periodic table song

							The Periodic Table
                           Triads
• 1829 – Döbereiner (1780-1849)
• Only 60 elements known
• Groups of 3’s
   – Melting points
   – Boiling points
   – Metallic properties
Cl, Br, I: similar chemical reactions
             nonmetallic
             diatomic gases
             form colorless acids
Ca, Sr, Ba
S, Se, Te
What do these triads have in common?
Elements in each triad are in the same
column or group on the Periodic Table
             Döbereiner's Lamp
• A lighter invented by the German chemist
  Johann Wolfgang Döbereiner.
• It is ignited by the action of hydrogen on a
  platinum sponge. Döbereiner observed that if
  a jet of hydrogen was directed at the platinum
  from a distance of 4 cm so that it was
  premixed with air, the platinum became red-
  hot, then white-hot and the jet ignited
  spontaneously. This discovery, in which fire
  was produced without flint and tinder
  or a match, quickly created an international
  sensation and was immediately tested and
  confirmed by many chemists and physicists.
• The Döbereiner-lighter was invented in 1823
  by Johann Wolfgang Döbereiner and was in
  production until ca. 1880.
• The lighter is exhibited in the Deutschen
  Museum and in the old pharmacy in the
  Heidelberg Castle.
Octaves
John Newlands (1837-1898)
• 1863
• Before 1860, atomic masses were
  unknown, uncertain, or incorrect
1. Arranged elements by
   atomic weights
2. Why do properties repeat every 8th element?
Elements are in the same group
Groups of 7—Law of Octaves
7 families of elements with similar properties
VIIIA –not yet discovered
• Members of the British Chemical Society
  laughed at this proposal.
• 30 years later he received an award for
  this achievement.
Dmitri Mendeleev (1834-1907)
 1. Arranged elements by atomic weights
  2. Predicted unknown elements and their
     properties   world fame!
  3. Predicted: Scandium, Gallium, Germanium
  4. Problem: Reversed Pairs
        Te and I
        Ar and K            Doomed his table
        Co and Ni
Either the weights were wrong or the arrangement was wrong
 Dmitri Mendeleev (1834-1907)
•1869
•13th of 17 children
•At age 20, the family moved to
Moscow to go to University
•Denied admission, so moved
to St. Petersburg and graduated
at the top of his class
•He got one haircut a year
Modern Periodic Table
Henry Moseley (1887-1915)

•   1913
•   Studied under Ernest Rutherford
1. Found reasons for the reversed pairs
2. Accurately determined atomic numbers
   (# of protons) using X-ray diffraction
3. Revised Periodic Chart:
Now based on atomic number NOT atomic weight
 Henry Mosely (untimely death)
• In 1914, he resigned at Manchester to
  return to Oxford to pursue his research,
  but when World War I broke out, he turned
  down a job offer and enlisted in the Royal
  Engineers.
• He fought at Gallipoli, where he was killed
  in action by a sniper in 1915.
             Periodic Law
• Properties of elements are a function of
  their atomic numbers
• Manhattan Project Scientists used atomic
  numbers and periodic law to predict and
  purify Uranium and Plutonium while
  making the A-bomb
• Robert Oppenheimer
• Upon seeing the
  A-bombs first trial quoted
  the Bhagavad-Gita

“Now I am become Death,
  the destroyer of worlds”
• Truman speaking
  about dropping the
  A-bomb
Tom Lehrer
                                            Tom Leher
                                            AKA Thomas Andrew Lehrer
Born: 9-Apr-1928
Birthplace: New York City

Gender: Male
Religion: Atheist
Race or Ethnicity: White
Occupation: Comic, Musician
Nationality: United States
Executive summary: Wretched songwriter
Military service: US Army (1955-57)
Father: (necktie manufacturer)
Brother: (1 brother)

   High School: (prep school, Connecticut)
   University: BA Mathematics, Harvard University (1947)
   University: MA, Harvard University (1948)
   University: PhD, Harvard University
   Teacher: MIT
   Teacher: Harvard University
   Teacher: Wellesley College
                                                                 • Periodic Table Song
   Professor: UC Santa Cruz (1972-)
                                                          Animated Element Song
   Phi Beta Kappa Society
   Edgar Allan Poe Award Raven Award (1954)               http://www.privatehand.com/flash/elements.html
   Jewish Ancestry

