Kelompok 3 - Kimia Unsur Golongan IIIa Dan IVa

ANALYTICAL CHEMISTRY

OlehFairuz Balqis

Helsya AnggitaKeynan HaqieRadjie FauzanTessa Sarah

Wida Rahmasariwida

• Boron family generally referred as group 13 elements in the periodic table. These consist of five elements namely boron, aluminum, gallium, indium, thallium as their family members. These metals are generally referred to as earth metals.

• Generally occur scarce in nature except aluminum• Posses three valence electrons • The carbon family consists of one metalloid (Boron) and four metals (Aluminium, Gallium,

Indium, and Thallium). • Soft and have low melting points except boron• Chemically reactive at moderate temperatures except boron• Ionization energy – In spite of the large nuclear charge and small size, the first ionization

energies of these elements are less than the corresponding values of s-block elements. This is because p-electrons are less penetrating and more shielded than s-electrons, i.e. they are farther from the nucleus and hence held less tightly than the s-electrons and thus can be easily removed.

• Electropositive (metallic) character increases from B to Tl. This is also indicated from the ionization energy values of these elements.

Boron Family

Boron

Physical characteristic

Chemical characteristic

uses

reactions

METALLOID

Physical characteristics of BoronState Solid

Color Black

Density 2.34 g/cm³

Melting point 2349 K

Boiling point 4200 K

Enthalpy of Vaporisation 480 kJ/mol

Chemical characteristics of BoronCrystal Structure rhombohedral

Electronegativity 2.04

Atomic Radii 85 pm

Atomic number 5Atomic mass 10.811 (7) g/mol Abundance 950 ppm

Uses of Boron

• Used with titanium and tungsten to make light weight heat resistant alloys. Also tennis rackets, regulators in nuclear plants, heat resistant glass and eye disinfectant.

• Boric acid (H3BO3) is used an insectiside, mostly against ants or cockroaches. Boron nitride is a material in which the extra electron of nitrogen (with respect to carbon) enables it to form structures that are isoelectronic with carbon allotropes.

• Sodium tetraborate decahydrate (Na2B4O7 - 10H2O) or borax, used in the production of adhesives, in anti-corrosion systems and many other uses.

Uses of Boron• Sodium tetraborate pentahydrate (Na2B4O7 - 5H2O),

which is used in large amounts in making insulating fiberglass and sodium perborate bleach.

• Orthoboric acid (H3BO3) or boric acid is used in the production of textile fiberglass, flat panel displays and eye drops.

• Boron slurry is used as an energetic material with very high energy density like rocket fuels and jet engines.

• Hard as well as a good conductor

Reactions of Boron

• Reactions with water Boron will not react with water under normal conditions.

• Reactions with air At higher temperatures, boron does burn in air to form boron(III) oxide, B2O3.

4B + 3O2(g) B2O3(s) • Reactions with halogens Boron reacts vigorously with

fluorine, chlorine, and bromine to form boron(III) trihalides. 2B(s) + 3F2(g) 2BF3(g)

2B(s) + 3Cl2(g) BCl3(g)

2B(s) + 3Br2(g) BBr3(g)

Reactions of Boron

• Reactions with acids Crystalline boron does not react with boiling hydrochloric acid (HCl) or boiling hydrofluoric acid (HF). Powdered boron oxidizes slowly when treated with concentrated nitric acid, HNO3.

Aluminium

reaction

Phisycal characteristic

Chemical characteristic

uses

METAL

Physical characteristics of AluminiumState solid

Color Bluish –white in its purest form, silvery in appearance while in general use

Density 2,70 g·cm−3

Boiling point 933,47 K

Melting point 2792 K

Enthalpy of fusion 10,71 kJ·mol−1

Enthalpy of Vaporisation 294,0 kJ·mol−1

Heat Capacity 24,200 J·mol−1·K−1

Chemical characteristics of AluminiumCrystal Structure Cubic closed packed

0,40494 nmElectronegativity 1,61

Ionization Potential 577,5 kJ·mol−1 , 1816,7 kJ·mol−1 ,

2744,8 kJ·mol−1

Atomic radii 118 pm

Covalen radii 118 pm

Abundance 82000 ppm

Reactions of Aluminium

• Reactions with water A thin layer of oxide prevents aluminium being attack by water.

