3. Nickel(Ni) Nickel is a silvery-white metal that is incredibly durable and has
a beautiful sheen. It is classified as a transition metal because
of its ability to accept and donate electrons to other
elements. Nickel has an atomic mass of 58.69, which makes it
one of the heavier elements on the periodic table.
Nickel was first isolated and classified as an element in 1751
by Axel Fredrik Cronstedt, who initially mistook the ore for
a copper mineral, in the cobalt mines of Los, Hälsingland,
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5. Reaction of nickel with acids
Nickel metal dissolves slowly in dilute sulphuric acid to form the aquated Ni(II) ion and hydrogen, H2. In
aqueous solution, Ni(II) is present as the complex ion [Ni(H2O)6]2+.
Ni(s) + H2SO4(aq) Ni2+(aq) + SO4
2−(aq) + H2(g)
The strongly oxidizing concentrated nitric acid, HNO3, reacts on the surface of iron and passivates the
surface.
6. Reaction of nickel with air
Nickel does not react with oxygen, O2 at room temperature, under normal conditions. Finely
divided nickel can burn, forming nickel(II) oxide, NiO.
2 Ni(s) + O2(g) 2 NiO(s)
7. Reaction of nickel with ammonia
Nickel(II)-ions are precipitated by ammonia as a green gelatinous precipitate of
nickel(II)hydroxide which dissolves forming a deep blue hexaaminenickel(II)
hydroxide at excess ammonia [4]
Ni2+(aq) + 2 OH−(aq) 2 Ni(OH)2(s) [light green]
Ni(OH)2(s) + 6 NH3(aq) [Ni(NH3)6]2+(aq) + 2 OH−(aq) [deep blue]
8. Reaction of nickel with dimethylglyoxim
Nickel(II) ions are precipitated by dimethylglyoxime under slightly alkaline conditions as a raspberry
colored complex.
9. Reaction of nickel with halogens
Nickel reacts slowly with halogens, forming the corresponding dihalides.
Ni(s) + Cl2(g) NiCl2(s) [yellow]
Ni(s) + Br2(g) NiBr2(s) [yellow]
Ni(s) + I2(g) NiI2(s) [black]
Nickel(II) can be oxidized to nickel(III) using Br2 under alkaline conditions
2 Ni(OH)2(s) + Br2(aq) + 2 OH−(aq) 2 Ni(OH)3(s) + 2 Br−(aq)
10. Reaction of nickel with hydroxide ions
Metallic nickel does not react with aqueous sodium hydroxide [4].
Nickel(II)-ions are precipitated by hydroxide ions forming a green gelatinous
precipitate [4]
Ni2+(aq) + 2 OH−(aq) 2 Ni(OH)2(s) [light green]
11. Reaction of nickel with sulfide
Nickel(II)-ions are precipitated by sulfide either using H2S and acetic acid (HCl
can't be used) or Na2S under neutral to alkaline conditions forming the black
NiS
Ni2+(aq) + S2−(aq) NiS(s) [black]
12. Reaction of nickel with water
Nickel metal does not react with water under normal conditions.
Nickel(II) ions complexes with water under acidic and neutral conditions forming
a light green hexaqua nickel ion [4].
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18. Palladium (Pd), chemical element, the least
dense and lowest-melting of the platinum
metals of Groups 8–10 (VIIIb), Periods 5 and 6, of
the periodic table, used especially as a catalyst (a
substance that speeds up chemical
reactions without changing their products) and
in alloys.
A precious gray-white metal, palladium is
extremely ductile and easily worked. Palladium is
not tarnished by the atmosphere at ordinary
temperatures.
It is a rare and lustrous silvery-white
metal discovered in 1803 by the English
chemist William Hyde Wollaston.
He noted that when he dissolved
ordinary platinum in aqua regia (nitric
acid + hydrochloric acid) not all of it
went into solution.
19.
20. Reaction of palladium with air
Palladium can be brought to react with oxygen, O2, by heating the palladium.
2 Pd(s) + O2(g) PdO(s) [black]
21. Reaction of palladium with halogens
Palladium will react with F2, Cl2 and Br2 forming palladium halides.
For fluorine, at mixture of Pd(II) and Pd(IV) is formed, and not Pd(III) as one could be led to believe:
2 Pd(s) + 3 F2(g) [Pd(II)Pd(IV)F6](s)
For chlorine, Pd(II)chloride is formed. Depending on the reaction conditions, two different forms are produced.
Pd(s) + Cl2(g) PdCl2(s)
For bromine, Pd(II)bromide is formed.
