(Honors) Intro to the Table(Honors) Intro to the Table http://youtu.be/5MMWpeJ5dn4

Dan Radcliffe Knows his elements!Dan Radcliffe Knows his elements! http://youtu.be/rSAaiYKF0cs

Elements Song:Elements Song: Periodic Table of Videos Crew:Periodic Table of Videos Crew:

http://youtu.be/afFw91fvNJM

A different SongA different Song http://www.youtube.com/watch?v=zUDDiWtFtEM&safe=active

Periodic Table Periodic Table of Elementsof Elements

Dmitri MendeleevDmitri Mendeleev

Russian chemist. Russian chemist.

Created first version of Created first version of periodic table.periodic table.

Predicted properties of Predicted properties of elements yet to be elements yet to be discovered. discovered.

Rockin the shaggy beard…

Mendeleev arranged Mendeleev arranged elements according to elements according to their atomic weights.their atomic weights.

Today they are arranged Today they are arranged by atomic number. by atomic number.

Development of the Table: 3:39http://youtu.be/nsbXp64YPRQ

Periodic LawPeriodic Law

Properties of elements are periodic Properties of elements are periodic functions of their atomic numbers.functions of their atomic numbers.

In other words, properties tend to repeat In other words, properties tend to repeat as you start a new period.as you start a new period.

Groups/FamiliesGroups/Families

Columns (1-18).Columns (1-18).

Elements have Elements have same number of valence electronssame number of valence electrons..

Have Have similarsimilar chemical properties. chemical properties.

Tend to form bonds in a similar way to get stable octet.Tend to form bonds in a similar way to get stable octet.

PeriodsPeriods

Rows (1-7).Rows (1-7).

Have same Have same number of number of occupied energy levelsoccupied energy levels..

They They do notdo not have similar have similar properties.properties.

Group 1: Alkali MetalsGroup 1: Alkali Metals

1 valence electron1 valence electron Form +1 IonsForm +1 Ions Very reactive Very reactive Found only in Found only in

compounds.compounds.

Rubidium http://youtu.be/uixxJtJPVXk

http://www.youtube.com/watch?feature=player_embedded&v=HY7mTCMvpEM

Group 2: Alkaline Earth MetalsGroup 2: Alkaline Earth Metals 2 valence electrons2 valence electrons Form +2 ionsForm +2 ions Very reactiveVery reactive Found only in Found only in

compoundscompounds

Group 2:

Some Alkaline Earth Metals

Group 17: HalogensGroup 17: Halogens

7 valence electrons7 valence electrons Form -1 ionsForm -1 ions Very reactiveVery reactive All nonmetalsAll nonmetals

IODINE

solid → gas

(sublimes)

Gas Liquid Solid

FLUORINE

Extremely reactive gas http://www.youtube.com/watch?

feature=player_embedded&v=u2ogMUDBaf4

Group 18: Noble GasesGroup 18: Noble Gases

Inert GasesInert Gases Not reactiveNot reactive Have stable octetHave stable octet

(except He)(except He) Monoatomic gasesMonoatomic gases

s, p, d, f, “Blocks”s, p, d, f, “Blocks”

Indicates what sublevel is being filled last Indicates what sublevel is being filled last in the atomin the atom

Lanthanide & Actinide SeriesLanthanide & Actinide Series

Two rows on the bottom of the tableTwo rows on the bottom of the table ““f” blockf” blockStart with lanthanum and actiniumStart with lanthanum and actinium

Transition MetalsTransition Metals

Metals in the “lower” Metals in the “lower” columns.columns.

(d-block metals)(d-block metals)

““Inner” transition Inner” transition metals are the two metals are the two bottom rowsbottom rows

(f-block metals)(f-block metals)

Transition MetalsTransition MetalsForm colored compounds and solutions.Form colored compounds and solutions.Often have multiple “oxidation states” (charges)Often have multiple “oxidation states” (charges)May involve d-sublevel electrons in forming May involve d-sublevel electrons in forming

bondsbonds

Man Made ElementsMan Made Elements::Elements that are not found naturally in the Elements that are not found naturally in the

earth’s crust.earth’s crust.Must be created through nuclear Must be created through nuclear

bombardment using particle accelerators.bombardment using particle accelerators.All elements above Uranium (Atomic #92)All elements above Uranium (Atomic #92)

Radioactive Elements:Radioactive Elements:All the isotopes of elements higher than All the isotopes of elements higher than

Bismuth (Atomic #83) are radioactive.Bismuth (Atomic #83) are radioactive.

Do we know our groups?Do we know our groups?Elements Song Again!Elements Song Again!http://youtu.be/zGM-wSKFBpohttp://youtu.be/zGM-wSKFBpo

Periodic Table Dating GamePeriodic Table Dating Game http://www.youtube.com/watch?v=A6cF0iWC3J4http://www.youtube.com/watch?v=A6cF0iWC3J4

Review QuestionReview Question::How many different ways is the structure How many different ways is the structure

of the Periodic Table related to the inner of the Periodic Table related to the inner structure of an atom? structure of an atom?

Think proton # and electron configuration!Think proton # and electron configuration!

