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Dmitri Mendeleev

• Published the 1st periodic table.
• Arranged elements according to ascending mass.

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Henry Moseley

• Published the current periodic table.
• Arranged elements according to ascending atomic
  ( of protons).
• The result is that elements having similar
  chemical properties can be found in the same
  column (or group).

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Arrangement

• There are 18 vertical columns on the periodic
  table (called groups, or families).
• Group members have the same of valence
  electrons and, therefore, similar chemical
  properties.

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Alkali Metals - Group 1

• Only have 1 valence electron.
• The most reactive metals on the periodic table.

• http//www.youtube.com/watch?vuixxJtJPVXkfeature
  related

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Alkaline Earth Metals - Group 2

• Have 2 valence electrons.
• Also reactive, although not as reactive as Group 1

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Transition MetalsGroups 3 -12

• Have more than 1, positive oxidation .
• Tend to form compounds having color.

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Halogens - Group 17

• Have 7 valence electrons.
• Most reactive nonmetals.
• Only group having all 3 phases of matter at room
  temperature.
• F2(g), Cl2(g), Br2(l), I2(s)

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Group 18 - Noble Gases

• Have 8 valence electrons (a full valence shell).
• Inactive, or inert. Already satisfied, so they
  dont react.

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Arrangement

• There are 7 horizontal rows on the table, called
  periods.
• The period number is equal to the number of
  occupied principle energy levels occupied in the
  element.

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Metals

• Tend to lose electrons when bonding, forming
  cations (positive ions).

• Properties
• Gray
• Shiny (luster)
• Malleable (can be bent)
• Ductile (can be drawn into wire)
• Good conductors
• High mp and bp

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Nonmetals

• Tend to gain electrons when bonding, forming
  anions (negative ions).
• Also includes the noble gases that, generally, do
  not bond at all.

• Properties
• Brittle
• Lower mp and bp than metals
• Poor conductors

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Metalloids

• Elements having both metallic and nonmetallic
  properties.
• Border the stairstep line.

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Periodic Properties

• You can predict certain properties about an
  element based on its location on the periodic
  table.

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Ionization Energy

• The energy required to remove the outermost
  electron from an element.
• Measured in kJ/mole.
• Rememberall elements want to be like their
  nearest noble gas partner having a full valence
  shell.
• Metals will have a low IE, and nonmetals will
  have a high IE.

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Electronegativity

• A measure of the ability of an atom to attract
  electrons.
• Rememberall elements want to be like their
  nearest noble gas partner having a full valence
  shell.
• Metals will have a low IE, and nonmetals will
  have a high IE.

e-
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Atomic Radius

• A measure of the distance from the center of the
  nucleus to the outermost valence shell.

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Ionization Energy Down a Group

• As we move down a group, the ionization energy
  decreases.
• As we go down a group, the distance from the
  outermost PEL to the nucleus increases, making it
  difficult for the nucleus to hang on to the
  electrons. This is called the shielding
  effect.

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Ionization EnergyAcross a Period

• Across a period, ionization energy increases as
  we move from metals to nonmetals.
• Metals want to lose their electrons and nonmetals
  want to gain them.
• Metals do not hold on to their electrons,
  tightly, and nonmetals do.

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Ionization Energy Trend
I.E. increases
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ElectronegativityDown a Group

• As we move down a group the electronegativity
  decreases.
• As we move down a group we add more principle
  energy levels.
• Due to the shielding effect, it becomes more
  difficult for larger atoms to attract electrons.

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ElectronegativityAcross a Period

• As we move across a period, electronegativity
  increases as we move from metals to nonmetals.
• Metals want to lose electrons and nonmetals want
  to gain them.
• Metals dont want anymore electrons, they want to
  lose the ones that they have. Nonmetals want to
  gain more, so they pull harder.

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Electronegativity Trend
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Atomic RadiusDown a Group

• As we move down a group, the atomic radius
  increases.
• As we move down a group we are adding entire
  PELS.

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Atomic RadiusAcross a Period

• As we move across a period, the atomic radius
  decreases.
• As we move across a period we are adding protons
  to the nucleus and electrons to the same valence
  shell.
• Protons are bigger and badder so they pull in
  on the valence shell stronger with each
  additional proton.

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Atomic Radius Trend
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Ionic Radius

• Metals lose electrons when they form an ion.
• The newly formed cation is smaller than the
  original atom.

Sodium, a metal, loses its valence electron which
decreases its radius.
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Ionic Radius

• Nonmetals gain electrons when they form an ion.
• The newly formed anion is larger than the
  original atom.

Chlorine, a nonmetal, gains an electron which
increases its radius.
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Metallic Properties

• As you move across a period you move from metals
  to metalloids to nonmetals.
• Metallic properties decrease as you move across a
  period.

• Look at group 14. As you move down the group you
  move from nonmetals to metalloids to metals.
• Metallic properties increase as you move down a
  group.