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ELEMENTS
Remember:
• Atoms of one type form an element
• Elements are the simplest form of a substance
• Every element is unique and has its own chemical and physical properties
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Dimitri Mendeleev• Russian chemist who
worked in the mid 1800’s
• Researched the 63 known elements
• Made cards for each element with all the facts he could find
• Developed the first periodic table by atomic mass
• Not perfect!!
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Henry Moseley• British scientist who
determined atomic numbers for the elements
• When elements arranged by atomic number and properties every element fell in place perfectly
• Periodic Law: Properties of elements repeat in a predictable way when atomic numbers are used to arrange elements into groups.
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Elements are arranged:
Vertically into Groups
Horizontally Into Periods
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Why?
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If you looked at one atom of every element in a group you would
see…
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Each atom has the same number of electrons in it’s outermost shell.
• An example…
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The group 2 atoms all have 2 electrons in their outer shells
Be (Beryllium)
Atom
Mg (Magnesium) Atom
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• The number of outer or “valence” electrons in an atom effects the way an atom joins with other atoms.
• The way atoms join determine many properties of the element.
• This is why elements within a group usually have similar properties.
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If you looked at an atom from each element in a period
you would see…
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Each atom has the same number of electron holding shells.
An example…
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The period 4 atoms each have 4 electron containing shells
K (Potassium)
AtomFe (Iron) Atom
Kr (Krypton)
Atom
4th Shell
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Each group has distinct properties
• The periodic Table is divided into several groups based on the properties of different atoms.
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Alkali Metals
Soft, silvery colored metals
Very reactive especially with water
Not found in pure form in nature
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Alkaline Earth Metals
Silvery-White Metals
Fairly reactive
Many are found in rocks in the earth’s crust
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Transition Metals
Malleable (easily bent/hammered into wires or sheets)
Most are good Conductors of electricity
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How many things can you think of that have Transition Metals in
them?
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Metalloids lie on either side of the “stairstep” line
They share properties with both metals and non-metals
Si (Silicon) and Ge (Germanium) are very important “semi-conductors”
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Where are semiconductors used?
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Nonmetals
Brittle
Do not conduct electricity
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Groups 13-16
Group 13Boron Group
Group 14Carbon Group
Group 15Nitrogen Group
Group 16 Oxygen Group
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Most are poisonous
Fairly reactive
Halogens
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Chlorine Gas was used as a chemical weapon during World War I.
It was used by the Nazis in World War II.
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Non-reactive
Gases at room temperature
Very Stable
Noble Gases
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WHY STABLE?
Noble gases have full valence levels!
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Actinide Series
•Share properties of Group 3 transition metals•Rare and some are radioactive•Elements with atomic numbers greater than 92 (Uranium) are synthetic.Lanthanide Series