1. Assignments
I have found related jognog quizzes you can do for extra point’s pts. to replace the missing naming HW. There is also a balancing equations page to use as make up points on those assignments. Jognog Code JSX4R7F
(All scores have to be greater than 85% to earn credits.)
In addition I have assigned you three periodic table jognog quizzes to go along with the power point I have assigned you for the break. Please have these completed by the time we are back at school.

2. Introduction to the Periodic Table
Atomic Number ● Symbol ● Atomic Weight
Element ● Compound ● Mixture

3. Periodicity Objectives
Be able to:
Explain how the early versions of the periodic table was organized by the following people
Mendeleev
Mosley
State the periodic law
Define Periods and groups/families of the table
Identify the following groupings in the table and their tables
Metals, non-metals, metalloids,
Alkali metals, Alkali earth metals, transition metals, Halogens, noble gases, Rare earth elements(Lanthanide and actinide series)
Describe the following trends in the periodic table. (Trends through the period and the family.)
Atomic Radii
Density
Ionization energy
Electron affinity/ electronegativity
List or identify the properties of the metals and non-metals.

4. Homework
Take notes on the previously listed objectives. You can also color in a periodic table to identify the areas required. Use the periodic tables in your notes or download one and use your smart phones to label it. Be resourceful. Also, I have assigned you two jognog quizzes to complete. You will only receive credit if you earn 85% or above.
Jognog code JSX4R7F

5. I made the PERIODIC TABLE !
I am Dmitri Mendeleev!
I made the PERIODIC TABLE !

6. Mendeleev’s Periodic Table
“I began to look about and write down the elements with their atomic weights and typical properties, analogous elements and like atomic weights on separate cards, and this soon convinced me that the properties of elements are in periodic dependence upon their atomic weights.” --Mendeleev, Principles of Chemistry, 1905, Vol. II

7. What is the PERIODIC TABLE?
Shows all known elements in the universe.
Organizes the elements by chemical properties.

8. How do you read the PERIODIC TABLE?

9. What is the ATOMIC NUMBER?
The number of protons found in the nucleus of an atom Or
The number of electrons surrounding the nucleus of an atom.

10. What is the SYMBOL?
An abbreviation of the element name.

11. What is the ATOMIC WEIGHT?
The number of protons and neutrons in the nucleus of an atom.

12. How do I find the number of protons, electrons, and neutrons in an element using the periodic table?
# of PROTONS = ATOMIC NUMBER
# of ELECTRONS = ATOMIC NUMBER
# of NEUTRONS = ATOMIC _ ATOMIC
WEIGHT NUMBER

13. Now you are almost as smart as I am!
But not as handsome!
Man, I look GOOD!

14. What is an ELEMENT? A substance composed of a single kind of atom.
Cannot be broken down into another substance by chemical or physical means.

15. What is a COMPOUND?
A substance in which two or more different elements are CHEMICALLY bonded together.

16. What is a MIXTURE?
Two or more substances that are mixed together but are NOT chemically bonded.

17. You are still not as handsome as the great Mendeleev!
I am working this beard!
Man, I look GOOD!

18. Worked with Rutherford
Henry Moseley ( )
English chemist
Worked with Rutherford
Proved Mendeleev’s arrangement of the periodic table to be correct – only, the periodic table was arranged according to atomic number, not atomic mass

19. The Periodic Law
States that when elements are arranged in order of increasing atomic number, their physical and chemical properties show a periodic pattern

20. How do we read the table?
The modern periodic table has 118 squares, which represent a unique element. The distinctive shape of the periodic table comes in part from the periodic law. Elements in the same column have similar properties. These columns are referred to as groups or families of elements. The horizontal rows of the periodic table are called periods. The elements in the periodic table are also grouped as metals, nonmetals, and semimetals. Metals make up most of the periodic table and are located in the center and at the left of the table. With the exception of hydrogen, nonmetals are on the right side, and semimetals are located between the metals and nonmetals.

21. metals, nonmetals and metalloids.

22. Nonmetals
Nonmetals
Metalloids
Good conductors of heat and electricity
Malleable
Ductile
Luster
Typically solids at room temperature
Solids, liquids and gases at room temperature
Solids are brittle and dull
Poor conductors of heat and electricity
Have properties of both metals and nonmetals
Mostly brittle solids
Intermediate conductors of electricity- AKA semiconductors

23. ALKALI METALS Readily react with water and air Extremely reactive
Silvery in appearance
Soft enough to cut with a knife
Lower densities than other metals
Lower melting points than other metals

24. ALKALINE-EARTH METALS
Harder & stronger than alkali metals
Higher densities & melting points than alkali metals
Less reactive than alkali metals

25. HALOGENS Most reactive nonmetals
React readily with most metals to form salts
Most electronegative elements

26. NOBLE GASES
Least reactive elements because their highest occupied energy levels are completely filled with an octet of electrons (except He, which only requires 2 electrons to be filled).

27. TRANSITION METALS High densities High melting points
Good conductors of heat & electricity
High luster
Less reactive than alkali and alkaline-earth metals

28. INNER TRANSITION (Rare Earth) METALS

29. Similar reactivity to alkaline-earth metals
LANTHANIDES
Soft, silvery metals
Similar reactivity to alkaline-earth metals

30. The first 4 have been found naturally on Earth
ACTINIDES
All radioactive
The first 4 have been found naturally on Earth

31. PERIODS

32. GROUPS

33. Atomic radius - Decreases across a period
Atomic radius - Decreases across a period. Protons are added to the nucleus moving across a period from left to right. This increases the charge of the nucleus and electrons are pulled closer to the nucleus.

34. Atomic Radii

35. Variations in Ionization Energies
Energy vs Atomic Number
Ionization Energy - The energy required to take an electron and become ionized. Chemical activity and bonding depends on taking or sharing electrons Getting to big makes it harder to hold onto E-. Being smaller allows you to grab E- from other atoms.

36. Ionization Energy Trends
INCREASES

37. Electronegativity
A measure of the ability of an atom in a chemical compound to attract a bonding pair of electrons
NOTE *Electronegativity is a property of atoms in compounds and thus differs from ionization energy and electron affinity, which are properties of isolated atoms*

38. Trends Increase across a period Decrease down a group
Effective nuclear charge increases
Decrease down a group
Increase in atomic size and increase in electron shielding decreases the effective nuclear charge
Electronegativity depends upon:
The number of protons in the nucleus
The distance from the nucleus
Electron shielding

39. Electronegativity trends
INCREASES

40. Big Picture
Fluorine and Francium are the most reactive elements. How do you asses an atoms reactivity? Reactivity depends on # of Protons, The distance from the nucleus and Electron shielding
Moving towards Fluorine on the table, protons increase. This means greater attraction to e- and grabbing free or weakly held e-.
Moving towards Francium the E- shells increase. Full electron shells means greater electron repulsion and less attractive forces to e- in the outer shell.

41. Electronegativity Trends
INCREASES
INCREASES