Metals, Non metals & Gases - Physical & Chemical Properties, Occurrence, Extraction etc.

1. UNIVERSITY OF GUYANA
DEPARTMENT OF CHEMISTRY
INORGANIC CHEMISTRY (CHM 3201)
END OF SEMESTER PRESENTATION
TOPIC
METALS, NON – METALS, NOBLE GASES:
OCCURRENCE & EXTRACTION
STUDENT : JOYLYN CONWAY
LECTURER: …….

2. OBJECTIVES
Metals
• Definition
• Physical & Chemical Properties
• Occurrence
• Extraction

3. OBJECTIVES
 Non Metals
• Definition
• Physical & Chemical Properties
• Occurrence
• Extraction
 Gases
• Extraction (Separation/Isolation)

6. METALS
A metal is basically a solid material, that is usually hard, shiny, malleable, fusible,
and ductile. It is a good thermal (heat) and electrical conductor.
On the periodic table as shown earlier, there is a distinct region where metallic
elements can be found. Examples:
Aluminum (Al) Silver (Ag) Titanium (Ti)
Gold (Au) Manganese (Mn) Lead (Pb)
Sodium (Na) Uranium (U) Mo (Molybdenum)
Iron (Fe) Cobalt (Co) W (Tungsten)

7. METALS – PHYSICAL PROPERTIES
• Good ELECTRICAL CONDUCTORS and HEAT
CONDUCTORS.
• Malleable - can be beaten into thin sheets.
• Ductile - can be stretched into wire.
• Possess metallic luster.
• Opaque as thin sheet.
• Solid at room temperature (EXCEPT Hg -Mercury).

8. METALS – CHEMICAL PROPERTIES
• Usually have 1-3 electrons in their outer shell.
• Lose their valence electrons easily, thus low ionization
energies. (they are commonly oxidized)
• Form oxides that are BASIC.
• Are good REDUCING AGENTS.
• Have lower ELECTRONEGATIVITIES.

9. METALS – CHEMICAL PROPERTIES
• Alkali metals are always 1+ (lose the electron in s
subshell)
• Alkaline earth metals are always 2+ (lose both electrons
in s subshell)
• Transition metal ions do not follow an obvious pattern,
2+ is common, and 1+ and 3+ are also observed

10. METALS – OCCURRENCE
• As stated under chemical properties they are good
reducing agents, as a consequence it is expected that
they are easily oxidized, thus yielding a compound that
is not the metal in its pure form. For this reason metals
are rarely found in their native form. Only some of
those that are less reactive are found in their free state in
the earth’s crust
E.g. Platinum (Pl), Copper(Cu) and Gold (Au),
Silver (Ag).

11. Metals commonly occur, as sulphide, oxide, halide and carbonates.
All the forms in which metals naturally occur whether in their natural
state or not, are as follows:
• Minerals – this is whereby metals occur in their free state in
the earth’s crust.
• Ores – This is a for of mineral which allows for the extraction
of metals
• Gangue – within ores there are impurities and rocks, and
surrounding clay and sand. These are referred to as Gangue.

12. METALS – OCCURRENCE CONT’D
• To obtain the metals from their impure form , some
natural chemical process has to occur, that would
reduce a compound of the metal or its ore. This yields
the metal in its pure form as small flakes or inclusions.

13. METALS – OCCURRENCE CONT’D
Oxides Carbonates Halides Sulphides Sulphates
Zincite (ZnO)
Marble or
limestone
(CaCO3)
Fluorspar (CaF2)
Zinc blende
(ZnS)
Galena (PbS)
Anglesite
(PbSO4)
Haematite
(Fe2O3.xH2O)
Magnetite
(Fe3O4)
Calamine
(ZnCO3)
Cryolite
(Na3AlF6)
Iron pyrites
(FeS2)
Baryl (BaSO4)
Bauxite
(Al2O3.2H2O)
Siderite (FeCO3)
Horn Silver
(AgCl)
Cinnabar (HgS)
Gypsum
(CaSO4.2H2O)
Cuprite (Cu2O)
Magnesite
(MgCO3)
Rock salt (NaCl)
Epsom salt
(MgSO4.7H2O)

