The Periodic Table Periodicity Unit IV Ch. 6. Pictionary Words Period Atomic radius Group Transition...

The Periodic TableThe Periodic Table

PeriodicityPeriodicity

Unit IVUnit IV

Ch. 6Ch. 6

Pictionary WordsPictionary Words

PeriodPeriod Atomic radius Atomic radius

GroupGroup Transition metal Transition metal

Metal Metal Reactivity Reactivity

MetalloidMetalloid Ionization energy Ionization energy

ElectronegativityElectronegativity

Non-metalNon-metal

Warm UpWarm Up

1. What do you KNOW about the periodic table?1. What do you KNOW about the periodic table?

2. What WOULD you like to know about the 2. What WOULD you like to know about the periodic table?periodic table?

3. What did you like to LEARN about the 3. What did you like to LEARN about the periodic table?periodic table?

Warm UpWarm Up

1.1. What is the law of octaves?What is the law of octaves?

2.2. Identify the groups that correspond to the Identify the groups that correspond to the following family names: alkali metals, alkali following family names: alkali metals, alkali earth metals, chalcogens, halogens, noble earth metals, chalcogens, halogens, noble gases and transition metals.gases and transition metals.

3.3. State the periodic law.State the periodic law.

4.4. Who is credited with organizing the modern Who is credited with organizing the modern periodic table. periodic table.

Warm Up-02/19/13Warm Up-02/19/13

1.1. Identify the family in which the following Identify the family in which the following appear: K, Cl, Pr, Ba, F, Mn, Th and W.appear: K, Cl, Pr, Ba, F, Mn, Th and W.

2.2. List 5 transition elements.List 5 transition elements.

3.3. The alkili metals are also known as what?The alkili metals are also known as what?

4.4. The alkili metals are also known as what?The alkili metals are also known as what?

5.5. The noble gas family is also known as what?The noble gas family is also known as what?

Warm Up-09/24/13Warm Up-09/24/13

1.1. Place the following elements in order from Place the following elements in order from largest to smallest: Si, Na, Ar, Al and S.largest to smallest: Si, Na, Ar, Al and S.

2.2. Place the following elements in order from Place the following elements in order from largest to smallest: Be, Ba, Ca, Mg, and Sr.largest to smallest: Be, Ba, Ca, Mg, and Sr.

3.3. Repeat questions 4 and 5 for ionic radius Repeat questions 4 and 5 for ionic radius excluding argon.excluding argon.

4.4. Place the following in order from greatest to Place the following in order from greatest to lowest ionization energies: Kr, Ne, Xe, He and lowest ionization energies: Kr, Ne, Xe, He and Ar.Ar.

Expectations:Expectations: 1.) Each group will have created a neat, 1.) Each group will have created a neat,

colorful, and easy to read periodic table. colorful, and easy to read periodic table. 2.) Atomic Number, Symbol and Name must 2.) Atomic Number, Symbol and Name must

be present.be present. 3.) Ionization/Electronegativity/Radii value 3.) Ionization/Electronegativity/Radii value

must be written in the place of the atomic massmust be written in the place of the atomic mass 4.) 3-d dimensions must be to scale4.) 3-d dimensions must be to scale

http://www.exo.net/~emuller/activities/Thehttp://www.exo.net/~emuller/activities/The%20Periodic%20Periodic%20Table.pdf%20Periodic%20Periodic%20Table.pdf

Atomic RadiusAtomic Radius- p. 914- 916 scale: 1 mm= - p. 914- 916 scale: 1 mm= 1pm.1pm.

Ionization EnergyIonization Energy- p. 914-916 scale: 1 mm= - p. 914-916 scale: 1 mm= 10 kJ/mol.10 kJ/mol.

Electronegativity-Electronegativity- p. 169 scale: 10 cm = 1 p. 169 scale: 10 cm = 1 Paulings.Paulings.

Ionic Radii-Ionic Radii- handout scale: 1 cm = .1 handout scale: 1 cm = .1 Angstroms.Angstroms.

Warm UpWarm Up1.1. If 1 mm= 1pm, how long would you cut a straw to represent If 1 mm= 1pm, how long would you cut a straw to represent

fluorine’s atomic radius?fluorine’s atomic radius?

2.2. If 1 mm= 1pm, how long would you cut a straw to represent If 1 mm= 1pm, how long would you cut a straw to represent germanium’s atomic radius?germanium’s atomic radius?

3.3. If 10 cm= 1 pauling, how long would you cut a straw to If 10 cm= 1 pauling, how long would you cut a straw to represent silver’s electronegativity?represent silver’s electronegativity?

