what is the atomic number

7/30/2019 What is the Atomic Number

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What is theAtomicNumber?

The numberofprotonsin thenucleusis called the atomicnumber.

Forsodium(Na) the atomicnumberis11.The atomicnumbertells you what theelementis(see theperiodic table).The atomicnumberof an element neverchanges.

What is the Mass Number?

The numberofprotons plus the numberofneutronsis called the massnumber.Sodium has 11 protons and 12 neutrons.The massnumberis 11 +12 = 23.The massnumberis the total numberofparticlesin the nucleus. The massnumberand the atomic numberare written above and below

thechemical symbolfor the element, as shown.

What is an Isotope?

Atomsof the same element may have differentnumbers

ofneutrons. These are called isotopes.For example, Chlorine (atomicnumber17)may have 18 or20 neutrons.The massnumberwill beeither17 + 18 = 35, or17+ 20 = 37.
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Isotopes of the same element have thesamechemical propertiesbecause the numberofprotons andelectronsare the same.

What are Electron Shells (energy levels)?

Electrons inatomsare in shells(shown ascirclesaround the nucleus).The shells can also be called energy levels.We will use the term shell rather than energy levelbut either is acceptable.

The maximumnumberofelectrons in eachshell,going from the middle to the outside, is 2, 8, 8, 18.Below is a picture of a potassium atom.Itselectron structureis2, 8, 8, 1.

An atom that has the maximumnumberofelectronsin its outer shell will be stable. This means thatit will notreact with otheratoms.It belongs to a group called thenoble gases.
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The electron shells are said to be full.The innershells of an atom are always full.

If the outer shell of an atom has less than

its maximumnumberofelectrons(see potassium above) then it will not be stable.It willreactwith otheratoms to get a full outer shell.

Ionsalso have a full outer shellofelectronsbut because they have a chargethey will react and formionic bonds

with otheroppositely chargedions

What is the Difference between anAtom and an Ion?

Anatomhas the same numberofprotonsandelectrons.An atom has nooverall electric charge.

If an atomloses orgainselectrons it is no longer called anatom.

It is called an ion. An ion has afullouter shellofelectrons.An ion has an electric charge.

Why do Chemical Reactions Happen?

Allchemical reactionshappen becauseatomsare trying to get afullouter shellofelectrons.

Thetotal numberofatoms isthe samebefore and afterthe reaction.

When an atomreacts with anotheratom to form achemical bond
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it will either1.Lose electronsto form a stablepositive ion.2.Gainelectronsto form a stable negativeion.

Or 3.Share electronsto form a stable moleculeWhat happens when a SodiumAtom becomes a SodiumIon?

Asodium atomhas 1 electronin itsouter shell.It is ingroup 1of the periodic table.

When sodiumreacts with non-metals (for example

chlorine) it willlose itsouter electron. Its outer shell will then have noelectrons.It is as though the outer shell has vanished. The next shellin is full.This fullinner shell becomes the newfullouter shell.

The sodiumatom loses its outer electron to become asodium ion.The sodium ion still has11 protons(11 positive charges)but now only 10 electrons (10 negative charges).The sodium ion has an extra positive charge, shown by
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the + sign.Allgroup 1metalswill form a 1+ ionwhen theyreact with non-metals.

The charge on the ion can also be shown as

and theelectron structurewritten as [2, 8]+

The charge on the sodium ion will make it react and formionic bonds with otheroppositely chargedions.Thefull outer shellofelectrons does not make the sodiumionunreactive (see anexample).

The Reaction between Sodium and Chlorine.

Chlorine has 7 electrons in itsouter shell.It is ingroup 7of the periodic table.

When an atom ofchlorine reactsit willgainone electron fromsodium.

The outer shell ofchlorine will thenhave 8 electrons and befull.The chlorideionwill have an extraelectron andtherefore an extranegative charge (shown as a - sign).
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Theelectrostaticforce ofattraction between theoppositely charged ions is called an ionicbond.

The electrons are shown as dots and crossesto show how they have moved during the reaction.In reality allelectrons are identical.

Thebalancedchemical equation for the above reaction is

Sodium + chlorine sodiumchloride.2Na(s) + Cl2 (g) 2NaCl(s)

Sodiumchloride is a crystalline ioniccompound.It forms agiantstructure.