• Reactions with air A thin layer of oxide prevents aluminium being attack by air. Aluminium will burn in oxygen with a brillian white flame to form aluminium trixode.

4Al + 3O2(g) 2Al2O3(s)

• Reactions with halogens Aluminium reacts vigorously with all halogens to form aluminium halides.

2Al(s) + 3Cl2(g) AlCl3(s)

2Al(s) + 3Br2(l) AlBr26(s)

2Al(s) + 3I2(l) l2I6(s)

• Reactions with acids Aluminium dissolves readily in dilute suphuric acid for form solutions containing the Al(III) ion and hydroden gas.

2Al(s) + 3H2SO4(aq) Al3+(aq) + 2SO4

2-(aq) + 3H2(g)

The reaction with dilute hydrochloric acid also yield the same Al(III) ion and hydrogen gas.

2Al(s) + 6HCl(aq) 2Al3+(aq) + 6Cl-

(aq) + 3H2(g)

• Reactions with bases Aluminium dissolves in sodium hydroxide to yield hydrogen gas and aluminates of the form [Al(OH)4]-.

2Al(s) + 2NaOH(aq) + 6H2O(l) 2Na+(aq) + 2[Al(OH)4]- + 3H2(g)

Reactions of Aluminium

• Kitchen utensils, building decorations, electrical transmission (not nearly as conductive as copper, but cheaper) as well as packaging (can, foil etc.).

• Aluminium alloys form vital components of aircraft and rockets as a result of their high strength to weight ratio. Alloys containing copper, magnesium, silicon, manganese and other metals are much stronger and more durable than aluminium, making aluminium useful in the manufacture of aircraft and rockets.

• Most electronic appliances that require cooling of their internal devices (like transistors, CPUs - semiconductors in general) have heat sinks that are made of aluminium due to its ease of manufacture and good heat conductivity.

• Aluminium oxide (Al2O3), alumina, is found naturally as corundum (rubies and sapphires), emery, and is used in glass making. Synthetic ruby and sapphire are used in lasers.

• Powdered aluminium is a commonly used silvering agent in paint. Aluminium flakes may also be included in undercoat paints, particularly wood primer - on drying, the flakes overlap to produce a water resistant barrier.

Uses of Aluminium

Physical Characteristic of Gallium

Color Silver White

State Solid at 298 K

Density 5.91g/cm3

Melting Point 302.91K (29.76°C)

Boiling Point 2477K (2204°C)

Enthalpy of Fusion 5.59 kJ mol-1

Enthalpy of Vaporisation 270.3 kJ mol-1

Heat Capacity 25.86 J mol-1 K-1

Chemical Characteristic of Gallium

Atomic Number 31

Atomic Mass 69.723 g/mol

Atomic Radii 130 pm

Abundance 18 ppm

Electronegativity 1.81

Electron Configuration [Ar] 3d10 4s2 4p1

Crystal Structure Orthorhombic

GALLIUMMETAL

REACTION

Reactions of GalliumReactions with bases

Gallium dissolves in aqueous alkali.

HAZARDS

Hazards of Gallium Harmful if swallowed, inhaled or of it comes in to contact with skin. Corrosive, causes burns. Some sources suggest that it may cause dermatitis from prolonged exposure; other tests have not caused a positive reaction. It will however stain your skin if you hold it in your bare hands.

Used in semiconductor production, quartz thermometers, laser diodes, used to locate tumors and for creating mirrors.

Gallium Gadolinium Garnet (Gd3Ga5O12) is a material with good optical properties, and is used in fabrication of various optical components and as substrate material for magneto-optical films.

