TRANSITION METALS

Group 9 members:

Jamella Chesney (group leader), Gibran Azeez, Shontel Baptiste, Yonnel Henry, Adiel Holligan, Kellyann Inniss, Melodie Lowe, Amrita Milling, Asaf Mohamed,

Abena Nedd, Daniel Persaud, Natasha Ramalho, Malini Tulsie

Subject: Chemistry

Class: Lower 6

Teacher: Mr. Latchman Tiwari

Date: November 30th, 2011

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CONTENTSIntroduction to Assignment……………………………………………………….…….page 3

Question One (1)………………………………………………………………..….……pages 4-6

Question Two (2)……………………………………………………………………….pages 7- 34

Reference…………..………………………………………………………..……….…page 35

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Introduction to Assignment

Task:

1) Describe the characteristics of the transition elements:

Physical characteristics

Trends (across periods 4-7)

Explain reason for the transition elements being between grps. 2 and 3

Compare to other elements in the P.T.

Types of intramolecular bonds existing

2) Determine the electronic configuration of transition metals and their ions:

Give brief background information on each metal

Electronic configurations: Use the Box method and dot and cross method on each

element in its natural state and ionic state, respectively. Include diagrams where

necessary.

State all the possible ions that can be formed from each element and their respective

colours.

In total there are 40 transition metals including two sets of series but we will only deal with 31 of

them.

The transition elements are those elements having a partially filled‘d’ or ‘f’ sub-shell in any

common oxidation state. The term "transition elements" most commonly refers to the d-block

transition elements. The first row of the transition metals is called the lanthanides or rare

earths. The second row consists of the actinides. All of the actinides are radioactive and those

above Z=92 are manmade in nuclear reactors or accelerators.

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QUESTION ONE

Characteristics of the Transition Elements

Reasons for transition metals being between group II and III on the periodic table

The elements of the second and third rows of the Periodic Table show gradual changes in properties across the table from left to right as expected. Consequently, the effects on atomic properties of the transition metals are: smaller atomic radius, increased first ionization energy, enhanced electro negativity and more nonmetallic character. The first ten elements called the first transition series are remarkably similar in their physical and chemical properties.

This general similarity in properties has been explained in terms of their relatively small difference in effective nuclear charge over the series. This occurs because each additional electron enters the penultimate 3d shell providing an effective shield between the nucleus and the outer 4s shell. Thus, the transition elements can be defined as those in which the d electron shells are being filled (except Sc and Zn where Sc (III) is d0 and Zn (II) is d10).

Comparing the properties of transition metals with those of alkali metals

Compared to the alkali metals, the transition metals:

o Are harder and stronger. They cannot be cut with a knife.

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o Are more dense. This means that in a fixed volume of metal there are more atoms of a transition metal than there are of an alkali metal

o have higher melting and boiling points – except mercuryo The transition metals are much less reactive than the alkali metals. They tend to react

relatively slowly, for example with air, water and acid.

Periodic trends of Transition Metals

Melting Point

Diagram showing the melting point of the elements of the first transition series

Transition metals have high melting points due to strong metallic bonds. The number of unpaired electrons in the outermost shell indicates the strength of the metallic bonds. Therefore, the more unpaired electrons present, the higher melting point will be. The first 4 elements in a row always have the highest melting points. However, as the unpaired d orbital electrons pair up, the melting point decreases. The last 5 elements in a row have a lower melting point than the first 4 elements. The last element in each row has the lowest melting point because the d orbital electrons are filled.

The metallic radius

The metallic radius decreases with the atomic number for the first 5 to 6 elements in a series and the metallic radius increases for the last few elements in a series. The reason the metallic radius

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behaves like this is due to the nuclear charge. As the number of electrons increases, the number of protons in the nucleus increases as well. As the number of protons in the nucleus increases, the atom is strongly shielding results in decrease of the atomic radius.