  FILMOGRAPHY AS ACTOR
  Hey, Mr. Producer! The Musical World of Cameron Mackintosh (8-Nov-1998) Himself

http://www.nndb.com/people/710/000022644/
           Element Puns
        Getting Punny With It

•John Enium’s Sister        • Ruthenium
•A crazy inmate             • Silicon
•Not fat                    • Tin
•What doctors do for sick   • Curium
people
• Assign HW elements #1-5
           Periodic Trends
• Draw the rough outline of the periodic
  table in this space.
    Reactivity
Group or Family




                                Non-
                                metals
                  Metals
                       Period
Atomic Size – add arrows to your table
                     Size
• Why?
• As the number of electrons grows
  the positive nucleus pulls them closer.




+
               +          +           +     +
                 Reactivity
Most active metal: Fr

Most active non-metal: F

More active?
     O or S
     Se or Br
     K or Ca
     Mg or Ca
     F or Ne
            II. Noble Gases

•Also known as: Rare Gases, Inert Gases
•Group VIII A
•Exist as monatomic gases
•Chemically inert (unreactive)
•Why are the noble gases so stable?
•They have a filled outer shell (ns2np6)   X
•Until 30 years ago, no noble gas compounds
were known
•Only Krypton and Xenon have formed chemical
compounds
     Xe(g) + 2 F2 (g)   XeF4 (s)
Reaction done at 400oC and
6 atmospheres of pressure (4560 mmHg)
• Helium: used as a coolant in refrigeration,
  deep sea diving, pressurized gas for
  rocket fuel, blimps
• Discovered on the sun with
  spectrophotometery before it was
  discovered on Earth
• Neon: used in signs
• Argon: used in incandescent light bulbs
Red = Ne
Others = Ar, Hg, phosphor
        III. Alkali Metals
1. Elements in Group IA
2. Occur in nature only as ions (+1)
3. All (except Hydrogen) posses:
      metallic properties
      silvery luster
      conductor of heat and electricity
      ductile
      malleable (can be cut with a knife)
4. Metal + H2O       H2 (g) + Base
   Alkaline means basic
   Basic solutions have a pH > 7
   Bases neutralize acids
5. Alkali Metals are very reactive
   --want to lose 1 electron to form a stable octet
   Alkali Metals = +1 ions
   K      K1+ + 1 e-
   X

Electron configuration of K1+ ion?
       1s2 2s2 2p6 3s2 3p6 (Just Like Ar)
       Filled outer shell = greater chemical stability
Reactivity increases with larger distance
  of e- from nucleus
                             Sodium Lake?
•   Reaction of Sodium with air: http://128.104.70.28/lab/CCA/MVHTM/NO_elt/Na_Air.HTM
•   Sodium with water: http://128.104.70.28/lab/CCA/MVHTM/NO_elt/Na_H2O.HTM
•   Potassium Air:
     –    http://128.104.70.28/lab/CCA/MVHTM/IL_elt/K_Air.HTM
•   Potassium Water:
     –    http://128.104.70.28/lab/CCA/MVHTM/IL_elt/K_H2O.HTM
•   Rubidium Air:
     –    http://128.104.70.28/lab/CCA/MVHTM/PR_elt/Rb_Air.HTM
•   Rubidium Water:
     –    http://128.104.70.28/lab/CCA/MVHTM/PR_elt/Rb_H2O.HTM
•   Cesium Air:
     –    http://128.104.70.28/lab/CCA/MVHTM/CmCz_elt/Cs_Air.HTM
•   Cesium Water:
     –    http://128.104.70.28/lab/CCA/MVHTM/CmCz_elt/Cs_H2O.HTM
•   Sodium Lake:http://www.theodoregray.com/PeriodicTable/Stories/011.2/Videos/SodiumLake01.html
6. Uses of Group IA Metals

