Periodic Table Periodic Table of Elementsof Elements

Bohr Model: and Valence electronsBohr Model: and Valence electrons http://youtu.be/trsln8RCEVohttp://youtu.be/trsln8RCEVo

CasseopiaCasseopia http://youtu.be/5MMWpeJ5dn4http://youtu.be/5MMWpeJ5dn4

Dan RadcliffeDan Radcliffe http://youtu.be/rSAaiYKF0cshttp://youtu.be/rSAaiYKF0cs

Bald Guy:Bald Guy: http://youtu.be/nsbXp64YPRQhttp://youtu.be/nsbXp64YPRQ

Song:Song: http://youtu.be/afFw91fvNJMhttp://youtu.be/afFw91fvNJM

http://youtu.be/zGM-wSKFBpohttp://youtu.be/zGM-wSKFBpo

Dmitri MendeleevDmitri Mendeleev

Russian chemist. Russian chemist.

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

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 on the table (1-18).Columns on the table (1-18).

Elements have the Elements have the same same number of valence electronsnumber of valence electrons..

Similar chemical properties.Similar chemical properties.

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

Periods (1-7)Periods (1-7)

The rows on the table.The rows on the table.

Have the same Have the same number number of occupied energy of occupied energy levelslevels..

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

Get to Know Your GroupsGet to Know Your Groups

Alkali MetalsAlkali Metals

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

compounds.compounds.

Rubidium

Comparing the Alkali MetalsComparing the Alkali Metals

http://youtu.be/uixxJtJPVXkhttp://youtu.be/uixxJtJPVXk

Alkaline Earth MetalsAlkaline Earth Metals

2 valence electrons2 valence electrons Form +2 ionsForm +2 ions Very reactiveVery reactive Found only in Found only in

compoundscompounds

HalogensHalogens

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

Noble GasesNoble 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

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 Metals

Form colored compounds and solutions.Form colored compounds and solutions.

Metals/Nonmetals/MetalloidsMetals/Nonmetals/Metalloids

MetalsMetals

Have lusterHave lusterMalleableMalleableDuctileDuctileConduct 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 Most elements along the “staircase”“staircase”

Can have properties of Can have properties of both metals and both metals and nonmetals.nonmetals.

B, Si, Ge, As, Sb, Te, AtB, Si, Ge, As, Sb, Te, At

Trends in the Period TableTrends in the Period 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.

Get out Reference Get out Reference Table STable S

Trends in RadiusTrends in Radius

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

Down a GroupDown a GroupSize increasesSize increases Why?Why?

You add You add new energy levelsnew energy levels

Across a PeriodAcross a PeriodSize decreasesSize decreasesWhy?Why?

Increasing Increasing nuclear chargenuclear charge pulls on the pulls on the energy levelsenergy levels

http://youtu.be/ba2yN2HtPTAhttp://youtu.be/ba2yN2HtPTA

Ionization EnergyIonization Energy

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

Get out Reference Get out Reference Table STable S

Trends in Ionization EnergyTrends in Ionization Energy

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.

Large Radius = Lower Ionization EnergyLarge Radius = Lower Ionization Energy

Why?Why?

The further the outmost electron to theThe further the outmost electron to the

nuclear pull the easier to remove it.nuclear pull the easier to remove it.

http://youtu.be/8F9nA4Fg3Rwhttp://youtu.be/8F9nA4Fg3Rw

ElectronegativityElectronegativity

The relative The relative attraction an atom attraction an atom has for electrons has for electrons involved in bond involved in bond formation.formation.

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

This can result in This can result in “polar” and “nonpolar” “polar” and “nonpolar” bonds.bonds.

Fluorine has the Fluorine has the highest EN value = 4highest EN value = 4

(The EN scale was (The EN scale was created by comparing created by comparing other elements to other elements to Fluorine)Fluorine)

Get out Reference Get out Reference Table STable S

Trends in ElectronegativityTrends in Electronegativity

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

http://youtu.be/93G_FqpGFGYhttp://youtu.be/93G_FqpGFGY

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