The Periodic Table

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The Periodic Table
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Early Organization

• As early as the early Greeks, scientists wanted
  to organize.
• They separated matter into Earth, Air, Fire and
  Water.
• They even had more detail such as combinations.
• For example Earth and Fire Lava
• Check out the game Little Alchemy on GOOGLE you
  might like it.

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History of the Periodic Table

• In the 1700s scientists had identified only 30
  elements
• In the 1800s there were 60

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History of the Periodic Table

• Early 1800s Dobereiner grouped elements into
  triads
• Li, Na, K

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History of the Periodic Table

• 1865 J.A.R. Newlands discovered properties
  repeated themselves every eighth element
• Called these octaves

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Mendeleev

• 1869 Dmitri Mendeleev produced the first periodic
  table for his students
• Left blanks where elements had yet to be
  discovered
• Was organized by atomic weight as that was the
  standard at the time.

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Here is one of the early official versions of
Mendeleevs Periodic Chart
Notice it is in German, even though Mendeleev
was Russian.
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Properties of Germanium as Predicted by Mendeleev Properties of Germanium as Predicted by Mendeleev Properties of Germanium as Predicted by Mendeleev Properties of Germanium as Predicted by Mendeleev Properties of Germanium as Predicted by Mendeleev
Properties of Ekasilicon Predicted in 1871 Properties of Ekasilicon Predicted in 1871 Properties of Ekasilicon Predicted in 1871 Properties of Ekasilicon Predicted in 1871 Properties of Ekasilicon Predicted in 1871

Atomic weightDensity  Specific heatMelting pointOxide formula  Oxide density  Chloride formula  bp of chloride Atomic weightDensity  Specific heatMelting pointOxide formula  Oxide density  Chloride formula  bp of chloride 725.5 g/cm30.31 J/(C  g)Very highRO24.7 g/cm3RCl4100C 725.5 g/cm30.31 J/(C  g)Very highRO24.7 g/cm3RCl4100C
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Properties ofGermanium Predictedin 1871 Observed  in1886
Atomic weightDensity  Specific heatMelting pointOxide formula  Oxide density  Cl-1 formula  bp of chloride 725.5 g/cm30.31 J/(C  g)Very highRO24.7 g/cm3RCl4100C 72.35.47 g/cm30.32 J/(C  g)960CGeO24.70 g/cm3GeCl486C
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HenryMoseley

• In 1913 Moseley assigned elements atomic numbers
  and rearranged periodic table.

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Table Terms

• Periodic Law when arranged by increasing atomic
  number elements repeat similar chemical and
  physical properties
• Groups or Families are the columns on the
  periodic table
• Periods are the rows going across.

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Major Groups on the Periodic Table

• Alkali Metals
• Alkaline Earth Metals
• Transition Metals
• Boron Group
• Carbon Group
• Nitrogen Group

• Oxygen Group (Chalcogens)
• Halogens
• Noble Gases
• Actinide Series
• Lanthanide Series

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Metals, Nonmetals, and Metalloids
6.1
Check out Theodore Grays App The elements
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Metals, Nonmetals, and Metalloids
6.1
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Metals, Nonmetals, and Metalloids
6.1

• Metals, Metalloids, and Nonmetals in the Periodic
  Table

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Metals, Nonmetals, and Metalloids
6.1

• Metals, Metalloids, and Nonmetals in the Periodic
  Table

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Metals, Nonmetals, and Metalloids
6.1
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Metals

• Good Conductors of heat and electricity
• Luster Shiny
• Malleable pounded into thin sheets
• Ductile pulled into a wire
• Mercury is the only liquid metal at room temp

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Non-Metals

• Most are gases
• Solids are brittle (S P)
• Bromine is the only liquid nonmetal at room temp

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Metalloids

• Properties of metals and non-metals
• Semi conductors
• Make very good computer chips

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Atomic Radius

• Atomic radius is the distance from the atoms
  nucleus to its outer edge.
• In the same energy level, more protons exert a
  stronger pull towards the nucleus

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Showing the Trend of Atomic Size
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Which has larger atomic radius?

• Na or Rb
• P or Cl
• You can tell by looking at the chart and knowing
  the trend.

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Ionization Energy

• Ionization energy is the energy needed to remove
  one electron
• Na (g) ? Na1 (g) 1 e-1
• Metals are more likely to give up an electron
  than nonmetals.

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Trends in Ionization Energy
It is good to know that Fluorine has the highest
Ionization Energy
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Which has larger ionization energy?

• H or Cs
• Li or N

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Ionic Radius

• Ionic radius is the distance from the ions
  nucleus to its outer edge.
• Non-metal ions get larger with a negative charge
• Metal ions get smaller with a positive charge
• This is because more protons are pulling on fewer
  electrons

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Anions are going to be larger than the atom.
Cations are going to be smaller than the atom.
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Trends in Ionic Size

• Relative Sizes of Some Atoms and Ions

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Which of the following is larger?

• O or O-2
• K or K

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Any Questions????
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Electronegativity

• Electronegativity reflects an atoms ability to
  attract electrons
• Cs Fr have the lowest electronegativities F
  has the highest

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Reactivity of Alkali and Alkaline Earth Metals

• Metals become more reactive as you move down the
  group
• Metals become less active when moving left to
  right

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Why Are There Patterns ?

• Elements have physical and chemical properties
  based upon their valence electrons.
• Valence electrons are the electrons in the outer
  most energy level (s p orbitals).
• The number of valence electrons may be determined
  by using the periodic table.

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Why Are There Patterns?

• When you look at an atom you are observing the
  valence electrons
• Duet rule - only 2 electrons fill the first
  energy level
• Octet rule 8 valence electrons is considered to
  be a full set

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Electron Affinity

• Electron affinity is the energy change that
  occurs when an atom gains an electron.
• F (g) e-1 ? F-1 (g)
• Most atoms give off energy when an electron is
  gained (negative).
• Nonmetals have more of an electron affinity than
  metals.
• EA decreases when moving down the group.
• EA increases moving from left to right in a
  period.

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