist
air or at elevated temperatures. Four allotropic
forms, or ferrites, are known: a, b, g, and d, with
transition points at 770, 928, and 1530°C. The a form
is magnetic, but when iron is transformed into the b
form, the magnetism disappears, although the
lattice remains unchanged.
Uses:
Iron is vital to plant and animal life. In humans, it
appears in the hemoglobin molecule. Iron metal is
usually alloyed with other metals and carbon for
commercial uses. Pig iron is an alloy containing about
3-5% carbon, with varying quantities of Si, S, P, and Mn.
Pig iron is brittle, hard, and fairly fusible and is used to
produce other iron alloys, including steel. Wrought iron
contains only a few tenths of a percent of carbon and is
malleable, tough, and less fusible than pig iron.
Wrought iron typically has a fibrous structure. Carbon
steel is an iron alloy with carbon and small amounts of
S, Si, Mn, and P. Alloy steels are carbon steels that
contain additives such as chromium, nickel, vanadium,
etc. Iron is the least expensive, most abundant, and
most used of all metals.
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Extraction:
Iron ore consists mostly of oxygen and iron atoms bonded
together into molecules. To convert these oxides of iron
to metallic iron, they must be smelted or sent through a
direct reduction process to remove the oxygen. Oxygeniron bonds are strong, and to remove the iron from the
oxygen, a stronger elemental bond must be presented to
attach to the oxygen. Carbon is used because the
strength of a carbon-oxygen bond is greater than that of
the iron-oxygen bond, and the process is done at high
temperatures. The iron ore must be powdered and mixed
with coke, which is essentially carbon, and the
combination must be burnt in the smelting process. The
carbon dioxide byproduct goes off into the atmosphere
and what is left is almost pure iron.
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Iron
On the right are some pictures of
Iron and where they can be used.
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Mercury (Hg)
Discovered:
The Babylonians, among the first people groups of
early civilization, is credited to be the first to put on
record the use of the element mercury. This was
some 3000 years ago when it was mixed freely with
other products. It was then sometimes added in
creams and ointments in dangerous proportions
because it was not yet known then as a chemical
element. At times poisoning was the result. The
discovery of mercury as an element was in the 18th
century.
Properties:
Mercury has a melting point of -38.842°C, boiling point of
356.58°C, specific gravity of 13.546 (20°C), and a valence of 1
or 2. Mercury is one of the few elements that is liquid at
ordinary room temperatures. Mercury is a heavy, silverywhite metal. It is a relatively poor conductor of heat, but a fair
conductor of electricity. Mercury readily forms alloys with
other metals, called amalgams. An electrical discharge will
cause mercury to combine with the noble gases argon,
krypton, neon, and xenon. Mercury and its compounds are
highly poisonous. Mercury is readily absorbed across
unbroken skin or though the respiratory or gastrointestinal
tract. It acts as a cumulative poison. Mercury is very volatile
in air. When room temperature air (20°C) is saturated with
mercury vapor, the concentration greatly exceeds the toxic
limit. The concentration, and thus the danger, increases at
higher temperatures.
Uses:
Mercury is amalgamated with gold to
facilitate the recovery of gold from its
ores. Mercury is used to make
thermometers, diffusion pumps,
barometers, mercury vapor lamps,
mercury switches, pesticides, batteries,
dental preparations, antifouling paints,
pigments,
and catalysts. Many of the salts
c
and organic mercury compounds are
important.
Extraction:
1. Cinnabar ore occurs in concentrated deposits located at
or near the surface. About 90% of these deposits are
deep enough to require underground mining with
tunnels. The remaining 10% can be excavated from open
pits.1 Cinnabar is dislodged from the surrounding rocks
by drilling and blasting with explosives or by the use of
power equipment. The ore is brought out of the mine on
conveyor belts or in trucks or trains.
2. Commercial-grade mercury is poured into wrought-iron
or steel flasks and sealed. Each flask contains 76 lb (34.5
kg) of mercury. Higher purity mercury is usually sealed
in smaller glass or plastic containers for shipment.
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Mercury
On the right are some pictures of
Mercury and where they can be used.
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Potassium (K)
Discovered:
Discoverer: Sir Humphrey Davy
Discover Location: London
Year: 1807
Properties:
Potassium's melting point is 63.25°C, boiling
point is 760°C, specific gravity is 0.862 (20°C),
with a valence of 1. Potassium is one of the most
reactive and electropositive of metals. The only
metal that is lighter than potassium is lithium.
The silvery white metal is soft (easily cut with a
knife). The metal must be stored in a mineral
oil, such as kerosene, as it oxidizes rapidly in
air and catches fire spontaneously when
exposed to water. Its decomposition in water
evolves hydrogen. Potassium and its salts will
color flames violet.
