the periodic table applied chemistry. elements there are approximately 116 elements in the periodic...

The The PeriodiPeriodi

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Applied Applied ChemistryChemistry

ElementsElements

There are approximately There are approximately 116116 elements elements in the periodic table.in the periodic table.

9292 elements occur naturally in nature. elements occur naturally in nature. Elements exist in the following three Elements exist in the following three

states: states: solid, liquid, and gassolid, liquid, and gas Elements can be found in all matter, Elements can be found in all matter,

including including livingliving things and the things and the environmentenvironment

All elements can be located in the All elements can be located in the periodic tableperiodic table..

Properties of ElementsProperties of Elements

Qualitative Properties: Qualitative Properties: properties properties describing appearance; descriptive describing appearance; descriptive using 5 sensesusing 5 senses Examples: Examples: Texture, color, shape, odorTexture, color, shape, odor

Quantitative Properties: Quantitative Properties: properties properties involving measurements (numbers)involving measurements (numbers)

Quantitative PropertiesQuantitative Properties Melting point – Temperature at which Melting point – Temperature at which

a a solidsolid changes to a changes to a liquid (liquid (+*/5701-+*3+*/5701-+*3))

Boiling point – Temperature at which Boiling point – Temperature at which a a liquidliquid changes to a changes to a gas (gas (ooC)C)..

Density – a measure of the amount Density – a measure of the amount of of massmass of an object divided by its of an object divided by its volumevolume Units are grams per milliliter (g/mL)Units are grams per milliliter (g/mL)

Properties of Properties of MetalsMetals At room temp, all are solid except for At room temp, all are solid except for

mercurymercury..

LusterLuster (A.K.A. Shininess) (A.K.A. Shininess)

Good Good conductorsconductors of heat and electricity. of heat and electricity.

High High densitydensity (ex. Dumbbell) (ex. Dumbbell)

HighHigh melting points melting points

Properties of Properties of MetalsMetals DuctileDuctile: can be drawn : can be drawn

out into thin wires.out into thin wires. MalleableMalleable: can be : can be

hammered into thin hammered into thin sheets.sheets.

Metals are found on the Metals are found on the leftleft side of the periodic side of the periodic table.table.

Metals make up Metals make up mostmost of of the periodic table.the periodic table.

NonmetalsNonmetals At room temperature, they are At room temperature, they are solids, liquids, solids, liquids,

or or gases.gases. No No luster (dull)luster (dull).. InsulatorsInsulators of heat and electricity. ( of heat and electricity. (Do notDo not

allow heat and electricity to flow through allow heat and electricity to flow through them.)them.)

BrittleBrittle, easy to break, easy to break Neither malleable or ductileNeither malleable or ductile Lower Lower boilingboiling points and points and meltingmelting points than points than

metals.metals. Located on the Located on the upper rightupper right side of the side of the

periodic table.periodic table.

Sulfur

Iodine

Metalloids (Semimetals)Metalloids (Semimetals) Have properties of both Have properties of both metalsmetals and and

nonmetalsnonmetals..

There are There are 7 7 metalloids in the periodic metalloids in the periodic table: table: Boron, Silicon, Germanium, Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium, & Arsenic, Antimony, Tellurium, & AstatineAstatine..

Located Located between the metals and between the metals and nonmetals, nonmetals, ALONGALONG the staircase . the staircase .

The Periodic TableThe Periodic Table

History of the Periodic TableHistory of the Periodic Table

Periodic – Periodic – repeating repeating patternpattern

Dobereiner (1829):Dobereiner (1829): found that some found that some elements have similar elements have similar propertiesproperties. . Grouped the elements in Grouped the elements in

groups of three called groups of three called triadstriads..

Triads on the Periodic TableTriads on the Periodic Table

Newlands (1867):Newlands (1867): saw that the saw that the properties of properties of elements repeat elements repeat every every 88 element. element. This is called the This is called the

Law of OctavesLaw of Octaves..

History of the Periodic TableHistory of the Periodic Table

History of the Periodic TableHistory of the Periodic Table

MendeleevMendeleev: : developed the first developed the first periodic tableperiodic table in in 1869.1869.

