Periodic+Table+Groups+Overview+Brief

Groups of the Periodic Table.

The alkali metals, found in group 1 of the periodic table (formerly known as group IA), are very reactive metals that do not occur freely in nature. These metals have only one electron in their outer shell. Therefore, they are ready to lose that one electron in ionic bonding with other elements. As with all metals, the alkali metals are malleable, ductile, and are good conductors of heat and electricity. The alkali metals are softer than most other metals. Cesium and francium are the most reactive elements in this group. Alkali metals can explode if they are exposed to water. Sodium and potassium are important in muscle and nerve function. Lithium is important in batteries and medicine. (Shiny/luster, soft, can be shaped, and can conduct electricity and heat. Highly reactive and reacts strongly with water and halogens. These elements tend to lose their one outer electron in chemical reactions.)

The alkaline earth elements are metallic elements found in the second group of the periodic table. All alkaline earth elements usually easily lose 2 electrons when bonding, making them very reactive. Because of their reactivity, the alkaline metals are not found free in nature. . As with all metals, the alkali metals are malleable, ductile, and are good conductors of heat and electricity. These elements lose two electrons when reacting. These metals are not as reactive as group one, but are much more reactive than the transition metals. Calcium is important in teeth and bones. Magnesium and Beryllium are important in making alloys that are light and strong. These alloys are important in vehicles and the aerospace industry.

The 38 elements in groups 3 through 12 of the periodic table are called "transition metals". As with all metals, the transition elements are both ductile and malleable, and conduct electricity and heat. The interesting thing about transition metals is that their outer electrons, or the electrons they use to combine with other elements, are present in more than one shell. This is the reason why they often have 1 to 3 electrons involved in bonding. There are three noteworthy elements in the transition metals family. These elements are iron, cobalt, and nickel, and they are the only elements known to produce a magnetic field.

Metals located in groups 13, 14, and 15. While these elements are ductile and malleable, they are not the same as the transition elements. These elements, unlike the transition elements, do not exhibit variable oxidation states, and their valence electrons are only present in their outer shell. All of these elements are solid, have a relatively high density, and are opaque. They have oxidation numbers of +3, ±4, and -3.

The thirty rare earth elements are composed of the lanthanide and actinide series. One element of the lanthanide series and most of the elements in the actinide series are called trans-uranium, which means synthetic or man-made. All of the rare earth metals are found in group 3 of the periodic table, and the 6th and 7th periods. The Rare Earth Elements are made up of two series of elements, the Lanthanide and Actinide Series.

Metalloids are the elements found along the stair-step line that distinguishes metals from non-metals. This line is drawn from between Boron and Aluminum to the border between Polonium and Astatine. The only exception to this is Aluminum, which is classified under "Other Metals". Metalloids have properties of both metals and non-metals. Some of the metalloids, such as silicon and germanium, are semi-conductors. This means that they can carry an electrical charge under special conditions. This property makes metalloids useful in computers and calculators

Non-metals are the elements in groups 14-16 of the periodic table. Non-metals are not able to conduct electricity or heat very well. As opposed to metals, non-metallic elements are very brittle, and cannot be rolled into wires or pounded into sheets. The non-metals exist in two of the three states of matter at room temperature: gases (such as oxygen) and solids (such as carbon). The non-metals have no metallic luster, and do not reflect light. Nonmetals can gain or lose 4 electrons, lose -3electrons, or lose -2 electrons when bonding.

The halogens are five non-metallic elements found in group 17 of the periodic table. The term "halogen" means "salt-former" and compounds containing halogens are called "salts". All halogens have 7 electrons in their outer shells, giving them an oxidation number of -1. The halogens exist, at room temperature, in all three states of matter:

The six noble gases are found in group 18 of the periodic table. These elements were considered to be inert gases until the 1960's, because their oxidation number of 0 prevents the noble gases from forming compounds readily. All noble gases have the maximum number of electrons possible in their outer shell (2 for Helium, 8 for all others), making them stable.

More: http://physicalsciencecottrell.wikispaces.com/Element+Families

Source: http://www.chemicalelements.com/groups/alkali.html

__What group activity:__

Reacts by losing one electrons Shiny and very soft Extremely reactive Conducts heat and electricity All will react strongly with water

Reacts by losing two electrons Shiny and soft Very Reactive Conducts heat and electricity All but one will react with water.

React slowly with water or not at all Shiny and most are hard Reactive to not very reactive Conducts heat and electricity Strong Many common and valuable metals

Softer or more brittle than transition metals Not as strong as the transition metals Tend to share electrons rather than lose them Able to conduct heat and electricity

Mixed with other metals to make alloys with special properties.

Many of these elements were made in laboratories.

Salt forming Gains or shares one electron in reactions Extremely reactive to very reactive Many are gases at normal temperatures

All are gases Extremely nonreactive Used in many types of lighting

Gains or shares three electrons when reacting

Gains, shares or loses four electrons when reacting

Gains or shares two electrons when reacting.

Malleable and ductile

Insulators and poor conductors

Dull and brittle