14. METALS – EXTRACTION
Metals can be extracted by two methods:
• Electrolytic Reduction
• Reduction
The choice of method depends on the reactivity of the metal.
Reactive metals are usually extracted by means of electrolytic
reduction, while those that are less reactive are extracted by
means of reduction with the use of C (carbon) and CO (carbon
monoxide)

15. • On the right is a pictorial
representation of the
“REACTIVITY SERIES OF
METAL”.
• This series can therefore be used to
determine which method of
extraction of metals is preferably
used.
As you go UP the series REACTIVITY
INCREASES, and as you go DOWN
the series REACTIVITY
DECREASES.

17. METALS – EXTRACTION
• Extraction of metal from its ore process, entail three
major steps:
• Concentration/Purification of Ore
• Reduction of metal
• Refining (Purification)

18. METAL - EXTRACTION (CONCENTRATION OF ORE)
• This step entails the removal of impurities, unwanted
substances (rocks & grits) that are associated with the
mineral ore. This can be done by means of the following
techniques:
• Hydraulic washing
• Froth floatation process
• Magnetic separation
• Chemical separation

19. METAL - EXTRACTION (CONCENTRATION OF ORE)
Hydraulic Washing
This technique basically involves gravity
separation. A stream of water flows
through a tube containing the metal ore
with it’s impurities (gangue). The ore is
denser and heavier than the gangue,
thus when a stream of water flows the
tubes it carries the gangue with it, leaving
behind the pure metal ore.

20. METAL - EXTRACTION (CONCENTRATION OF ORE)
Froth Floatation Process
This process is more than likely specific to
sulphide ores only. The sulphide ores are
usually ground to a powdered form, which
has an oil detergent mixture added to it to
yield an emulsion. The emulsion is stirred
and aerated to so as to allow the oil and froth
to float to the surface with the sulphide ores.
While the non polar gangue remains at the
bottom of the flask. The mineral rich froth is
obtained and allowed to settle.

21. METAL - EXTRACTION (CONCENTRATION OF ORE)
Magnetic Separation
This method can only be utilized if
the metal and its ore has different
magnetic properties. The method
entails the grounding of the metal and
its ore also. After which the powder is
rolled over a magnetic roller, which
causes the magnetic substances to
attract towards the belt, leaving behind
the non magnetic particles.

22. METAL – EXTRACTION (REDUCTION OF METAL)
• This procedure basically entails the obtaining of the metal, by
reducing it from its metal oxide form.
• This procedure deals with whether the metal will be extracted by
“REDUCTION” or “ELECTROLYTIC REDUCTION” based
on their reactivity.
• Those metal ores that occur as sulphides and carbonates, rather
as oxides, usually have to be converted to oxides, prior to
reduction, since it is easier to obtain metals once in their oxide
form.

23. METAL – EXTRACTION (REDUCTION OF METAL)
• They are two methods in which sulphides/carbonates can be
converted to oxides:
1.Calcination - Heating of the ore in the absence of oxygen
e.g. ZnCO3 ZnO + CO2
2. Roasting – Heating of the ore in the presence of oxygen
e.g. 2 ZnS + 2 O2 3 ZnO + SO2HEAT
HEAT

24. METAL – EXTRACTION (REDUCTION OF METAL)
REDUCTION
• The oxide of the metal is then reduced by means of a reducing
agent in the presence of heat. Such an agent can either be C or
CO (recall the Ellingham Diagrams)
ZnO + C Zn + CO
ZnO + CO Zn + CO2
HEAT
HEAT

25. METAL – EXTRACTION (REDUCTION OF METAL)
Other Examples :
HgS – Cinnabar
(Name of Ore)
N.B. Examples previously shown are specific to metals
found low or in the middle of the reactivity series.

