Announcements

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Announcements

• Friday
• Quiz
• Journal Check 12 entries
• Data Table Outline
• Experimental Design Due

MON TUES WEDS THURS FRI SAT SUN
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The Periodic Table

• How is the periodic table put together?

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(No Transcript)
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What is the Periodic Table?

• It is an organizational system for elements.
• Periodic Table Song ASAPscience
• Periodic Table Song Meet the Elements

Picture from www.chem4kids.com
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Who created it?

• The quest for a systematic arrangement of the
  elements started with the discovery of individual
  elements.
•   By 1860 about 60 elements were known and a
  method was needed for organization. 
• In 1869, Russian chemist Dimitri Mendeleev
  proposed arranging elements by atomic weights and
  properties.
• The table contained gaps but Mendeleev predicted
  the discovery of new elements.

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Mendeleevs Table
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So how is it arranged?

• The genius of the periodic table is that it is
  organized like a big grid.
• The elements are placed in specific places
  because of the way they look and act.
• If you have ever looked at a grid,
• you know that there are rows (left to right)
• and columns (up and down). The periodic table has
  rows and columns, too, and they each mean
  something different.
• quoted from http//www.chem4kids.com/files/elem_pe
  rtable.html

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Periods Rows

• Even though they skip some squares in between,
  all of the rows go left to right. When you look
  at a periodic table, each of the rows is
  considered to be a different period (Get it? Like
  PERIODic table.)
• quoted from http//www.chem4kids.com/files/elem_pe
  rtable.html

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Across the Periodic Table

• Periods Are arranged horizontally across the
  periodic table (rows 1-7)
• These elements have the same number of valence
  shells.

2nd Period
6th Period
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Periods Rows

• In the periodic table, elements have something in
  common if they are in the same row.
• All of the elements in a period have the same
  number of atomic orbitals.
• Every element in the top row (the first period)
  has one orbital for its electrons. All of the
  elements in the second row (the second period)
  have two orbitals for their electrons. It goes
  down the periodic table like that.
• quoted from http//www.chem4kids.com/files/elem_pe
  rtable.html

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And you got your groups

• The periodic table has a special name for its
  columns, too. When a column goes from top to
  bottom, it's called a group.
• quoted from http//www.chem4kids.com/files/elem_pe
  rtable.html

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Down the Periodic Table

• Family Are arranged vertically down the periodic
  table (columns or group, 1- 18 or 1-8 A,B)
• These elements have the same number electrons in
  the outer most shells, the valence shell.

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Groups Columns

• The elements in a group have the same number of
  electrons in their outer orbital.
• Every element in the first column (group one) has
  one electron in its outer shell. Every element on
  the second column (group two) has two electrons
  in the outer shell. As you keep counting the
  columns, you'll know how many electrons are in
  the outer shell.
• There are some exceptions to the order when you
  look at the transition elements, but you get the
  general idea.

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What do all the numbers mean ?
From www.science-class.net
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Periodic Table Metallic arrangement

• Layout of the Periodic Table Metals vs.
  nonmetals

Nonmetals
Metals
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Other than periods and groups, the table is
divided into families.
From www.science-class.net
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9.16 WARM UP

• What are 3 ways the periodic table is organized?
• 1.
• 2.
• 3.

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Announcements

• See front board
• Experimental Design hard copy
• Bring science fair journals on Friday
• Quiz Friday

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9.16 WARM UP

• What are 3 ways the periodic table is organized?
• 1. Atomic number
• 2. Properties and characteristics
• 3. Valence electrons
• 4. State of Matter
• 5. Metal Properties

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Getting to know the families

• Groups will discuss each family
• Find
• 3 characteristics
• 2 common examples
• Alkali Metals, Alkaline Earth Metals, Transition
  Metals, Rare Earth Metals, Other Metals,
  Non-Metals, Metalloids, Halogens, Noble Gases

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• Alkali Metals 120
• Alkaline Earth 121
• Transition Metals 122
• Lanthanides 122
• Actinides 124
• Metalloids 135

• Carbon Family 130
• Nitrogen Family 131
• Oxygen Family 132
• Halogen Family 133
• Noble Gases 134
• Hydrogen 134

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ALKALI METALS

• very reactive metals that do not occur freely in
  nature
• malleable, ductile, good conductors of heat and
  electricity.
• can explode if they are exposed to water

From www.science-class.net
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ALKLINE EARTH METALS

• metals
• very reactive
• not found free in nature

From www.science-class.net
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TRANSITION METALS

• ductile and malleable, and conduct electricity
  and heat
• iron, cobalt, and nickel, are the only elements
  known to produce a magnetic field.

From www.science-class.net
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RARE EARTH ELEMENTS

• many are man-made

From www.science-class.net
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OTHER METALS

• are ductile and malleable
• are solid, have a high density,

From www.science-class.net
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METALLOIDS

• have properties of both metals and non-metals
• some of the metalloids are semi-conductors. This
  means that they can carry an electrical charge
  under special conditions. This property makes
  metalloids useful in computers and calculators

From www.science-class.net
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NON-METALS

• not able to conduct electricity or heat very well
• very brittle
• Do not reflect light.

From www.science-class.net
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HALOGENS

• "halogen" means "salt-former" and compounds
  containing halogens are called "salts"
• exist in all three states of matter

From www.science-class.net
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NOBLE GASES

• do not form compounds easily
• Happy/Inert Elements (Full outer shells)

From www.science-class.net
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Trends
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Trend 1. Electron Configuration

• Top has fewer electrons, bottom (NE corner) has
  the most
• Electrons increase as you move across and down

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2. Trend in Atomic Radius

• Atomic Radius
• The size of the atom as determined by the
  boundaries of the valence e-. Largest atomic
  species are those found in the SW corner since
  these atoms have the largest n

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3.Trend in Ionization Potential
Ionization potential The energy required to
remove the valence electron from the atom.
Largest toward NE corner of PT since these atoms
hold on to their valence e- the tightest.
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4. Trend in Electron Affinity
Electron Affinity The energy release when an
electron is added to an atom. Most favorable
toward NE corner of PT since these atoms have a
great affinity for e-. (Likelihood to gain an
electron)
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Trends on a graph
3. Ionization Energy Largest toward NE of PT 4.
Electron Affinity Most favorable NE of PT
2. Atomic Radius Z Largest toward SW corner
of PT
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5. Trends with Metals

• Becomes less metal-like from left to right
• More metallic from top to bottom

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Secret Words

• Saying is
• _ _ _ _ _ _ _ _ _ _ _
• _ _ _ _ _ happy.