Family or Group – a vertical column on the Periodic Table made up of similar elements

Period or Series – A horizontal row on the periodic table . The period indicates the number of orbits.

Noble Gases

Last column on periodic table

Noble gases have complete outer energy levels

(8 e- in their outer orbit, except Helium

which has 2e- in its only energy level, remember the 1st orbit is filled with 2

e-)  

Noble Gases

Characteristics:  1) Stable electron arrangement (8 outer

electrons)2) Extremely high Ionization Energy3) Tend not to form ions4) Inert - tend not to take part in chemical changes5) Very low melting points and boiling points making them gases at room temperature.

Hydrogen

Has only one electron

Can gain 1 electron to become a -1 ion Or

Lose 1 electron to become a +1 ion

Metals

Elements on left side of the Periodic Table. Metals tend to:

1) form + ions by giving up electrons.2) good conductors of electricity and heat3) react with acids4) react with non-metals5) they do not react with each other

Metals

6) Malleable – able to be bent or hammered without breaking

7) Ductile – able to stretch to form wire8) Solid at room temperature (except

Mercury)9) Luster10) Sliver color (except gold and copper)

NonmetalsElements on right side of the Periodic Table. (Not including Column 18 – the noble gases).

 Characteristics:  1) Form negative ions

2) React with metals3) Poor conductors of heat and electricity4) Do not react with acids5) React with each other6) Brittle7) Dull in appearance

Metalloids

Elements adjacent to the stair-case like line between metals and nonmetals.

 

Metalloids have characteristics ofboth metals and non-metals.

Characteristics:

1) solid at room temp.2) Poor conductors of electricity at low temperature3) Good conductors of electricity at high temperatures

 

Alkali MetalsFirst column on the Periodic Table.

Characteristics: 1) Metals2) Very soft (can be cut with a butter

knife)3) One electron in their outer orbit (they

form +1 ions by losing this electron).4) Low Ionization Energy and

Electronegativity making it easy to remove electrons.

Alkali Metals

5) Highly reactive (react violently with water, acids and peroxides) Due to this high reactivity these elements are never found in pure form in rocks.

6) Reactivity increases going down the family.

7) Form very strong bonds.

Alkaline Earth MetalsSecond column on periodic table.

 Characteristics:

1) Metals2) Two electrons in their outer

orbit(form +2 ions by losing both electrons)

3) Ionization energy and electronegativity slightly higher than the alkali metals

Alkaline Earth Metals

4) Still highly reactive but a little less reactive than alkali metals. Due to their reactivity these elements are never found in pure form in rocks.

5) Reactivity increases down the family

6) Form slightly weaker bonds than the alkali metals.

7) Slightly harder than the alkali metals

HalogensNext to last column on Periodic table.

Characteristics:1) Non-metals 2) 7 electrons in their outer orbit

(gain 1 e- to become –1 ions)3) very high ionization energy and

electronegativity making it easy for them to gain electrons.

4) Highly reactive

Halogens

5) Reactivity increases going up the family

6) React with all elements on the P.T. except He, Ne and Ar

7) Do not occur as individual (unbonded atoms) in nature

Diatomic ElementsDiatomic molecule – a molecule made up of 2 atoms

of the same element. There are seven elements that will form diatomic molecules any time they are present in their pure

form. These elements are:  Hydrogen (H2)

Nitrogen (N2)

Oxygen (O2)

Fluorine (F2)

Chlorine(Cl2)

Bromine(Br2)

Iodine(I2)