The periodic table and Subatomic particles

1
The periodic table and Subatomic particles
2
Bell Work

• Write the formula for
• Dicarbon tetrachloride
• Hydrosulfuric acid

3
Review - The atom

• Building block of matter
• Each element is made up of only one kind of atom
• We have approximately 116 elements located on the
  periodic table

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Introduction to the periodic table

• Symbols and names
• Approximately 109 elements on the periodic table,
  we are not going to focus on elements 110-118.
• The elements are named for properties, place of
  discovery, or people who discovered them
• Symbols consist of 1, 2, or 3 letters. The first
  letter is always capitalized.

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By observing the properties of the elements on
the periodic table

• The periodic table is an arrangement of elements,
  in order of increasing atomic number, in
  horizontal rows of such a length that elements
  with similar chemical properties fall directly
  beneath one another in vertical groups.

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Lets color the periodic table to help us learn
about the different parts

• Get the following colors please
• Black, red, brown, yellow, orange, pink, purple,
  light green, light blue, dark blue, dark green
• Color Hydrogen light black you still have to be
  able to read through the color.
• Color group (column) 1 red.
• Color group 2 brown.

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• Color the Lanthanides orange. (elements 57-71)
• Color the Actinides pink. (elements 89-103)
• Color the Metalloids purple (elements 5, 14,
  32, 33, 51, 52, 84, 85)
• Color group 17 light green (except for element
  85).
• Color groups 3-12 light blue. (and elements 31,
  49, 81, 50, 82, 83)
• Color Aluminum dark blue.
• Color group 18 yellow.
• Color any remaining element that has not been
  colored yet dark green.

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Lets make a legend

• On the back of your paper
• Black hydrogen
• Red alkali metals
• Brown alkaline earth metals
• Yellow noble gases
• Orange lanthanides
• Pink actinides
• Purple metalloids
• Light blue transition metals
• Dark blue aluminum
• Light green halogens
• Dark green CNO group

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Aqua- Alkali metals yellow- Alkaline Earth
metals Orange- Transition MetalsLight pink/Dark
pink- Inner transitional metals Dark Blue- other
metalsLight Blue- Metalloids White-
Non-metalslight brown- Halogens Neon green-
Nobel Gases
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Early scientists and the periodic table

• Noticed trends in the properties of the elements
  and began grouping them in various ways

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Dmitri Mendeleev 1871

• Introduced the first modern periodic table
• Listed elements in columns in order of increasing
  atomic mass
• Only about 70 elements were known
• Arranged columns so the elements with the most
  similar properties were side by side
• Left blank spaces
• Predicted properties of missing elements
• Remarkably accurate

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Henry Moseley -- 1913

• Determined atomic number
• Arranged the elements in the periodic table by
  their atomic number
• Is used today

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Periodic Law

• Periodic Law when the elements are arranged in
  order of increasing atomic numbers, there is a
  periodic repetition of their physical and
  chemical properties

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The Modern Periodic Table

• Group Each vertical column
• Also called a family
• Have similar physical and chemical properties
• Identified by a
• number (1-18)

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Group A Representative Elements

• These elements have more predictable bonding
  properties due outer electrons (valence).
• Main group elements
• Group A includes the first two columns and the
  last six.
• Only need to memorize four group names
• Alkali metals (IA or 1A)
• Alkaline earth metals (IIA or 2A)
• Halogens (VI A or 6A)
• Noble Gases (VIII or 8A)

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Group B elements

• Groups 3 12 on the periodic table
• Called the transition elements

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The Modern Periodic Table

• Periods horizontal rows (7 of them)
• Elements in the same period do not have similar
  properties in terms of reactions
• Number of elements per period
• 2 (period 1) to 32 (periods 6 and 7)

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Metals

• Most elements are metals. 88 elements to the left
  of the stair-step line are metals or metal like
  elements.
• Physical Properties of Metals
• Normally solids (Hg is an exception)
• Luster (shininess)
• Good conductors of heat and electricity
• High density (heavy for their size)
• High melting point
• Ductile (most metals can be drawn out into thin
  wires)
• Malleable (most metals can be hammered into thin
  sheets)

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Metals

• Chemical Properties of Metals
• Easily lose electrons
• Corrode easily. Corrosion is a gradual wearing
  away. (Example silver tarnishing and iron
  rusting)

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Non-metals

• Nonmetals are found to the right of the
  stair-step line.
• Their characteristics are opposite those of
  metals.
• Physical Properties of Nonmetals
• No luster (dull appearance)
• Poor conductor of heat and
• electricity
• Brittle (breaks easily)
• Not ductile
• Not malleable
• Low density
• Low melting point

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Non-metals

• Chemical Properties of Nonmetals
• Tend to gain electrons (becoming negatively
  charged ions, anions)
• Since metals tend to lose electrons and nonmetals
  tend to gain electrons, metals and nonmetals like
  to form compounds with each other. These
  compounds are called ionic compounds.

