The Periodic Table

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The Periodic Table
Good morning! Please get your notebook and be in
your seat when the bell rings. Warm-up Complete
the chart using your periodic table.
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Bens Chem Videos

• Periodic Table Video
• http//www.youtube.com/watch?veJp6xkd4SAIlistPL
  J9LZQTiBOFFDw-QjstExbB0P5E9v_Zuhindex9
• Periodic Law http//www.youtube.com/watch?voFnRvS
  YMioA

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Dmitri Mendeleev Created The Periodic Table
http//upload.wikimedia.org/wikipedia/commons/b/b3
/Medeleeff_by_repin.jpg

• HOW HIS WORKED
• Elements arranged in rows (periods) by increasing
  atomic mass.
• Elements arranged in columns (families) by the
  way they reacted.

• SOME PROBLEMS
• Left blank spaces for what he said were
  undiscovered elements. (Turned out he was
  right!)
• Pattern of increasing atomic mass was broken to
  keep similar reacting elements together.

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The Current Periodic Table
http//www.chemistryexplained.com/Ma-Na/Moseley-He
nry.html

• In 1913, Henry G.J. Moseley, an English
  scientist, arranged the elements based on
  increasing atomic number.

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Groups

• Vertical columns are called groups or families
• Groups are numbered 1 to 18.
• Number the groups at the top of each column on
  your periodic table.

GROUP
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GroupsHeres Where the Periodic Table Gets
Useful!!
Why?

• Elements in the same group have similar chemical
  and physical properties!!
• Example Elements in Group 1 are highly reactive
  and can be explosive in water. http//www.teachert
  ube.com/viewVideo.php?video_id41344

• They have the same number of valence electrons.
• http//www.tutorvista.com/content/science/science-
  i/structure-atom/valence-shell-electron.php

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Valence Electrons

• Electrons farthest away from the nucleus are most
  loosely held.
• Ranges from 1 to 8 valence electrons
• Many properties of the atom, and therefore of an
  element, are determined by the number of valence
  electrons.

• http//www.tutorvista.com/content/science/science-
  i/structure-atom/valence-shell-electron.php

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Periods

• Horizontal rows numbered 1 to 7.
• Elements in the same period have the same number
  of electron shells or energy levels.
• Number the Periods on the left side of each row
  on your periodic table.

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Properties of Elements on the Periodic Table

• An elements physical and chemical properties can
  be predicted from its location in the periodic
  table
• Example Sodium is more reactive than Aluminum
• Reactivity in metals decreases as you go from
  left to right.
• For nonmetals, the opposite is true. Nonmetals in
  Groups 14 through 17 become more reactive from
  left to right. Group 18, the Noble Gases, are an
  exception.

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Metals
Copper
Aluminum

• Left/Middle of Periodic Table
• Shiny, metallic
• Conduct heat and electricity
• Malleable and ductile (reshape)
• Lose valence electrons in a reaction

Gold
Nickel
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Metalloids

• Zigzag on Periodic Table where
• metals and nonmetals meet
• Mostly shiny, metallic looking
• Only semi-conductive
• Often combined with non-metals

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Non-Metals
Helium
Neon

• Right side of Periodic Table
• Dull, not shiny, many are GAS
• Do not conduct heat or electricity
• Crumble or break if solid
• (non-malleable/ductile)

• Gain or share electrons in a chemical reaction

Iodine
Chlorine
Carbon
Sulfur
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Hydrogen

• Belongs to a family of its own.
• Diatomic, reactive gas.
• Was involved in the explosion
• of the Hindenburg aircraft.
• Promising as an alternative
• fuel source for automobiles

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Alkali Metals

• 1st column on the periodic table (Group 1) not
  including hydrogen.
• Very reactive metals
• Always combined with something else in nature
  (like in salt).
• Soft enough to cut with a butter knife
• 1 valence electron

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Alkaline Earth Metals

• Second column on the periodic table. (Group 2)
• Reactive metals
• Always combined with nonmetals in nature.
• Several are important mineral nutrients (Mg and
  Ca)
• 2 valence electrons

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Transition Metals

• Elements in groups 3-12
• Less reactive harder metals
• Includes metals used in jewelry and construction.

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Boron Family

• Elements in group 13
• Aluminum metal was once rare and expensive, not a
  disposable metal.

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Carbon Family

• Elements in group 14
• Contains elements important to life and
  computers.
• Carbon is the basis for an entire branch of
  chemistry.
• Silicon and Germanium are important
  semiconductors.

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Nitrogen Family

• Elements in group 15
• Nitrogen makes up over ¾ of Earths atmosphere.
• Nitrogen and phosphorus are both important in
  living things.
• Most of the worlds nitrogen is not available to
  living things.
• The red stuff on the tip of matches is phosphorus.

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Oxygen Family

• Elements in group 16
• Oxygen is necessary for respiration.
• Many things that stink, contain sulfur (rotten
  eggs, garlic, skunks,etc.)

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Halogens

• Elements in group 17, also called Halides
• Very reactive, volatile, diatomic, nonmetals
• Always found combined with other element in
  nature
• Used as disinfectants and to strengthen teeth

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The Noble Gases

• Elements in group 18
• VERY unreactive (STABLE), monatomic gases
• Used in lighted neon signs
• Used in blimps to fix the Hindenburg problem.
• Have a full valence shell.

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Lanthanide Series

• One of two rows that sits off to the bottom of
  the periodic table
• Reactive
• Fairly soft metals

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Actinide Series

• Also towards bottom of periodic table
• All are radioactive, some are not found in
  nature
• Some with higher atomic numbers have only been
  made in labs

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Electron Configuration
Click on the video links for explanations of
electron configuration.
http//www.youtube.com/watch?v2AFPfg0Como
http//www.youtube.com/watch?vjtYzEzykFdg
http//www.chemprofessor.com/periodicqm.htm
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Pre-APPeriodic Trends

• Reactivity how likely or how vigorously an atom
  is to react with another substance.
• Non-Metals
• Period - reactivity increases as you go from left
  to right, except for Group 18
• Group reactivity decreases as you go down the
  group
• Metals
• Period reactivity decreases as you go from left
  to right
• Group reactivity increases as you go down a
  group

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Pre-APPeriodic Trends

• Atomic Radius related to the atoms volume.
• Period atomic radius decreases as you go from
  left to right
• Group atomic radius increases as you go down a
  group

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Pre-APPeriodic Trends

• Electronegativity the atoms desire to grab
  another atoms electrons.
• Period electronegativity increases as you go
  from left to right.
• Group electronegativity decreases as you go
  down a group

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Pre-APPeriodic Trends

• Ionization Energy amount of energy needed to
  remove the outermost electron. Closely related to
  electronegativity.
• Period Ionization energy increases as you go
  from left to right.
• Group Ionization energy decreases as you go
  down a group

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Pre-APPeriodic Trends

• Melting Point
• Metals the melting point for metals decreases
  as you go down a group
• Non-Metals the melting point for non-metals
  increases as you go down a group