Valency, OxidationState and IonicCompounds.

When a metal reacts with a non-metal,the metal will loseelectronsto form apositive ion
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and the non-metal will gainelectrons to form anegativeion.

Thecompoundwhich is formed will be ionic.

It will form agiantstructure(also called a giant ioniclattice).If you do not know whether an element is a metal ora non-metal seethe periodic table

The valency (combining power) of a metal is the sameas its oxidationstate (the charge on the ion).

The numberofelectrons that a metal will loseis the same as itsgroup numberin the periodic table.

A metal in group 1 will form a 1+ion

(Valency1,oxidationstate1+).

A metal in group 2 will form a 2+ion

(Valency2, oxidation state2+).

The numberofelectrons that a non-metal will gainwill be 8 minus its group number.A non-metal in group 6 will form a 2

-ion

(Valency 2, oxidationstate 2-).

A non-metal in group 7 will form a 1-ion

(Valency 1, oxidationstate 1-).

A non-metalion is negative because it has gainedelectrons

Magnesium is ingroup 2of theperiodic table.A magnesiumatomwilllose 2 electronsto form astable2

+

ion.
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Oxygen is in group 6of the periodic table.An oxygenatom will gain2 electrons to form a stable 2

-

ion.

In this example theelectronsare shown asdots andcrosses.You will often see electrons drawn like this in books.

Theionic bondbetween magnesium and oxygen isstrongerthan the ionicbond betweensodium and chlorinebecause of the greatercharge on the ions.Magnesiumoxide has ahighermelting pointbecause of the strongerbond.

magnesium + oxygen magnesiumoxide.2Mg(s) + O2(g) 2MgO(s)
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9/31

Lithiumis ingroup 1of theperiodic table.A lithiumatomwilllose 1 electronto form astable1

+ion.

Oxygen is in group 6of the periodic table.

An oxygenatom will gain2 electrons to form a stable 2-ion.

In this example theelectronsare shown asdots andcrosses.

Two lithiumatoms will each give one electron to theoxygen atom.

The atoms becomeions.

Theelectrostaticattraction between the oppositelycharged ionsforms the ionicbond between lithium and oxygen.

Theformulaforlithiumoxide is Li2O.

lithium+ oxygen lithiumoxide.4Li(s) + O2(g) 2Li2O(s)
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10/31

Magnesium is ingroup 2of theperiodic table.A magnesiumatomwilllose 2 electronsto form astable2

+ion.

Chlorine is in group 7 of the periodic table.A chlorineatom will gain1 electron to form a stable 1

-ion.

In this example theelectronsare shown asdotsandcrosses.

Two chlorineatoms will each gainone electron fromthe magnesium atom. The atoms becomeions.

The attraction between theoppositely charged ionsforms the ionicbond between magnesium and chlorine.Theformulaformagnesiumchloride is MgCl2.

magnesium +chlorine magnesiumchloride.Mg(s) + Cl2(g) MgCl2(s)

The Electron Structure ofIons andNoble Gases are theSame.
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11/31

The noble gases are in group 0 of theperiodic table.They will notreact with otheratomsbecause they haveafullouter shellofelectronsandno overall charge.

Atomswhich have lost orgainedelectrons to formionswillalsohave a fullouter shell ofelectrons but because they havea chargethey will formionicbondswith otheroppositelychargedions.

Ions and noble gases both have afullouter shellofelectronsand therefore can have thesameelectron structure.

A Li+ionhas thesameelectron structure as Helium.

A Mg2+

ionhas the same electron structureas a Na

+ionand a O

2-ion.

It is the electron structure ofNeon (see previous pages).

A Cl-ionhas the same electron structure asArgon.

The electron structure ofHelium is 2.Neon is 2, 8.

Argon is 2, 8, 8.

INamesofIonicCompounds.

The names ofmetalelements do not changewhen they becomeions.
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12/31

If you do not know whether anelement isa metal or a non-metal seethe periodic table

ons are said to have a noble gaselectron structure

Metalsform positively charged ions called cations.Examples areLi

+, Na

+, K

+, Mg

2+, Ca

2+,Al

3+.

The above ions are calledlithium, sodium, potassium,magnesium, calcium and aluminium.

