The Periodic Table

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The Periodic Table
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The Father of the Periodic TableDimitri Mendeleev

• Mendeleev was the first scientist to notice the
  relationship between the elements
• Arranged his periodic table by atomic mass
• Said properties of unknown elements could be
  predicted by the properties of elements around
  the missing element
• Moseley later discovered that the periodic nature
  of the elements was associated with atomic
  number, not atomic mass

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Valence Electrons

• Outermost (last shell) electrons in an atom
• Electrons available for interactions with valence
  electrons of other atoms in chemical reactions

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Metalloid

• Six elements Boron, Silicon, Germanium, Arsenic,
  Antimony and Tellurium
• Elements found along the stair-step line that
  separates metals from non-metals.
• Chemical elements with properties that are
  in-between or a mixture of those of metals and
  nonmetals
• Have a metallic appearance but they are brittle
  and only fair conductors of electricity

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The Periodic Table
Column Group or Family 18 columns on the
Periodic Table
Row Period 7 rows on the Periodic Table
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Metals, Nonmetals, and Semi-metals
Hydrogen Only nonmetal on the metal side
Nonmetals are on the right of the stair-step
Metals are to the left of the stair- step
Semi-metals, metalloids, touch the
stair-step
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What is luster, malleable and ductile?

• Luster describes the way a surface reflects
  lighttherefore metallic luster would be shiny
  like a metal object.

• Malleable means to be able to press or pound the
  substance into sheets or different shapes.

• Ductile means that the substance can be drawn out
  into thin wires.

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The Groups of the Periodic Table

• Group 1 The Alkali Metals
• Most reactive metals on the PT
• Reactive in water and air thus stored in oil
• Rarely found free in nature
• Charge of 1 1 valence electron (1 electron in
  the outer shell)

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The Groups of the Periodic Table

• Group 2 The Alkaline Earth Metals
• Still quite reactive
• React with water to form bases and hydrogen gas
• Have a silvery luster
• Good conductors of heat and electricity
• Charge of 2 2 valence electrons (2 electrons
  in outer shell)

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T he Groups of the Periodic Table

• Groups 3-12 Transition Metals
• Found freely and in compounds in nature
• Great conductors of electricity
• Mixed with paints to achieve bright colors
• include radioactive elements 89 through 109
• include Mercury, the only metal that is liquid at
  room temperature
• Have a silvery luster, except Copper and Gold
• Charge is usually 2 but can varyusually 2
  valence electrons (2 in outer shell)

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T he Groups of the Periodic Table

• Group 13 Boron Family
• Metallic (except Boron, which is a solid
  metalloid)
• Scarce in nature (except Aluminum, which is the
  most abundant metallic element
• Charge is 3 3 valence electrons

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The Groups of the Periodic Table

• Group 14 The Carbon Family
• Contains elements that can form unusual bonds
  (Carbon and Silicon)
• Includes a nonmetal (Carbon), two metalloids
  (Silicon and Germanium) and two metals (Tin and
  Lead)
• Relatively unreactive
• Charge is 4 or -4 contains 4 valence electrons

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T he Groups of the Periodic Table

• Group 15 The Nitrogen Family
• Consists of two nonmetals (Nitrogen and
  Phosphorus), two metalloids (Arsenic and
  Antimony), and one metal (Bismuth)
• Nitrogen is most commonly found as atmospheric
  gas
• Range from very abundant elements (Nitrogen and
  Phosphorus) to relatively rare elements (Arsenic,
  Antimony, and Bismuth)
• Solids at room temperature, except Nitrogen
• Charge is -3 contains 5 valence electrons

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The Groups of the Periodic Table

• Group 16 The Oxygen Family
• Consists of three nonmetals (Oxygen, Sulfur, and
  Selenium), one metalloid (Tellurium), and one
  metal (Polonium)
• Also known as the Chalcogens
• Charge is -2 6 valence electrons

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T he Groups of the Periodic Table

• Group 17 The Halogens
• Most reactive nonmetals, with Fluorine being the
  most reactive of all nonmetals
• Found in the rocks of Earth's crust and dissolved
  in sea water
• Exist as a gas at room temperature (F2 and Cl2),
  a liquid (Br2), and a solid (I2 and At)
• Charge is -1 7 valence electrons

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T he Groups of the Periodic Table

• Group 18 The Noble Gases (The Inert Gases)
• Nonreactive
• Colorless gases
• Nonmetal
• Charge is 0 2 or 8 valence electrons- have a
  full outer energy level

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Special Rows on the PT
Lanthanides
Actinides
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Lanthanides Family

• Very reactive burns easily in air
• 15 soft metals
• Once called the Rare Earth Elements
• Relatively abundant in Earth's crust
• Found in Row 6 of the periodic table between
  Groups 3 and 4
• Occur together in nature, and they are very
  difficult to separate from each other
• Silvery-white metals that tarnish when exposed to
  air, forming their oxides

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Actinides Family

• All are radioactive.
• 15 very dense metals- tarnish in air.
• Actinides combine directly with most nonmetals