the history of the modern periodic table. history of the periodic table dmitri mendeleev – first...
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The History of the Modern
Periodic Table
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History of the Periodic Table
• Dmitri Mendeleev – first to organize elements according to their properties
• Mendeleev ordered the elements according to increasing atomic mass
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Henry Mosely
• British Scientist 1911
• Re-ordered the periodic table in order of Proincreasing atomic number instead of mass.
• blems with the Mendeleev table disappeared.
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History of the Periodic Table
• Periodic Law: The physical & chemical properties of the elements are periodic functions of their atomic numbers.
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History of the Periodic Table
• Periodic Table: arrangement of elements in order of their atomic numbers so that elements with similar properties fall in the same column.
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Periodic Table Geography
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The horizontal rows of the periodic table are called PERIODS.
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The vertical columns of the periodic table are called GROUPS, or FAMILIES.
The elements in any group of the periodic table have similar physical and chemical properties!
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Alkali Metals (yellow)
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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
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Alkaline Earth Metals(Blue)
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Alkaline Earth Metals
• Second column on the periodic table. (Group 2)
• Reactive metals that are always combined with nonmetals in nature.
• Several of these elements are important mineral nutrients (such as Mg and Ca
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Transition Metals (orange!)
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Transition Metals
• Elements in groups 3-12• Less reactive harder
metals• Includes metals used in
jewelry and construction.
• Metals used “as metal.”
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Halogens (green)
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Halogens
• Elements in group 17• Very reactive, volatile,
diatomic, nonmetals• Always found combined
with other elements in nature .
• Used as disinfectants and to strengthen teeth.
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Noble Gases (Red)
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The Noble Gases• Elements in group 18• VERY unreactive,
monatomic gases• Do not combine with
other elements• Used in lighted “neon”
signs• Have a full valence
shell.
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The Odd Ones
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Hydrogen
• Hydrogen belongs to a family of its own.
• Hydrogen is a diatomic, reactive gas.
• Hydrogen is promising as an alternative fuel source for automobiles
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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
the atmosphere.• Nitrogen and phosphorus are
both important in living things.
• Most of the world’s nitrogen is not available to living things.
• The red stuff on the tip of matches is phosphorus.
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Metalloids
• Along the stair step line of the periodic table
• Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium
• Have characteristics of both metals and nonmetals
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The periodic table is the most important tool in the chemist’s toolbox!
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Metals, Nonmetals, and Metalloids
Metallic character increases down and to the left on the table and nonmetallic character
increases up and to the right on the table.
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Atomic Radii Increase
Ato
mic
Rad
ii I
ncr
ease
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Valence Electrons
• electrons available to be lost, gained, or shared in the formation of chemical compounds
• usually in the outermost s and p orbitals for main group elements (Families 1 & 2, and Families 13-18)
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Valence Electrons for each group
• Group 1: valency +1
• Group 2: +2
• Group 3: +3
• Group 4: 4
• Group 5: -3
• Group 6: -2
• Group 7: -1
• Group 8: 0 stable. does not like to react with others.
• With each electron shell wanting to gain up to 8 electrons on outer shell
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• An electron configuration shows the number of electrons in each orbital in a particular atom.
• Keep this in mind about the number of valence electrons and the Roman numeral column number: The IA family has 1 valence electron; the IIA family has 2 valence electrons; the VIIA family has 7 valence electrons; and the VIIIA family has 8 valence electrons. So for the families labeled with a Roman numeral and an A, the Roman numeral gives the number of valence electrons.
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Neutral Atoms vs. Ions
• Cations – form positive ions by losing electrons (metals)
• Anions – form negative ions by gaining electrons (nonmetals)
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Ionization Energy• Energy required to remove one electron
from a neutral atom of an element.• Increases left to right across the periodic
table.• Increases going from the bottom to the
top of a group.• For each successive electron in an atom
that is removed, the ionization energy increases.
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Ionization Energies Increase
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Electron Affinity• energy change that occurs when a neutral atom gains an
electron• Most atoms release energy when they acquire electrons.
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Electronegativity• measure of an atom’s ability to attract electrons
in a chemical compound• If electron affinity is high, electronegativity will be
high.
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Periodic Table
LanthanidesActinides
Alkaline Metals
Alkaline Earth Metals
Transition Metals
Noble Gases
Halogens
Metalloids
Group 15 pnictogensGroup 16 chalcogens
Group 13 boron familyGroup 14 carbon family
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Metals, Nonmetals, and Metalloids
Metallic character increases down and to the left on the table and nonmetallic character increases up and to the right on the table.
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Periodic Table w/ orbitals
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Interactive Periodic Table
• http://center.acs.org/periodic/tools/PT.html