Ionization energy

By definition, ionization energy is how much energy is required to remove one electron from an element to the outer shell. Ionization energy increases from left to right due to the number of valance electrons increase from left to right in the periodic table. Ionization energy also increases from bottom to top. Electro negativity and Bond Polarity

Electro negativity is the ability of an atom to pull electrons to it. In the periodic table, electro negativity increases from left to right and from bottom to top. In all cases, if electrons are not being shared equally between atoms, the bonds will be polar. On the other hand, if electrons are being shared equally, the bonds will be non-polar.

Atomic Radius

Although there is a slight contraction at the beginning of the series, the atoms are all much the same size.

Colored compounds

We observe color as varying frequencies of electromagnetic radiation in the visible region of the electromagnetic spectrum. Different colors result from the changed composition of light after it has been reflected, transmitted or absorbed after hitting a substance. Because of their structure, transition metals form many different colored ions and complexes. Color even varies between the different ions of a single element - MnO4

− (Mn in oxidation state 7+) is a purple compound, whereas Mn2+ is pale-pink.

The color of a complex depends on:

the nature of the metal ion, specifically the number of electrons in the d orbital the arrangement of the ligands around the metal ion (for example geometric isomers can

display different colors) the nature of the ligands surrounding the metal ion. The stronger the ligands then the

greater the energy difference between the split high and low 3d groups.

Properties and Characteristics of Transition Elements

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They often form colored compounds. They can have a variety of different oxidation states. At least one of their compounds has an incomplete d-electron sub-shell. They are often good catalysts. They are silvery-blue at room temperature (except copper and gold). They are solids at room temperature (except mercury). They form complex ions (aqua ions included). They are often paramagnetic.

QUESTION TWO

Scandium (Sc)

This is a silvery-white metallic transition metal.

Date of Discovery: 1879Discoverer: Lars NilsonName Origin: ScandinaviaUses: No uses knownObtained From: minerals (thortveitile, wiikite)

Atomic Number: 21

Number of Neutrons: 24

Period: 4

Block in periodic table: d-block

Classification: Metallic

Melting Point: 1539.0 °C (1812.15 K, 2802.2 °F) 

Boiling Point: 2832.0 °C (3105.15 K, 5129.6 °F)

Crystal Structure: Hexagonal

Electronic Configuration of the Scandium Element

1s2 2s2 2p6 3s2 3p6 3d1 4s2 

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Electronic Configuration of the Scandium Ion

Sc3+

1s2 2s2 2p6 3s2 3p6 

Common Ionic States of Scandium.

Scandium has one common ionic state Sc3+. This is because bonding is only involved with the 4s electrons.

Common Ionic Compounds of Scandium

Scandium Sulphide - Sc2S3

Scandium(III) oxide, Sc2O3

Titanium (Ti)

It is a strong, lustrous, corrosion-resistant transition metal with a silver color.

Date of Discovery: 1791Discoverer: William GregorName Origin: From the Greek word titanos (Titans)Uses: paint, rubberObtained From: minerals (ilmenite, rutile)

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Atomic Number: 22Neutron number: 26Period: 4Block in periodic table: d-blockColour: SilverClassification: MetallicMelting Point: 1660.0 °C (1933.15 K, 3020.0 °F)Boiling Point: 3287.0 °C (3560.15 K, 5948.6 °F) Crystal Structure: Hexagonal

Electronic Configuration of Titanium

1s2 2s2 2p6 3s2 3p6 3d2 4s2

 

Common Ionic States of Titanium

Titanium has four ionic states 1+, 2+, 3+, 4+. This is due to bonding with all the 4s electrons and all the unpaired 3d electrons. The maximum ionic state is 4+ because the maximum amount of electrons available for bonding is 4.

Common Ionic Compounds of Titanium

Titanium carbide, Ti C

Titanium(IV) oxide  TiO2

Titanium disilicide Ti Si 2

Vanadium (V)

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 It is a hard, silvery gray, ductile and malleable transition metal .

