The Periodic Table. During the nineteenth century, chemists began to categorize the elements...
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Transcript of The Periodic Table. During the nineteenth century, chemists began to categorize the elements...
![Page 1: The Periodic Table. During the nineteenth century, chemists began to categorize the elements according to similarities in their physical and chemical.](https://reader036.fdocuments.net/reader036/viewer/2022062802/56649eac5503460f94bb2439/html5/thumbnails/1.jpg)
The Periodic Table
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During the nineteenth century, chemists began to categorize
the elements according to similarities in their physical and chemical properties. The end result of these studies was our
modern periodic table.
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Dmitri Mendeleev
1834 - 1907
In 1869 he published a table of the elements organized by increasing atomic mass.
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Lothar Meyer
1830 - 1895
At the same time, he published his own table of the elements organized by increasing atomic mass.
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Henry Moseley
1887 - 1915
In 1913, through his work with X-rays, he determined the actual nuclear charge (atomic number) of the elements*. He rearranged the elements in order of increasing atomic number.*“There is in the atom a fundamental quantity which increases by regular steps as we pass from each element to the next. This quantity can only be the charge on the central positive nucleus.”
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Periodic Table Geography
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Periodic Table
• Columns called Families/Groups– Family # indicates # valence (outer shell)
electrons– Elements in same family have similar
properties• Rows called Periods
– Row # indicates # energy levels in atom
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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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Metals/Nonmetals/Semiconductors
• Metals: excellent conductors of heat & electricity; have luster, are ductile/malleable
• Nonmetals: poor conductors of heat & electricity; are dull & brittle
• Semiconductors(Metalloids): elements that under certain conditions conduct heat & electricity
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Families of Elements
• Family 1: Alkali Metals• Family 2: Alkaline Earth Metals• Families 3 to 12: Transition Metals• Family 13: Boron Family• Family 14: Carbon Family• Family 15: Nitrogen Family• Family 16: Oxygen Family• Family 17: Halogens• Family 18: Noble Gases• Three general groups: metals, nonmetals, &
semiconductors(metalloids)
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Periodic Table
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Periodic LawWhen elements are arranged in order of increasing atomic number, there is a periodic pattern in their physical and chemical properties.
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Alkali Metals
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Alkaline Earth Metals
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Transition Metals
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Metals• Alkali metals (Family 1)
– Very reactive– Has 1 valence electron– When ionized has charge of 1+
• Alkaline Earth metals (Family 2)– Reactive– Has 2 valence electrons– When ionized has charge of 2+
• Transition metals (Families 3 to 12)– Somewhat reactive– Valence electron number varies– Ionized charge varies
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InnerTransition Metals
These elements are also called the rare-earth
elements.
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Halogens
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Noble Gases
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Nonmetals• Include H, some elements from families 13 to 16, all
elements from families 17 & 18. Zig-zag line divides metals from nonmetals.
• Inert gases are unreactive; contain 8 valence electrons• Halogens are very reactive; contain 7 valence
electrons; gain electrons becoming negatively charged
• Elements in other families gain electrons to become negatively charged
• These elements plentiful on Earth
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Semiconductors(aka Metalloids)
• Located along the zig-zag line• Includes:
– Boron (B); Silicon (Si), Germanium (Ge), Arsenic (As), Antimony (Sb), Tellurium (Te), Polonium (Po)
• Notice that Al is not considered a metalloid, it is considered a metal
• Conduct heat & electricity under certain conditions• B is hard & added to steel to increase hardness; Sb is
bluish-white and shin, Te is silvery-white & electrical conductivity increases with light exposure, Si important in solar cells & integrated circuits
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#1. Atomic Size - Group trends• As we increase the
atomic number (or go down a group). . .
• each atom has another energy level,
• so the atoms get
bigger.
HLi
Na
K
Rb
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#1. Atomic Size - Period Trends• Going from left to right across a period, the size
gets smaller.
• Electrons are in the same energy level.
• But, there is more nuclear charge.
• Outermost electrons are pulled closer.
Na Mg Al Si P S Cl Ar
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#2. Trends in Ionization Energy
• Ionization energy is the amount of energy required to completely remove an electron (from a gaseous atom).
• Removing one electron makes a 1+ ion.
• The energy required to remove only the first electron is called the first ionization energy.
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Ionization Energy
• The second ionization energy is the energy required to remove the second electron.– Always greater than first IE.
• The third IE is the energy required to remove a third electron.– Greater than 1st or 2nd IE.
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#3. Trends in Electronegativity• Electronegativity is the tendency for an
atom to attract electrons to itself when it is chemically combined with another element.
• They share the electron, but how equally do they share it?
• An element with a big electronegativity means it pulls the electron towards itself strongly!
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Electronegativity Group Trend• The further down a group, the
farther the electron is away from the nucleus, plus the more electrons an atom has.
• Thus, more willing to share.• Low electronegativity.
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Electronegativity Period Trend• Metals are at the left of the table.
• They let their electrons go easily
• Thus, low electronegativity
• At the right end are the nonmetals.
• They want more electrons.
• Try to take them away from others
• High electronegativity.
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The periodic table is the most important tool in the chemist’s
toolbox!