4.4. If 10 cm= 1 pauling, how long would you cut a straw to If 10 cm= 1 pauling, how long would you cut a straw to represent gold’s electronegativity?represent gold’s electronegativity?

5.5. If 1 mm= 10 kJ/mol., how long would you cut a straw to If 1 mm= 10 kJ/mol., how long would you cut a straw to represent neon’s ionization energy?represent neon’s ionization energy?

6.6. If 1 mm= 10 kJ/mol., how long would you cut a straw to If 1 mm= 10 kJ/mol., how long would you cut a straw to represent potassium’s ionization energy?represent potassium’s ionization energy?

Warm UpWarm Up1.1. If 1 mm= 1pm, how long would you cut a straw to represent If 1 mm= 1pm, how long would you cut a straw to represent

gallium's atomic radius?gallium's atomic radius?

2.2. If 1 mm= 1pm, how long would you cut a straw to represent If 1 mm= 1pm, how long would you cut a straw to represent oxygen’s atomic radius?oxygen’s atomic radius?

3.3. If 10 cm= 1 pauling, how long would you cut a straw to If 10 cm= 1 pauling, how long would you cut a straw to represent manganese's electronegativity?represent manganese's electronegativity?

4.4. If 1 mm= 1 pauling, how long would you cut a straw to If 1 mm= 1 pauling, how long would you cut a straw to represent calcium’s electronegativity?represent calcium’s electronegativity?

5.5. If 1 mm= 10 kJ/mol., how long would you cut a straw to If 1 mm= 10 kJ/mol., how long would you cut a straw to represent kripton’s ionization energy?represent kripton’s ionization energy?

Johann Dobereiner, 1817Johann Dobereiner, 1817

TriadsTriads

Groups of three elements having similar physical Groups of three elements having similar physical and chemical properties.and chemical properties.

These three elements are in the same Group or These three elements are in the same Group or FamilyFamily

John Newlands, 1863John Newlands, 1863

Arranged elements in order of their atomic masses. Arranged elements in order of their atomic masses.

Noticed that their properties repeated every 8th Noticed that their properties repeated every 8th elementelement

Law of OctavesLaw of OctavesThe same properties repeat every eighth elementThe same properties repeat every eighth element

Dmitri Mendeleev, 1869Dmitri Mendeleev, 1869

Believed that similar properties occurred after Believed that similar properties occurred after periods that could vary in lengthperiods that could vary in length

Properties of the elements repeat in an orderly Properties of the elements repeat in an orderly way. Such a pattern is “periodic”way. Such a pattern is “periodic”

The Periodic LawThe Periodic Law““The properties of the elements are a periodic The properties of the elements are a periodic

function of their atomic masses”function of their atomic masses”

Henry Moseley, 1913Henry Moseley, 1913

Using X-Rays, he showed that the nucleus had a Using X-Rays, he showed that the nucleus had a positive charge. Thus, the Periodic Law was positive charge. Thus, the Periodic Law was revised:revised:

Periodic Law

Properties of the elements are a periodic function of their atomic numbers

Electron Configuration andElectron Configuration andThe Periodic TableThe Periodic Table

Electron Configuration determines a chemical's reactivity.Electron Configuration determines a chemical's reactivity.

s-Block Elements (Groups 1 and 2; or Groups I A and II A)s-Block Elements (Groups 1 and 2; or Groups I A and II A)

Outermost electrons are added to an s-orbitalOutermost electrons are added to an s-orbital Group 1: sGroup 1: s11 - - Alkali MetalsAlkali Metals

Group 2: sGroup 2: s22 - - Alkaline Earth MetalsAlkaline Earth Metals


p-Block Elements (Groups 13-18; Groups III A through p-Block Elements (Groups 13-18; Groups III A through VIII A)VIII A)

Outermost electrons are added to a p-orbital Outermost electrons are added to a p-orbital

Group 13: pGroup 13: p11



Group 16: pGroup 16: p44 - - ChalcogensChalcogens

Group 17: pGroup 17: p55 - - HalogensHalogens

Group 18: pGroup 18: p66 - - Noble GasesNoble Gases ( (Inert GasesInert Gases) )


d-Block Elements (Groups 3-12; Groups I B through VIII B)d-Block Elements (Groups 3-12; Groups I B through VIII B)

Outermost electrons are added to a d-orbital Outermost electrons are added to a d-orbital

Known as the Known as the transition metalstransition metals

All metals All metals


Reading the electron configuration directly off the Reading the electron configuration directly off the Periodic Table.Periodic Table.

s-Block s-Block

p-Block p-Block

Main Group Elements (s- & p-blocks)Main Group Elements (s- & p-blocks)

d-Block (Transition Elements)d-Block (Transition Elements)

f-Block (Lanthanides and Actinides)f-Block (Lanthanides and Actinides)

Warm UpWarm Up1.1. What are the three largest divisions within the What are the three largest divisions within the

periodic table?periodic table?

