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

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

4. 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 - )

5. Noble Gases Characteristics: 1)Stable electron arrangement (8 outer electrons) 2)Extremely high Ionization Energy 3)Tend not to form ions 4)Inert - tend not to take part in chemical changes 5)Very low melting points and boiling points making them gases at room temperature.

7. Hydrogen Has only one electron Can gain 1 electron to become a -1 ion Or Lose 1 electron to become a +1 ion

9. 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 heat 3) react with acids 4) react with non-metals 5)they do not react with each other

10. Metals 6)Malleable – able to be bent or hammered without breaking 7)Ductile – able to stretch to form wire 8)Solid at room temperature (except Mercury) 9)Luster 10) Sliver color (except gold and copper)

12. Nonmetals Elements on right side of the Periodic Table. (Not including Column 18 – the noble gases). Characteristics: 1) Form negative ions 2) React with metals 3) Poor conductors of heat and electricity 4) Do not react with acids 5) React with each other 6) Brittle 7) Dull in appearance

14. Metalloids Elements adjacent to the stair-case like line between metals and nonmetals. Metalloids have characteristics of both metals and non-metals. Characteristics: 1) solid at room temp. 2) Poor conductors of electricity at low temperature 3) Good conductors of electricity at high temperatures

16. Alkali Metals First column on the Periodic Table. Characteristics: 1)Metals 2)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.

17. 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.

19. Alkaline Earth Metals Second column on periodic table. Characteristics: 1)Metals 2)Two electrons in their outer orbit(form +2 ions by losing both electrons) 3)Ionization energy and electronegativity slightly higher than the alkali metals

20. 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

22. Halogens Next 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

23. 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

24. Diatomic Elements Diatomic 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 (H 2 ) Nitrogen (N 2 ) Oxygen (O 2 ) Fluorine (F 2 ) Chlorine(Cl 2 ) Bromine(Br 2 ) Iodine(I 2 )