The Periodic Table

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The Periodic Table
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The Periodic Table

• is a chart that organizes all the elements in a
  way that shows patterns both similarities and
  differences among the elements.
• Elements are listed by increasing atomic number.

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• The horizontal rows are called periods. There
  are 7 periods.
• The vertical columns are called groups. There
  are 18 groups.
• Elements in the same group have similar chemical
  properties.

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Periods

• Each period corresponds to the energy levels
  found outside an atoms nucleus
• The period that an element is located in tells
  you what the highest energy level is that will
  contain electrons

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Periods

• The most energy levels found in an atom
  (currently) is seven which corresponds to the
  seven periods in the table
• Example
• Potassium (K) is located in period 4 and thus
  will have its valence electrons in the fourth
  energy level

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Special Groups

• Group 1 elements are known as the alkali metals.
• Group 2 elements are known as the alkaline earth
  metals.
• Group 17 elements are called halogens.
• Group 18 elements are called noble gases.
• Groups 3-12 are called transition metals.
• The Lanthanides and Actinides are the excerpts at
  the bottom.

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Group 1 Alkali Metals

• Have only one e- in the valence shell
• Most reactive of all metals reactivity
  increases as you go down the group
• Hydrogen is an exception!
• Has one valence electron but is classified as a
  non-metal

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Group 2 Alkaline Earth Metals

• Has two e- in valence shell
• Become increasingly soluble with increase in
  temperature

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Group 18 Noble Gases

• Generally are chemically inert meaning they do
  not react with other elements
• This is because they already have 8e- in their
  valence shell causing them to be stable
• (He only has 2 valence e-)
• Only He and Ne are truly inert others will
  react in limited amounts under specific
  conditions

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Group 17 Halogens

• Halogen means salt former form salts when
  reacting with a metal
• Most exist as diatomic molecules in gaseous state
  
• Ex. Cl2
• All are one e- short of a full valence shell
  causing them to be very reactive
• Are non-metals

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Transition and Rare Earth Metals

• Some of the rest of the elements in the periodic
  table fall under these two categories
• Transition metals are groups 3 12
• Rare earth (inner transition) metals are broken
  down further into actinides and lanthanides

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Transition and Rare Earth Metals
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Representative Elements

• Groups 1, 2 (s block) and 13-18 (p block) are
  often called representative elements. They are
  sometimes labelled 1A, 2A, 3A, 8A

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• These elements are called the representative
  elements

8A0
1A
2A
3A
4A
5A
6A
7A
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The Periodic Table
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• There are 3 major sections of elements in the
  periodic table
• Metals
• Non-metals
• Metalloids
• Metals are located to the left of the staircase
  line and non-metals are to the right (except H).
  Metalloids border the line.

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Properties of Metals

• Physical Properties

• Chemical Properties

• Luster (shiny)
• Good conductors
• High density
• High melting point
• Malleable/bendable
• Solid at room temperature (except Hg)

• Easily lose electrons
• Corrode easily (ex rusting or tarnishing)
• Low electronegativity

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Properties of Non-metals

• Physical Properties
• Dull
• Poor conductor
• Brittle
• Not malleable
• Low density and melting point
• Chemical Property
• Tend to gain electrons
• High electronegativity

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Properties of Metalloids

• Metalloids border the staircase and tend to
  have some properties of both metals and
  non-metals.
• solids
• can lose or gain electrons
• semi-conductors of electricity (Conduct heat and
  electricity better than non metal but not as well
  as metals
• Shiny or dull
• Malleable

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The Periodic Table