THE PERIODIC TABLE

THE PERIODIC TABLE

THE PERIODIC TABLE

Not to be confused with this one

Not to be confused with this one

I. Introduction The Periodic Table isa table of the elements arranged according to repeated changes in chemical properties.

I. THE PERIODIC TABLEHistorical DevelopmentHistory records the isolation of the first element (phosphorous) in 1649. By 1869, a total of 63 elements had been isolated, but there was still no organized means to arrange them. Then along came a Russian named Mendeleev

I. THE PERIODIC TABLEHistorical Development2. Originally developed by Dimitri Mendeleev He arranged the elements in order of increasing atomic masses

B. Historical DevelopmentMendeleevs table had blank spaces. This caused Mendeleev to hypothesize that there other unknown elements. This bold hypothesis allowed Mendeleev to predict the properties and the mass numbers of these undiscovered elements.

B. Historical DevelopmentModern P.T. Made by Henry Moseley Elements are arranged by increasing atomic number and similarity of properties.

II.ORGANIZATION OF THE P. T.GROUPS OR FAMILIES The vertical columns in the periodic tableIncrease in atomic number as one goes down a family

II.ORGANIZATION OF THE P. T.GROUPS OR FAMILIES Two main groups:Group A: Representative ElementsGroup B: Transition Elements

Group AGroup BGroup A

A. GROUPS OR FAMILIES4. Elements in the same family haveSimilar propertiesThe same number of electrons in their outer (valence) energy level

II.ORGANIZATION OF THE P. T. Periods or SeriesThe horizontal rows Increase in atomic number from left to rightEach represents a new valence energy level

Lanthanide Series Rare Earth Metals B. Periods

Actinide Series All are radioactiveSome are not found in natureTransuranium Elements:B. PeriodsElements above atomic # 92. All are synthetic

Note: Together the Lanthanide Series and Actinide Series are referred to as theB. PeriodsInner Transition ElementsC. Element location on the PTUse the period and group numbers as an address to help locate an elementIII.Metals, Nonmetals, Metalloids

III.Metals, Nonmetals, Metalloids

III.Metals, Nonmetals, Metalloids

III.Metals, Nonmetals, Metalloids

III.Metals, Nonmetals, MetalloidsA. Stair Step Line Separates Metals, Nonmetals and metalloids

Left: metalsRight: nonmetalsTouching line: metalloids

Look at the stair step line on your P.T.

Look at the stair step line on your P.T.III.Metals, Nonmetals, Metalloids

Look to the Left of the Line

Look to the Left of the Line

III.Metals, Nonmetals, MetalloidsB. Metals Most elements are metals (88)Examples: Zinc, iron, copperLocated to the left of the stair step lineException ?

B. Metals Physical PropertiesLuster (shininess) Good conductors of heat and electricity High density (heavy for their size) High melting point Ductile (drawn out into thin wires) Malleable (hammered into thin sheets)

5. Chemical PropertiesEasily lose electrons B. Metals

Corrode easily.

31Corrosion is a gradual wearing away. (Example: silver tarnishing and iron rusting)

ELements to the Left of the Line Lose eLectrons

III.Metals, Nonmetals, MetalloidsC. Nonmetals Examples: P, C, S Located to the right of the stair step lineException: H is a nonmetal

C. Nonmetals3. Physical Properties dull Poor conductor of heat and electricity Brittle (breaks easily) Not ductile Not malleable Low density Low melting point

C. Nonmetals3. Chemical Properties Tend to gain electrons

Elements to the riGhtof the line Gain electrons

D. MetalloidsExamples: Si, B, AsOn the stair step lineException: Al is a metalB

SiIII.Metals, Nonmetals, MetalloidsD. Metalloids Physical PropertiesSolids Can be shiny or dull Can be ductile or notCan be malleable or brittleSemiconductors - Conduct heat and electricity better than nonmetals but not as well as metals The Periodic TableGetting back to it

IV.The FamiliesA. Alkali Metal FamilyGroup IAPropertiesLowest densities 1 valence electron Largest atomic radii Highly reactive Stored under keroseneNot found free in nature

IV.The FamiliesB. Alkaline Earth Metal FamilyGroup IIAPropertiesTwo electrons in the outer shell 2nd highest reactive metalsNot found free in nature

