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Ch 5Ch 5

Periodic TablePeriodic Table

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PeriodsPeriods

Rows are called periods. Rows are called periods. Period number indicates the highest Period number indicates the highest

occupied energy level of the electrons. occupied energy level of the electrons. The two named periods are the lanthanide The two named periods are the lanthanide

and actinide series found at the bottom of and actinide series found at the bottom of the periodic table.the periodic table.

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Lanthanide and Actinide SeriesLanthanide and Actinide Series

These two periods of elements are broken These two periods of elements are broken apart from the rest due to the fact that are apart from the rest due to the fact that are man-made. man-made.

Lanthanides are shiny metals that are not Lanthanides are shiny metals that are not very reactive. very reactive.

Actinides are all radioactive metals and Actinides are all radioactive metals and are somewhat reactive.are somewhat reactive.

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Groups Groups

Columns are called groups.Columns are called groups.Each group consists of a specific family of Each group consists of a specific family of

elements that share similar properties.elements that share similar properties.These families includeThese families include

AlkaliAlkaliAlkalineAlkalineTransitionTransitionHalogenHalogenNoble gas Noble gas

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Alkali FamilyAlkali Family

Alkali metals belong to group 1.Alkali metals belong to group 1.They are soft, silvery metals with a low They are soft, silvery metals with a low

melting point. melting point. They are the most reactive metal group. They are the most reactive metal group. Their normal state of matter is solid.Their normal state of matter is solid.

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Alkaline FamilyAlkaline Family

Alkaline metals belong to group 2.Alkaline metals belong to group 2.They are harder, denser, and have a They are harder, denser, and have a

higher melting than alkali metals.higher melting than alkali metals.They are only slightly less reactive. They are only slightly less reactive. Their normal state of matter is solid.Their normal state of matter is solid.

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Transition FamilyTransition Family

Transition metals belong to group 3-12. Transition metals belong to group 3-12. They have typical metal properties such as They have typical metal properties such as

a very high luster and good conduction.a very high luster and good conduction.They are so unreactive that they normally They are so unreactive that they normally

exist in nature as lone elements. exist in nature as lone elements. Their normal state of matter is solid.Their normal state of matter is solid.

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Halogen FamilyHalogen Family

Halogens belong to group 17.Halogens belong to group 17.They are the most reactive nonmetal They are the most reactive nonmetal

group.group.They typically react with metals to form They typically react with metals to form

salts.salts.The normal states of these elements The normal states of these elements

include two solids, one liquid, and two include two solids, one liquid, and two gases. gases.

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Noble Gas FamilyNoble Gas Family

Noble gases belong to group 18.Noble gases belong to group 18.They are unreactive nonmetals.They are unreactive nonmetals.They normally exist in nature as lone They normally exist in nature as lone

elements.elements.Their normal state of matter is gas.Their normal state of matter is gas.

1111

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TrendsTrends The periodic table is arranged in a very organized way The periodic table is arranged in a very organized way

with distinct patterns. It can offers many clues that may with distinct patterns. It can offers many clues that may be helpful through this class.be helpful through this class.

Some of the periodic trends include:Some of the periodic trends include: Valence electronsValence electrons Oxidation numbersOxidation numbers ReactivityReactivity Sates of matterSates of matter Metallic propertiesMetallic properties Energy level blocksEnergy level blocks Ionization energyIonization energy Atomic radiiAtomic radii Ionic radiiIonic radii ElectronegativityElectronegativity

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Valence ElectronsValence Electrons

Valence electrons are the outer electrons Valence electrons are the outer electrons available to be lost, gained, or shared available to be lost, gained, or shared when bonding.when bonding.

The last digit in the group number The last digit in the group number indicates the number of valence electrons.indicates the number of valence electrons.

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Oxidation NumbersOxidation Numbers Oxidation number Oxidation number is the number assigned to an atom in is the number assigned to an atom in

an ionic compound. an ionic compound. It indicates the number of electrons and how the It indicates the number of electrons and how the

electrons are used while bonding.electrons are used while bonding. It proceeds across the groups starting at group 1, It proceeds across the groups starting at group 1,

skipping over transition elements, and ending at group skipping over transition elements, and ending at group 18.18.

