1. 3.3 – NOTES – The Groups of the Periodic Table

2. A.9 The Elements
Two major classifications of elements are metals and nonmetals
Metalloids are intermediates between the two main groups and are located along the stairstep between metals and nonmetals
Metalloids have properties of both metals and nonmetals

4. A.10 Organization of the Periodic Table
Horizontal rows are called periods
Contain electrons in the same energy level
Metals are on the left and nonmetals are on the right
Vertical columns are called groups or families

5. 1 2
3-12 13 14 15 16 17 18
Lanthanide Series
Actinide Series

6. Group 1 Called the alkali metals React very violently with water
All of these elements are metals except hydrogen
1 valence electron
Very soft, very reactive
Examples and other information
sodium, lithium, potassium

7. Group 2 Called the alkaline earth metals
Also very reactive, but not as much as group 1
2 valence electrons
Examples and other information
Magnesium and Calcium

8. Groups 3-12 Called the transition metals Very stable elements
Valence electrons don’t follow pattern
Mercury is the only liquid metal at room temperature
Examples and other information
Copper, iron, gold, silver, nickel
Inner transition
Actually located between groups 2 and 3 in periods 6 and 7,
but placed two rows below the periodic table to
conserve space
Very rare elements
Lanthanide Metals contain elements 57-70
Actinide Metals contain elements
all radioactive, some naturally occurring others are synthetic

9. Group 17 Called the Halogens All nonmetal elements Very Reactive
Elements in all three states of matter (Solid, Liquid, Gas)
7 valence electrons
Examples and other information
Iodine, Bromine, Fluorine

10. Group 18 Called the Noble Gases Do not react to form compounds
Have 8 valence electrons
All Gases
Examples and other information
Helium, Neon, Argon, Krypton, Xenon, Radon

11. Groups are mixed groups and contain both solids, liquids, and gases. They are named by the first element in the group. These elements vary in properties and uses
Group 13 is the Boron group, 3 valence electrons
Group 14 is the Carbon group, 4 valence electrons
Group 15 is the Nitrogen group, 5 valence electrons
Group 16 is the Oxygen group, 6 valence electrons

14. A.11 Predicting Properties
Periodic properties: vary among elements according to trends that repeat as atomic number increases
Properties can be estimated by elements above and below on the table
Mendeleev was unaware of several elements when he designed the periodic table, but he guessed at their existence and properties based on the elements surrounding the empty spaces