The names ofnon-metal elementsdo change when they become ions.Non-metalsformnegatively chargedions called anions.Examples areF

-, Cl

-, Br

-, I

-, O

2-, S

2-.

If there is only 1non-metal in the ioniccompoundthename ends in ide.

The above ions are calledfluoride, chloride, bromide,iodide, oxide and sulfide.

So, lithium + chlorine lithiumchloride.2Li(s) + Cl2(g) 2LiCl(s)

potassium + bromine potassiumbromide.2K(s) + Br2(l) 2KBr(s)

If there are 2non-metals and the second one is oxygenthename ends in ate.

Why is the formula ofsodiumoxideNa2OandnotNaO orNaO2?
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13/31

Theionicsolid must have the same numberofplus and minuscharges.IfNa

+forms a compound with O

2-,

then the formula will be Na2O.Two sodium ions (each 1+) will be needed

to balance the charge on oneoxygenion (2-).

Sodium hasvalency1, oxygen hasvalency 2.

Examples offormulaeof otherioniccompoundsfrom the elements on theprevious pageare

LiF, LiCl, LiBr, LiI, 1

+

with 1

-

NaF,NaCl,NaBr,NaI, givesKF,KCl,KBr,KI, 1 to 1.

Li2O,Na2O,K2O, 1+with 2

-

Li2S,Na2S,K2S, gives 2 to 1.

MgF2,MgCl2,MgBr2,MgI2, 2+with 1

-

CaF2,

CaCl2,

CaBr2,

CaI2, gives 1 to 2.

MgO,CaO,MgS, CaS, 2+with 2

-gives 1 to 1.

AlF3,AlCl3,AlBr3,AlI3,3+

with 1-gives 1 to 3.

Al2O3,Al2S3, 3+

with 2-gives 2 to 3

Below is a small piece of a giantionicstructure.

It is also called a giant ionic lattice.The word "giant" means that ahugenumberofparticlesare present (compare this with the wordsimple).

A giant ionicstructureis made from a hugenumberofions.
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14/31

The red balls are positiveions and the blue balls arenegativeions. Theelectrostaticattraction between theoppositely chargedions is called an ionicbond

(compare this with acovalent bond).

The structureextends (repeats itself) in alldirectionsgiving a crystal with a regular arrangement ofions calleda lattice. The crystal is said to be highlyordered.

Forsodiumchloridethe red balls may representNa+ions

and the blue balls may representCl-ions.

All ionic solids have a similar structureto thatshown above but they maynot beidentical.Differences ofpacking and the relative size and amountsofions will give differentcrystalvariations.

When metalsreact withnon-metalsthey form anioniccompound.

Ionshave a charge becauseelectronsare lost orgained informing anionicbond.

An ioniccompound has strongforces ofattractionbetween the ions in alldirections and forms agiantstructure.
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15/31

Ionicbonds are strong.Allioniccompounds are solid at roomtemperature.Solid ioniccompounds do notconductelectricity

because the ions are notfree tomove.

If the solid is heated until itmelts, the liquid willconductelectricity because the ions are mobile(they can move). When electricity flows throughan ioniccompound the ions become separated andturned intoelements. This happens duringelectrolysis.

If the ionic solid is dissolved in asolvent(for example water), the particles of the solventovercometheforceofattractionbetween the ionsand separate the ionsfrom each other to form asolution.The solution will conductelectricitybecause the ions are now free to move.The liquid which conductselectricityis called theelectrolyte.

What is Covalent Bonding?

When non-metals react with non-metals theyshareelectronsand form acovalent bond.Covalent means sharing.If you do not know whether anelementisa metal or a non-metal, seethe periodic table.

A covalent bond forms because of theelectrostaticattractionbetween thenucleiof theatoms(that are positive)and the shared electrons (that are negative).
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There are noionspresent (no + or- charges) because theelectrons are shared, not transferredfrom one atomtoanother.

One pairofshared electrons form asinglecovalent bond.Two pairs ofshared electrons form adoublecovalentbond.Three pairs ofshared electrons form atriplecovalentbond.

Only covalent compounds are called molecules.

If the compound isionicit is not called a molecule.

Covalentcompoundscontaining a small numberofatomsare called simplemolecules.Simplemeansthat only a small numberofatomsare present.If a hugenumberofatoms arepresent it would be called agiantmolecule.