Uses:
Potash is in high demand as a
fertilizer. Potassium, found in most
soils, is an element that is essential for
plant growth. An alloy of potassium
and sodium is used as a heat transfer
medium. Potassium salts have many
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commercial uses.
Extraction:
Potassium is gained either immediately by
electrolysis of Potassium salts or by
reaction of Na with Potassium salts.
Potassium is relatively easy to purify
once it has been produced by either
method, though "crude" commercial
potassium is often sold directly after
electrolysis. Obviously, both processes
require very high temperature, as
Potassium salts have to be molten to
conduct electricity.
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Potassium
On the right are some pictures of
Potassium and where they can be
used.
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Magnesium (Mg)
Discovered:
Discoverer: Joseph Black
Discovered Location: Bordeux ,
France
Year: 1755
Properties:
Magnesium has a melting point of
648.8°C, boiling point of 1090°C,
specific gravity of 1.738 (20°C), and
valence of 2. Magnesium metal is light
(one-third lighter than aluminum),
silvery-white, and relatively tough. The
metal tarnishes slightly in air. Finely
divided magnesium ignites upon
heating in air, burning with a bright
white flam
Uses:
Magnesium is used in pyrotechnic and incendiary
devices. It is alloyed with other metals to make them
lighter and more easily welded, with applications in the
aerospace industry. Magnesium is added to many
propellants. It is used as a reducing agent in the
preparation of uranium and other metals that are
purified from their salts. Magnetite is used in
refectories. Magnesium hydroxide (milk of magnesia),
sulfate (Epsom salts), chloride, and citrate are used in
medicine. Organic magnesium compounds have many
uses. Magnesium is essential for plant and animal
nutrition. Chlorophyll is a magnesium-centered
porphyry.
c
Extraction:
Magnesium metal is strong reducing agent
and therefore, cannot be obtained by
chemical reduction method. It is
extracted by electrolysis of fused
anhydrous salts. A number of methods
are available for the extraction of
magnesium metal from its ores. The most
widely used method is based on the
electrolysis of magnesium chloride
obtained from the seawater.
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Magnesium
On the right are some pictures of
Magnesium and where they can
be used.
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Titanium (Ti)
Discovered:
Discoverer: William Gregor
Discovered Location: England
Year: 1791
Uses:
Titanium is important for alloying with aluminum, molybdenum, iron,
manganese, and other metals. Titanium alloys are used in situations where
lightweight strength and ability to withstand temperature extremes are
required (e.g., aerospace applications). Titanium may be used in
desalination plants. The metal is frequently used for components which must
be exposed to seawater. A titanium anode coated with platinum may be used
to provide cathodic corrosion protection from seawater. Because it is inert in
the body, titanium metal has surgical applications. Titanium dioxide is used
to make man-made gemstones, although the resulting stone is relatively soft.
The asterism of star sapphires and rubies is a result of the present of TiO2.
Titanium dioxide is used in house paint and artist paint. The paint is
permanent and provides good coverage. It is an excellent reflector of
infrared radiation. The paint is also used in solar observatories. Titanium
oxide pigments account for the largest use of the element. Titanium oxide is
used in some cosmetics to disperse light. Titanium tetrachloride is used to
iridize glass. Since the compound fumes strongly in air, it is also used to
produce smoke screens.
c
Properties:
Titanium has a melting point of 1660 +/- 10°C, boiling point of
3287°C, specific gravity of 4.54, with a valence of 2, 3, or 4. Pure
titanium is a lustrous white metal with low density, high strength,
and high corrosion resistance. It is resistant to dilute sulfuric and
hydrochloric acids, moist chlorine gas, most organic acids, and
chloride solutions. Titanium is only ductile when it is free of oxygen.
Titanium burns in air and is the only element that burns in nitrogen.
Titanium is dimorphic, with the hexagonal a form slowly changing to
the cubic be form around 880°C. The metal combines with oxygen
at red heat temperatures and with chlorine at 550°C. Titanium is as
strong as steel, but it is 45% lighter. The metal is 60% heavier than
aluminum, but it is twice as strong. Titanium metal is considered to
be physiologically inert. Pure titanium dioxide is reasonably clear,
with an extremely high index of refraction and an optical dispersion
higher than that of diamond. Natural titanium becomes highly
radioactive upon bombardment with deuterons.
Extraction:
Conversion of titanium (IV) oxide, TiO2, into
titanium(IV) chloride, TiCl4The ore rutile (impure
titanium(IV) oxide) is heated with chlorine and
coke at a temperature of about 900°C. Other metal
chlorides are formed as well because of other
metal compounds in the ore. Very pure liquid
titanium (IV) chloride can be separated from the
other chlorides by fractional distillation under an
argon or nitrogen atmosphere, and is stored in
totally dry tanks.
