element and coumponds ppt

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Br ( Bromine )



Characteristic

Physical Chemical

Elemental bromine exists asa diatomic molecule, Br2. It is a dense,

mobile, slightly transparent reddish-brown liquid, that evaporates easilyat standard temperature andpressures to give an orange vapor (itscolor resembles nitrogen dioxide) thathas a strongly disagreeable odorresembling that of chlorine. It is one ofonly two elements on the periodictable that are liquids at roomtemperature (mercury is the other,although caesium , gallium ,

and rubidium melt just above roomtemperature).

Being less reactive than chlorine butmore reactive than iodine, bromine

reacts vigorously with metals,especially in the presence of water, togive bromide salts. It is also reactivetoward most organic compounds,especially upon illumination,conditions that favor the dissociationof the diatomic molecule into bromineradicals:Br2 2 Br·It bonds easily with manyelements and has astrong bleaching action.

Bromine is slightly soluble in water,but it is highly soluble in organicsolvents such as carbondisulfide, carbontetrachloride, aliphatic alcohols,and acetic acid.



Identification

+ AgNO3 (aq) beige precipitate formed

+ Ammonia solution insoluble precipitate, dissolve if excess ammonia

+ HNO3 insoluble

in a solution of PbCH3COO2 white precipitate soluble in hot water



FunctionBromine is used for disinfecting, flame retardant ,water purification compounds, dyes , medicines ,sanitary cleaners, inorganic bromides for photography (silverbromide (AgBr) ) and others. Organic bromides arealso important.

Another utility include: Sodium bromide (NaBr) asa nerve sedative, Methylbromide (CH3Br)substances firefighters, and Ethylene dibromida (C2H4Br2) was added to gasoline to turn into PbBr2 Pb.



Storage



Compound of Bromine



Aluminium bromide AlBr3

Aluminium bromide is any chemical compound with theempirical formula AlBrx. The species called "aluminiumtribromide," is the most common aluminium bromide. Thespecies aluminium monobromide forms from the reactionof HBr with Al metal at high temperature. Itdisproportionates near room temperature:6/n "[AlBr]n" → Al2Br6 + 4 Al This reaction is reversed at temperatures > 1000 °C.

The anhydrous form is used as a catalyst for the Friedel-

Crafts alkylation reaction. Its catalytic activity is similar toanhydrous aluminum chloride. However, commercialapplications are rare.



Hydrogen Bromide HBrHydrogen bromide is the diatomic molecule HBr. HBr isa gas at standard conditions. Hydrobromic acid formsupon dissolving HBr in water. Conversely, HBr can beliberated from hydrobromic acid solutions with the additionof a dehydration agent, but not by distillation. Hydrogenbromide and hydrobromic acid are, therefore, not thesame, but they are related. Commonly, chemists refer tohydrobromic acid as "HBr", and this usage, whileunderstood by most chemists, is imprecise and can beconfusing to the non-specialist.



Mercury ( Hg )



Characteristic

Physical Chemical

Mercury is a heavy, silvery-whitemetal. As compared to other metals, it

is a poor conductor of heat, but a fairconductor of electricity.

Mercury has an exceptionally lowmelting temperature for a d-block

metal. mercury has a uniqueelectronic configuration whereelectrons fill up all the available 1s,2s, 2p, 3s, 3p, 3d, 4s, 4p, 4d, 4f, 5s,5p, 5d and 6s subshells. As suchconfiguration strongly resists removalof an electron, mercury behavessimilarly tonoble gas elements, whichform weak bonds and thus easilymelting solids. The stability of the 6sshell is due to the presence of a filled

4f shell. An f shell poorly screens thenuclear charge that increases theattractiveCoulomb interaction of the6s shell and the nucleus(see lanthanide contraction).



Physical Chemical

The absence of a filledinner fshell is the reason forthe much higher meltingtemperature of cadmium.Metals such as gold have

atoms with one less 6selectron than mercury.Those electrons are moreeasily removed and areshared between the goldatoms forming relatively

strong metallic bonds.[2][5] At its melting point (−38.86

°C), the density of mercuryis[6] 13.534 g/cm3.



Identification



FunctionUsed in thermometers, barometers, diffusion pumps,coulometers, fluorescent lamps, mercury switches,insectisides, and batteries. Gaseous mercury is used inmercury-vapour lamps. It is found in paint, batteries,thermometers, electrical equipment, fluorescent lights andplastics. Batteries account for 88% of the mercury contentin municipal solid waste.Mercury was once used in the amalgamation process ofrefining gold and silver ores.