Metals/Nonmetals/MetalloidsMetals/Nonmetals/Metalloids

MetalsMetals

LusterLusterMalleableMalleableDuctileDuctileConduct heat and electricityConduct heat and electricityTend to lose valence electrons and form Tend to lose valence electrons and form

positive ionspositive ionsAll solids (except Hg)All solids (except Hg)

NonmetalsNonmetals

No lusterNo luster Brittle (if solid)Brittle (if solid) Don’t conductDon’t conduct Tend to gain valence electrons Tend to gain valence electrons

and form negative ionsand form negative ions Can be solid ( I, C, P, S) , liquid (Br), Can be solid ( I, C, P, S) , liquid (Br),

or gases (F, Cl, N, O) or gases (F, Cl, N, O) Hydrogen is considered a nonmetalHydrogen is considered a nonmetal

Metalloids (Semimetals)Metalloids (Semimetals)

Most elements along the “staircase”Most elements along the “staircase” Can have properties of both metals and nonmetals.Can have properties of both metals and nonmetals. B, Si, Ge, As, Sb, Te, AtB, Si, Ge, As, Sb, Te, At

Trends in the Periodic TableTrends in the Periodic Table

Atomic RadiusAtomic Radius

Distance from the nucleus of an atom to Distance from the nucleus of an atom to the outer edge of it’s electron cloud.the outer edge of it’s electron cloud.

Trends in RadiusTrends in Radius(Use Table S)(Use Table S)

Down a GroupDown a Group

Ex: Group 1 What happens?Ex: Group 1 What happens?

Across a PeriodAcross a Period

Ex: Period 2Ex: Period 2 What happens?What happens?

Li

Na

K

Rb

Cs

Fr

Li Be B C N O F Ne

Let’s Think:Let’s Think:Can you come up with a reason why you Can you come up with a reason why you think this trend happens?think this trend happens?

How might it be related to electron shells and How might it be related to electron shells and electron repulsion?electron repulsion?

How might it be related to the pull of nuclear How might it be related to the pull of nuclear charge?charge?

Down a Group: Down a Group: Size increasesSize increases Add Add new energy levelsnew energy levelsGreater shielding from core electronsGreater shielding from core electronsOuter electrons further from nucleus Outer electrons further from nucleus

so less attractive forceso less attractive force

Across a Period: Across a Period: Size decreasesSize decreases Increasing Increasing nuclear chargenuclear charge pulls on same # of pulls on same # of

energy levelsenergy levelsNo increase in shielding effectNo increase in shielding effect

http://youtu.be/ba2yN2HtPTAhttp://youtu.be/ba2yN2HtPTAhttp://www.youtube.com/watch?v=VopLrkfXfGw&safe=activehttp://www.youtube.com/watch?v=VopLrkfXfGw&safe=active

Helpful Tutorial:Helpful Tutorial: http://www.youtube.com/watch?v=k9NrwDaMRQk&safe=activehttp://www.youtube.com/watch?v=k9NrwDaMRQk&safe=active

Ionization Ionization EnergyEnergy

Energy required to Energy required to remove the remove the outermost electron outermost electron from an atom.from an atom.

Trends in Trends in IonizationIonization Energy Energy(Use Table S)(Use Table S)

Down a GroupDown a Group

Ex: Group 1 What happens?Ex: Group 1 What happens?

Across a PeriodAcross a Period

Ex: Period 2Ex: Period 2 What happens?What happens?

LiNaKRbCsFr

Li Be B C N O F Ne

What is the trend?What is the trend?

Directly related to Atomic Radius.Directly related to Atomic Radius.

Larger Radius = Lower Ionization EnergyLarger Radius = Lower Ionization Energy

Why?Why?

The further the outermostThe further the outermost

electron is from theelectron is from the

nuclear pull, the easier itnuclear pull, the easier it

is to remove.is to remove.

The more shells of kernelThe more shells of kernel

electrons around theelectrons around the

nucleus the greater thenucleus the greater the

““shielding effect”.shielding effect”.

ElectronegativityElectronegativity

Attraction an atom Attraction an atom has for electrons has for electrons involved in bond involved in bond formation.formation.

ElectronegativityElectronegativity

The higher the EN value the more the atom “pulls” The higher the EN value the more the atom “pulls” on electrons involved in a bond.on electrons involved in a bond.

Like a “tug of war” for electrons in the bondLike a “tug of war” for electrons in the bond

Polarity of BondsPolarity of Bonds

Polar Bond:Polar Bond: unequalunequal electron sharing electron sharingatoms have atoms have different ENdifferent EN

valuesvalues

Nonpolar BondNonpolar Bond: : equalequal electron sharing electron sharingAtoms have Atoms have same ENsame EN

valuesvalues

Fluorine has the Fluorine has the highest EN value = 4highest EN value = 4 EN scale was created EN scale was created

by comparing other by comparing other elements to Fluorineelements to Fluorine

Nonmetals generally Nonmetals generally have much higher EN have much higher EN values than metalsvalues than metals

Trends in ElectronegativityTrends in Electronegativity (Use Table S) (Use Table S)

Down a GroupDown a Group

Ex: Group 1 What happens?Ex: Group 1 What happens?

Across a PeriodAcross a Period

Ex: Period 2Ex: Period 2 What happens?What happens?

LiNaKRbCsFr

Li Be B C N O F Ne

What was the trend?What was the trend?

What is the relationship to atomic radius?What is the relationship to atomic radius?

What elements don’t have really have What elements don’t have really have electronegativity values? Why is that?electronegativity values? Why is that?

http://youtu.be/93G_FqpGFGY

http://www.youtube.com/watch?v=YZ8izzEq6zI&safe=active

Metallic/NonMetallic Metallic/NonMetallic CharacterCharacter

More “Metallic”:More “Metallic”: Large radiusLarge radius Low Ionization EnergyLow Ionization Energy Low ElectronegativityLow Electronegativity

More “Non Metallic”:More “Non Metallic”: Small radiusSmall radius High Ionization EnergyHigh Ionization Energy High ElectronegativityHigh Electronegativity http://www.youtube.com/watch?

feature=player_embedded&v=hANWofStHrk

Crash Course Video(13 minutes)Crash Course Video(13 minutes)http://www.youtube.com/watch?http://www.youtube.com/watch?

v=0RRVV4Diomg&safe=activev=0RRVV4Diomg&safe=active