26. METAL – EXTRACTION (REDUCTION OF METAL)
• For the extraction of metals high in the reactivity series,
recall these are done by means of electrolytic reduction.
• The molten chloride of the metal is reduced
electrolytically to obtain the metal.
• During electrolysis, electrons are being added directly to
the metal ions at the cathode (reduction)

28. METALS – EXTRACTION (REFINING (PURIFICATION))
1. Liquation
• Metals with low melting points are suitable for this method e.g Sn,
Pb
• The metal impurities are place into a liquefied form
• A sloping hearth of a furnace is used on which the metal is placed
and melted.
• As a consequence of the heating the pure metal melts and flows
down the slope, while the impurities with higher melting points
remain behind.

29. PICTORIAL REPRESENTTION OF REFINING OF METAL
BY MEANS OF LIQUATION

30. METALS – EXTRACTION (REFINING (PURIFICATION))
2. Electrorefining
• Recall electrolysis was used to obtain the metal from
its ore. Electrolysis can be further be applied, this time
with aim of purifying the extracted metal.
• This method entails the use of a block of impure metal
to be made the anode and a thin sheet of pure metal to
be made the cathode of an electrolytic cell containing an
aqueous solution of the metal salt.

31. PICTORIAL REPRESENTTION OF REFINING OF METAL
BY MEANS OF ELECTROREFINING

33. SUMMARY OF EXTRACTION OF METAL PROCEDURES

34. SUMMARY OF EXTRACTION OF METAL PROCEDURES
BASED ON REACTIVITY

36. NON METALS
• The are naturally occurring elements that do not portray
the same chemical and physical properties as those of
metals. Non metals are not good thermal or electrical
conductors . They are non – lustrous, brittle and range
from hard to soft.
• Seventeen elements on the periodic tale are generally
classified as being non metals, of which each of them falls
under at least one state of matter (solid, gas, liquid)

37. NON METALS
Solid Gas Liquid
Carbon (C) Hydrogen (H) Argon (Ar) Bromine (Br)
Phosphorus (P) Helium (He) Krypton (Kr)
Sulfur (S) Oxygen (O) Xenon (Xe)
Selenium (Se) Nitrogen (N) Radon (Rn)
Iodine (I) Neon (Ne)
Fluorine (F)
Chlorine (Cl)

38. NON-METALS – PHYSICAL PROPERTIES
• Low Melting Points for solids and liquids
• Low boiling Points for solids and liquids
• Graphite (Carbon) has an exception, it is a good
conductor of electricity
• Not ductile
• Seven non-metals exist under standard conditions
as diatomic molecules:

39. NON-METALS – PHYSICAL PROPERTIES
• H2(g)
• N2(g)
• O2(g)
• F2(g)
• Cl2(g)
• Br2(l)
• I2(l) (volatile liquid - evaporates readily)

40. NON-METALS – PHYSICAL PROPERTIES
• In terms of their electronic configuration, the
outermost electron shells of most nonmetals
are incomplete. These elements therefore
attempt to gain electrons. The exceptions are
the noble gases, which are unreactive
because their outermost electron shells are
complete.

41. NON-METALS – CHEMICAL PROPERTIES
• Have a tendency to gain or share electrons with
other atoms. They are electronegative in
character.
• React with oxygen to form acidic or neutral
oxides.

42. NON-METALS – CHEMICAL PROPERTIES
• Non-metals do not react with water.
• Non-metals react with chlorine to form
covalent chlorides.

43. NON-METALS – CHEMICAL PROPERTIES
• Non-metals react with hydrogen to
form covalent Hydrides

44. NON –METALS – OCCURRENCE
• Hydrogen, carbon, nitrogen, oxygen, sulfur, and the noble gases
can be found in the form of free (uncombined) elements as well
as compounds in nature.
• The remaining non metals are found as compounds in nature.
Similar to that of metals they occur as:
Carbonates (CO32− ) Halides (RX) Phosphates(PO43− )
Sulfides (S2− ) Nitrates (NO3–)
Sulfates (SO42-) Oxides (O2–)

45. NON METAL – EXTRACTION
• Bromine is commonly found in sea water as halides. However
in some cases it is required in its elemental state, as a
consequence it has to be extracted, this is completed under four
(4) stages.
1. Oxidation of bromide ions Br– to bromine Br2
2. Removal of bromine vapour
3. Reduction of bromine Br2 to hydrobromic acid HBr
4. Oxidation of hydrobromic acid HBr to bromine Br2

46. NON METAL – EXTRACTION
Stage 1: Oxidation of bromide ions Br– to bromine Br2
Bromine is removed from the sea water by
displacement of the bromide ions using chlorine:
Cl2(aq) + 2Br–(aq) ==> 2Cl–(aq) + Br2(aq)
Stage 2: Removal of bromine vapour
The bromine mixture is air blown. This extracts the
easily vaporized bromine.