Date of Discovery: 1830Discoverer: Nils SefstromName Origin: After Vanadis (Scandinavian goddess)Uses: catalyst, dye, color-fixerObtained From: minerals (patronite, vanadinite)Atomic Number: 23

Number of Neutrons: 28

Period: 4

Block in periodic table: d-block

Melting Point: 1890.0 °C (2163.15 K, 3434.0 °F) 

Boiling Point: 3380.0 °C (3653.15 K, 6116.0 °F)

Crystal Structure: Cubic

Electronic Configuration of Vanadium Element

1s2 2s2 2p6 3s2 3p6 3d3 4s2

Common Ionic States of Vanadium

Vanadium has five ionic states 2+, 2+, 3+, 4+, 5+.

Common Ionic Compounds of Vandium

Vanadium(IV) oxide  VO2

Vanadium(V) fluoride  VF5.

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Vanadium(II) chloride  VCl2

Chromium ( Cr)

It is a steely-gray, lustrous, hard metal that takes a high polish and has a high melting point. It is also odorless, tasteless, and malleable.

Date of Discovery: 1797Discoverer: Louis VauquelinName Origin: From the Greek word chrôma (color)Uses: Stainless steelObtained From: Chromite

Atomic number: 24.

Electronic Configuration:

1s2 2s2 2p6 3s2 3p6 3d5 4s1 OR [Ar] 3d5 4s1

Common Ionic States of Chromium

It has six ionic states 1+, 2+, 3+, 4+, 5+, 6+

Examples of possible ions and compounds:

Hydroxide: Cr(OH)3, green in colour

Chlorides: Cr2Cl3, green in colour

Sulphates: Cr2(SO4)3 • 12(H2O), reddish brown (anhydrous), purple (hydrated)

Nitrates: [Cr(H2O)6](NO3)3•3H2O, blue-violet in colour (anhydrous)

Manganese (Mn)

It is found as a free element in nature (often in combination with iron), and in many minerals. As a free element, manganese is a metal with important industrial metal alloy uses, particularly in stainless steels.

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Date of Discovery: 1774Discoverer: Johann GahnName Origin: From the Latin word mangnes (magnet)Uses: steel, batteries, ceramicsObtained From: pyrolusite, psilomelane, rhodochrosite

Electronic Configuration:

1s22s22p63s23p64s23d5

Ions:

It has seven ionic states 1+, 2+, 3+, 4+, 5+, 6+, 7+

Examples if Ionic compounds:

Oxides: MnO, green in colour

Dioxides: MnO2, brown-black in colour

Bromide: MnBr2, pink in colour

Iron (Fe)

Iron is a metal in the first transition series. It is the most common element (by mass) forming the planet Earth as a whole. Iron's very common presence in rocky planets like Earth is due to its abundant production as a result of fusion in high-mass stars, where the production of nickel-56 (which decays to iron) is the last nuclear fusion reaction that is exothermic.

Date of Discovery: Known to the ancientsDiscoverer: UnknownName Origin: LatinSymbol Origin: From the Latin word ferrum (iron)Uses: steel, haemoglobin (carries oxygen in blood)

Electronic configuration:

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1s2 2s2 2p6 3s2 3p6 4s2 3d6.

Total number of possible ions:

Fe1+

1s2 2s2 2p6 3s2 3p6 4s2 3d5

Fe2+

1s2 2s2 2p6 3s2 3p6 4s2 3d4

Fe3+

1s2 2s2 2p6 3s2 3p6 4s2 3d3

Fe4+

1s2 2s2 2p6 3s2 3p6 4s2 3d2

Fe5+

1s2 2s2 2p6 3s2 3p6 4s2 3d1

Fe6+

1s2 2s2 2p6 3s2 3p6 4s2

Cobalt (Co)

Date of Discovery: 1737Discoverer: George BrandtName Origin: From the German word kobalt (evil spirit)Uses: magnets, ceramics, special glassesObtained From: arsenic, oxygen, sulfur, cobaltine

 

Atomic Number: 27 Number of Neutrons: 32 Melting Point: 1495.0 °C (1768.15 K, 2723.0 °F) Boiling Point: 2870.0 °C (3143.15 K, 5198.0 °F) 

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Crystal Structure: Hexagonal Colour: silver

Electronic configuration

1s2 2s2 2p6 3s2 3p6 3d3 4s2 3d4

Common Ionic States of Cobalt

Cobalt has five ionic states 1+, 2+, 3+, 4+, 5+.

