The Periodic Table of Elements

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The Periodic Table of Elements

• Not just a table, the key to matter!!!!!!!

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One of the greatest songs!

• http//www.privatehand.com/flash/elements.html

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The Wonders of the Periodic Table
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Arranging the Elements

• Dmitri Mendeleev (1887), a Russian scientist,
  looked at the chemical and physical properties of
  elements and organized them on the basis of their
  similarities
• By arranging the 63 known elements, he found that
  by placing them by increasing atomic weight he
  could put them into 7 groups, or columns.
• He found the pattern, all the elements in a
  column have the same valences, the number of
  electrons in the outer shell

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The Modern Periodic Table

• British scientist, Henry Mosley, arranged the
  elements according to their atomic number
• The Periodic Law states that the physical and
  chemical properties of the elements are periodic
  functions of their atomic number

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Design of the Periodic Table

• Classification system used to organize all the
  elements
• Information can be obtained about each element
  just by where it is placed in the periodic table!

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Columns

• Called groups or families
• Have similar, but not identical properties

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Rows

• Also called periods
• Elements are not alike in the rows
• First element in a row is an extremely active
  solid, where as the last is always an inactive
  gas
• There are 7 periods, with period 6 separated out
  to make the periodic table shorter
• Each of the rows fills the same electron orbits

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Columns and Rows
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Element Key, each element has their own.
Number of protons
mass - number number of neutrons
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It is just the beginning!!!!
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Lets look at what we have
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Most of the 109 elements are classified as metals

• Physical properties
• Luster or shininess
• Ductile means made into thin wires
• Malleable means hammered into thin sheets
• Allows heat and electricity to pass through
• Have a high density

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Chemical Properties of Metals

• Depends on the number of electrons in the outer
  shell of the atom
• These outer shell electrons are weakly held and
  tend to be lost when they chemically combined
• Easily react with water and gases in the
  atmosphere
• Metals are corrosive, they wear away
• ex. rust and tarnish

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Position of Elements
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Nonmetals

• Physical properties are opposite of metals, they
  are dull, brittle, and break easily, they are not
  ductile or malleable, and they can be a solid,
  liquid, or a gas
• Chemical properties are determined by the number
  of electrons in their outer shell
• Last row has 8 electrons in their outer shell, so
  they are non reactive

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Metalloids

• They have properties of both metals and nonmetals
• Metal-like
• They conduct heat and electricity, but not as
  well as metals
• Can be shiny or dull
• Are ductile and malleable
• Include boron, silicon, germanium, arsenic,
  antimony, tellurium, polonium, and astatine

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Chemical Families

• Elements within the same family on the periodic
  table have similar properties because they have
  the same number of valence electrons

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Alkali MetalsGroup 1

• Single electron in their outer shell
• Soft, silver-white, and shiny
• Can be cut with a knife
• Good conductors of heat and electricity
• So highly reactive they are never found free in
  nature
• Violent reaction in water

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Li
K
Na
Cs
Rb
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Alkaline Earth MetalsGroup 2

• They have 2 electrons in their outer shell
• Not quite as reactive as the alkali metals
  because they loose 2 electrons when combining
  chemically
• Never found free in nature because they are so
  reactive
• Calcium and magnesium are important part of this
  family

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Be
Mg
Ca
Ba
Ra
Sr
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The Transition MetalsGroups 3-12

• They have two electrons in their outer shell
  except Cr, Cu, Nb, Mo, Ru, Rh, Ag, PT, and Au
  have one.
• These share electrons when they combine
  chemically
• Conduct heat and electricity
• Many are familiar gold, silver, zinc, iron,
  nickel, copper, and tin

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Zinc
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Boron FamilyGroup 13

• They have 3 valence electrons in their outer
  shell
• Boron is metalloid, while aluminum, and the rest
  of the family are metals
• Aluminum is the most abundant metal and the 3rd
  most abundant element in the Earths crust
• Family includes boron, aluminum, gallium,
  indium, and thallium

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aluminum
indium
boron
thallium
gallium
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Carbon FamilyGroup 14

• Has 4 valence electrons in their outer shells
• Carbon is a nonmetal, silicon and germanium are
  metalloids
• Carbon makes over 5 million different compounds
  and is the basis of life
• Silicon is the second most abundant element in
  the Earth crust, important in computer chips
• Family includes carbon, silicon, germanium, tin,
  and lead

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carbon
silicon
tin
lead
germanium
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Nitrogen FamilyGroup 15

• Have 5 valence electrons in their outer shells
• Tend to share electron when they chemically
  combined
• Nitrogen is the most abundant element in the
  earths atmosphere
• Phosphorus is an active nonmetal that is not
  found free in nature
• Family includes nitrogen, phosphorus, arsenic,
  antimony, and bismuth

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phosphorus
nitrogen
antimony
bismuth
arsenic
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Oxygen FamilyGroup 16

• Have 6 valence electrons in their outer shell
• They share electrons when chemically combined
• Oxygen is the most abundant element in the
  Earths crust and second most abundant element in
  the atmosphere
• Oxygen is an extremely reactive element and
  combines with almost all other elements
• Family members include oxygen, sulfur, selenium,
  tellurium, and polonium

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oxygen
sulfur
polonium
tellurium
selenium
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The HalogensGroup 17

• Have 7 valence electrons in their outer shell
• They are the most reactive nonmetals
• Never found free in nature
• They share or gain one electron when they
  chemically combined
• Halogen means salt formers and all compounds with
  halogens are called salts.
• Astatine is a metalloid
• Family members include chlorine, fluorine,
  bromine, iodine, and astatine

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chlorine
fluorine
bromine
astatine
iodine
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Noble GasesGroup 18

• They have 8 electrons in their outer shell,
  except helium which has 2, means they are
  normally un-reactive
• Also known as the inert gases
• Found in small amount is the Earths atmosphere,
  argon the most common
• Family members include helium, neon, argon,
  krypton, xenon, and radon

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After failing 3 chemistry tests, Jake and Jacks
parents wall papered their room with the
Periodic Table!!!!!!
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Rare-Earth Elements

• These have properties that are similar to one
  another
• All have 2 valence electrons
• They have been moved to the bottom to make the
  periodic table easier to read
• First row is the lanthanide series, shiny, soft,
  malleable metals, that are conductive
• The second row is the actinide series, all are
  radioactive and only the first four are present
  in nature
• Elements numbered 92-118 are all synthetic and
  radioactive
• Uranium is the best known rare-earth metal

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Lanthanoid Series
Uranium
Samarium
Cerium
Lanthanum
Praseodymiun
Neptunium
Actinium
Thorium
Neodymiun
Ytterbium
Proctactinium
Actinoid Series
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Periodic Properties of the Elements

• Certain properties of elements vary in regular
  ways from left to right across a period. These
  properties include electron arrangement,
  reactivity, atomic size, and metallic properties

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Valence Electrons
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Ionic Charges
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Atomic Radius
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