The numbers are: +1, +2, +3, +4, -3, -2, -1, 0.The numbers are: +1, +2, +3, +4, -3, -2, -1, 0. Elements with positive oxidation numbers lose the Elements with positive oxidation numbers lose the

specified amount of electrons to form positive cations.specified amount of electrons to form positive cations. Elements with negative oxidation numbers gain the Elements with negative oxidation numbers gain the

specified amount of electrons to form negative anions.specified amount of electrons to form negative anions.

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ReactivityReactivity

Reactivity increases as you go down a Reactivity increases as you go down a metallic group.metallic group.

Reactivity decreases as you go down a Reactivity decreases as you go down a nonmetallic group.nonmetallic group.

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States of MatterStates of Matter

With the exception of hydrogen, solids are With the exception of hydrogen, solids are located on the left of the periodic table and located on the left of the periodic table and gases on the right.gases on the right.

The only two liquids are mercury (a liquid The only two liquids are mercury (a liquid metal) and bromine (a liquid nonmetal).metal) and bromine (a liquid nonmetal).

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Metallic PropertiesMetallic Properties

There is a stair step line that divides the There is a stair step line that divides the periodic table into metals and nonmetals.periodic table into metals and nonmetals.

Everything to the left of the line is a metal Everything to the left of the line is a metal and everything to the right is a nonmetal.and everything to the right is a nonmetal.

With the exception of aluminum (a metal), With the exception of aluminum (a metal), everything touching the line is a metalloid.everything touching the line is a metalloid.

A metalloid shares characteristics of both A metalloid shares characteristics of both metals and nonmetals and exist as very metals and nonmetals and exist as very brittle solids.brittle solids.

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Energy Level BlocksEnergy Level Blocks Groups are divided into blocks based on Groups are divided into blocks based on sublevelssublevels. .

There is an s-block, p-block, d-block, and f-block.There is an s-block, p-block, d-block, and f-block. S-block is group 1 and 2. Group 1 electron S-block is group 1 and 2. Group 1 electron

configurations end with nsconfigurations end with ns11, group 2 end with ns, group 2 end with ns22. . P-block is group 13 through 18. Electron configurations P-block is group 13 through 18. Electron configurations

proceed as npproceed as np11, np, np22, np, np33, np, np44, np, np55, and np, and np66.. The n in each electron configuration indicates the main The n in each electron configuration indicates the main

energy level and can be found from the period number.energy level and can be found from the period number. D-block is group 3-12. At this block electron D-block is group 3-12. At this block electron

configuration rules have to be followed closely and there configuration rules have to be followed closely and there is no general trend.is no general trend.

F-block does not belong to any groups. Rather, it F-block does not belong to any groups. Rather, it belongs to period 8 and 9, the lanthanide and actinide belongs to period 8 and 9, the lanthanide and actinide series. series.

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Blue= s blockYellow= p blockRed= d blockGreen= f block

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Ionization EnergyIonization Energy

Ionization energy is the energy required to Ionization energy is the energy required to remove one electron from a neutral atom remove one electron from a neutral atom to form an ion.to form an ion.

The trends are:The trends are: Increase across a period Increase across a period Decrease down a group Decrease down a group IE increases with each successive ionizationIE increases with each successive ionization

2222

ElectronegativityElectronegativity

ElectronegativityElectronegativity is a measure of the ability is a measure of the ability of an atom to attract electrons.of an atom to attract electrons.

The trends are:The trends are: Increase across periodIncrease across periodDecrease down a groupDecrease down a group

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Atomic RadiiAtomic Radii

Atomic radii is a measurement of half the Atomic radii is a measurement of half the distance between the nuclei of two distance between the nuclei of two identical atoms that are bonded.identical atoms that are bonded.

The trends are:The trends are:Decrease across a period Decrease across a period Increases down a group Increases down a group

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Ionic RadiiIonic Radii

Ionic radii is the radius of an ion formed by the Ionic radii is the radius of an ion formed by the element.element.

Group 1-14 have positive oxidation numbers and Group 1-14 have positive oxidation numbers and therefore lose electrons to form cations.therefore lose electrons to form cations.

Formation of a positive cation causes decrease Formation of a positive cation causes decrease in size from atomic radii. in size from atomic radii.

Group 15-18 have negative oxidation numbers Group 15-18 have negative oxidation numbers and therefore gain electrons to form anions.and therefore gain electrons to form anions.

Formation of a negative anion cause increase in Formation of a negative anion cause increase in size from atomic radii.size from atomic radii.