Why does a Chlorine Molecule have a Covalent Bond?

Chlorine is anon-metal.A chlorineatomhas 7electronsin itsouter shell.Chlorine is ingroup 7of theperiodic table.Two chlorine atoms will eachshare one electronto get afullouter shelland form astableCl2molecule

This is a picture of the shared electrons making a covalentbondin a chlorine molecule. Chlorine is asimple molecule.
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By sharing the two electrons where the shells toucheach chlorineatom can count 8 electrons in itsouter shell.These fullouter shells with theirshared electronsare now stable and the Cl2molecule will notreact furtherwith otherchlorine atoms.

One pairofshared electrons form asinglecovalent bond.

There are noionspresent (no + or- charges) inchlorinegasbecause the electrons are shared,not transferredfrom one atom toanother.Chlorine does formhydrogen ionswhen it isdissolvedin waterto becomechloric acid.

What is a Hydrogen Molecule?

Hydrogen is anon-metal.Hydrogen has only oneelectron.Two hydrogenatomswill eachshare theirone electron toform acovalent bondand make a hydrogenmolecule(H2).
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This is a picture of a hydrogen molecule.

By sharing the two electrons where the shells toucheach hydrogenatom can count 2 electrons in itsoutershell.These fullouter shells with theirshared electrons are nowstable.The H2molecule will notreact further with otherhydrogenatoms.

The pairofshared electrons between the two hydrogenatoms

form asinglecovalent bond.

The structural formula of a hydrogen molecule is written

There are noionspresent (no + or- charges) inhydrogengasbecause the electrons are shared,not transferredfrom one atom toanother.

What is an Oxygen Molecule?
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19/31

Oxygen is anon-metal.An oxygenatomhas 6electronsin itsouter shell.Oxygen is ingroup 6of theperiodic table.

Two oxygenatomswill eachsharetwo electrons to formtwocovalent bondsand make an oxygenmolecule(O2).

This is a picture of an oxygen molecule.

By sharing the four electrons where the shells toucheach oxygenatom can count 8 electrons in itsouter shell.These fullouter shells with theirshared electrons

are now stable, and the O2molecule willnot (normally)react further with otheroxygen atoms.

Note the 2 pairs (4 electrons)shared between the atoms.Each electron pairisone bond.Oxygen has two bondsbetween its atoms.This is called adoublebond.

The structural formula of an oxygen molecule is written

There are noionspresent (no + or- charges) inoxygengas
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because the electrons are shared,not transferredfrom one atom toanother.

What is a Carbon Dioxide Molecule?

Oxygen and carbon are bothnon-metals.An oxygenatomhas 6electronsin itsouter shell.Oxygen is ingroup 6of theperiodic table.

A carbon atom has 4electrons in itsouter shell.Carbon is in group 4 of the periodic table.

Two oxygenatomsand 1 carbon atom will each

sharetwo electrons to formfourcovalent bondsand make a carbon dioxidemolecule(CO2).

This is a picture of a carbon dioxide molecule.

By sharing the four electrons where the shells touch eachoxygen and carbonatom can count 8 electrons in its outershell.These fullouter shells with theirshared electronsare now stable, and the CO2molecule willnot react further with otheroxygenorcarbon atoms.
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Each electron pairisone bond.Carbon and oxygen have two bonds each between theiratoms.

This is called adoublebond.

The structural formula of a carbon dioxide molecule iswritten

There are noionspresent (no + or- charges)incarbon dioxide gasbecause the electrons are shared,

not transferredfrom one atom toanother.Carbon dioxide does formhydrogen ionswhen it isdissolvedin water(or rain water)to become aweakacidcalledcarbonic acid

What are the Properties ofSimpleMolecules?(compare these withgiantmoleculesand

ioniccompounds).

When non-metalsreact with non-metalsacovalently bonded moleculeis formed.

Covalent bonds are strong but only existbetween theatomsof the molecule.The force ofattraction between molecules

(called the intermolecular force)is veryweak (compare this withionic bonding).The picture below shows the forces ofattractionbetween two molecules ofoxygengas.
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The weak force between molecules means that very littleenergyis needed to separatethem. Many molecular compoundsareliquid orgas at roomtemperature.

