The Periodic Table and the Elements

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Presentation transcript:

The Periodic Table and the Elements What is the periodic table ? What information is obtained from the table ? How can elemental properties be predicted base on the PT ?

Elements are arranged: Vertically into Groups Groups are also called Families. Horizontally Into Periods

Why?

If you looked at one atom of every element in a group you would see…

Each atom has the same number of electrons in it’s outermost shell. An example…

The group 2 atoms all have 2 electrons in their outer shells Be (Beryllium) Atom Mg (Magnesium) Atom

The number of outer or “valence” electrons in an atom effects the way an atom bonds. The way an atom bonds determines many properties of the element. This is why elements within a group usually have similar properties.

If you looked at an atom from each element in a period you would see…

Each atom has the same number of electron holding shells. An example…

The period 4 atoms each have 4 electron containing shells 4th Shell K (Potassium) Atom Kr (Krypton) Atom Fe (Iron) Atom

Each group has distinct properties The periodic Table is divided into several groups based on the properties of different atoms.

Soft, silvery colored metals http://www.lyon.edu/webdata/Users/DMcDowell/GenChem/alkalishow.html Alkali Metals Soft, silvery colored metals Very reactive!!!

Alkali Metals reacting with water: Li (Lithium) Na (Sodium) K (Potassium) Rb (Rubidium) Cs (Cesium) What would you expect from Francium?!?!

Alkaline Earth Metals Silvery-White Metals Fairly reactive Many are found in rocks in the earth’s crust

Transition Metals Most are good conductors of electricity and heat Malleable (easily bent/hammered) and ductile (can be formed into wires)

How many things can you think of that have Transition Metals in them?

Metalloids lie on either side of these “stairsteps” They share properties with both metals and non-metals Si (Silicon) and Ge (Germanium) are very important “semi-conductors”

What are semiconductors used in?

Nonmetals Brittle Do not conduct electricity

Halogens Most are Poisonous Fairly reactive

Chlorine Gas was used as a chemical weapon during World War I. It was used by the Nazis in World War II.

Noble Gases Unreactive Gases at room temperature

Jellyfish lamps made with noble gases artist- Eric Ehlenberger

Colors Noble Gases produce in lamp tubes: Ne (Neon): orange-red Hg (Mercury): light blue Ar (Argon): pale lavender He (Helium): pale peach Kr (Krypton): pale silver Xe (Xenon): pale, deep blue

Lanthanide Series Actinide Series

Trends on the Periodic Table Atomic # increases going from left to right therefore the number of electrons increases from left to right. However, even though you have more electrons in the shells the atomic size actually decreases from left to right. This is because of electron shielding. Electrons repel against each other. More electrons= more repulsion=larger radius

The Periodic Table 02

2. Trend in Atomic Radius Atomic Radius: The size of at atomic specie as determine by the boundaries of the valence e-. Largest atomic species are those found in the SW corner since these atoms have the largest n, but the smallest Zeff.

Atomic radii