Gallium is the rarest component of new photovoltaic compounds (such as copper indium gallium selenium sulphide or Cu(In,Ga)(Se,S)2, recently announced by South African researchers) for use in solar panels as an alternative to crystalline silicon, which is currently in short supply. It has been suggested that a liquid gallium-tin alloy could be used to cool computer chips in place of water. As it conducts heat approximately 65 times better than water it makes a considerably better coolant.

USESUses of Gallium

GALLIUM

Physical Characteristic of Indium

Color Silvery Lustrous Grey

State Solid at 298 K

Density 7.31g/cm3

Melting Point 429.75K (156.6°C)

Boiling Point 2345K (2072°C)

Enthalpy of Fusion 3.27 kJ mol-1

Enthalpy of Vaporisation 231.8 kJ mol-1

Heat Capacity 26.74 J mol-1 K-1

Chemical Characteristic of IndiumAtomic Number 49

Atomic Mass 114.818 (3) g/mol

Atomic Radii 155 pm

Abundance 0.049 ppm

Electronegativity 1.78

Electron Configuration [Kr] 4d10 5s2 5p1

Crystal Structure Tetragonal

INDIUMMETAL

REACTIONReactions of Indium

Reactions with bases

Unlike gallium (in the same group as indium), indium will not dissolve in aqueous alkali solutions.

Hazards of Indium

Pure indium in metal form is considered non-toxic. However, all indium compounds should be regarded as highly toxic. Indium compounds damage the heart, kidney, and liver, and may be teratogenic.

HAZARDS

The first large-scale application for indium was as a coating for bearings in high-performance aircraft engines during World War II.

Afterwards, production gradually increased as new uses were found in fusible alloys, solders, and electronics.

In the 1950s, tiny beads of it were used for the emitters and collectors of alloy junction transistors.

In the middle and late 1980s, the development of indium phosphide semiconductors and indium tin oxide thin films for liquid crystal displays (LCD) aroused much interest.

By 1992, the thin-film application had become the largest end use.

USESUses of Indium

INDIUM

Physical Characteristic of Thallium

Color Silvery White

State solid at 298 K

Density 11.85g/cm3

Melting Point 1746K (1473°C)

Boiling Point 1746K (1473°C)

Enthalpy of Fusion 4.31 kJ mol-1

Enthalpy of Vaporisation 166.1 kJ mol-1

Heat Capacity 26.32 J mol-1 K-1

Chemical Characteristic of Thallium

Atomic Number 81

Atomic Mass 204.383 g/mol

Atomic Radii 190 pm

Abundance 0.6 ppm

Electronegativity 1.62

Electron Configuration

[ Xe ] 4f14 5d10 6s2 6p1

Crystal Structure Hexagonal close packed

ThalliumMETAL

Reactions of Thallium• Reactions with water Thallium tarnishes slowly in moist air or dissolves in

water to yield poisonous thallium(I) hydroxide. 2Tl(s) + 2H2O(l)2TlOH(aq) + H2(g)

• Reactions with air An oxide layer protects thallium form further reaction with air. When heated strongly in air the poisonous thallium(I) oxide is formed.

2Tl(s) + O2(g)Tl2O(s) • Reactions with halogens Thallium reacts vigorously with fluorine, chlorine

and bromine to form poisonous dihalides. 2Tl(s) + 3F2(g) 2TlF3(s)

2Tl(s) + 3Cl2(g) 2TlCl3(s)

2Tl(s) + 3Br2(l) 2TlBr3(s) • Reactions with acids Thallium dissolves slowly in sulphuric acid and

hydrochloric acid as the product, poisonous thallium(I) salts, are not vey soluble.

• Thallium has been used in the production of high-density glasses, combined with sulfur or selenium and arsenic, that have low melting points in the range of 125 and 150°C. These glasses have room temperature properties that are similar to ordinary glasses and are durable, insoluble in water and have unique refractive indices.

• Infrared lenses• Thallium amalgam is used in thermometers for low temperature, because it

freezes at -58°C (pure mercury freezes at -38°C).