 

Nickel (Ni)

Date of Discovery: 1751Discoverer: Alex CronstedtName Origin: From the German word kupfernickel (false copper)Uses: electroplating metal alloys, nickel-cadmium batteriesObtained From: pentlandite

           Atomic Number: 28 Number of Neutrons: 31 Melting Point: 1453.0 °C (1726.15 K, 2647.4 °F) Boiling Point: 2732.0 °C (3005.15 K, 4949.6 °F) Crystal Structure: Cubic Color: white

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Electronic configuration

1s2 2s2 2p6 3s2 3p6 3d3 4s2 3d6

Common Ionic States of Nickel

Nickel has four ionic states 1+, 2+, 3+, 4+.

Copper (Cu)

Date of Discovery: Known to the ancientsName Origin: From the Latin word cypriumUses: electrical conductor, jewelry, coinsObtained From: chalcopyrite, coveline, chalcosine

Atomic Number: 29 

Number of Neutrons: 35 

Melting Point: 1083.0 °C (1356.15 K, 1981.4 °F) 

Boiling Point: 2567.0 °C (2840.15 K, 4652.6 °F) 

Crystal Structure: Cubic 

Color: red/orange

Electronic Configuration of Copper

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1s2 2s2 2p6 3s2 3p6 3d3 4s2 3d7

  Common Ionic States of Copper

Copper has three ionic states 1+, 2+, 3+.

Colour: Blue

Zinc (Zn)

Zinc is a bluish silver, lustrous metal that tarnishes in moist air, producing a layer of carbonate. Zinc reacts with both acids and alkalis and is a fair conductor of electricity. It burns in air with a bright bluish-green flame producing white clouds of the oxide. Zinc is essential for good health and is only toxic in large amounts.

Date of Discovery: 1746Discoverer: Andreas MarggrafName Origin: From the German word zin (meaning tin)Uses: metal coating, rust protection, brass, bronze, nickelObtained From: zinc blend, calamine

State: SolidMelting point: 692.68 K (419.53oC)Boiling point: 1183 K (910oC)1st ionization energy: 906.4 kJ mol-1

2nd ionization energy:1733.2 kJ mol-1

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Structure: Hexagonal and closely packedColour: Bluish silver

Electron configuration:[Ar] 3d10 4s2

Shells: 2, 8, 18, 2STRUCTURE OF A ZINC BLENDE

Ions:

Zinc forms only 2+ ions and these are colourless.

In chemical compounds zinc exhibits almost exclusively a +2 oxidation. There are however, a few compounds of zinc in the +1 state but there are no reports of zinc in the +3 state at all.

Yttrium (Y)

Yttrium is a soft, silvery metal which usually exists in colourless compounds. It is relatively stable in air as a result of an oxide that forms on its surface. Yttrium also dissolves oxygen gas in relatively high concentrations.

Date of Discovery: 1794Discoverer: Johann GadolinName Origin: After Ytterby (a town in Sweden)Uses: color TV's, radarsObtained From: monazite, xenotime, yettriac

Melting point: 1798 K (1525oC)Boiling point: 3613 K (3340oC)

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1st ionization energy: 615.6 kJ mol-1

Shells: 2, 8, 18, 9, 2Structure: Hexagonal and closely packed

Electron configuration:

[Kr] 4d1 5s2

Ions:

Yttrium forms only 3+ ions

Zirconium (Zr)

Zirconium is a strong, malleable, ductile, lustrous, grayish-white metal. It is generally exceptionally resistant to corrosion but is, however, rapidly attacked by hydrofluoric acid, even at low concentrations. Powdered zirconium can spontaneously ignite in air and exposed surfaces form a protective layer.