Storage



Compound of Mercury



Mercury(II) sulfate, commonly called mercuric sulfate is the chemicalcompound HgSO4. It is an odorless solid that forms white granules orcrystalline powder. In water, it separates into an insoluble sulfate with a yellowcolor and sulfuric acid.

An acidic solution of mercury sulfate is known as Denigés' reagent. It wascommonly used throughout the 20th century as a qualitative analysis reagent. IfDenigés' reagent is added to a solution containing compounds that havetertiary alcohols, a yellow or red precipitate will form



Mercury(II) chloride or mercuricchloride (formerly corrosive sublimate ), is the chemicalcompound with the formula HgCl2. This whitecrystalline solid is a laboratory reagent and a molecularcompound. It is no longer used for medicinal purposes

(e.g. treatment of syphilis) because it is highly toxic andsuperior treatments have become available.Mercury(II) chloride was used as a photographicintensifier to produce positive pictures in the collodionprocess of the 1800s. When applied to a negative, themercury(II) chloride whitens and thickens the image,thereby increasing the opacity of the shadows andcreating the illusion of a positive image



B ( Boron )



Characteristic

Physical Chemical

Boron is a chemical element in theperiodic table that has the

symbol W and atomicnumber 5. Elementsof trivalent metalloids, boron borax numerous in stone. There aretwoallotropesof boron; amorphous boron is

a brown powder, but metallic boron isblack.Loud metallic form (9.3 inthe Moh scale) and abad conductor in room temperatures.Never found free in nature.

Elemental boron is rare and poorlystudied because the material is

extremely difficult to prepare. Moststudies on "boron" involve samplesthat contain small amounts of carbon.Chemically, boron behaves moreclosely to silicon than to aluminium.Crystalline boron is chemically inert

and resistant to attack by boilinghydrofluoric or hydrochloric acid.When finely divided, it is attackedslowly by hot concentrated hydrogenperoxide, hot concentrated nitric acid,hot sulfuric acid or hot mixture ofsulfuric and chromic acids.[16][32]The rate of oxidation of borondepends upon the crystallinity, particlesize, purity and temperature. Borondoes not react with air at room

temperature, but at highertemperatures it burns to form boron



Identification



FunctionApproximately 35% of the productionof boron used dipabrik manufacture highly resistantborosilicate at high temperature heating, 20% of the productionof boron as sodiumcompounds are used asingredients peroksoborat NaBO3 washing detergents are

veryeffective at temperatures of 90 degree Celcius . Asa vital component in nuclear power plants because ofitsability to absorb neutrons as, fire wood filler, and asa flux in soldering process



Storage



Compound of Bromine



Boric Acid

1. ortoborat acid ( H3BO3 )2. metaborat acid ( HBO2 )3. tetraborat acid ( H2B4O7 )

form of white crystals, solublein cold water and hot water. can be obtained fromthehydrolysis of boron halides, can be obtained from theoxidation of boron withhydrogenperoxide. in acidic water solution of aweak mono and not acting as a proton donor but as

a lewis acidboric acid has a layered structure of acircular field with the connecting hydrogenbonds.molten boric acid dissolves metaloxides produce borate glasses. pyrex borosilicateglass containing compounds



Tetraflouroborat Acid HBF4

is a strong acid and therefore can not be obtained asHBF4. Is common in the trade as an acid solution ofTetraflouroborat with a content of about 40%



Al ( Aluminium )



Characteristic

Physical Chemical

- Density lightweight (only2.7 g / cm ³, while

the iron ± 8.1 g / cm ³)- Good corrosion resistance- Electricity and heat dissipation isgood- Easy fabrication / in form- Its strength is low but the

integration (alloying) strength can beimproved

Pure aluminum , silvery white metalhaving the desired characteristics

of the metal. Heislight, not magnetic and noteasily splashed, a second metal easiest in terms of formation,and sixth interms of ductility.



Identification







Storage



Compound of Alumunium



Alumunium oxide Al2O3

Aluminum oxide is a chemical compound of aluminum andoxygen , with the chemicalformula Al2O3. Mineralname is alumina,and in the mining, ceramic and materials

engineering more of these compounds are called by thename of alumina.



Tetraflouroborat Acid HBF4

· At room temperature, solid aluminum chloride havingan ionic lattice with a lot of covalent character.· At temperatures around 180-190 ° C (depending on the

pressure), aluminum chloride is transformed into theform of the molecule, Al2Cl6. This causes it to melt orevaporate because of the attractivenessintermolekulernya weakened.· With a slight increase in temperature will break intosimpler molecules of AlCl3.

