This chemistry project document summarizes the properties and characteristics of different groups of elements on the periodic table. It describes the alkali metals, alkali earth metals, transition metals, metalloids, non-metals, halogens, noble gases, and rare earth metals. It also discusses atomic properties such as atomic radius, ionic radius, ionization energy, and electronegativity.

1. Chemistry Project
By Joe Carrillo

2. alkali metals
• Lithium. Sodium, Potassium, Rubidium, cesium*, Francium*.
• These are found in group 1A, with one electron in their valence shell.
• They are highly reactive and aren’t found in nature.
• Their physical characteristic is malleability, ductile, and good conductors of
electricity.
• The elements marked with a * in the upper right corner are the most reactive and
will explode with contact to water.
• http://www.chemicalelements.com/groups/nonmetals.html

3. Alkali earth metals
• Beryllium, Magnesium, Calcium, Strontium, Barium, Radium.
• These elements are found in the second row of the periodic table.
• All of these elements have an oxidation number of+2, which makes very reactive
to other elements and compounds.
• Like the Alkali metals they are not found free in nature.
• http://www.chemicalelements.com/groups/nonmetals.html

4. Transition metals
• Examples: Iron*, Cobalt*, Nickel*, Copper, Zinc, Platinum, Gold, Mercury.
• There are 38 transition metals, and they are found in groups 3- 12.
• Like all metals they are malleable, shiny, ductile and good conductors of electricity and
heat.
• there electrons they use to combine with other elements, are present in more than one
shell.
• several common oxidation states.
• The marked* elements are the only elements to produce a magnetic force field.
• The size is determined by the 4s electrons. The pull of the increasing number of protons
in the nucleus is more or less offset by the extra screening due to the increasing
number of 3d electrons.
• http://www.chemguide.co.uk/atoms/properties/atradius.html
• http://www.chemicalelements.com/groups/nonmetals.html

5. metalloids
• Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium, Polonium.
• Found on the “stair steps” on the periodic table. Aluminum is an exception and is
classified as “ other metals.”
• Properties of both metals and non metals. Some are semi-conductors silicon and
germanium.
• They are useful in computers and calculators.
• http://www.chemicalelements.com/groups/nonmetals.html

6. Non-metals
• Hydrogen, Carbon, Nitrogen, Oxygen, Prosperous, Sulfur,.
• Don’t conduct electricity / heat very well. Unlike metals they are brittle and break
easily. Don’t reflect light.
• exist in two of the three states of matter, Gases and Solids.
• oxidation numbers of ±4, -3, and -2.
• http://www.chemicalelements.com/groups/nonmetals.html

7. halogens
• Group 17
• Solid- Iodine, Astatine
• Liquid- Bromine
• Gas- Fluorine, Chlorine
• Halogen means “salt former”, the outer ring has seven eclectrons always.
• oxidation number of -1
• They exist in all 3 forms of matter at room temp.
http://www.chemicalelements.com/groups/nonmetals.html

8. Noble gasses
• Helium, neon, argon, Krypton, xenon, radon.
• Their oxidation charge is zero which makes it very difficult for compounds to be
formed.
• The valence ring is full except for helium with only 2 electrons in its outer ring .
• http://www.chemicalelements.com/groups/nonmetals.html

9. Rare earth metals
• thirty rare earth elements are composed of the lanthanide and actinide series.
• On element from the lanthanide series is “man made” and most of the actinide
series are man made.
• Found in group 3, 6, and 7 of periodic table.
• http://www.chemicalelements.com/groups/nonmetals.html

10. Atomic radius
• Atomic radius generally increases as you move down a group.
• Definition: is half of the distance between the centers of two atoms of that
element that are just touching each other.
• Generally, the atomic radius decreases across a period from left to right and
increases down a given group.
• http://chemistry.about.com/od/periodictableelements/a/periodictrends.htm

11. Ionic radius
• Ionic radii are difficult to measure with any degree of certainty, and vary according
to the environment of the ion.
• several different measures of ionic radii in use.
• an atom doesn't have a fixed radius. The radius of an atom can only be found by
measuring the distance between the nuclei of two touching atoms, and then
halving that distance.
• http://www.chemguide.co.uk/atoms/properties/atradius.html

12. Ionization energy
• one mole of a substance (molar ionization energy or enthalpy) and reported in
kJ/mol. In atomic physics the ionization energy is typically measured in the unit
electron volt eV). Large atoms or molecules have a low ionization energy, while
small molecules tend to have higher ionization energies.
• http://en.wikipedia.org/wiki/Ionization_energ
y

13. Electro negativity
• The amount of energy required to remove an electron from an atom, forming a
cation.
• A property of an atom which increases with its tendency to attract the electrons of
a bond.
Examples: The chlorine atom has a higher electronegativity than the hydrogen
atom, so the bonding electrons will be closer to the Cl than to the H in the HCl
molecule.
• http://chemistry.about.com/od/chemistryglossary/a/Electronegdef.htm