They have low melting andboilingpoints.

Note that when a molecular compoundmelts orboils,moleculesseparate from each otherbut the covalent bond between theatoms of the moleculedoes not break. The molecule is the same moleculein the solid, liquid orgas state.

If the covalent bondbreaks,the moleculeis said to decompose (split up!).

Moleculesdo not have a charge (noions) because theelectronsareshared between atoms to form acovalentbond.Molecular substances will thereforenotconductelectricityWhat is a GiantMolecule? - What is Carbon?

Acovalently bondedsubstance containing a hugenumberofatoms is called a giantmoleculeor agiantcovalentlattice.
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There are four examples ofmolecules (made fromnon-metals)which form giantstructures. They aresilicon, silicon

dioxideandtwo forms of theelementcarboncalleddiamondandgraphite(polymersare adifferentkind oflargemolecule).

When two (ormore)forms of an elementexist in the same physical state, they are called allotropes.Diamond and graphite are allotropes ofcarbon.

Carbon can exist asfullerenesas well as diamond andgraphite.

Carbon and siliconare both ingroup 4of theperiodic table.They both need to form 4 bonds withthemselves orotherelements. They havevalency4.Valency is the combining powerof an atom.

(with the exception ofgraphitewhich is a giantmolecule).

What is the Structure ofDiamondand Silicon?

Diamond is aformof theelementcarbon- see alsographite.
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In the picture ofdiamond above, eachblueballrepresents a carbonatom. The structure has billionsofatoms forming hexagons andextendsinalldirections.

Allof thecovalent bondsin diamond areidentical.It forms agiantmolecular structure.

A crystal ofdiamond is onegiantmolecule!

The covalent bonds are very strong.Diamond is thehardestnaturally occurring material. It does notconductelectricity.

Silicon (used in microchips forcomputers) has thesame structure, with eachblueballbeing a siliconatom.

Silicon dioxide (SiO2) issand (also called silica).SiO2has a similar structure and also forms a giantmolecule.

What is theStructure ofGraphite?
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Whenever you come across carbon, as areactantorelectrode,carbon means graphite notdiamond.

It can be written C(gr) but is usually written as just C.

Graphite consists of many flat layers ofhexagons(like a wire fence).The layers are called graphene sheets.Each carbon atom is joined tothree othercarbonatoms.Each layeris itself agiantmoleculewith very strongcovalent bonds.

Carbon is ingroup 4of theperiodic tableand so it has fourelectronsin itsouter shell.Three electrons are used forbonding in the graphenesheet.The fourth electron between thelayers isdelocalised(it is afree electron).

Between the layers thebonds are weak. Free electronsbetweenthe layers allows graphite toconduct electricityandheat.
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The layers can easily slide over each other makinggraphite softand slippery and anexcellent lubricant (like oil).

See alsocarbon fibresandfullerenes.

What are the Properties ofGiantMolecules?

Giant moleculesincludediamond,graphite,siliconandsilicon dioxide.

Giant Molecules have highmelting and boiling points

due to strongcovalent bonds.

They arevery hard(due to strongcovalent bonds).

They do notdissolve in water.

They do not conduct electricityas a solid (exceptgraphite)or as a liquid because there are no ions

What are the Properties ofCarbon Fibres?

CarbonFibresare very thin (see nano particles).They are less than one hundredth of a millimeterindiameter.They can be more than three times as strong assteelbut with less than one quarterof thedensity.

How is Carbon Fibres Made?

Carbon fibres are made by heating longpolymerchainscontaining carbon and otheratoms until there is only
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carbon left.The chains are heated where there is nooxygento prevent the carbon atomsreactingto formcarbon

dioxide.

What are the Uses ofCarbon Fibres?

Carbon fibresare used to reinforce a large numberofmaterials.The materials are mainlypolymers

called carbon fibre reinforced plastic.The carbon fibres make the polymer stronger.

Carbon fibres are used to makean increasingly largenumberofproductsincludingaircraft,cars, boats, sports equipment(fishing rods, tennis rackets, golf clubs) and bicycles.

See alsographiteandfullerenes.

What is Metallic Bonding?

Metals form a giant structure(likeioniccompoundsandgiantmolecules).
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what is the atomic number

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