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The Periodic Table!
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Important People to Remember Dmitri Mendeleev
- published 1st periodic table in 1869- arranged elements by atomic mass
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Important People to Remember
Henry Moseley- arranged the periodic table for
today- arranged elements by atomic
number
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Groups and Periods On the periodic table: Elements are arranged according to
similar properties. Periods Groups
Copyright © 2008 by Pearson Education, Inc.Publishing as Benjamin Cummings
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Metals, Nonmetals, and MetalloidsThe heavy zigzag line separates metals and nonmetals.• Metals are located to
the left.• Nonmetals are located
to the right. • Metalloids are located
along the heavy zigzag line between the metals and nonmetals.
Copyright © 2008 by Pearson Education, Inc.Publishing as Benjamin Cummings
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Metals To the left of the Zigzag Malleable (smashed into thin sheets) Ductile (stretched into wires) Conduct heat and electricity Shiny Reactive High Melting Points Mostly Solids at room temperature
- except Hg (liquid)
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Examples of Metals Fe
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Non-Metals
Right of the zigzag (Upper right side) Poor conductor of electricity Dull Brittle Low Melting Points Mostly gases at room temperature
- Liquid (Bromine)- Solids (Sulfur, Phosphorus, Carbon)
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Examples of Nonmetals
Sulfur
Carbon
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Metalloids
Along the zigzag line! Has properties of both metals AND
nonmetals! Somewhat shiny solids, not much
luster Semiconductive B, Si, Ge, As, Sb, Te, Po, At
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Examples of Metalloids
Silicon
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Names of Some Representative Elements• Several groups of
representative elements are known by common names.
Copyright © 2008 by Pearson Education, Inc.Publishing as Benjamin Cummings
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Alkali Metals Group 1: Li, Na, K, Rb, Cs, Fr VERY reactive Soft Metals Rarely exist in nature alone Form salts when combined
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Alkaline Earth Metals Group 2: Be, Mg, Ca, Sr,
Ba, Ra Reactive Found in compounds that
are in the Earth’s Crust More dense and harder
than alkali metals
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Transition Metals In the middle (d-
block) Much LESS reactive Electron in highest
energy level can change
Therefore when they form ions, their charges can vary.
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Examples:
Cu+1
Cu+2
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Halogens Group 7: F, Cl, Br, I, At Most reactive non metals Fluorine most reactive non metal Physical properties very within
group
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Noble Gases Group 8: He, Ne, Ar, Kr, Xe,
Rn Don’t react or combine with
anyone! (Unless forced) INERT GASES
Low Boiling Points All gases at room temperture
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Lanthanides
Elements 58-71 - All occur in nature except 61
Rare earth metals Very reactive High melting points and boiling
points Used in lamps, lasers, magnets, and
motion picture projectors.
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Actinides
Elements 90-103 Most are synthetic (man-made) Almost all are radio active Very dense Can be found in smoke detectors,
nuclear weapons, and radio active minerals
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Periodic Law
- Periodic Law = trends that occur throughout the periodic table
- -Atomic Radius -Ionization Energy -Electronegativity
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How are the elements organized? Atoms in the same group have the
same number of valence electrons. Outer shell = valence shell
(outside electrons) 8 valence electrons= stable Valence electrons determine
reactivity and how strongly an atom will bond with other atoms.
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Determine Valence Electrons
- These atoms want 8 valence electrons
- Is it easier for them to gain or lose a certain amount of electrons?
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Atomic Radius Trend
What is atomic radius?
- Distance from the nucleus to the valence electrons
- It’s the size of the atom!
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Atomic Radius
-As you go across the period what happens to the atomic radius?
-As you go down a group what happens to the atomic radius?
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Atomic Radius Trend
As you go across a period, the number of protons increases (e- increase too, but on the same energy level). More p+ can pull in e- closer, decreasing the radius.
More attractions = SMALL atomic radius
As you go down a group, e- are added to new energy levels. Each level is further from the nucleus, which increases the radius.
More energy levels = LARGE atomic radius
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Electronegativity Electronegativity is the atom’s want to
gain electrons
An atoms LOVE for electrons!!
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Electronegativity
- What happens when you go across a period?
- Down a group?
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Electronegativity As you go across a period, electrons are held more closely because the
atomic radius decreases. It is easier to attract electrons, so electronegativity increases.
Small radius (more attractions) = HIGH electronegativity
As you move down a group, electrons are further away from nucleus because the atomic radius increases. It is harder to attract electrons, so electronegativity decreases.
Large radius (less attractions) = LOW electronegativity
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Electronegativity
Look at the dot structures!
The atom that wants to GAIN electrons will have a high electronegativity!
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Ionization energy
Ionization Energy is the energy needed to remove a valence electron
-What do see as you go across the period?
-What happens to the energy going down a group?
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Ionization energy •As you go across a period, electrons are held more closely
because the atomic radius decreases. It is easier to attract electrons, so electronegativity increases.
Small radius (more attractions) = HIGH ionization energy
As you go down a group, electrons are further from nucleus because the atomic radius increases. It takes less energy to remove an electron, so the ionization energy decreases.
Large radius (less attractions) = LOW ionization energy
You can also look at the dot structures!