Arranged the Arranged the periodic table in periodic table in order of increasing order of increasing atomic massatomic mass..

Dimitri Mendeleev:Dimitri Mendeleev: 1869 1869 Predicted the Predicted the

properties of properties of undiscoveredundiscovered elementselements and left and left blank spots in the blank spots in the periodic table for periodic table for these elements.these elements.

11stst Periodic Law Periodic Law: the : the propertiesproperties of elements of elements recur at certain recur at certain intervals of intervals of increasing increasing atomic massatomic mass..

History of the Periodic TableHistory of the Periodic Table MoseleyMoseley (1911), he (1911), he

reorganized the periodic reorganized the periodic table in order of increasing table in order of increasing atomic number atomic number (protons).(protons).

Modern Periodic LawModern Periodic Law – the – the propertiesproperties of elements of elements recur at certain intervals of recur at certain intervals of atomic number.atomic number.

““Properties are periodic”Properties are periodic”

Organization of the Organization of the Periodic TablePeriodic Table

PeriodPeriod: Horizontal Rows in : Horizontal Rows in the periodic tablethe periodic table There are There are 77 periods in the periods in the

periodic table.periodic table. Elements in a period Elements in a period do NOTdo NOT

have similar properties.have similar properties.

Group or FamilyGroup or Family: Vertical : Vertical Columns in the periodic tableColumns in the periodic table There are There are 1818 groups in the periodic groups in the periodic

table.table. Numbered from Numbered from 1 to 18 or1 to 18 or 1A, 2A, 1A, 2A,

(B groups), 3A through 8A.(B groups), 3A through 8A. Elements in the same group Elements in the same group havehave

similar propertiessimilar properties..

Organization of the Organization of the Periodic TablePeriodic Table

Elements in the same group Elements in the same group havehave similar propertiessimilar properties. . Why?Why? Elements in the same group have the Elements in the same group have the

same number of same number of VALENCEVALENCE electrons. electrons. ValenceValence electrons are those electrons are those

electrons in the outer energy level.electrons in the outer energy level. The maximum number of valence The maximum number of valence

electrons is electrons is 88..

Organization of the Organization of the Periodic TablePeriodic Table

1A 1

2A2

3A 4A 5A 6A 7A13 14 15 16 17

8A18

1 = Alkali Metals and Hydrogen Group

13 = Boron Group

18 = Noble Gas Group

17 = Halogen Group

16 = Oxygen or Chalcogen Group

15= Nitrogen Group

14 = Carbon Group

2 = Alkaline Earth Metals

Transition Group

Lanthanide Series

Actinide Series

Inner Transition

3 4 5 6 7 8 9 10 11 12

Groups in the periodic tableGroups in the periodic table HydrogenHydrogen: Group : Group 1 or 1A/IA1 or 1A/IA

1 1 valence electronvalence electron

Alkali MetalsAlkali Metals: Group : Group 1 or 1A/IA1 or 1A/IA 11 valence electron valence electron MostMost reactive metals reactive metals As you go down a group, reactivity As you go down a group, reactivity

increasesincreases..

Groups in the periodic tableGroups in the periodic table

Alkaline Earth MetalsAlkaline Earth Metals: Group : Group 2 or 2 or 2A/IIA2A/IIA 22 Valence electrons Valence electrons Very reactiveVery reactive

Boron GroupBoron Group: Group : Group 13 or 3A/IIIA13 or 3A/IIIA 3 3 Valence electronsValence electrons

Carbon GroupCarbon Group: Group : Group 14 or 4A/IVA14 or 4A/IVA 44 Valence electrons Valence electrons

Groups in the periodic tableGroups in the periodic table

Nitrogen GroupNitrogen Group: Group : Group 15 or 5A/VA15 or 5A/VA 5 5 Valence electronsValence electrons

Oxygen Group or Chalcogen GroupOxygen Group or Chalcogen Group: Group : Group 16 or 6A/VIA16 or 6A/VIA 6 6 Valence electronsValence electrons