2.2. What are the characteristics of metals?What are the characteristics of metals?

3.3. What are the characteristics of non-metals?What are the characteristics of non-metals?

4.4. What are the characteristics of metalloids?What are the characteristics of metalloids?

5.5. What is the rule of thumb for metals?What is the rule of thumb for metals?

6.6. What is the rule of thumb for non-metals?What is the rule of thumb for non-metals?

7.7. State the octet rule?State the octet rule?

Categories of ElementsCategories of Elements

MetalsMetals - hard and shiny; conduct electricity - hard and shiny; conduct electricity

NonmetalsNonmetals - gases or brittle solids; good - gases or brittle solids; good insulatorsinsulators

MetalloidsMetalloids - properties of both metals and - properties of both metals and nonmetalsnonmetals

Rule of Thumb:Rule of Thumb:

Metals have 1-3 electrons in outer levelMetals have 1-3 electrons in outer level

Nonmetals have >5 electrons in the outer levelNonmetals have >5 electrons in the outer level

The Octet RuleThe Octet Rule

Eight electrons in the outer level render Eight electrons in the outer level render an atom essentially unreactivean atom essentially unreactive

Rule of Thumb:Rule of Thumb:

An atom having a filled or half filled An atom having a filled or half filled sublevel is slightly more stable (less sublevel is slightly more stable (less reactive) than an atom without a filled or reactive) than an atom without a filled or half-filled sublevel.half-filled sublevel.

Relative Atomic StabilityRelative Atomic Stability

Decreasing order of stabilityDecreasing order of stability

Full outer shell (sFull outer shell (s2 2 and pand p66))

Full sublevel (sFull sublevel (s22))

Half-filled sublevelHalf-filled sublevel

No special arrangementNo special arrangement

Electron Sublevel StructureElectron Sublevel Structure

If the last electron for an atom is in a full or If the last electron for an atom is in a full or half-full sublevel, then the atom is half-full sublevel, then the atom is inherently more stable. inherently more stable.

Periodic PropertiesPeriodic Properties

Atomic RadiiAtomic Radii

Ionic Radii Ionic Radii

First Ionization EnergyFirst Ionization Energy

Electronegativity Electronegativity

----------------------------------------------------------

Electron AffinityElectron Affinity

Oxidation NumbersOxidation Numbers

Warm UpWarm Up1.1. What happens to atomic radius as you go down the periodic What happens to atomic radius as you go down the periodic

table?table?

2.2. What is ionization energy?What is ionization energy?

3.3. As atomic number increases in a period, what happens to As atomic number increases in a period, what happens to ionization energy?ionization energy?

4.4. As atomic number increases in a group, what happens to As atomic number increases in a group, what happens to ionization energy?ionization energy?

5.5. List three factors that affect ionization energy?List three factors that affect ionization energy?

6.6. Define electronegativity?Define electronegativity?

7.7. What happens to electronegativity as you move left to right What happens to electronegativity as you move left to right across the periodic table?across the periodic table?

8.8. What happens to electronegativity as you move top to bottom What happens to electronegativity as you move top to bottom across the periodic table?across the periodic table?

Atomic RadiusAtomic Radius

As the principal quantum number (n) increases, the size As the principal quantum number (n) increases, the size of the electron cloud increases. That is, the atomic of the electron cloud increases. That is, the atomic size increases as you size increases as you go down the tablego down the table..

The reason for this is that you are The reason for this is that you are adding energy levelsadding energy levels as you go down the table (1, 2, 3,...).as you go down the table (1, 2, 3,...).

The positive charge of the nucleus increase as you go The positive charge of the nucleus increase as you go from from left to rightleft to right across the table. This increase in across the table. This increase in nuclear charge increases the pull on the electron nuclear charge increases the pull on the electron cloud by the nucleus - pulling the the electron cloud cloud by the nucleus - pulling the the electron cloud in tighter to the nucleus. Thus, the atoms decrease in in tighter to the nucleus. Thus, the atoms decrease in size.size.

Ionic RadiiIonic Radii

Metallic IonsMetallic IonsFormed by the Formed by the lossloss of electrons of electronsSmaller than the atoms from which they Smaller than the atoms from which they

were formedwere formed

Nonmetallic IonsNonmetallic IonsFormed by the Formed by the gaingain of electrons of electronsLarger than the atoms from which they were Larger than the atoms from which they were

formedformed

First Ionization EnergyFirst Ionization Energy

The energy required to remove the most loosely-held The energy required to remove the most loosely-held electron from a neutral atom. electron from a neutral atom.