Thallium and its compounds are highly toxic and should be handled with

great care. Thallium is a suspected human carcinogen. Thallium was once

an effective murder weapon before its effects became understood and an

antidote (prussian blue) discovered.

Uses of Thallium

Hazards of Thallium

Chemical Characteristic of Ununtrium

Atomic Number 113

Atomic Mass [284] g/mol

Electron Configuration

[Rn] 5f14 6d10 7s2 7p1

Classification Metallic

Availability Shyntetic

Created by bombarding americium-243 atoms with calcium-48 atoms.

Experiments resulting in the formation of element 113 were reported in February 2004 following experiments carried out between 14 July - 10 August 2003 involving scientists at Dubna (Joint Institute for Nuclear Research at the U400 cyclotron with the Dubna gas-filled recoil separator, DGFRS) in Russia

CARBON FAMILY• The carbon family consists of carbon, silicon, germanium, tin and lead.• Carbon family elements contain atoms that have 4 electrons in their outer

energy level.• As you move down the periodic table in the carbon family the atomic

radius increases while ionization energy decreases.• The carbon family consists of one nonmetal (carbon), two metalloids

(silicon and germanium) and two metals (tin and lead). • The carbon family elements tend to be fairly unreactive.• The elements tend to form covalent compounds, though tin and lead also

form ionic compounds.• Carbon family elements exist free in nature and in compounds.

Physical Characteristic of Carbon

Color Graphite : BlackDiamond : colourless

State solid at 298 K

Density Graphite : 2.267 g/cm3

Diamond : 3.513 g/cm3

Melting Point 3800 K (3527°C)

Boiling Point 4300 K (4027°C)

Enthalpy of Fusion 105.0 kJ mol-1

Enthalpy of Vaporisation 710.9 kJ mol-1

Heat Capacity 8.517 J mol-1 K-1

Chemical Characteristic of Carbon

Atomic Number 6

Atomic Mass 12.0107 g/mol

Atomic Radii 70 pm

Abundance 480 ppm

Electronegativity 2.55

Electron Configuration 1s2 2s2 2p2

Crystal Structure Hexagonal close packed

CARBON (C)

NON METAL

Reactions of Carbon• Reactions with water Carbon, either as graphite or diamond does not react

with water under normal conditions. Under more forceful conditions, the reaction becomes important. In industry, water is blown through hot coke. The resulting gas is called water gas and is a mixture of hydrogen (H2, 50%), carbon monoxide (CO, 40%), carbon dioxide (CO2, 5%), nitrogen and methane (N2 + CH4, 5%). It is an important feedstock gas for the chemical industry.

C + H2O CO + H2

• Reactions with air Carbon, as graphite, burns in oxygen to form gaseous carbon(IV) dioxide. Carbon, as diamond, also burns in air when heated to 600-800°C to also form carbon(IV) oxide.

C(s) + O2(g) CO2(g) • Reactions with halogens Graphite reacts with fluorine (but none of the other halogens) at high temperatures to make a mixture of carbon tetrafluoride, CF4, together with some C2F6 and C5F12.

C(s) + excess F2(g) CF4(g) + C2F6 + C5F12• Reactions with bases Graphite reacts with hot concentrated nitric acid to form

mellitic acid, C6(CO2H)6.

Carbon-14 which is radioactive is used in "carbon dating" (telling how old something is

by determining the amount of Carbon-14 present in the item being tested as compared to a

standard value for a similar object which is new). Diamond is a gemstone and used for

drilling/cutting.Graphite is used in pencils, as a lubricant,

and to protect against rust.Charcoal is used to remove toxins, tastes,

and odors.

