1. The Periodic Table
A guide.

2. The Periodic Table Is a valuable tool to chemists
Gives a lot of information about the elements
Can be used to predict properties of elements

3. What’s on the P.T.? All the elements discovered to date!
92 naturally occurring elements
26 man-made elements

4. How is the P.T. organized? In order of increasing atomic number!
With elements that have similar properties in the same column.
So what is with the 2 rows of elements at the bottom? Where do they fit in?

5. This is where the 2 rows really belong.
So why is it never shown there?
It would make the P.T. too long to fit on a single page.

6. Elements can be metals, nonmetals or metalloids.
Are lustrous (shiny)
Are good conductors of heat and electricity
Are ductile (able to be drawn into wire)
Are malleable (can be pounded into thin sheets
Malleability-
Ductility-

7. Metals on the P.T.
Metals

8. Nonmetals on the P.T.
Nonmetals

9. S
Nonmetals
Are BRITTLE (shatter easily when hit) solids, or liquid or gas at room temperature
Are INSULATORS of heat and electricity
Solids are DULL Cl

10. Metalloids Are between the metals and the nonmetals on the P.T.
Can have properties of both metals and nonmetals
There are 7 METALLOIDS-
Boron
Silicon
Germanium
Arsenic
Antimony
Tellurium
Polonium

11. Arrangement The vertical columns are called GROUPS or families.
All the elements in a group have similar chemical and physical properties!
There are 18 groups on the P.T.
Some are important enough to be named!
The horizontal rows are called PERIODS.
There are 7 periods on the P.T.

12. Alkali Metals – Group 1 Very reactive metals
React vigorously with water and oxygen in the air
Produce bases (alkalis) when reacting with water

13. Alkaline Earth Metals – Group 2
Reactive metals (but not as much as the alkali metals)
The “earth” part of the name comes from being found in compounds within rocks and minerals

14. Halogens – Group 17 Are very reactive nonmetals
name means “salt former” & compounds made with halogens are called salts

15. Noble Gases – Group 18 Are mostly nonreactive nonmetals
Before the 1960s they were considered completely nonreactive
Now we know they can be made to react a little

16. Transition Metals – Groups 3 - 12
Are great conductors!

17. Inner Transition Metals – the 2 lower rows on the P.T.
Are more reactive than the transition metals
Top row called the LANTHANIDES
Bottom row called the ACTINIDES

18. Metalloids

19. Physical/Chemical Properties of Elements on the P.T.
Elements in groups share similar chemical and physical properties.
These similarities can be used to predict trends among the elements on the P.T.

20. Periodic Trends of Elements – some definitions
Atomic radius
Considered to be half the distance between the nuclei of 2 of the same element bonded together

21. Ionic Radius – same as an atomic radius but for ions
An ion – a positively or negatively charged atom made by gaining or losing electrons

22. Ionization energy-
Energy needed to remove an electron from an atom to make it an ion
Metals usually give up electrons more easily than nonmetals do.

23. Electronegativity
The attraction an atom has for another element’s electrons

24. Periodic Trends – the important 2 elements to remember

25. Why these 2 elements? Francium (Fr) Fluorine (F)
Largest atomic & ionic radius
Lowest ionization energy & electronegativity
Fluorine (F)
Smallest atomic & ionic radius
Highest ionization energy & electronegativity
All trends can be figured out if you remember these 2 elements!!!!!!!!!!!!!!!

26. Periodic Trends
Choose any set of elements in a row or in a column and discuss what happens to their trends.