Pd(s) + Br2(g) PdBr2(s) [red-black]
22. Uses of Palladuim
The largest use of palladium today is in
catalytic converters.Palladium is also
used in jewelry, dentistry, watch making,
blood sugar test strips, aircraft spark
plugs, surgical instruments, and electrical
contacts,hydrogen purification, chemical
applications, groundwater
treatment.Palladium is also used to make
professional transverse (concert or
classical) flutes.
23. Isotopes Isotope Atomic mass
Natural
abundance (%)
Half life Mode of decay
102Pd 101.906 1.02 - -
104Pd 103.904 11.14 - -
105Pd 104.905 22.33 - -
106Pd 105.903 27.33 - -
108Pd 107.904 26.46 - -
110Pd 109.905 11.72 - -
Palladium is more reactive than the other platinum metals. For example,
it is attacked more readily by acids than any of the other platinum
metals. It dissolves slowly in nitric acid to give palladium(II) nitrate,
Pd(NO3)2, and with concentrated sulfuric acid it yields palladium(II)
sulfate, PdSO4∙2H2O. In its sponge form it will dissolve even
in hydrochloric acid in the presence of chlorine or oxygen.
26. Platinum is a silvery metallic chemical element, a
member of the six transition elements in Group VIII of
the periodic table known collectively as the platinum
metals (ruthenium, rhodium, palladium, osmium,
iridium, and platinum). Platinum has the symbol Pt, its
atomic number is 78, and its atomic weight is 195.09.
27. History
The first European reference to platinum appears in 1557 in
the writings of the Italian humanist Julius Caesar Scaliger as a
description of an unknown noble metal found
between Darién and Mexico, "which no fire nor any Spanish
artifice has yet been able to liquefy".
In 1735, Antonio de Ulloa and Jorge Juan y Santacilia saw
Native Americans mining platinum while the Spaniards were
travelling through Colombia and Peru for eight years. Ulloa
and Juan found mines with the whitish metal nuggets and
took them home to Spain. Antonio de Ulloa returned to Spain
and established the first mineralogy lab in Spain and was the
first to systematically study platinum, which was in 1748.
28.
29. Platinum has six naturally occurring isotopes:
190
Pt, 192
Pt, 194
Pt, 195
Pt, 196
Pt, and 198
Pt. The most abundant of these is 195
Pt, comprising 33.83% of all platinum.
Main isotopes Decay
abundance half-life (t1/2) mode product
190
Pt 0.0120% 4.83×10
11
y α 186
Os
192
Pt 0.782% stable
193
Pt synth 50 y ε 193
Ir
194
Pt 32.9% stable
195
Pt 33.8% stable
196
Pt 25.2% stable
198
Pt 7.36% stable
30. Physical properties
Pure platinum is a lustrous, ductile, and malleable, silver-white
metal.Platinum is more ductile than gold, silver or copper, thus
being the most ductile of pure metals, but it is less malleable
than gold.
Its physical characteristics and chemical stability make it useful
for industrial applications.Its resistance to wear and tarnish is
well suited to use in fine jewellery.
Platinum being dissolved in hot aqua regia
Chemical properties
Platinum has excellent resistance to corrosion. Bulk platinum does
not oxidize in air at any temperature, but it forms a thin surface film
of PtO2 that can be easily removed by heating to about 400 °C.
31. Reaction of platinum with air
Platinum metal does not normally react with air.
Reaction of platinum with halogens
Platinum will react with F2, Cl2, Br2 and I2 forming platinum halides.
For fluorine, at mixture of platinum(VI) fluoride, PtF6, and the tetrameric platinum(V) fluoride,
(PtF5)4 is formed, depending on the reaction conditions. The tetrameric platinum(V) fluoride
disproportionates into platinum(VI) fluoride and platinum(IV) fluoride, PtF4:
Pt(s) + 3 F2(g) PtF6(s) [dark red]
4 Pt(s) + 10 F2(g) (PtF5)4(s) [deep red]
(PtF5)4(s) PtF6(s) + PtF4(s) [yellow brown]
32. Reaction of platinum with halogens
For chlorine Pt(II)chloride and Pt(IV)chloride is formed, depending on reaction conditions.
Pt(II)chloride comes in two forms.
Pt(s) + Cl2(g) PtCl2(s) [brown black]
Pt(s) + 2 Cl2(g) PtCl4(s) [dark red or olive green]
For bromine and iodine, Pt(IV)halides formed.
Pt(s) + 2 Br2(g) PtBr4(s) [brown black]
Pt(s) + 2 I2(g) PtI4(s) [brown black]
33. Reaction of platinum with water
Platinum does not react with hydrogen, but hydrogen can be
dissolved in platinum.
Reaction of platinum with hydrogen
Platinum metal does not normally react with water.
