1. Aim: How are Elements Organized in the Periodic Table?
DO Now:
1. How would you organize these buttons?
2. How do you think elements are organized in the periodic table?
3. Write at least one trend you notice about the elements in the periodic table.

2. History of the Periodic Table
The first periodic table was developed in Russia in 1869 by chemist Dmtri Mendeleev; he arranged the elements in order of increasing atomic mass.
The modern periodic law states: elements are arranged in order of increasing atomic numbers.
Chemists use the properties of elements to sort them into groups.

3. Periods and Groups Periods Groups or Families Vertical columns
Horizontal rows
The # of the period indicates the # of energy levels (shells) in the element
The # of valence electrons (electrons in outer shell) increases from right to left
Properties of elements change across a period
Vertical columns
Most elements within the same group have the same number of valence electrons (electrons in outermost shell); therefore, have similar chemical properties

4. Three Classes of Elements
Metals
Alkali Metals
Alkaline Earth Metals
Transition Metals
Inner Transition Metals
Metalloids
Nonmetals
Halogen
Noble Gases

6. Metals vs Non Metals Properties Metals
solids at room temperature are malleable
are ductile
have luster
good conductors of heat and electricity
Properties of Nonmetals
many are gases at room temperature
not malleable, tend to be brittle in the solid phase.
surface is dull
poor conductors of heat and electricity

7. Metallic Character
The metallic character of an element can be defined as how readily an atom can lose an electron.
Metallic characteristics decrease from left to right across a period, and  increase down a group.

9. Alkali Metals and Alkaline Earth Metal
Alkaline Earth Metals
Group 1
Most active metals in the periodic table
All react vigorously with water to produce H2(g)
They are shiny, have the consistency of clay, and are easily cut with a knife.
Reactivity increases as you go down this period
Group 2
Second most active metals

11. Transition Metals and Inner Transition Metals
The elements in Groups 3 through 12
Typically hard solids with high melting points, with the exception of mercury
Form colored compounds.
Are good conductors of heat and electricity.
Can be hammered or bent into shape easily.(malleable)
Are less reactive than alkali metals such as sodium.

13. Metalloids
They can be found adjacent to the stair-step line in the periodic table.
Have properties similar to those of metals and nonmetals.
Solids
Can be shiny or dull
Ductile
Malleable
Conduct heat and electricity better than nonmetals but not as well as metals

14. Metalloids Cont.
boron (B), silicon (Si), germanium (Ge), arsenic (As), antimony (Sb), tellurium (Te), and polonium (Po) are the elements found along the step like line between metals and non-metals of the periodic table.

16. Halogens
Group 17
Halogens have 7 valence electrons, which explains why they are the most active non-metals
Have low melting points and boiling points
Chemical reactivity decreases as you go down the group

18. Noble Gases Group 18 Colorless gases
Do not chemically react with other elements (inert or stable)
Are isolated atoms

19. Activity
Given the blank periodic table fill in each category with a different color.
Alkali Earth Metals Nonmetals
2. Alkaline Earth Metals 7. Nobles Gases
3. Transition Metals Metalloids
4. Inner transition Metals 9. Other Metals
5. Metalloids Halogens