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Titanium
On the right are some pictures of
Titanium and where they can be
used.
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Zinc (Zn)
Discovered:
Discoverer: Andreas Marggraf
Discovered Location: Germany
Year: 1746
Uses:
Zinc is used to form numerous alloys, including brass, bronze,
nickel silver, soft solder, Geman silver, spring brass, and
aluminum solder. Zinc is used to make die castings for use in the
electrical, automotive, and hardware industries. The alloy
Prestal, consisting of 78% zinc and 22% aluminum, is nearly as
strong as steel yet exhibits super plasticity. Zinc is used to
galvanize other metals to prevent corrosion. Zinc oxide is used
in paints, rubbers, cosmetics, plastics, inks, soap, batteries,
pharmaceuticals, and many other products. Other zinc
compounds are also widely used, such as zinc sulfide (luminous
dials and fluorescent lights) and ZrZn2 (ferromagnetic
materials). Zinc is an essential element for humans and other
animal nutrition. Zinc-deficient animals require 50% more food
to gain the same weight as animals with sufficient zinc. Zinc
metal is not considered toxic, but if fresh zinc oxide is inhaled it
can cause a disorder referred to as zinc chills or oxide shakes.
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Properties:
Zinc has a melting point of 419.58°C,
boiling point of 907°C, specific gravity
of 7.133 (25°C), with a valence of 2.
Zinc is a lustous blue-white metal. It is
brittle at low temperatures, but
becomes malleable at 100-150°C. It is
a fair electrical conductor. Zinc burns
in air at high red heat, evolving white
clouds of zinc oxide.
Extraction:
Add hydrochloric acid. The zinc
will form zinc chloride and the
sand will remain unchanged.
You can then filter it to get the
zinc chloride dissolved in the
filtered solution and the sand
left in the filter.
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Zinc
On the right are some pictures of
Titanium and where they can be
used.
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Extractions
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
Chemical series produced by arranging
the metals in order of their ease of
reaction with reagents such as oxygen,
water, and acids. An example of such an
arrangement, starting with the most
reactive, is: potassium, sodium, calcium,
magnesium, aluminum, zinc, iron, tin, lead,
copper, silver, gold. This arrangement
aids the understanding of the properties
of metals, helps to explain differences
between them, and enables predictions to
be made about a metal's behavior, based
on a knowledge of its position or
properties. It also allows prediction of the
relative stability of the compounds
formed by an element: the more reactive
the metal, the more stable its compounds
are likely to be.

The position of a metal in the series
determines the reactions of the metal with
various reagents, the displacement of one
metal from its compound by another
metal, and the method of extraction of a
metal from its ore.
Metal:
Date Discovered:
Mercury
Babylonian
Iron
Egyptian
Zinc
1746
Magnesium
1755
Titanium
1791
Calcium
1807
Potassium
1808
Aluminum
1825
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Timeline Of Events
This is the timeline of the metals I did just before.
As you can see from above going down it shows which time period each metal
was discovered. First Mercury was discovered by the Babylonians and then
Iron was later discovered by the Egyptians. We do not know the exact time
periods but we do the the tribes and civilizations which discovered it. Next
Zinc and Magnesium were discovered only 9 years away from each other.
Later in 1791, Titanium was discovered. In 1807 Calcium was discovered and a
year after that Potassium was discovered. In 1826 Aluminum was discovered.
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AOI Relating to Metals
Human Ingenuity
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Metals are well suited to sustainable development goals. They are not biodegradable and have
virtually an unlimited lifespan and the potential for unlimited recyclability. Thus metals can be
considered as renewable materials. However mineral resources, the source of primary metals,
are “non-renewable” as their supply is finite, but this does not necessarily mean scarcity. In
this paper the results from a series of Life Cycle Assessments of primary metal production
processes for copper, nickel, lead, zinc, aluminum and steel have been used to examine how
metals may contribute to society’s transition to sustainable development. Particular issues
considered include: •
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Current metal reserves and how these may change in the future,
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Some of the environmental impacts (Total Energy, Global Warming Potential and Acidification
Potential) associated with primary metal production and how they will be exacerbated by
declining ore grades
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New processing technologies with lower energy consumptions and improved metal extraction
efficiencies that will reduce reserve depletion and environmental impacts,
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Increasing the utilization of “metals in use” by recycling, with particular reference to
aluminum, •
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The potential impact of a carbon tax on metal prices and how this may influence the ways in
which metals are used in the future.
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The End
By Mahum Mujeeb 8A