Periodic Table Study Guide 8 th Grade Mrs. Jenkins How to Draw Lewis Structures.
Unit 3: The Periodic Table - Mrs. Rhee Science
Transcript of Unit 3: The Periodic Table - Mrs. Rhee Science
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Unit 3: The Periodic Table
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The Periodic Law:
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The Periodic Law:When the elements are arranged by increasing atomic number,
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The Periodic Law:When the elements are arranged by increasing atomic number, there is a periodic repetition of their chemical and physical properties.
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Dmitri Mendeleev (1834-1907)
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Dmitri Mendeleev (1834-1907)
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Dmitri Mendeleev (1834-1907)∙ First to notice the element's periodic repetition of properties.
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Dmitri Mendeleev (1834-1907)∙ First to notice the element's periodic repetition of properties.∙ Designed the first periodic table (in 1869)
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Today's Modern Periodic Table
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Today's Modern Periodic Table(see back inside cover of text)
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Wall Poster:
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See Handout,The Divided Periodic Table
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Periods:Horizontal rows, numbered 1-7.
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Families (or Groups):
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Families (or Groups):Vertical columns, numbered 1-18
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Families (or Groups):Vertical columns, numbered 1-18(also 1A - 8 A)
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Family Names"
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Family Names" 1" Alkali metals (not hydrogen)
"
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Family Names" 1" Alkali metals" 2 " Alkaline earth metals"
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Family Names" 1" Alkali metals" 2 " Alkaline earth metals" 3-12 " The transition metals"
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Family Names" 1" Alkali metals" 2 " Alkaline earth metals" 3-12 " The transition metals" 13 " The Boron family"
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Family Names" 1" Alkali metals" 2 " Alkaline earth metals" 3-12 " The transition metals" 13 " The Boron family" 14 " The Carbon family"
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Family Names" 1" Alkali metals" 2 " Alkaline earth metals" 3-12 " The transition metals" 13 " The Boron family" 14 " The Carbon family" 15 " The Nitrogen family"
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Family Names" 1" Alkali metals" 2 " Alkaline earth metals" 3-12 " The transition metals" 13 " The Boron family" 14 " The Carbon family" 15 " The Nitrogen family" 16 " The Oxygen family"
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" 17 " The Halogens"
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" 17 " The Halogens" 18 " The Noble Gases
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Semimetals(semiconductors or metalloids):
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Semimetals (or metalloids):Elements that have properties of both metals and nonmetals.
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Metals:
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Metals:Those elements that are a good conductors of heat or electricity and generally shiny;
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Metals:Those elements that are a good conductors of heat or electricity and generally shiny; most are solid, ductile, and malleable.
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Nonmetals:
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Nonmetals:Those elements that are generally gasses or dull, brittle solids and are poor conductors of heat and electricity.
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The Inner Transition Metals:
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The Inner Transition Metals:
Elements 58-71are called the Lanthanide series
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The Inner Transition Metals:
Elements 58-71are called the Lanthanide series
Elements 90-103 are called the Actinide series
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The Periodic Table can be broken into s, p, d, and f blocks,
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The Periodic Table can be broken into s, p, d, and f blocks, corresponding directly with the predictions made by quantum mechanics.
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By knowing an element's location on the Periodic Table, its electron configuration can be easily determined.
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Valence Electrons
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Valence Electrons (p152)•Responsible for an atom's chemical properties.
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Valence Electrons (p152)•Responsible for an atom's chemical properties.
•Are lost, gained, or shared to form chemical bonds.
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•Only found in the outermost energy level of an atom... therefore,
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•Only found in the outermost energy level of an atom... therefore, only belong to the outermost and sublevels.
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•Only found in the outermost energy level of an atom... therefore, only belong to the outermost s and p sublevels.
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•Only found in the outermost energy level of an atom... therefore, only belong to the outermost s and p sublevels.
Making the maximum number of valence electrons any atom can have...
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•Only found in the outermost energy level of an atom... therefore, only belong to the outermost s and p sublevels.
Making the maximum number of valence electrons any atom can have... 8 !
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The numbering 1A - 8A is used to indicate the number of valence electrons in those families.
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The numbering 1A - 8A is used to indicate the number of valence electrons in those families.
Therefore the transition elements all have only 2 valence electrons!
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Valence Shell:
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Valence Shell: The region of space occupied by an atom's valence electrons.
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The Octet Rule
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The Octet RuleAtoms tend to lose, gain, or share electrons to obtain a
"stable octet."
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The Octet RuleAtoms tend to lose, gain, or share electrons to obtain a
"stable octet."
(The configurationof a noble gas!)
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Ionic Charge overview:
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Ionic Charge overview:
Metals lose valence electrons to become positive ions ("cations").
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Ionic Charge overview:
Metals lose valence electrons to become positive ions ("cations").
