Chapter 5 p.123 Periodic Table

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Chapter 5 p.123 Periodic Table

• Periodic means
• Repeating pattern
• Dimitri Mendeleev Russian chemist,
• 1866, published in 1869
• Mendeleev- discovered pattern by chemical
  properties----
• left empty spaces
• 42 yrs later
• Henry Mosely English chemist 1911
• Modern definition of Atomic modern
  organization of Periodic Table.

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• PT divided into two sections
• Metals / non-metals via stair steps
• Metals on the left of stairs
• Metals conduct electricity heat
• Non-metals on the right of stairs
• Non-metals do not conduct electricity very well
  and heat only slightly. Most are gases and
  powders.
• Metalloids
• Elements touching the stair steps
• Exclude Boron and Aluminum
• Properties of both, cant make up their mind
• Semi-conductors .used in computer chips

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• Elements going sideways period
• Elements going down group or family
• Period numbers down side tell largest occupied
  energy level.
• Group numbers across the top tell number of
  valence electrons.
• there are some deviations
• transition elements, the group equal the sum
  of the s d electrons.

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Important Concept

• There are patterns to the Periodic Table called
  the Periodic Law
• 1 Groups or families exhibit same
  characteristics.
• Note outer valence electrons determine chemical
  properties SO..all elements in a group or family
  will have similar chemical properties.
• Official way to say it The physical
  chemical properties of elements are a periodic
  function of their atomic number.

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• Group 1 Alkali Metals
• Very reactive, explosive, does not exist pure in
  nature
• Group 2 Alkaline-Earth Metals
• Very reactive but not as active as group 1 does
  not exist pure in nature
• Group 3-12 Transition Metals
• Less reactive, some not reactive, good conductors
  of electricity, heat
• Group 17 Halogens
• Very reactive, gases
• Group 18 Noble Gases
• Not reactive, inert,
• Lanthanides
• Extremely similar, tedious to distinction
• Actinides
• Radioactive, short life

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• Group 1 s block Alkali Metals
• all elements in group 1 have 1 valence e-
• hence all have similar properties.
• Extremely reactive..explosive
• Not found in pure state in nature
• Combines vigorously with non-metals
• Usually stored under kerosene
• Going down group lower melting point
• Li depression, bipolar, ..Gastonia
• Na Cl NaCl .salt..electrolytes, got to have
  it.
• bottled water?????? . Gatorade
• K Cl KCl .saltmuscle cramps. eat bananas

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• Group 2 Alkaline-Earth Metals s2 block
• harder, denser, stronger
• too reactive to be found in purity in nature
• Be emeralds.green fireworks
• Mg white fireworks, very hard,
• Ca Ca3PO4 bones ,
• CaCO3 Concrete , Marble, limestone
• Chlorophyll in plants is calcium based
• Sr Red fireworks
• Ba Medicine tracking, white chalky stuff people
  drink, isotopes
• With a color pencil lightly color in groups 1
  2 to color code the s block on your periodic
  block

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• HYDROGEN
• doesnt share same properties as group 1
• is placed above group 1 because it does have the
  1s1 orbital filled.

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• Transitional Metals groups 3-12 color code
• in each case the sum of outer s electrons and d
  electrons group number
• Fe, Co, Ni, make steel, only these can make
  a magnet
• Al most abundant metal on earth
• Fe second abundant, most used 1
• Group 11
• Cu
• Ag
• Au coinage metals, nonreactive ,can be pure on
  earth.
• Group 12
• Zn used in plating ZnO
• Cd rechargeable batteries
• Hg poisonous, accumulates in bodies,
  thermometers

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Charles Martin hall was a 21 yr old college
student in 1884 in Ohio when he first became
interested in aluminum. One of his professors
commented that anyone who could manufacture
aluminum cheaply would make a fortune, and Hall
decided to give a try. Working in a wooden
shed near his house with an iron frying pan, a
blacksmiths forge as a heat and crude galvanic
cells (batteries). Hall found that he could
produce aluminum by passing an electric current
through molten Al2O3Na3AlF6 mixture. By a
strange coincidence, Paul Heroult, a Frenchman
died the same year as Hall, and had made the same
discovery about the same time.
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• Non-metals color code entire p block
• begin to fill p sublevel
• of valence electrons group -10
• Most are gases _at_ room temp
• 1 non-metal is a liquid at room temp Br
• Poor conductors of electricity and heat
• Group 17 Halogens
• F most chemically reactive
• Use to etch glass and tooth decay
• Cl disinfective . Swimming pools
• Br lipstick, dyes
• I thyroid medicine, purple vapor
• Sublimination solid gas
• CO2 solid gas never gets wet,
  never a liquid

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• Note
• Diatomic Molecules
• 2 atoms of same element chemically combine in
  nature
• N2 O2 F2
• Cl2
• Br2
• I2
• H2
• When writing these you must write them as
  diatomic !!!!! Or it will be wrong!!!!
• Noble Gases group 18 inert .filled energy
  orbital
• Laser Light shows, Neon lights

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• Carbon
• 3 forms called allotropes p. 626 in book
• Allotrope same element different structural
  form
• Diamond.. Atoms in a pyramid
• Graphite .. Atoms in layers. pencil
• Fullerenes.Atoms in a spherecoal
• periodic table based on carbon-12
• Silicon
• sand, SiO2 .. Glass, computer chips
• Nitrogen
• each breath is 80 N2, diatomic, fertilizers,
  TNT, dynamite

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• Phosphorus
• Fertilizers, Match heads
• Antimony Bismuth
• Added to other metals to lower melting point
• Automatic fire sprinkler
• Oxygen
• 20 of air , diatomic, 2 allotropes
• Ozone, O3 .. How made ?????

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• Alloys
• Brass Cu Zn
• Bronze Cu Sn
• Sterling Silver Cu Ag
• Pewter Cu Sn Sb
• Gold
• 100 gold 24 karat
• 92 gold 22 karat.8 copper
• 58 gold 14 karat 42 copper
• 50 gold 12 karat .50 copper
• What property does copper add to the gold?
• What makes your skin turn green with fake gold?

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• Without looking at periodic table
• For the electron configuration write
• Group Period Block
• A. (Rn) 7s1
• B. (He) 2s2
• C. (Ar) 3d104s1
• D. (Kr) 5s24d105p3
• E. (Ar) 3d74s2
• Open books p. 156 29,30,31 ---15 minutes

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