The Periodic Table

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History

• The Periodic Table

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• Memorize the periodic table by Monday
• History of the periodic table

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Newlsands

• John Newlands (1837, English)
• Law of Octaves (every 8th element was grouped
  together)
• Ordered elements by atomic mass

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Mendeleev

• Dmitri Mendeleev (1869, Russian)
• Also organized elements by increasing atomic
  mass.
• Elements with similar properties were grouped
  together.

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Mendeleev

• Dmitri Mendeleev (1869, Russian)
• Predicted properties of undiscovered elements.

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Moseley

• Henry Mosely (1913, British)
• Organized elements by increasing atomic number.
• Resolved discrepancies in Mendeleevs
  arrangement.
• This is the way the current Periodic Table is
  arranged.

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Organization of theElements

• The Periodic Table

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Metallic Character

• Metals
• Nonmetals
• Metalloids

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Metals

• Most of the periodic table is made of metals!
• Form positive ions
• Metals are good conductors of heat and
  electricity
• Metals are malleable
• Metals are ductile
• Metals have high tensile strength
• Metals have luster

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Examples of Metals
Potassium, K reacts with water and must be stored
in kerosene
Copper, Cu, is a relatively soft metal, and a
very good electrical conductor.
Zinc, Zn, is more stable than potassium
Mercury, Hg, is the only metal that exists as a
liquid at room temperature
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Properties of Nonmetals

• Nonmetals are poor conductors of heat and
  electricity
• Nonmetals tend to be brittle
• Many nonmetals are gases at room
  temperature

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Examples of Nonmetals
Microspheres of phosphorus, P, a reactive
nonmetal
Sulfur, S, was once known as brimstone
Graphite is not the only pure form of carbon, C.
Diamond is also carbon the color comes from
impurities caught within the crystal structure
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Properties of Metalloids
Metalloids straddle the border between metals and
nonmetals on the periodic table.

• They have properties of both metals and
  nonmetals.
• Metalloids are more brittle than metals, less
  brittle than most nonmetallic solids
• Metalloids are semiconductors of electricity
• Some metalloids possess metallic luster

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Silicon, Si A Metalloid

• Silicon has metallic luster
• Silicon is brittle like a nonmetal
• Silicon is a semiconductor of electricity

Other metalloids include

• Boron, B
• Germanium, Ge
• Arsenic, As
• Antimony, Sb
• Tellurium, Te

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Metals vs. Nonmetals
Metals Nonmetals
Luster High-shiny Dull
Conductor Good for heat and electricity poor
Malleable Yes-hammered into sheets No-brittle
Ductile Yes-pulled into wires No-brittle
Melting point High Low
Density High low
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Chemical Reactivity

• Families
• Similar valence e- within a group result in
  similar chemical properties

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Chemical Reactivity

• Alkali Metals
• Alkaline Earth Metals
• Transition Metals
• Halogens
• Noble Gases

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Blocks

• Main Group Elements (s p blocks)
• Transition Metals (d block)
• Inner Transition Metals (f block)

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Periodic Trends

• The Periodic Table

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Periodic Law

• When elements are arranged in order of increasing
  atomic , elements with similar properties appear
  at regular intervals.

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Other Properties

• Atomic Radius
• size of atom

• First Ionization Energy
• Energy required to remove one e- from a neutral
  atom.

• Melting/Boiling Point

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Atomic Radius

• Atomic Radius

K
Na
Li
Ar
Ne
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Atomic Radius

• Atomic Radius

• Increases to the LEFT and DOWN

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Atomic Radius

• Why larger going down?
• Higher energy levels have larger orbitals
• Shielding - core e- block the attraction between
  the nucleus and the valence e-
• Why smaller to the right?
• Increased nuclear charge without additional
  shielding pulls e- in tighter

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Ionization Energy

• First Ionization Energy

He
Ne
Ar
Li
Na
K
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Ionization Energy

• First Ionization Energy

• Increases UP and to the RIGHT

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Ionization Energy

• Why opposite of atomic radius?
• In small atoms, e- are close to the nucleus where
  the attraction is stronger
• Why small jumps within each group?
• Stable e- configurations dont want to lose e-

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Ionization Energy

• Successive Ionization Energies

• Large jump in I.E. occurs when a CORE e- is
  removed.

• Mg 1st I.E. 736 kJ
• 2nd I.E. 1,445 kJ
• Core e- 3rd I.E. 7,730 kJ

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Ionization Energy

• Successive Ionization Energies

• Large jump in I.E. occurs when a CORE e- is
  removed.

• Al 1st I.E. 577 kJ
• 2nd I.E. 1,815 kJ
• 3rd I.E. 2,740 kJ
• Core e- 4th I.E. 11,600 kJ

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Melting/Boiling Point

• Melting/Boiling Point

• Highest in the middle of a period.

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Ionic Radius

• Ionic Radius

• Cations ()
• lose e-
• smaller

• Anions ()
• gain e-
• larger

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Examples

• Which atom has the larger radius?

• Be or Ba
• Ca or Br

Ba Ca
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Examples

• Which atom has the higher 1st I.E.?

• N or Bi
• Ba or Ne

N Ne
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Examples

• Which atom has the higher melting/boiling point?

• Li or C
• Cr or Kr

C Cr
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Examples

• Which particle has the larger radius?

• S or S2-
• Al or Al3

S2- Al
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Chinese Periodic Table
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Periodic Table
Hydrogen most abundant gas in the universe, 1
valence electron, often exists as a single proton.
Transition Metals multiple charges, bright
colored, used in building, coins, and jewelry
Alkaline Earth Metals 2 valence electrons, 2 ion
Halogens Salt formers, 7 valence electrons,
-1 ion, most reactive nonmetals
Noble Gases all have full valence shell of 8
electrons, except He which has 2. Inert
(unreactive) gases.
Alkali Metals 1 valence electron, forms 1 ion,
most reactive metals, combine with halogens to
form salts. Soft silvery white. Most reactive is
at the bottom.
Rare Earth or Inner Transition Metals Many
synthetic, rare, or radioactive elements.
Divided into Lanthanides and Actinides