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Metalloids

• Physical Properties of Metalloids
• Solids
• Can be shiny or dull
• Ductile
• Malleable
• Conduct heat and electricity better than
  nonmetals but not as well as metals
• Have properties of both metals and nonmetals
• Group of elements that exist between the metals
  and the nonmetals
• These elements particularly Si are used in
  semiconductors
• B, Si, Ge, As, Sb, Te, Po, At

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Group 1 (or IA) Alkali Metals

• 1st column on P.T. , does not include Hydrogen
  (H)
• Can cut these metals with a knife
• They are so reactive to oxygen and water that
  they do not occur in nature in their pure state
  and must be stored under some inert liquid to
  keep them from reacting.

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Alkali metals (cont.)

• Their reactivity increases as you go down the
  group because their size increases making it
  easier for an electron to be removed.
• Ex. Francium (Fr) more reactive than Sodium (Na)
• When in water form basic solution (pH7)
• They all contain one valence electron which is
  given up easily in a chemical compound.

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Sodium (Na) and Water
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Group 2 or II A- Alkaline Earth Metals

• Second column on the periodic table
• They are not as soft as the Group 1 metals.
• They are too reactive to occur in nature in their
  pure state, but NOT as reactive as alkali metals.
• They react more mildly with oxygen to produce
  oxides of metals and will only react with water
  at temperatures where the water is steam.
• Their reactivity increases as you go down the
  column due to the increase in size and ease that
  electrons can be removed.
• Found on earths crust

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Group 17 of VII A- Halogens

• Very reactive since they need only one electron
  to become like a noble gas (8 valence electrons,
  octet)
• The halogens are five non-metallic elements found
  in group 7 A or group 17 of the periodic table.
• The term "halogen" means "salt-former" and
  compounds containing halogens are called "salts".
  

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Group 17 or VII A Halogens (continued)

• None of the halogens can be found in nature in
  their elemental form.
• All form diatomic molecules (F2, Cl2, Br2, and
  I2)
• The halogens exist, at room temperature, in all
  three states of matter
• Solid- Iodine, Astatine
• Liquid- Bromine
• Gas- Fluorine, Chlorine

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Interesting facts about Halogens (not on test)

• Fluoride ions are found in minerals such as
  fluorite (CaF2) and cryolite (Na3AlF6).
• Chloride ions are found in rock salt (NaCl), the
  oceans, which are roughly 2 Cl- ion by weight,
  and in lakes that have a high salt content, such
  as the Great Salt Lake in Utah, which is 9 Cl-
  ion by weight.
• Both bromide and iodide ions are found at low
  concentrations in the oceans, as well as in brine
  wells in Louisiana, California, and Michigan.

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Group 18 or group VIII A - Noble Gases

• Have a complete octet, 8 electrons in outer shell
  (valence shell)
• Very stable and un-reactive (inert)

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Group B - Transition Metals

• The lower middle section of the P.T.
• DO NOT need to memorize the column names
• These metals have multiple oxidation numbers
  (charges), which means that they can bond in
  multiple ways.
• These are the d area elements

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Inner Transitional Metals or Rare Earth Metals

• Lathanide series begins with Lathanum (La) and
  ends with Lutetium (Lu)
• Actinide series begins with Actinium and ends at
  Lawrencium(Lr)
• These are the f area elements

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Why use roman numerals?

• The roman numeral at the top of the main-group
  families indicates the number of valence (outer
  shell) electrons in that element
• Valence electrons are normally considered to be
  only the s and p electrons in the outermost
  energy level

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Of the 113 elements

• Only two (Hg and Br) are liquids under normal
  conditions
• The noble gases, H, N,O, F, and Cl are gases at
  room temperature
• The remaining elements are solids

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Diatomics

• Elements that naturally occur bonded to
  themselves
• Hydrogen H2
• Nitrogen N2
• Oxygen O2
• Fluorine F2
• Chlorine Cl2
• Bromine Br2
• Iodine I2

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Other elements to know

• Sulfur usually exists as S8
• Phosphorus usually exists as P4

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Allotropes

• Most elements in the periodic table exist in
  nature in only one form
• Others have multiple forms that are these are
  called allotropes
• For example carbon exists as graphite, diamond,
  and the newly discovered buckminsterfullerene
• Graphite conducts electricity and is slippery
  enough to be used as a metal lubricant
• Diamond is the hardest of all natural materials
  and are used in industrial grinding machines
• Buckminsterfullerence is the form with 60 carbon
  atoms in clusters

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Examples of allotropes

• Arsenic
• Gray allotrope is metallic
• Yellow allotrope of As4 molecule is nonmetallic
• Oxygen
• Phosphorus
• One is white burns spontaneously in air
• Red and black allotropes are long chains of atoms
  that are more stable
• Selenium
• Sulfur
• One is the S8 molecule that is nonmetallic
• Another is semi-metallic
• Tin
• Three allotropes one that has a distinctly
  metallic look and two that are white crystals

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Now that we can understand the periodic table

• Lets go on to looking at the atoms of the
  elements