Nonmetals and semimetalsusually gain valence electrons to become negative ions ("anions")
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Ionic Charge Trend:
Family" Charge
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Ionic Charge Trend:
Family" ChargeAlkali metals" +1
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Ionic Charge Trend:
Family" ChargeAlkali metals" +1" "Alkaline earth metals" +2
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Ionic Charge Trend:
Family" ChargeAlkali metals" +1" "Alkaline earth metals" +2Boron" +3
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Ionic Charge Trend:
Family" ChargeAlkali metals" +1" "Alkaline earth metals" +2Boron" +3Carbon (nonmetals)" -4
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Ionic Charge Trend:
Family" ChargeAlkali metals" +1" "Alkaline earth metals" +2Boron" +3Carbon (nonmetals)" -4Nitrogen (nonmetals)" -3
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Ionic Charge Trend:
Family" ChargeAlkali metals" +1" "Alkaline earth metals" +2Boron" +3Carbon (nonmetals)" -4Nitrogen (nonmetals)" -3
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Ionic Charge Trend:
Family" ChargeAlkali metals" +1" "Alkaline earth metals" +2Boron" +3Carbon (nonmetals)" -4Nitrogen (nonmetals)" -3Oxygen (nonmetals)" -2
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Ionic Charge Trend:
Family" ChargeAlkali metals" +1" "Alkaline earth metals" +2Boron" +3Carbon (nonmetals)" -4Nitrogen (nonmetals)" -3Oxygen (nonmetals)" -2Halogens" -1
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Ionic Charge Trend:
Family" ChargeAlkali metals" +1" "Alkaline earth metals" +2Boron" +3Carbon (nonmetals)" -4Nitrogen (nonmetals)" -3Oxygen (nonmetals)" -2Halogens" -1Noble Gases" 0
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Diatomic Elements:
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Diatomic Elements: Elements that are found in nature as pairs of atoms; two identical atoms bonded together.
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The Super Seven: H2 , N2 , O2 , F2 , Cl2, Br2 , and I2
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Periodic Properties (Section 5.3)
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Periodic Properties (Section 5.3)
Atomic Radius: the distance from the center of an atom's nucleus to its outermost electron.
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Periodic Properties (Section 5.3)
Atomic Radius: the distance from the center of an atom's nucleus to its outermost electron.
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(See Figure 3.2, page 143)
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Trend:
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Trend:
Increases as you move down a family (electrons added to higher energy levels)
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Trend:
Increases as you move down a family (electrons added to higher energy levels) Decreases as you move across a period (due to the increase in nuclear charge)
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Ionic Radius (figure 3.9, see p151)
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Ionic Radius:
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Trend:
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Trend:
Increases as electrons are added (anions)
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Trend:
Increases as electrons are added (anions)
Decreases as electrons are lost (cations)
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Ionization Energy: energy required
to remove the outermost electrons
from a gaseous atom.
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Ionization Energy: energy required to remove the outermost electron from a *gaseous atom.
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Ionization Energy: energy required to remove the outermost electron from a *gaseous atom.
*a single, isolated atom.
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Ionization Energy: energy required to remove the outermost electron from a *gaseous atom.(Turns the atom into a positive ion.)
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Ionization Energy: energy required to remove the outermost electron from a *gaseous atom.(Turns the atom into a positive ion.)
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(See Page 146)
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Trend:Increases as you move across a period
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Trend:Increases as you move across a period (because the atoms get smaller!)
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Trend:Increases as you move across a period (because the atoms get smaller!)
Decreases as you move down a family
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Trend:Increases as you move across a period (because the atoms get smaller!)
Decreases as you move down a family (because the atoms get larger!)
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(See figure 3.6, page 147)
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(See figure 3.6, page 147)
It takes a great deal more energyto remove a core electron!!!
There will be a huge jump in ionizationenergy when removing these!
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Electronegativity:
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Electronegativity: ability of an atom to attract electrons in a chemical bond.
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Electronegativity: ability of an atom to attract electrons in a chemical bond.
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(See Figure 3.11, page 153)
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Trend:Increases as you move across a period
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Trend:Increases as you move across a period (because the atoms get smaller!)
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Trend:Increases as you move across a period (because the atoms get smaller!)
Decreases as you move down a family
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Trend:Increases as you move across a period (because the atoms get smaller!)
Decreases as you move down a family (because the atoms get larger!)
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Shielding effect:
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Shielding effect:The repulsive force exerted on valence electrons by core electrons.
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Shielding effect:The repulsive force exerted on valence electrons by core electrons. -
- lowers ionization energy
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Shielding effect:The repulsive force exerted on valence electrons by core electrons. -
- lowers ionization energy - lowers electronegativity
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Shielding effect:The repulsive force exerted on valence electrons by core electrons. -
- lowers ionization energy - lowers electronegativity - increases atomic radius