Halogen GroupHalogen Group: Group : Group 17 or 7A/VIIA17 or 7A/VIIA 77 Valence electrons Valence electrons Used in Used in photographyphotography MostMost reactive nonmetals reactive nonmetals

Groups in the periodic tableGroups in the periodic table

Noble Gas GroupNoble Gas Group – Group – Group 18 or 8A/VIIIA18 or 8A/VIIIA 88 Valence electrons Valence electrons (Helium only has 2)(Helium only has 2) Do not react with other elements: known Do not react with other elements: known

as as INERTINERT Have a complete outer shell of electrons Have a complete outer shell of electrons

known as a known as a full stable octetfull stable octet ““Everyone wants to be like a noble gas.”Everyone wants to be like a noble gas.”

Groups in the periodic tableGroups in the periodic table Transition MetalsTransition Metals: Groups : Groups 3-123-12

Inner Transition MetalsInner Transition Metals: Bottom of PT : Bottom of PT LanthanideLanthanide Series or Rare Earth Elements Series or Rare Earth Elements

(Cerium through Lutetium)(Cerium through Lutetium) Actinide SeriesActinide Series

(Thorium through Lawrencium)(Thorium through Lawrencium)

Transuranium ElementsTransuranium Elements: : allall elements elements after uranium (atomic #92)after uranium (atomic #92) these elements are these elements are manmademanmade elements elements

Groups in the periodic tableGroups in the periodic table

IMPORTANT NOTE: IMPORTANT NOTE: Members of a group have Members of a group have similarsimilar chemical chemical properties, because they properties, because they have the same number of have the same number of valence valence electrons.electrons.

Trends in the Periodic TableTrends in the Periodic Table The most reactive The most reactive metalsmetals are the are the alkali alkali

metals.metals.

Metals becomeMetals become more more reactive as you reactive as you move down a family.move down a family.

The The most reactive metalmost reactive metal is is FranciumFrancium..

Trends in the Periodic TableTrends in the Periodic Table

The most reactive The most reactive nonmetalsnonmetals are the are the halogenshalogens..

Nonmetals become Nonmetals become lessless reactive as reactive as you move down a family.you move down a family.

The The most reactive nonmetalmost reactive nonmetal is is fluorinefluorine..

Trends in the Periodic TableTrends in the Periodic TableAtomic RadiiAtomic Radii

The distance between the The distance between the nucleusnucleus and and the outermost the outermost electronselectrons in an atom. in an atom.

Unit = Unit = picometer (pm)picometer (pm)

IncreasesIncreases as you go down a group. as you go down a group.

Decreases Decreases as you go left to right as you go left to right across a period.across a period.

Atomic Radius Examples:Atomic Radius Examples:

Which has a Which has a largerlarger atomic atomic radius?radius? Potassium or CesiumPotassium or Cesium Sodium or ChlorineSodium or Chlorine Silicon or LeadSilicon or Lead Lithium or OxygenLithium or Oxygen

Trends in the Periodic TableTrends in the Periodic TableIonization EnergyIonization Energy

The energy needed to The energy needed to removeremove a a valence electron from an atom. valence electron from an atom.

Unit = Unit = kJ/mol (kilojoules per kJ/mol (kilojoules per mole)mole)

IncreasesIncreases as you go from left to right as you go from left to right across a period.across a period.

DecreasesDecreases as you go down a group. as you go down a group.

Ionization Energy of the 1Ionization Energy of the 1stst 20 20 ElementsElements

Trends in the Periodic TableTrends in the Periodic TableIonization EnergyIonization Energy

The ionization energy for the noble The ionization energy for the noble gases is very gases is very highhigh because they do because they do not want to give up any electrons. not want to give up any electrons. (They have a stable octet.)(They have a stable octet.)

The energy needed to remove each The energy needed to remove each successive electron successive electron increasesincreases..

Ionization Energy Ionization Energy Examples:Examples:

Which has a Which has a largerlarger ionization ionization energy?energy? Silicon or chlorineSilicon or chlorine Lithium or rubidiumLithium or rubidium Sulfur or telluriumSulfur or tellurium Calcium or bromineCalcium or bromine