Solid aluminum chloride does not conduct electricity atroom temperature because the ions are not movingfreely. Fusion of aluminum chloride (only possible byraising the pressure) does not conduct electricitybecause of the absence of ions.



Cl ( Chlor )



Characteristic

Physical Chemical

At standard temperature andpressure, two chlorine atoms form

the diatomic molecule Cl2. This is ayellow-green gas that has itsdistinctive strong smell, the smell ofbleach. The bonding between the twoatoms is relatively weak (only 242.580±0.004 kJ/mol), which makes the

Cl2 molecule highly reactive. Theboiling point at regular atmosphere isaround −34 ˚C, but it can be liquefied

at room temperature with pressuresabove 8 atmospheres.

Along with fluorine, bromine, iodine,and astatine, chlorine is a member of

the halogen series that forms thegroup 17 (formerly VII, VIIA, or VIIB)of the periodic table. Chlorine formscompounds with almost all of theelements to give compounds that areusually called chlorides. Chlorine gas

reacts with most organic compounds,and will even sluggishly support thecombustion of hydrocarbons.



Identification







Storage



Compound of Chlor



Magnesium Chloride MgCl2

Magnesium chloride is also an ionic compound, but withthe arrangement of the ions is more complicated becausethe amount of chloride ions are two times more than

magnesium ions.

Same with sodium chloride, the heat necessary toovercome the attraction between the ions is also large, sothe melting point and boiling point is also high.

Solid magnesium chloride is not a conductor of electricitybecause the ions are not moving freely. However,electrolysis can be experienced when the ions becomefree due to melting.

Magnesium chloride is soluble in water produces a weak

acid solution (pH = approximately 6).

If magnesium ions from the lattice is broken down andtransformed into the solid solution, there is sufficientattraction between the ions 2 + and water molecules toform coordination bonds (dative covalent) betweenmagnesium ions and the lone pair of electrons around the



Sodium Chloride NaCl

In addition to the familiar uses of salt in cooking, salt isalso used in many applications, from manufacturing pulpand paper, to setting dyes in textiles and fabric, to

producing soaps, detergents, and other bath products. Itis the major source of industrial chlorine and sodiumhydroxide, and used in almost every industry.



N ( Nitrogen )

Ch t i ti



Characteristic

Physical

Phase gas

Density (0 °C, 101.325 kPa)

1.251 g/LLiquid density atb.p. 0.808 g·cm

−3

Melting point 63.15 K, -210.00 °C, -346.00 °F

Boiling point 77.36 K, -195.79 °C, -320.33 °F

Triple point 63.1526 K (-210°C), 12.53 kPa

Critical point 126.19 K, 3.3978 MPa

Heat of fusion (N2) 0.72 kJ·mol−1

Heat of vaporization (N2) 5.56 kJ·mol−1

Molar heat capacity (N2)

29.124 J·mol−1

·K−1



CharacteristicChemical

Gas in the form of colorless, tasteless, and odorlessSoluble in water, and classified as an element that isdifficult to react because its binding energy isvery large. Nitrogen reacts only at relatively hightemperatures with the aid of a catalyst



Identification







Storage



Compound of Nitrogen

A i NH



Ammonium NH3

is a distinctive smelling gas, and colorless, and poisonous.and easily melt if given thepressureusefulness :

primary use as a raw material for making ZAraw materials other compounds suchas nitric acid, ammonium chloride, and ammonium nitratein the ice plant is used as a coolant, becausethe liquid ammonia evaporates andabsorbs lots of heatas a rocket fuel that can burn ownself when

mixed produce an oxidant nitrogen gas and heat



Nitric acid HNO3

The chemical compound nitric acid (HNO3) is akind of colorless corrosive liquid, and isa toxic acid which can cause burns. Solution

of nitric acid with nitric acid content of more than86% nitric acid known as smokeless, and can bedivided into two types ofacid,white fuming nitric acid and red fuming nitric acid.Nitric acid is usually used in laboratories asa reagent. This solution was also used to

manufacture explosive materials suchas nitroglycerin, trinitrotoluene (TNT) andSiklotrimetilenatrinitramin (RDX), and also for the manufactureof ammonium nitrate.Nitric acid is also used in the metallurgy and refining asit can react with themetal. Whenmixed with hydrochloric acid, the mixture will form aqua regia, one of thefew reagentsthat dissolves gold and platinum.Nitric acid is also a component of acid rain.

element and coumponds ppt

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