Date of Discovery: 1789Discoverer: Martin KlaprothName Origin: zircon (mineral)Uses: nuclear applicationsObtained From: zircon, baddeleyite

Melting point: 2123 K (1850oC)Boiling point: 4673 K (4400oC)1st ionization energy: 640.1 kJ mol-1

2nd ionization energy:1266.8 kJ mol-1

3rd ionization energy:2218.2 kJ mol-1

Shells: 2, 8, 18, 10, 2Structure: Hexagonal and closely packed

Electronic configuration:

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[Kr] 4d2 5s2

Ions:

Zirconium is predominantly in +4 oxidation state in it compounds. Some less stable compounds, however, are known in which the oxidation sate is +3.

Niobium (Nb)

Niobium is a shiny, white, soft, and ductile metal, and takes on a bluish tinge when

exposed to air at room temperatures for a long time. The metal starts to oxidize in air at high

temperatures, and when handled hot must be done so under a protective atmosphere so as to

minimize oxide production.

Date of Discovery: 1801

Discoverer: Charles Hatchet

Name Origin: After Niobe, daughter of mythical king (Tantalus)

Uses: No uses known

Obtained From: columbite

Electronic Configuration

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1s2

2s2 2p6

3s2 3p6 3d10

4s2 4p6 4d4

5s1

Molybdenum (Mo)

Molybdenum is a silvery-white, hard, transition metal. Molybdenum is used in alloys, electrodes and catalysts. The World War 2 German artillery piece called "Big Bertha" contains molybdenum as an essential component of its steel.

Date of Discovery: 1778Discoverer: Carl Wilhelm ScheeleName Origin: From the Greek word molubdos (lead)Uses: aircraft, missilesObtained From: molybdenite, wulfenite

Electronic Configuration

Technetium (Tc)

Technetium is a silvery-grey metal that tarnishes slowly in moist air. Until 1960, technetium was available only in small amounts. The chemistry of technetium is related to that of rhenium.

Date of Discovery: 1937Discoverer: Carlo PerrierName Origin: From the Greek word technêtos (artificial)Uses: Tc-99m is used for radioactive tracing in medicineObtained From: Man-made

Electronic Configuration

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1s2

2s2 2p6

3s2 3p6 3d10

4s2 4p6 4d5

5s1

Element Melting point (°C)

Boiling Point (°C)

First Ionization Energy (kJ/mol)

Colour in natural state

Atomic Radius (pm)

Niobium 2477 4744 652.1 Grey metallic 146

Molybdenum 2623 4639 684.9 Grey metallic 139

Technetium 2157 4265 702.4 Silver grey metallic 138

Ruthenium (Ru)

Ruthenium is a very rare, hard, lustrous, brittle, silvery-white metal that does not tarnish at room temperature. The metal is unaffected by air, water and acids. It reacts with molten alkali and halogens and can oxidize explosively.

Date of Discovery: 1844Discoverer: Karl KlausName Origin: From the Latin word Ruthenia (Russia)Uses: platinum alloysObtained From: pentlandite, pyroxinite

Ions:

3+

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1s2

2s2 2p6

3s2 3p6 3d10

4s2 4p6 4d6

5s1

Electronic configuration: 

[Kr] 4d7 5s1

Most stable oxidation state is 4+

Rhodium ( Rh)

Rhodium is a rare, hard, silvery-white, lustrous metal . It is highly reflective and extremely resistant to corrosion. It is not attacked by most acids. Rhodium's salts form rose-colored aqueous solutions. This is used as an automobile catalyst converter in an automobile, in making electrical contacts and in making ornaments e.g. jewellery (coating).

Date of Discovery: 1803Discoverer: William WollastonName Origin: From the Greek word rhodon (rose)Obtained From: by-product of nickel production

Electronic configuration

[Kr] 4d8 5s1

Oxidation States

Most stable oxidation state is 3+

Palladium (Pd)

Palladium was discovered by William.H. Wollaston in 1803 in platinum ore. He isolated palladium metal in a series of chemical reactions, finally heating palladium cyanide to extract palladium metal. The element is named after the Greek goddess of wisdom "Pallas'.

It has the following ions:

1+, 2+ , 3+

Electron configuration: 

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[Kr] 4d10

 Silver (Ag)

Silver is a soft, white, lustrous transition metal. It has the highest electrical conductivity of any element and the highest thermal conductivity of any metal. The metal occurs naturally in its pure, free form (native silver), as an alloy with gold and other metals.

