1. Chapter 4 Notes: The Periodic Table
Mostly memorization no math involve

2. How would you organize the following items?
1) Organize, closet, computer and grocery store. If you are working at a hardware store (ACE, do it center, Lowes, Home depot) figure this task out (dairy, meat, cans etc..)
Work with your table partner and ready to present to the class
2) How is the periodic table arranged? (students go to the board and write their lay out)

3. Chp 4-1 Periodic Law
Periodic law - periodic table is organized based on the atomic #, chemical & physical properties of the elements
Mendeleev is the creator of the periodic table used atomic mass
1st periodic table in 1869 arranged by mass

4. The Periodic Table Group Period A vertical columns
Elements in a group share the same chemical properties
Period
A horizontal rows
Elements in the same period have the same number of energy levels

5. The Periodic Table
Elements’ chemical properties are determined by the number of valence electrons
Valence electrons are electrons that are in the outermost energy level of an atom (in the S and P orbital)

6. Main Group Elements
Transition Elements
Inner Transition
Elements

7. Main Group

8. Metals Properties

9. Metals Properties Most elements are metals
They are good conductors of electricity
Most are ductile (can be rolled into wire) and malleable (can be hammered or rolled into sheets)
Can form alloys - solid or liquid mixtures of metals
Talk about wires (landline, and internet) that are used as conductor – Expensive speakers with gold coating for better sounds (Beats by Dre headphones)

10. Check-In
A = metals B = non metals C = metalloids Classify the following elements: 1.Na 2.H 3.C 4.Ca 5.Si 6.W

11. Alkali Metals
Group 1
Highly reactive (easily combine with other elements)
React with water to make alkaline (basic) solutions
Will give away 1 valence electron
Found in nature as compounds
Electrolytes Lithium burns red and use in battery (lithium-ion) Potassium helps muscles contract

12. Alkaline Earth Metals Group 2 2nd most reactive group
Found in nature in compounds
Give away 2 v.e.
Calcium build bones
Magnesium deficient can lead to depression. Cerebral spinal fluid (CSF) magnesium has been found low in treatment-resistant suicidal depression patients

13. Transition Metals d and f blocks
Most lanthanides and actinides (f-block) are radioactive.
Generally less reactive than alkali and alkaline earth metals
Do not have identical outer electron configurations Common metals that a person will think of (copper, iron, gold, silver, zinc)

14. Halogens Group 17 Gain 1 electron in reactions
React with metals to form salts
Halogens are non-metals
Seven valence electrons making them highly reactive
Halogens are oxidants (elements that grab electrons and mess up the cells in your body)

15. Noble Gases Group 18 Not reactive at all
Eight valence electrons makes them very stable (outermost energy level is full)
Also called inert gases because of their low reactivity

16. Hydrogen Most common element in the universe
Found in many organic compounds
Fuel source for the sun (nuclear fusion) Unlike all other elements
Highly reactive

17. Chp 4-3 Periodic Trends Atomic radius Ionization energy
Electronegativity
Electron affinity

18. Periodic Trends
Atomic Radius: The estimated distance from the nucleus to the outer most electrons
Increases down a group
As electrons energy levels are added, the nucleus becomes larger
Decreases across a period
# protons increases which pulled the v.e. closer to the nucleus

19. Atomic Radius Trend Radius decreases Radius Increases Radius decreases
Based on the picture what trend do you see? In term of atomic size
Radius decreases

20. Periodic Trends
Ionization Energy - The energy required to remove one electron from an atom or ion
Decreases down a group
Electrons are farther from the nucleus and easier to remove
Increases across a period
Electrons are closer to the nucleus

21. Periodic Trends
Electronegativity - the ability of an atom to attract electrons to itself
Decreases down a group
Increases across a period
How many like to have a car or an A in chemistry?
Decreases down a group because the radius is too big, harder to attract electrons

22. Periodic Trends
Electron Affinity - the energy change that occurs when an electron is added to a neutral atom
Decreases down a group
Increases across a period

23. Example Consider the following elements: Na, Al, P, Cl
Largest and smallest radius?
Highest electronegavity?
Largest radius = Na smallest = Cl
Highest electronegavity = Cl

24. Fill in your periodic table
Color and label each of these:
Main-group metals
Transition metals
Lanthanides and Actinides
Nonmetals
Noble Gases
Metalloids
Label with arrows each of these trends:
Atomic Radius
Ionization energy
Electronegativity
Electron affinity
Reactivity (this is different on each side of the PT)