Uses

Silicon (Sc)

Physical Characteristic of Silicon

Color dark grey with a bluish tinge

State solid at 298 K

Density 2.33g/cm3

Melting Point 1687K (1414°C)

Boiling Point 3173K (2900°C)

Enthalpy of Fusion

39.6 kJ mol-1

Enthalpy of Vaporisation

383.3 kJ mol-1

Heat Capacity

19.789 J mol-1 K-1

Chemical Characteristic of Silicon

Atomic Number 14

Atomic Mass 28.0855 g/mol

Atomic Radii 110 pm

Abundance 2.771 x 105 ppm

Electronegativity 1.90

Electron Configuration

1s2 2s2 2p6 3s2 3p2 

Crystal Structure

Diamond

METALloid

Reactions of Silicon• Reactions with water a surface layer of oxide makes silicon unreactive to water.• Reactions with air it will not react with oxygen below temperatures of 900°C,

above this the reaction with oxygen gives silicon dioxide.

Si(s) + O2(g) SiO2(s)

At temperatures >1400°C the silicon will react with nitrogen to give silicon nitrides.

2Si(s) + N2(g) 2SiN(s)

3Si(s) + 2N2(g) Si3N4(s) • Reactions with halogens silicon reacts vigorously with all the halogens to form

tetrahalides, the reaction with fluorine takes place at room temperature, the others require heating over 300°C.

Si(s) + 2F2(g) SiF4(g)

Si(s) + 2Cl2(g) iCl4(g)

Si(s) + 2Br2(l) SiBr4(l)

Si(s) + 2I2(l) SiI4(s)

• Reactions with acids Under normal conditions silicon does not react with most acids, but is dissolved by hydrofluoric acid.

Si(s) + 6HF(aq) [SiF6]2-(aq) + 2H+

(aq) + 2H2(g)

• Reactions with basesSilicon is attacked by bases such as aqueous sodium hydroxide to give silicates.

Si(s) + 4NaOH(aq) [SiO4]4-(aq) + 4Na+

(aq) + 2H2(g)

Reactions of Silicon

Used in glass as silicon dioxide (SiO2). It is used as a semiconductor to make microchips for electronics Silicon is also used in solar cells, tools, cement, LCDs, grease and oils.

Fine powder is highly flammable. A serious lung disease known as silicosis often occurred in miners, stonecutters, and others who were engaged in work where siliceous dust was inhaled in great quantities.

Uses of Silicon

Hazards of Silicon

Ge(Germanium)

METALLOID

Chemical Properties of Germanium

Atomic Number32

Atomic Mass72.64 g/mol

Atomic Radii125 pm

Abundance1.8 ppm

Electronegativity2.01

Electron Configuration

[Ar] 3d10 4s2 4p2

Crystal StructureCubic close

packed

Physical Properties of Germanium

Color Greyish white

State solid at 298 K

Density 5.323g/cm3

Melting Point 1211.4K (938.3°C)

Boiling Point 3093K (2820°C)

Enthalpy of Fusion 34.7 kJ mol-1

Enthalpy of Vaporisation 327.6 kJ mol-1

Heat Capacity 23.222 J mol-1 K-1

Uses

Germanium is an important semiconductor material. It is commonly doped with arsenic or gallium at the level of one part per 1010 for electronics. Germanium is also used as an alloying agent, a catalyst, and as a phosphor for fluorescent lamps. The element and its oxide are used in highly sensitive infrared detectors and other optical devices. The high index of refraction and dispersion of germanium oxide has led to its use in glasses for use in microscope and camera lenses. Organic germanium compounds have a relatively low toxicity to mammals, but are lethal to certain bacteria, giving these compounds potential medical importance.

Reactions of Germanium

Reactions with water

• The thin oxide layer renders germanium more or less inert to water.

Reactions with air

•The surface of lumps of germanium is protected by a very thin layer of germanium dioxide. At red heat, germanium reacts with oxygen in air to from germanium dioxide.•Ge(s) + O2(g) GeO2(s)

Natural Abundance

Germanium has been detected in the atmosphere

of. Its abundance in the Earth's crust is

approximately 1.6 ppm

There are only a few minerals

like argyrodite, briartite, germanite,

and renierite that contain appreciable

amounts of germanium

Sn (Timah)

METAL

Physical & Chemical Properties of TinPhysical Properties of Tin

• Color : silvery lustrous grey• State : solid at 298 K• Density : (white) 7.265g/cm &