47. NON METAL – EXTRACTION
Stage 3: Reduction of bromine Br2 to hydrobromic acid HBr
• A fine mist of sulphur dioxide and water are mixed with
the bromine vapour.
• The hydrogen bromide and sulphuric acid mist formed
are removed from the air by passing the mist through a
layer of glass fibre, causing the acids to condense, which
yields a concentrated solution of hydrobromic acid.
Br2(aq) + SO2(g) + 2H2O(l) ==> 2HBr(aq) + H2SO4(aq)

48. NON METAL – EXTRACTION
Stage 4: Oxidation of hydrobromic acid HBr to bromine Br2
• Steam and chlorine are blown through the acid solution to
reform bromine by oxidation of the bromide ion:
Cl2(aq) + 2HBr(aq) ==> 2HCl(aq) + Br2(g)
• The bromine vapour is removed from the mixture by steam
distillation.
• The hot vapour mixture is condensed to form an aqueous
layer of bromine, which is then dried using concentrated
sulphuric acid.

51. EXTRACTION OF OXYGEN & NITROGEN GAS
• The atmosphere comprises of approximately 78% N2 ,
21% O2 , 0.9% Ar and 0.04% CO2.
• These three gases are separated into their individual
components by means of fractional distillation.
• In order for this to be done the air must be
LIQUEFIED.

52. EXTRACTION OF N2 & O2 - FRACTIONAL DISTILLATION
• Air is filtered to remove dust, and then cooled in stages until it reaches –200°C.
At this temperature it is a liquid. The air has been liquefied.
• water vapour condenses, and is removed using absorbent filters
• carbon dioxide freezes at -79°C, and is removed
• Oxygen liquefies at -183°C
• Argon liquefies at -186°C
• Nitrogen liquefies at -196°C
• The Ar, N2 and O2 gases are then separated by means of fractional
distillation, on the basis of the temperatures at which they liquefy.

54. EXTRACTION (ISOLATION/SEPARATION)
OF NOBLE GASES
• The air is comprised of other gases (i.e. Noble Gases) .
Argon, Neon, Krypton and Xenon, are all gases that are
by products of fractional distillation that yields Nitrogen
and Oxygen gas. However the extraction of Ar can be
done in the same way as that of nitrogen and oxygen.
• N.B. The gases are all mixed together
• Neon, Krypton and Xenon can be extracted by means of
DEWAR’S METHOD

55. EXTRACTION OF NOBLE GASES – DEWAR’S METHOD
• The mixture of noble gases is separated into individual
constituents by the use of coconut charcoal which adsorbs
different gases at different temperatures.
• Argon, Krypton and Neon – After ½ hour at 173K, only
these noble gases are adsorbed by the charcoal, while helium
and neon remain unabsorbed.
• The mixture of helium and neon is kept in contact with the
coconut charcoal at 93K which completely adsorbs neon
leaving free helium.

56. EXTRACTION OF NOBLE GASES – DEWAR’S METHOD
• The charcoal at 173K containing argon, krypton and
xenon is placed in contact with another charcoal at
the temperature of the liquid air when argon diffuse
into the other charcoal.
• The temperature of the first charcoal (temp.173K)
still containing krypton and xenon is raised to 183K
when krypton is set free while xenon remain
adsorbed in the charcoal. When it is heated, xenon
is recovered.

57. PICTORIAL REPRESENTATION OF THE APPARATUS
USED TO CARRY OUT DEWAR’S METHOD

58. EXTRACTION OF RADON
• Radon however is obtained by radioactive
disintegration of radium-226

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