The Periodic Table

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The Periodic Table

• Chapter 5

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Alchemy Diderot's Alchemical Chart of
Affinities (1778)
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Dalton's elements and symbols (1808)
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The Bayley Pyramid Periodic Table
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Mohammed Abubakr's circular periodic table is one
alternative to the standard periodic table of the
elements.
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A Spiral Periodic Table by Prof. Thoedor Benfey
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Spiral Periodic Table
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The Dufour Periodictree
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AtomFlowers A periodic table that gives a
representation of the electron orbitals that look
like flowers
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Chinese periodic table
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Chapter 5 section 1pg 126-129
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Organizing the Elements

• 1750 17 elements known
• Mostly common metals
• After 1750, more chemists begin to study elements
  ?many more elements discovered faster
• Needed a way to organize elements
• 1789 Antoine Lavoisier grouped elements based on
  type
• Metals, nonmetals, gases earths
• 1860 Mendeleev

• What was going on in history during this time?
• Why is this organization limited?

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Mendeleevs Periodic Table

• Organized elements like a deck of cards
• 1st ? order by mass
• 2nd ? property patterns
• esp. rxns with O H

• Draw an example of ordering strategy

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A
2
4
5
6
8
7
9
10
Q
J
K
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Mendeleevs Periodic Table

• Organized elements like a deck of cards
• 1st ? order by mass
• 2nd ? property patterns
• esp. rxns with O H
• Rows (called periods)
• Mass increases from left to right
• Columns (called groups)
• Mass increases from top to bottom
• Similar properties

• Draw an example of ordering strategy
• Draw a small periodic table to illustrate rows
  and columns

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groups
periods
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Mendeleevs Periodic Table

• Left blanks for elements not discovered yet
• Why remember Mendeleev if he wasnt the first to
  come up with a P.T.?
• Best organization strategy
• Used to make accurate predictions about what
  elements were yet to be discovered

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Mendeleevs Periodic Table

• EX Gallium
• Predicted similar properties to aluminum
• Soft metal
• Low melting point
• Density 5.9 g/cm3
• Truth about gallium
• Soft metal
• Melting pt 29.7C
• Density 5.91 g/cm3
• Further proof his PT was good
• Discovery of scandium and germanium

Would gallium be a solid, liquid or gas at
room temperature (20-22C)?
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Check your understanding

• Pg 126 reading strategy
• Pg 127 figure 3
• Pg 129 figure 4 (already done ?)
• Pg 129 assessment, 1-8

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REMINDER!!!

• Open note reading quiz

WARNING
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Chapter 5 section 2pg 130-138
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5.2

• More on Mendeleev (note 1860)
• Did not know about protons
• Did not know that all atoms in an element have
  the same of protons
• His PT arranged by mass, ours by atomic

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5.2

• Periods
• Rows (side-to-side)
• of periods of electron energy levels
• Groups
• Columns (up-and-down)
• Similar properties
• Similar electron configuration
• Determines chemical properties

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5.2

• Atomic mass
• given on PT is an average of the elements
  isotope masses
• Weighted avg.s
• Atomic mass avg. mass of isotopes compared to
  how common they are
• AMU
• Atomic Mass Unit
• Unit of mass for atoms (like grams but much
  smaller!)

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5.2

• Classes of Elements
• Solid, liquid, gas ? dependant on temp.
• Occur naturally vs. those that do not
  (man-made)
• Metals, nonmetals, metalloids

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5.2

• Metals
• Most elements are metals (75!)
• Physical properties
• Good conductors
• Solids at room temp. (except for Hg)
• Malleable
• ductile
• Chemical properties
• Some are reactive, others are not
  (to rust or not to rust?)

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5.2

• Special Metals
• Transition metals
• Chemical properties
• Form compounds with distinctive colors
• Lanthanide actinide series

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5.2

• Nonmetals
• Physical properties
• Poor conductors
• Brittle
• Most are gasses at room temp. (low bp)
• Chemical properties
• Vary ? some very reactive, others not at all
• Most reactive group 17
• Least reactive group 18

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5.2

• Metalloids
• Physical properties
• Conductivity varies with temp.
• Semi-conductors ? computer chips
  ? Silicon Valley

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Chapter 5 section 3pg 139-149
Part I pg 139 ions Part II pg 140-145 Part
III pg 146-149
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5.3 Part I

• Valence electrons
• Electrons in the outermost energy level
• Chemical properties depend on the number of
  valence electrons
• What does this mean after learning about the
  organization of the PT?
• Groups have similar properties so they must also
  have similar s of valence electrons

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5.3 Part I

• Octet
• magic in chemistry
• Valence orbitals can hold no more than 8 e-
• All atoms want a full valence (8 e-) or none (all
  or nothing)
• Exceptions H He

Why?
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5.3 Part I

• Ions
• Atoms that gain or loose e- to fill or empty the
  valence orbital

1p
1
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5.3 Part I

• Ions
• Atoms that gain or loose e- to fill or empty the
  valence orbital

2p
Ø
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5.3 Part I

• Ions
• Atoms that gain or loose e- to fill or empty the
  valence orbital

3p
1
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5.3 Part I

• Ions
• Atoms that gain or loose e- to fill or empty the
  valence orbital

4p
2
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5.3 Part I

• Ions
• Atoms that gain or loose e- to fill or empty the
  valence orbital

5p
3
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5.3 Part I

• Ions
• Atoms that gain or loose e- to fill or empty the
  valence orbital

6p
4

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5.3 Part I

• Ions
• Atoms that gain or loose e- to fill or empty the
  valence orbital

6p
-4

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5.3 Part I

• Ions
• Atoms that gain or loose e- to fill or empty the
  valence orbital

7p
-3

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5.3 Part I

• Ions
• Atoms that gain or loose e- to fill or empty the
  valence orbital

8p
-2

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5.3 Part I

• Ions
• Atoms that gain or loose e- to fill or empty the
  valence orbital

9p
-1

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5.3 Part I

• Ions
• Atoms that gain or loose e- to fill or empty the
  valence orbital

10p
Ø

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5.3 Part I

• Ions
• Atoms that gain or loose e- to fill or empty the
  valence orbital

11p
1

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5.3 Part II

• Groups
• Alkali Metals
• Alkaline Earth Metals
• Transition Metals
• Boron Family
• Carbon Family
• Nitrogen Family
• Oxygen Family
• Halogens
• Noble Gases

• Group
• 1
• 2
• 3-12
• 13
• 14
• 15
• 16
• 17
• 18

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5.3 Part II

• For each group
• List the elements in that group
• How many valence electrons do they have?
• What kind of ions do they form?
• Are they reactive?
• What are some of their physical and chemical
  properties?
• Where are they found?
• What are they used for?

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5.3 Part III

• Elemental Friends Foes
• Add to your group list

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Transition Metals

• Groups 3-12

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Transition Metals

• 1st elements discovered
• Make colorful compounds
• Often used to tint/color glass
• Metals
• Good conductors
• Malleable
• Ductile
• Solids at room temp. (exception Hg)

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Transition Metals

• All ions are positively charged
• Valence electron s vary ?
  Type of ion formed varies
• Example Iron Fe2 and Fe3

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Transition Metals

• Most mined
• Many uses
• Wires
• Construction
• Decoration