Li   somewhat rare
     occurs in nature as Li1+ ions in several types of
     rocks
     lowest density of any metal
     used in ceramics and drugs (anti-psychotic)
Na   very abundant, but never found as a pure metal
     usually in chloride form
     In soil, seawater, plants, animals
     hard to find anything without Na+
NaHCO3—baking soda
NaHCO3 + H2O—soda water
Na2CO3—soda cracker
         (yeast dough neutralized with soda)
NaNO3—fertilizers
Na2B4O7•10H2O—Borax (washing soda)
K     many uses
      very abundant
KBr     sedatives and photography
K2CO3   potash—used in fertilizers, glass making, soap
KNO3     saltpeter—black gun powder, curing meat,
                   fireworks
• Which is the most reactive alkali metal?
  Why?
  – Fr, farthest down the table,
    electrons lost are FAR from the + nucleus
• What does “alkali” mean?
  – Base forming….Alkali flats out in Utah
• Why aren’t there any pure Na or K deposits
  on earth?
  – Explode with H2O
     Alkali Metals—Group IA




Li                            Na



              K
          Element Puns
       Getting Punny With It

• When people die they …      • argon
                              (or barium)
•What a torpedoed ship does
                              • zinc
•50% of element 67
                              • hafnium
•Male of the Ganese tribe
                              • manganese
          Element Puns
       Getting Punny With It

• A 2000 pound coffin    • Krypton
•What some classes do,   •Boron
  but not this one       •Rubidium
•Land of the Frogs
IV. Halogens—Group VIIA
   “salt forming”
   non metals          X

1. Ions tend to gain 1 e- to form a
   stable octet
2. Form –1 ions
    Cl + 1 e-       Cl1-
         Halogen Reactions
• Halogen and Hydrogen       Acid
•         Cl2 + H2     HCl
• Halogen + Metal    Salt
         Na + Cl2     NaCl
• Try these dot diagrams:
    Cl        Cl-        Cl2

    Cl        Cl-       Cl Cl
• Which is more stable a chlorine atom, ion, or
  molecule? Why?
  – The ion, a completely full, unshared outer shell.
• Why are halogens so reactive?
  – Only need to gain 1 e-


• Which is more reactive, Cl2 or F2?
  – Fluorine, electrons are closer to the positive
    nucleus.
• What are the problems with freon?
         – Reacts with ozone layer




http://env.chass.utoronto.ca/env200y/know/ozonehole3d.gif
• Which is the most stable halogen?
  – Lower down the group
• What is the molecular weight of Chlorine
  gas?
             g
   Cl2   71
            mol
                              Halogen   High Intensity
                                        Discharge
                                        (HID)
                                        XENON




Chlorine, Bromine, Fluorine
& Iodine
  V. Alkaline Earth Metals
1. Elements in Group IIA
2. Occur in nature as ions (+2)
3. 2 e- in their outer shells     X


4. Metal + H2O      H2 (g) + Base
   Alkaline means basic
   Basic solutions have a pH > 7
   Bases neutralize acids
       Alkaline Earth Metals
• Essential for life:
• Without Ca+2 organisms die
  – Muscle action, energy use, hormone
    signaling, blood clotting etc.
• Mg+2 is needed for photosynthesis and
  many protein jobs.
        Calcium compounds
• CaO “lime” mortar,    “Wild” Iowa
  bricks, steel
• CaCO3 “limestone” a
  key component of
  rock formations,
  fossils, and shells
• CaCl2 is used to
  de-ice roads
• Why are alkali metals more reactive?
  – Only need to lose 1 electron,
    alkaline need to lose 2. Also
    alkaline have a filled s sublevel
    increasing stability
• Which is more stable, Ca+2 of Ca?
  – Ca+2 due to a full octet (e- config of Argon)
Reactions of Alkaline Earth Metals
• Alkaline + Halogen   a salt
           Mg + Cl2  MgCl2
• Alkaline + Oxygen    oxide
           Sr + O2   SrO
• Alkaline + Water   a base (DEMO Ca and Mg)
     Ca + 2 H2O     Ca(OH)2 + H2 (g)
• Short 1 min movie of Group I and II Rxn’s
           Element Puns
        Getting Punny With It