(grey) 5.768g/cm• Melting Point :

505.08K (231.93°C)• Boiling Point : 2875K (2602°C)• Enthalpy of Fusion : 7.2 kJ mol-1

• Enthalpy of Vaporisation : 296.2 kJ mol-1

• Heat Capacity : 27.112 J mol-1 K-1

Chemical Properties of Tin

Atomic Number : 50Atomic Mass : 118.710 g/mol Atomic Radii : 145 pmAbundance : 2.2 ppmElectronegativity : 1.96Electron Configuration :[Kr] 4d10 5s2 5p2 Crystal Structure :Tetragonal

USES OF TIN

Used as a coating for steel cans. Also in solder (33%Sn:67%Pb), bronze (20%Sn:80%Cu), and pewter. Stannous fluoride (SnF5), a

compound of tin and fluorine is used in some toothpaste. It is also used in the manufacture of super conducting magnets. While tin

has many uses in alloys, it has few uses in it's pure elemental form. Tin foil was once a common wrapping material for foods and drugs; now replaced by the use of aluminium foil, which is

commonly referred to as tin foil. In 2006, the categories of tin use were solder (52%), tinplate (16%), chemicals (13%), brass and

bronze (5.5%), glass (2%), and variety of other applications (11%).

REACTIONS OF TIN

It is stable to water under ambient conditions but on heating with steam, tin reacts with water to from tin dioxide and hydrogen. Sn(s) + 2H2O(g) SnO2(s) + 2H2(g)

Reactions with

water

It is stable in air under ambient conditions but on heating in air or oxygen, tin reacts with oxygen to from tin dioxide.Sn(s) + O2(g) SnO2(g)

Reactions with air

Pb (lead)

Pb (which also called “lead”) is a metal element which have atomic number 82. in latin, it’s called plumbum, and in Indonesian usually

called “Timbal” or “Timah hitam”

Lead can be extracted from the earth primarily in form of “galena” (PbS, which is

86,6% lead)

METAL

Physical characteristic:

Phase soiid

Density (standard room temperature)

11.34 g/cm³

Liquid density 10.66 g/cm³

Melting point 600.61 K(327.46 °C, 621.43 °F)

Boiling point 2022 K(1749 °C, 3180 °F)

Melting heat 4.77 kJ/mol

Boiling heat 179.5 kJ/mol

Heat capacity (25 °C) 26.650 J/(mol·K)

Electronegativity 2.33 (Skala Pauling)

Ionization energy

First : 715.6 KJ/molSecond : 1450.5 kJ/molThird : 3081.5 kJ/mol

Abundance 14 ppm

Atomic radius 180 ppm

Crystal Structure Cubic Close Packed

Chemical characteristic

Reactions of Lead

in Reactions with water The surface of lead is covered by a thin layer of oxide that means it will not react under normal conditions

In Reactions with air

Only upon heating lead to 600-800°C does lead react with oxygen in air to from lead oxide.

2Pb(s) + O2(g)2PbO(s)

Functions of Lead

• Used in solder, as a colouring agent in ceramic glazes (red and yellow), shielding against radiation, roofing, in (lead-acid) batteries and ammunition.

UUQ (Ununquadium)

This item is purely synthetic and is not available commercially.

METAL

Physical characteristic:

Phase presumably a solid at 298 K

Density (standard room temperature)

Unknown

Liquid density Unknown

Melting point Unknown

Boiling point Unknown

Melting heat Unknown

Boiling heat Unknown

Heat capacity Unknown

Chemical characteristic

Electronegativity No data

Ionization energy(detil)

No data

Electron configuration

[Rn] 5f14 6d10 7s2 7p2 (guess based

on lead)

Reactions of Uuq

As only so little ununquadium has ever been made it's reactivity is unknown. It is expected that its behaviour would be similar to that of

lead, immediately above it in the periodic table, and tin (two places above it).

Functions of Uuq

Ununquadium is a synthetic and highly unstable element. No useful or commercial

ununquadium compounds exist yet.