1. The Periodic Table
J. McLeod
H. Chemistry

3. Essential Question
How is the periodic table arranged?

4. A little history… Dmitri Mendeleev: 1st Periodic Table
organized the periodic table by increasing atomic mass
Left empty spaces
Predicted properties of unknown elements

5. Mendeleev’s Table

6. A little more history...
Henry Moseley: Modern Periodic Table ( )
There were small problems with Mendeleev’s table.
Used information he found about isotopes to modify Mendeleev’s table
Determined that elements are put in order by their atomic number

7. Elements are arranged:
Vertically into Groups/Families
Horizontally Into Periods

8. Why?

9. If you looked at one atom of every element in a group you would see…
Each atom has the same number of valence electrons Electrons in the outermost energy level (shell)

10. The group 2 atoms all have 2 electrons in their outer shells
Be (Beryllium)
Atom
Mg (Magnesium) Atom

11. The number of outer or valence electrons in an atom effects the way an atom bonds.
The way an atom bonds determines many properties of the element.
This is why elements within a group usually have similar properties.

12. If you looked at an atom from each element in a period you would see…
Each atom has the same number of energy levels.

13. The period 4 atoms each have 4 energy levels
4th Shell
Kr (Krypton)
Atom
Fe (Iron) Atom
K (Potassium) Atom

14. Divisions of the Table
The Periodic Table is divided into regions based on general properties
Include:
Metals
Non-metals
Metalloids

16. Metals Left side of the stairs Forms cations by losing electrons
High Melting Points
Solids at room temperature (except Hg)
Metallic luster
Malleable and ductile
Good conductors of heat and electricity

17. Non-metals Right side of the stairs Forms anions by gaining electrons
Low Melting Points
Gases or solids at room temperature (except Br2)
Brittle solids (Which means what?)
Insulators (poor conductors or heat & electricity)

18. Metalloids Have properties of both metals and non-metals
Semi-conductors
Solids

19. Ticket Out The Door:
State whether the following are metals, nonmetals, or metalloids and then predict a property that they may have:
Potassium
Iodine
Antimony

21. Bellwork
What are the vertical columns of the PT called? What do they have in common?
What are the horizontal rows called? What do they have in common?

22. Groups

23. Hydrogen Belongs to a family of its own. Is a diatomic, reactive gas.
Was involved in the explosion of the Hindenberg.
Is promising as an alternative fuel source for automobiles

24. Alkali Metals Group 1 Soft, silvery colored metals 1 valence e-
Very reactive!!!

25. Alkali Metal Video
What trend in reactivity is seen amongst the alkali metals?
What would you expect from Francium?!?!

26. Alkaline Earth Metals Group 2 Silvery-white metals 2 valence e-
Fairly reactive
Many are found in rocks in the earth’s crust

27. Transition Metals Most are good conductors heat & electricity
Malleable (easily bent or hammered into wires or sheets)

28. How many things can you think of that have Transition Metals in them?
Write as many down as you can in 1 minute.

30. Halogens Group 17 Have 7 Valence electrons Most are poisonous
Cl2 was used as a chemical weapon during WWI and WWII

31. Halogens
What trend in reactivity is seen amongst the Halogens?

32. Noble Gases Group 18 8 Valence Electrons Very unreactive
Gases at room temperature

33. Jellyfish lamps made with noble gases artist- Eric Ehlenberger

34. Lanthanides & Actinides
Located at the bottom of the Periodic Table
Rare Earth Metals
Lanthanide Series
Actinide Series

35. Summing it up: Ticket out the Door
State which group each of the following elements belongs to and give a property of the element.
Lithium
Chlorine
Uranium
Krypton
Strontium
Chromium

36. Bellwork What is the most reactive metal?
What is the most reactive nonmetal?
How many energy levels does Strontium have?
How many valence electrons does Aluminum have?

37. Blank Periodic Table
Write the names of the families in their respective columns
Alkali Metals, Alkaline Earth Metals, Halogens, & Noble Gases
Label the two rows with their respective names
Lanthanides & Actinides
Outline the metals in RED
Outline the metalloids in GREEN
Outline the non-metals in BLUE
Draw an arrow showing reactivity of METALS
Draw an arrow showing reactivity of NONMETALS

38. Periodicity
The properties of the elements on the periodic table create trends as you move around.
Trends move left-right & up-down

39. Reactivity of Metals Towards Francium Inc. down a column
Inc. right to left across a period
Why?
Increase in Size (value of n)
Larger in size
Increase Shielding effect
Weaker nuclear charge
Decrease ionization energy
Towards Francium Fr

40. Reactivity of Nonmetals
Inc. up a column
Inc. left to right across a period
Why?
Decrease in size (value of n)
Smaller in size
Decrease Shielding effect
Stronger nuclear charge
Increase ionization energy F
Towards Fluorine

41. Atomic Radius ½ the distance between two adjacent nuclei
…increases as we go down a column
WHY?
add a new energy level each time
…increases as we go right to left across a period
Decrease in nuclear charge

42. Atomic Radii = 1 Angstrom IA IIA IIIA IVA VA VIA VIIA Li Na K Rb Cs ClP Si Al Br Se As Ge Ga I Te Sb Sn In Tl Pb Bi Mg Ca Sr Ba Be F O N C B
IA IIA IIIA IVA VA VIA VIIA
= 1 Angstrom

43. Ionic Radius the size of an ion cations anions Ca atom Ca+2 ion
Cl atom
Cl-1 ion
20 p+
20 p+
17 p+
17 p+
20 e–
18 e–
17 e–
18 e–
Cl1– Ca Cl
Ca2+
cations lose electrons-
smaller
Anions gain electrons
larger

44. Atomic Radii Ionic Radii
IA IIA IIIA IVA VA VIA VIIA Li Na K Rb Cs Cl S P Si Al Br Se As Ge Ga I Te Sb Sn In Tl Pb Bi Mg Ca Sr Ba Be B C N O F
Atomic
Radii
0.95
Li1+
Be2+
Na1+
Mg2+
Cl1-
N3-
O2-
F1-
S2-
Se2-
Br1-
Te2-
I1-
Al3+
Ga3+
In3+
Tl3+
Ca2+
K1+
Sr2+
Rb1+
Cs1+
Ba2+
Ionic
Radii
Cations: smaller
than parent atoms
Anions: LARGER
than parent atoms
= 1 Angstrom

45. Ionization Energy Ionization Energy increases
the energy required to remove an e– from an atom
…increases as we go up a column
WHY?
shielding effect - increase in the number of energy levels
…increases as we go from left to right across a period
Nonmetals tend to gain electrons… high 1st ionization energy.
Metals tend to lose electrons… low first ionization energy He
Ionization Energy increases

46. Electronegativity electronegativity increases
the tendency for a bonded atom to attract electrons to itself
…increases as we go up a column
…increases as we go left to right across a period
WHY?
Nonmetals tend to gain electrons… high electronegativity
Metals tend to lose electrons… low electronegativity F
electronegativity increases

47. Periodic Table
On the periodic table on the next page of your notes… draw out all of the trends if you have not done so already.