Date of Discovery: Known to the ancientsDiscoverer: UnknownName Origin: From the Old English word seolfor (silver)Symbol Origin: From the Latin word argentum (silver)Uses: jewelry, photography, electrical conductorObtained From: ores

Electronic configuration:

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 4d10 OR [Kr] 5s1 4d10

Total number of possible ions:

The possible ions that can be formed from silver are:

Ag+1, ag2+

Examples of compounds formed with the ion are:

Oxide(s) / air: Ag2O, AgO ⇒ black in colour

Chloride(s): AgCl ⇒ white in colour

-E.g. reacts with these ligands according to the following equations:

Iodide: AgI ⇒ yellow in colour (insoluble)

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Cadmium (Cd)

Cadmium is a soft, malleable, ductile, bluish-white divalent metal. It is similar in many respects to zinc but forms complex compounds. Unlike other metals, cadmium is resistant to corrosion and as a result it is used as a protective layer when deposited on other metals.

Date of Discovery: 1817Discoverer: Fredrich StromeyerName Origin: From the Greek word kadmeiaUses: poisonous, nickel-cadmium batteriesObtained From: by-product of zinc refining

Electronic configuration:

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 OR [Kr] 5s2 4d10

Ions and examples of compounds:

Cd2+

Sulphide: CdS, yellow in colour- E.g. can react with hydrochloric acid

Fluoride: CdF2, grey or white greyHydroxide: Cd(OH)2, white in colour

- E.g. can react with hydrochloric acid, sulfuric acid and nitric acid

Lanthanum (La)

Lanthanum is a soft, malleable, silvery white metal which has hexagonal crystal structure at room temperature. Lanthanum easily is oxidized (a centimeter-sized sample will completely oxidize within a year) and is therefore used as in elemental form only for research purposes.

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Electronic configuration:

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5d1 6s2 OR [Kr] 5d1 6s2

Total number of possible ions:

Halogens: LaF3 (pale yellow), LaCl3 (white), LaI3, LaBr3 (white)

Water: La(OH)3, white in colour

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6

 

Hafnium (Hf)

Date of Discovery: 1923Discoverer: Dirk CosterName Origin: From the Latin word Hafnia (Copenhagen)Uses: nuclear reactorsObtained From: zircon

Hafnium ductile metal, silvery in colour and is used in nuclear reactor rods as it is a good absorber of neutrons and has high corrosion resistant ability. Hafnium is also found in gas filled and incandescent lights.

Atomic Number: 72

Melting Point: 2506 K (2233°C or 4051°F)

Boiling Point: 4876 K (4603°C or 8317°F)

State at Room Temperature: Solid

Element Classification: Metal

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Period Number: 6    

Group Number: 4    

Electronic Configuration

The electronic configuration of hafnium is:

[Xe] 4f14 5d2 6s2

Diagram showing electron shells of Hafnium

E. C. -2, 8, 18, 32, 10, 2

Ions

The number of possible ions that can be formed from hafnium are:

Hf1+, Hf2+, Hf4+

Examples of compounds formed with ions:

Hf1+ forms:

Hafnium carbide (HfC), which has the highest melting point of any known two-element compound (the most refractory compound).

Hf2+ forms :

Hafnium oxide (HfO2).

Hf4+ forms:

Hafnium fluoride (HfF4)

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Tantalum (Ta)

Tantalum is a chemical element with the symbol Ta and atomic number 73. The name is derived from the name Tantalus, a character in Greek mythology. Tantalum is a rare, hard metal with a blue gray colour. It is highly corrosion resistant.

