Objective/Warm-Up

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Objective/Warm-Up

• SWBAT identify families on the periodic table.
• SWBAT describe periodic trends.
• Identify the following elements as metals,
  non-metals, or semi-metals.
• Fe Cl
• Cu Rn
• F Ra
• Si U

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http//web.buddyproject.org/web017/web017/metals.h
tml
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Vertical columns are called Groups or Families
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• Elements have same of valence electrons.
• Elements react in similar fashion.

Family
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Horizontal rows are called Periods
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• Elements have the same n (principal energy level)

Period
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Color the Periodic Table

• Need 9 different colors (or 8 white)

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Colored Image of Families on the Periodic Table
Alkali Metals
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Colored Image of Families on the Periodic Table
Alkaline Earth Metals
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Colored Image of Families on the Periodic Table
Transition Metals
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Colored Image of Families on the Periodic Table
Inner Transition Metals or Rare Earth Metals
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Colored Image of Families on the Periodic Table
Noble Gases or Inert Gases
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Colored Image of Families on the Periodic Table
Halogens
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Colored Image of Families on the Periodic Table
Other Non-Metals Semi-Metals or
Metalloids Other Metals
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Colored Image of Families on the Periodic Table
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Homework

• EC Riddles Due Friday
• P. 141 5-11, 13, 16 Due Monday

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Objective/Warm-Up

• SWBAT define and predict periodic trends.
• To which family or group does each element
  belong?
• Na
• F
• Kr
• Sr
• Fe
• Es

Alkali metals
Halogens
Noble Gases
Alkaline earth metals
transition metals
Inner transition metals
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Atomic Radius-half the distance between the
nuclei of two like atoms
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Ionization energy-energy required to remove an
electron
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Electronegativity-the tendency of atoms to
attract electrons
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Electron Affinity-the amount of energy needed to
add an electron
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http//web.buddyproject.org/web017/web017/metals.h
tml
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Objective/Warm-Up

• SWBAT describe and apply periodic trends.
• Warm-Up Explain how atomic radius changes across
  and down the periodic table.
• HW p. 121 3, 4, 6, 7, 9, 10, 12, 13 Due
  Thursday, Quiz Friday

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Ionic Radius-positive ions (cations) are smaller
than the atoms from which they are formed,
negative ions (anions) are larger than the atoms
from which they are formed.
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Shielding and Nuclear Charge

• Shielding explains family trends. As you move
  down a family, there are more energy levels. More
  energy levels means the valence electrons are
  further away from the nucleus. With more energy
  levels, the radius is larger and the electrons
  are more easily removed, meaning a lower
  Ionization energy.
• Example Li has a smaller radius and larger
  ionization energy than Na.

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• Nuclear charge explains period trends. As you
  move across a period, the energy level stays the
  same, what changes is the number of protons and
  electrons. With more protons, the electrons are
  pulled in closer, resulting in a smaller nucleus,
  making it more difficult to remove an electron
  (thus a higher IE).
• Example Li has a larger radius and lower
  ionization energy than Be.

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What can you get from looking at the electron
configuration?

• The elements with a greater ionization energy
  would rather not lose their electrons to be ions
  because they need them to closer to complete.
• The more energy levels, the greater the radius
• The elements with a higher electronegativity pull
  on their electrons because they dont want to
  lose them. They need them to be closer to
  complete.
• O He 2s2 2p4
• S Ne 3s2 3p4
• Se Ar 4s2 3d10 4p4

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Wrap-Up

• Explain shielding and nuclear charge.

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• Atomic Radius-half the distance between the
  nuclei of two like atoms
• Ionization energy-energy required to remove an
  electron
• Electronegativity-the tendency of atoms to
  attract electrons when in a bond
• Electron Affinity- the energy change when an
  electron is added to a neutral atom
• Ionic Radius-positive ions (cations) are smaller
  than the atoms from which they are formed,
  negative ions (anions) are larger than the atoms
  from which they are formed.

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Review-How to compare elements and their
properties

• Easy way to remember things
• All the properties increase as you go from left
  to right and bottom to top except for atomic
  radius.
• Notice that Helium has the smallest atomic
  radius, but Francium has a very large atomic
  radius.

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Electronegativity
Electronegativity
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Objective/Warm-up

• SWBAT compare and contrast the contributions of
  Mendeleev and Moseley to the development of the
  periodic table.
• SWBAT identify families on the periodic table.
• Name what families or groups each element belongs
  to
• - Ag
• - Cl
• - Pb
• - Ca

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Wrap-Up

• Why does radius increase down a family, but
  decrease across a period?
• How does this relate to the trends for ionization
  energy?
• HW P. 141 5-11, 13, 16 Due Monday

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Who Organized and Arranged the First Periodic
Table?
Dmitri Mendeleev
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Medeleev predicted what the element with a mass
of 70 would be like
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Medeleevs work allowed him to predict
undiscovered elements
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Unfortunately, Medeleevs work was not 100
accurate.

• Mendeleev used atomic mass to arrange his
  periodic table
• Now, we use atomic number!!!
• In Mendeleevs table some of the elements
  appeared to be misplaced because their properties
  didnt match the rest of the elements in the
  column.
• He was able to predict properties of unknown
  elements.

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Henry Moseley a young scientist - fixed the
problem!

• 50 years later- Henry Moseley, discovered atomic
  number ( of protons)
• Atomic number gives a better fit!

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• Fill in the Venn Diagram.

Mendeleev
Moseley
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• Periodic Law the physical and chemical
  properties of the elements are periodic functions
  of their atomic numbers.

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The Periodic Table The 3 Major Types of Elements

• The elements on the periodic table fall into 3
  main categories
• Metals
• Nonmetals
• Metalloids

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Metals

• Physical Properties
• Metallic luster (shiny),
• good conductors of electricity and heat,
• high density,
• high melting points,
• ductile (can be made into thin wires),
• malleable (can be made into thin sheets)
• Chemical Properties
• Usually give up their valence electrons when
  bonding,
• corrosion occurs when the element reacts with
  water or oxygen.

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Metalloids or Semi-Metals

• Elements that are on either side of the dark
  zigzag line are metalloids.
• They have properties of both metals and
  nonmetals.
• Metalloid means metallike.
• Solids that can be shiny or dull.
• Conduct heat and electricity better than
  nonmetals, but not as well as metals.
• They are ductile and malleable.

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Nonmetals

• Physical Properties
• No luster (no shine),
• dull in appearance,
• poor conductors of heat and electricity,
• cannot be made into wire or thin sheets
  (nonductile/nonmalleable),
• lower density,
• lower melting point.
• Chemical Properties
• Usually gain valence electrons when bonding.

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http//web.buddyproject.org/web017/web017/metals.h
tml
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http//www.windows2universe.org/earth/geology/meta
ls.html