• A flower you might raise      •Germanium
•The lone ranger’s horse        •Silver
•What a farmer did with seeds   •Sodium
•The outer covering of an ox    •Oxide
                      Iron
• “The skeleton of our modern civilization”
• Steel – Iron and carbon and other metals.
  chrome steel, nickel steel, titanium, etc.
• 5% of the earth’s crust
• Found in earth as Fe2O3
• Mesabi Range – Minn.
  Large Deposits.
Bessemer Converter
used to convert
iron ore to iron
                   Copper

•   Large deposits in N. Michigan
•   Conductor of electricity (wires)
•   Cooking pots – (heat conductor)
•   Brass – alloy of Cu + Zn
•   Bronze – alloy of Cu + Sn
copper ore



                 copper kettle



  copper roofs
                 Lead
• Pb Plumbum        Plumbing
• Mineral Point – SW Wisconsin
• Obtained from PbS (Galena) ore
• Lead Salts are poisonous
  White lead – paint
• Batteries – wet cells
  Pb and Sulfuric Acid in cars
• Pewter – Lead and Tin
Galena
                     Zinc

• Use in dry cell batteries (flashlight)
• Galvanized Iron – Zinc “dipped”
  protects from rusting.
• Sacrificial Zn on your outboard motor
                        Tin

• Coating for Iron (steel) “tin” cans
• Napoleon’s Coat – tin pest
  brittle when cold
                    Mercury

•   Found in cinnabar (HgS)
•   Spain – large producer
•   13.6 times more dense than water
•   freezing point = - 38.9º C
•   vapor is poisonous (breathing)
•   liquid can be absorbed through the skin
    (touching)
Mercury   Cinnabar
                       Silver

•   A “Noble” metal
•   Relatively unreactive
•   The best conductor
•   Uses:
    Silverware, jewelry
    Mirrors (silvered)
    Photography – Ag+ ions are sensitive to light
    Dental Fillings – amalgam
          Hg and Ag mixture
                 Aluminum

• Most abundant metal in earth’s crust (8.1%)
• electrolytically extracted from bauxite
  (Charles Martin Hall)
• In 1855 – 3 times the value of silver
• Washington Memorial had an Aluminum cap
• 50% used in structural alloys, ships, planes,
  cars, buildings
• Household utensils – foil, pans
• AlCl3 is in many antiperspirants
• Linked to Alzheimer’s and brain lesions.
• Charles Martin Hall
      Washington
      Monument


Aluminum
                           Gold

• Most malleable and ductile
  metal
• Gold leaf 1/250,000 inch thick

• Not attacked by individual acids
  only Aqua regia (HNO3 + HCl)

• Pure Gold = 24 carats
  14 carat = 14 parts Au and 10
  parts other metals
               Silicon

• Second most common element
  (28% of earth’s crust)
• Exists as silica – SiO2
  sand, clay, glass, asbestos
• Uses:
  Microchips
  Carborundum – SiC
Silicon
                    Sulfur
• Brimstone H2S and SO2
• Paper industry bleaching dioxins
    – That Wisconsin Rapids smell
•   SO2 – Acid Rain
•   80% of sulfur mined in Texas and Louisiana
•   Production of H2SO4
•   Found in proteins
    “perming” hair
Sulfur




         Sulfur Hot Springs
Yellowstone
    Transition Elements – Groups B
•   10 columns – filling d orbitals
•   Structural uses
•   85% must be imported
•   Also needed in living organisms
•   Iron – Zinc – Copper - Manganese
• Lanthanoid Series
  – 14 Elements – filling f orbitals
  – lanthanum    utterbium
• Actinoid Series
  – 14 Elements – filling 5f orbitals
• The lanthanoids and actinoids were once
  called “rare earth elements”
• Why?
• ‘Earth’ refers to the oxide form of these
  elements. These elements were first
  isolated in this form.
                   Coinage
• Many transition
  metals are coinage
  metals
• What properties are
  desired in a coin
  metal?
• Unreactive,
  inexpensive, can form
  durable alloys,
  resistant to corrosion.