Date of Discovery: 1802Discoverer: Anders EkebergName Origin: After king Tantalus (Greek mythology)Uses: capacitors, camera lensesObtained From: tantalite

Atomic Number: 73Melting Point: 3290 K (3017°C or 5463°F)

Boiling Point: 5731 K (5458°C or 9856°F)

Phase at Room Temperature: Solid

Element Classification: Metal

Period: 6    

Electronic configuration

[Xe] 4f14 5d3 6s2

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Ions

The number of possible ions that can be formed from tantalum are:

Ta1+, Ta2+, Ta3+, Ta4+, Ta5+

Some examples of compounds form with the above ions:

Ta1+ forms: [Xe] 4f14 5d3 6s1

Ta2H

Ta2+ forms: [Xe] 4f14 5d3

TaO2

Ta3+ forms: [Xe] 4f14 5d2

TaCl3

Tungsten (W)

Tungsten trioxide is then heated with carbon or hydrogen gas (H2), forming tungsten metal and carbon dioxide (CO2) or tungsten metal and water vapor (H2O). Pure tungsten is a steel grey or whitish metal. It has the highest melting point and lowest vapour pressure of all metals.

Date of Discovery: 1783Discoverer: Fausto and Juan Jose de Elhuyar

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Name Origin: From the Swedish words tung sten (heavy stone)Symbol Origin: From wolfram (its German name)Uses: used widely in electronics industryObtained From: scheelite, wolframite

Atomic Number: 74

Melting Point: 3695 K (3422°C or 6192°F)

Boiling Point: 5828 K (5555°C or 10031°F)

Phase at Room Temperature: Solid

Element Classification: Metal

Period Number: 6    

Electron configuration

[Xe] 4f14 5d4 6s2

E. C. - 2, 8, 18, 32,12,2

Ions

The possible ions that can be formed from tungsten are:

W2+, W3+, W4+, W5+, W6+

The compounds these ions form are:

Tungsten hexafluoride: WF6

Tungsten dichloride: WCl2

Tungsten diiodide: WI2

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Rhenium (Re)

Rhenium is used in flash lamps for photography and for filaments in mass spectrographs and ion gages, but is most frequently used as an alloying agent in tungsten and molybdenum and as a catalyst for performing certain reactions to a type of hydrocarbon known as an olefin.

Date of Discovery: 1925Discoverer: Walter NoddackName Origin: From Rhines provinces of GermanyUses: filaments for mass spectrographsObtained From: gadolinite, molybdeniteAtomic Number: 75Melting Point: 3459 K (3186°C or 5767°F)Boiling Point: 5869 K (5596°C or 10105°F)Phase at Room Temperature: SolidElement Classification: MetalPeriod Number: 6    Ionization Energy: 7.88 eV

Ions:

+7, +6, +4

1s2

2s2 2p6

3s2 3p6 3d10

4s2 4p6 4d10 4f14

5s2 5p6 5d5

6s2

Electron Configuration:

Osmium (Os)

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Metallic osmium is hard, brittle and very difficult to make. Powdered osmium is easier to make but emits osmium tetroxide (OsO4) when it is exposed to the air. Unfortunately, osmium tetroxide smells bad and is very poisonous. Because of these problems, osmium is primarily used to make very hard alloys.

Date of Discovery: 1803Discoverer: Smithson TenantName Origin: From the Greek word osmë (odor)Uses: tip gold pen points, instrument pivots, electrical light filamentsObtained From: ores that contain platinum

Atomic Number: 76Melting Point: 3306 K (3033°C or 5491°F)Boiling Point: 5285 K (5012°C or 9054°F)Phase at Room Temperature: SolidElement Classification: MetalPeriod Number: 6    Ionization Energy: 8.7 eV

Electronic configuration:

1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5d6 6s2

Ions: Os+4, Os+3

Iridium (Ir)

Date of Discovery: 1804Discoverer: S. TenantName Origin: From the Latin word iridis (rainbow)Uses: tip gold pens, crucible and special containersObtained From: gravel deposits with platinum

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Pure iridium is very brittle and is nearly impossible to machine. It is primarily used as a hardening agent for platinum. Platinum-iridium alloys are used to make crucibles and other high temperature equipment. Iridium is also alloyed with osmium to make the tips of fountain pens and compass bearings.

