1. Chapter 6 The Periodic Table and Periodic Law

2. Chapter 6 Standards
CHEM.A Explain how the periodicity of chemical properties led to the arrangement of elements on the periodic table.
CHEM.A Compare and/or predict the properties (e.g., electron affinity, ionization energy, chemical reactivity, electronegativity, atomic radius) of selected elements by using their locations on the periodic table and known trends.

3. Development of the Modern Periodic Table
Section 6.1
Development of the Modern Periodic Table

4. Objectives
Trace the development and Identify key features of the periodic table.

5. Key Terms Periodic law Group Period Representative elements
Transition elements
Metals
Alkali metals
Transition metals
Inner transition metals
Nonmetals
Halogens
Noble gases
metalloid

6. History 1790s, French scientist Lavoisier 23 elements
1800s: electricity and spectrometer

7. John Newlands Patterns on the periodic table Law of octaves
Elements on the eights had similarities

9. Meyer & Mendeleev 1869: connection between atomic mass and properties
Mendeleev published first
Left holes of undiscovered elements
Predicted properties of undiscovered elements- Sc, Ga, Ge

10. Moseley Problems with Mendeleev Rows by increasing atomic mass
Moseley used atomic number instead

11. The Periodic Law
There is periodic repetition of chemical and physical properties when elements are arranged by increasing atomic number.

12. The Modern Periodic Table
Horizontal rows- periods (7)
Vertical columns- groups or families (18)

13. Groups 1,2 and 13-18= Representative Elements
Groups 3-12= Transition Elements

14. Metals shiny, smooth solid room temperature
good conductors of heat and electricity

15. Alkali Metals
Group1 (excluding hydrogen)
highly reactive

16. Alkaline Earth Metals
Group 2
highly reactive (not as much as 1)

17. Group B Metals Transition metals elements contained in D block
Inner transition metals
the lanthanide (4f) and actinide (5f) series

18. Nonmetals
Generally a gas or a brittle, dull solids
Poor conductors

19. Nonmetal Families Halogens= group17 REALLY REACTIVE
Noble Gases= group18
Unreactive/stable (all valence electrons are filled)

20. Metalloids Have characteristics of both metals and nonmetals
B, Si, Ge, As, Sb, Te, At
Separate metals on the left from nonmetals on the right

22. Homework
Worksheet

23. Classification of the Elements
Section 6.2
Classification of the Elements

24. Objectives
Explain why elements in the same group have similar properties
Identify the four blocks of the periodic table based on electron configuration

25. Valence Electrons
The properties of elements in each group are similar because they have same number of valence electrons

26. Valence Electrons and Period Number
Energy level of valence electrons = period on the table
Ex: Lithium: period 2, valence electron in 2nd energy level (1s22s1)

27. Valence Electrons and Group Number
Group number (1A-8A) = number of valence electrons

28. REVIEW 4 different energy sublevels s, p, d, and f S block= 1A and 2A
holds max of 2 electrons
P block= 3A through 8A
max holds 6 electrons
S block must fill before P block can fill
Noble gases are stable because of filled S and P blocks

29. REVIEW D block = transition metals F block= inner transition metals
max of 10 electrons
F block= inner transition metals
unpredictable manner of filling
max of 14 electrons

30. Reactivity Trends Increases down the table for the metals
Decreases down the table for the nonmetals
                                                                                                                                        

31. Homework
Worksheet