Periodic Table Groups printable pdf download

Investigative Science –P

Friday September 4th, 2015

ERIODIC

ABLE GROUPS

Perry High School

Notebook pages: 72-73

Mr. Pomerantz_________________________________________________________________________Page 1 of 4

There are two main groups on the periodic table: metals and nonmetals. The left-side of the table contains elements with

the greatest metallic properties. As you move from left to right, the elements become less metallic with the far right side

of the table consisting of nonmetals. The elements in the middle of the table are “transition” elements because they are

changing from metallic properties to nonmetallic properties. Elements touching a zigzag line, on the right side of the

table, are metalloids because they have both metallic and nonmetallic properties.

The table is in vertical columns called “groups” or “families” and horizontal rows called “periods”. Each arrangement is

significant. The elements in each vertical column or group have similar properties. Group 1 elements all have one

electron in their outer shells. This gives them similar properties. Group 2 elements all have 2 electrons in their outer

shells. This also gives them similar properties. Not all of the groups, however, hold true for this pattern. The elements in

the first period or row all have one shell. The elements in period 2 all have 2 shells. The elements in period 3 have 3

shells and so on.

There are a number of major groups with similar properties. They are as follows:

Hydrogen: this element does not match the properties of any other group so it stands alone. It is above group 1 but it is

not part of that group. It is a very reactive, flammable, colorless, odorless gas at room temperature. Hydrogen has only 1

valence electron.

Group 1: Alkali metals – These metals are extremely reactive and never exist in nature in their pure forms. Scientists

keep pure alkali metals in mineral oil or kerosene, preventing any explosive reactions with water they are silver colored

and shiny. Their density is extremely low, making soft enough to cut with a knife. They conduct heat and electricity.

Alkali metals have 1 valence electron.

Group 2: Alkaline-earth Metals – Alkaline-earth metals are slightly less reactive than alkali metals. However alkaline-

earth metals are still to reactive to be found alone in nature; they are common in rock formations. They are silver

colored, have higher densities then alkali metals, and possess 2 valence electrons.

Groups 3-12: Transition Metals-these metals have a range of reactivity and wide range of properties. In general, they are

shiny and good conductors of heat and electricity. They are malleable and ductile, like all metals. They also have higher

densities and melting points than groups 1 and 2. Iron, cobalt and nickel are transition metals and they are the only

known element to produce a magnetic field. Transition metals have 1or 2 valence electrons.

Lanthanides (58-71) and Actinides (90-103): These transition metals can be found at the bottom of the table so the table

is not too wide. The elements in these two periods share many properties. The lanthanides are shiny and reactive. The

actinides are radioactive and are therefore unstable. Elements 90-103 do not exist in nature but scientists can

manufacture them in a lab.

Group 13: Boron group – Contains 1 metalloid, 4 metals and all are reactive. Aluminum is in this group. It is also the

most abundant metal in the earth’s crust. Elements in the boron group have 3 valence electrons.

Group 14: Carbon Group – Contains 1 nonmetal, 2 metalloids, and 2 metals and the elements have different reactivity.

These elements have 4 valence electrons.

Group 15: Nitrogen Group – Contains 2 nonmetals, 2 metalloids, and 1 metal element. Reactivity of these elements is

variable, but they all have 5 valence electrons.

Group 16: Oxygen Group contains 3 nonmetals, 1 metalloid, and 1 metal. All the elements are reactive and have 6

valence electrons.

Group 17: Halogens – All the halogens are nonmetals and all are very reactive. They are poor conductors of heat and

electricity and tend to form “salts” with metals. NaCl, for example: Na (sodium) is metal and Cl (chlorine) is a halogen.

Halogens can be solid, liquid or gas at room temperature. All the halogens have 7 valence electrons.

Group 18: Nobel gases – These are non-reactive, nonmetals. All are colorless and odorless gases at room temperature.

All are found in Earth’s atmosphere in small amounts and all have a stable arrangement of 8 valence electrons.

Periodic Table Groups

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