Increases as atomic number increases in any period. Increases as atomic number increases in any period.

Decreases as the atomic number increases in any Decreases as the atomic number increases in any group.group.

Affected by:Affected by:Shielding EffectShielding EffectRadius of the atomRadius of the atomNuclear ChargeNuclear ChargeElectron Sublevel StructureElectron Sublevel Structure

Factors Affecting Ionization EnergyFactors Affecting Ionization Energy

Nuclear ChargeNuclear Charge - ionization energy is proportional to - ionization energy is proportional to the nuclear chargethe nuclear charge

Shielding EffectShielding Effect - Ionization energy is inversely - Ionization energy is inversely proportional to the shielding effect proportional to the shielding effect

RadiusRadius - Ionization energy is inversely proportional to - Ionization energy is inversely proportional to the distance between the nucleus and the outer the distance between the nucleus and the outer electrons electrons

SublevelSublevel - an electron from a full or half-full sublevel - an electron from a full or half-full sublevel requires additional energy to be removedrequires additional energy to be removed

Metals - LowMetals - Low ionization energyionization energyNonmetals - High ionization energyNonmetals - High ionization energy


Electronegativity indicates the ability of an Electronegativity indicates the ability of an element’s atom to attract electrons in a element’s atom to attract electrons in a chemical bond.chemical bond.


Influenced by the same factors which affect Influenced by the same factors which affect ionization energy and electron affinity ionization energy and electron affinity

Size Size Shielding effect Shielding effect Nuclear charge Nuclear charge

The Trends (in the Periodic Table) are the same The Trends (in the Periodic Table) are the same

increases from left to right increases from left to right

increases from bottom to top increases from bottom to top


The most active metals have the lowest The most active metals have the lowest electronegativityelectronegativity

The most active nonmetals have the highest The most active nonmetals have the highest electronegativityelectronegativity

Nuclear ChargeNuclear Charge

As the positive charge of the nucleus As the positive charge of the nucleus increases, it becomes increasingly increases, it becomes increasingly harder to remove an electron from an harder to remove an electron from an outer shellouter shell

Tends to Tends to raiseraise the First Ionization Energy the First Ionization Energy

Shielding EffectShielding Effect

The effect when “inner” electrons block the The effect when “inner” electrons block the attraction of the nucleus for the outer attraction of the nucleus for the outer electronselectrons

Tends to Tends to lowerlower the First Ionization Energy the First Ionization Energy

RadiusRadius

Ionization energy is inversely proportional to the Ionization energy is inversely proportional to the distance between the nucleus and the outer distance between the nucleus and the outer electrons electrons

Tends to Tends to lowerlower the First Ionization Energy the First Ionization Energy

SublevelSublevel

An electron from a full or half-full sublevel requires An electron from a full or half-full sublevel requires additional energy to be removedadditional energy to be removed

If a sublevel is full or half-filled, then this tends to If a sublevel is full or half-filled, then this tends to raise the First Ionization Energyraise the First Ionization Energy

Electron AffinityElectron Affinity

The attraction an The attraction an isolatedisolated atom has for an atom has for an additional electronadditional electron

Shows the same trend as First Ionization Shows the same trend as First Ionization Energy (increases from left to right, and Energy (increases from left to right, and decreases from the top down).decreases from the top down).

Oxidation NumbersOxidation Numbers

Group 1Group 1 lose 1 electron lose 1 electron +1+1

Group 2 Group 2 lose 2 electrons lose 2 electrons +2+2

Group 3-12 Group 3-12 multiple gain/loss multiple gain/loss

Group 13 Group 13 lose 3 electrons lose 3 electrons +3+3

Group 14 Group 14 lose/gain 2,4 electronslose/gain 2,4 electrons ±4, +2±4, +2

Group 15 Group 15 gain 3 electrons gain 3 electrons -3-3

Group 16 Group 16 gain 2 electrons gain 2 electrons -2-2

Group 17 Group 17 gain 1 electron gain 1 electron -1-1

Group 18 Group 18 stable stable 00

LEO says GERLEO says GER

Warm UpWarm Up

1.1. What is the oxidation number for group 1?What is the oxidation number for group 1?







8.8. Name the following groups: 1, 2, 16,17 and 18.Name the following groups: 1, 2, 16,17 and 18.

Web ActivityWeb Activity

http://www.learner.org/http://www.learner.org/interactives/periodic/interactives/periodic/groups_interactive.htmlgroups_interactive.html

The Periodic Table Periodicity Unit IV Ch. 6. Pictionary Words Period Atomic radius Group Transition...

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