Atomic Number: 77Melting Point: 2719 K (2446°C or 4435°F)Boiling Point: 4701 K (4428°C or 8002°F)Phase at Room Temperature: SolidElement Classification: MetalPeriod Number: 6    Ionization Energy: 9.1 eV

Electronic configuration:

1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5d7 6s2

Ions:

Ir+1, Ir+2 , Ir+3 ,Ir+4, Ir+5, Ir6+

Platinum (Pt)

It is a dense, malleable, ductile, precious, gray-white transition metal. Even though it has six naturally occurring isotopes, platinum is one of the rarest elements in the Earth's crust and has an average abundance of approximately 0.005 mg/kg. It occurs in some nickel and copper ores along with some native deposits

Date of Discovery: 1735Discoverer: Julius ScaligerName Origin: From the Spanish word platina (little silver)Uses: jewelry, containers, catalystObtained From: platinum ores

Electronic configuration

[Xe] 4f14 5d9 6s1

Ionic state:

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The most common oxidation states of platinum are +2 and +4. The +1 and +3 oxidation states are less common. As a soft acid, platinum has a great affinity for sulfur, such as on dimethyl sulfoxide (DMSO); numerous DMSO complexes have been reported and care should be taken in the choice of reaction solvent.

Gold (Au)

Gold is a dense, soft, shiny, malleable and ductile metal. Pure gold has a bright yellow color and luster traditionally considered attractive, which it maintains without oxidizing in air or water. Chemically, gold is a transition metal and a group 11 element. It is one of the least reactive solid chemical elements. Gold is the most malleable and ductile of all metals.

Date of Discovery: circa 3000 BCDiscoverer: UnknownName Origin: From the Old English word geolo (yellow)Symbol Origin: From the Latin word aurum (gold)Uses: electronics, jewelry, coinsObtained From: crust of the earth, copper ores

Electronic configuration:

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6s 1 OR [Xe] 4f 14 5d 10 6s 1

Ions:

Common oxidation states of gold include +1 (gold(I) or aurous compounds) and +3 (gold(III) or auric compounds). Gold ions in solution are readily reduced and precipitated out as gold metal by adding any other metal as the reducing agent. The added metal is oxidized and dissolves allowing the gold to be displaced from solution and be recovered as a solid precipitate.

Mercury (Hg)

It is a poor conductor of heat, but a fair conductor of electricity. Like silver, mercury reacts with atmospheric hydrogen sulfide. Mercury even reacts with solid sulfur flakes, which are used in mercury spill kits to absorb mercury vapors.

Date of Discovery: Known to the ancientsDiscoverer: UnknownName Origin: After the planet MercurySymbol Origin: From the Latin word hydrargyrum (liquid silver)

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Uses: thermometers, barometers, fluorescent lamps, batteriesObtained From: cinnabar ore

Electronic configuration:

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10

Ions:

Common oxidation states of mercury include +2.

Actinium (Ac)

A soft, silvery-white radioactive metal, actinium reacts rapidly with oxygen and moisture in air forming a white coating of actinium oxide that prevents further oxidation.

Electronic configuration:

[Rn] 6d 1 7s 2

Ions:

Ac+3

As most lanthanides and actinides, actinium assumes oxidation state +3 in nearly all its chemical compounds. Actinium is found only in traces in uranium ores as 227Ac isotope, which decays with a half-life of 21.773 years, predominantly emitting beta particles.

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REFERENCE Petrucci, Ralph. General Chemistry: Principles & Modern Applications. 9th ed. Upper

Saddle River, New Jersey 2007.

Zener, C. Interaction Between the d-shell in the Transition Metal. Physical Review. 81.4

(1951).

Cotton, F. Albert; Wilkinson, G.; Murillo, C. A. (1999). Advanced Inorganic Chemistry

(6th ed.). New York: Wiley.

http://www.chemicalelements.com/elements/uub.html

http://www.bbc.co.uk/schools/gcsebit...ev_print.shtml

http://www.msm.cam.ac.uk/doitpoms/tl...c/printall.php

http://www.shodor.org/chemviz/ioniza...ackground.html

http://www.transtutors.com/chemistry...ng-points.aspx

http://www.chemicool.com/elements/zirconium.html

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