IV.The FamiliesC. Transition MetalsGroup B FamiliesPropertiesCan have varying numbers of valence electrons Form brightly colored compoundsIV.The FamiliesD. Boron FamilyGroup IIIA Al is the most abundant metal in the Earths crust 3. PropertiesHave 3 valence e- Contains metals & metalloids

IV.The FamiliesE. Carbon FamilyGroup IVA Properties1. Have 4 valence electrons 2. Family contains metals, metalloids, and nonmetalsForms of carbon: diamond, coal, cokeSi second most abundant element in the Earths crust

IV.The FamiliesF. Nitrogen FamilyGroup VA PropertiesHave 5 valence electrons Contains metals, metalloids, and nonmetalsN makes up 80% of air

IV.The FamiliesG. Oxygen Family Group VIA PropertiesHave 6 valence electrons O most abundant element on earth

IV.The FamiliesH. Halogen FamilyGroup VIIA PropertiesHave 7 valence electrons Most reactive nonmetalsReact with IA and IIA family members to form salts F the most chemically reactive of all elements

IV.The FamiliesI. Noble Gas FamilyGroup VIIIA PropertiesHave 8 valence e- (full valence energy level) Inert, stable, non-reactiveAll are gases Low boiling pointsPeriodic Trends

A. Periodic LawWhen elements are arranged in order of increasing atomic #, elements with similar properties appear at regular intervals.

B. Chemical ReactivityFamiliesSimilar valence e- within a group result in similar chemical properties

B. Chemical ReactivityAlkali MetalsAlkaline Earth MetalsTransition MetalsHalogensNoble GasesC. Other PropertiesAtomic Radiussize of atom

1998 LOGALFirst Ionization EnergyEnergy required to remove one e- from a neutral atom.

1998 LOGALMelting/Boiling PointD. Atomic RadiusAtomic Radius

LiArNeKNa

D. Atomic RadiusAtomic RadiusIncreases to the LEFT and DOWN

D. Atomic RadiusWhy larger going down?Higher energy levels have larger orbitalsShielding - core e- block the attraction between the nucleus and the valence e-Why smaller to the right? Increased nuclear charge without additional shielding pulls e- in tighterE. Ionization EnergyFirst Ionization Energy

KNaLiArNeHe

E. Ionization EnergyFirst Ionization EnergyIncreases UP and to the RIGHTE. Ionization EnergyWhy opposite of atomic radius?In small atoms, e- are close to the nucleus where the attraction is stronger

F. Melting/Boiling PointMelting/Boiling PointHighest in the middle of a period.G. Ionic RadiusIonic RadiusCations (+)lose e-smaller

2002 Prentice-Hall, Inc.Anions ()gain e-largerExamplesWhich atom has the larger radius?Beor BaCa or BrBaCaExamplesWhich atom has the higher 1st I.E.?N or BiBaor NeNNeExamplesWhich atom has the higher melting/boiling point?LiorCCrorKrCCrExamplesWhich particle has the larger radius?S or S2-Alor Al3+S2-Al

Chart237541521118877706664701861601431171101049994231197

Atomic NumberAtomic Radius (pm)

Sheet113713122542372315251941119005887996771088770140686613149641682107020801118649812160736131435771411778715110106316104100017991255189415191923141820197590

Sheet100000000000000000000

Atomic NumberAtomic Radius (pm)

Sheet2

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Chart237541521118877706664701861601431171101049994231197

Atomic NumberAtomic Radius (pm)

Sheet113713122542372315251941119005887996771088770140686613149641682107020801118649812160736131435771411778715110106316104100017991255189415191923141820197590

Sheet100000000000000000000

Atomic NumberAtomic Radius (pm)

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1

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Chart237541521118877706664701861601431171101049994231197

Atomic NumberAtomic Radius (pm)

Sheet113713122542372315251941119005887996771088770140686613149641682107020801118649812160736131435771411778715110106316104100017991255189415191923141820197590

Sheet100000000000000000000

Atomic NumberAtomic Radius (pm)

Sheet2

Sheet3

1

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7

Chart213122372519900799108814061314168220804987365777871063100012551519418590

Atomic Number1st Ionization Energy (kJ)

Sheet113713122542372315251941119005887996771088770140686613149641682107020801118649812160736131435771411778715110106316104100017991255189415191923141820197590

Sheet1

Atomic NumberAtomic Radius (pm)

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1

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