1. 5.2 Electron Configuration & The Periodic Table
Chapter 5
The Periodic Law
5.2 Electron Configuration & The Periodic Table

2. In the modern periodic table, elements are arranged in order of increasing atomic number.

3. METALS METALLOIDS NONMETALS
In the periodic table below, indicate the location of the groups, periods, alkali metals, alkaline earth metals, halogens, noble gases, lanthanides, actinides, transition metals, inner transition metals, main group elements, metals, nonmetals and metalloids.
METALS
METALLOIDS
NONMETALS

4. 80% of elements are metals.
Most solids (Hg is liquid)
Luster – shiny.
Ductile – drawn into thin wires.
Malleable – hammered into sheets.
Conductors of heat and electricity.
Include transition metals – “bridge” between elements on left & right of table
80% of elements are metals.

5. Uses of Iron, Copper, and Aluminum
The metals iron, copper, and aluminum have many important uses. How each metal is used is determined by its properties.

6. Nonmetals Properties are generally opposite of metals
Poor conductors of heat
and electricity
Low boiling points
Most are gases at room temperature
Few are brittle solids (break easily), phosphorus and sulfur
One, bromine, is a dark red liquid
Chemical properties vary

7. Metalloids stair-step pattern 6 elements
Have properties similar to metals and non-metals
Ability to conduct heat and electricity varies with temp
Better than non-metals but not metals
*The behavior of a metalloid can be controlled by changing conditions.

8. Uses of Metalloids
If a small amount of boron is mixed with silicon, the mixture is a good conductor of electric current. Silicon can be cut into wafers, and used to make computer chips.

9. Let’s Compare! Metals 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

10. Sublevel Blocks on the Periodic Table1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
Sublevel Blocks on the Periodic Table

11. PERIODS

12. GROUPS

13. In the periodic table below, indicate the location of the groups, periods, alkali metals, alkaline earth metals, halogens, noble gases, lanthanides, actinides, transition metals, inner transition metals, main group elements, metals, nonmetals and metalloids.
MAIN GROUP ELEMENTS

14. s-Block Elements: Group 1
s1 - ALKALI METALS

15. 1s1 1s22s1 1s22s22p63s1 1s22s22p63s23p64s1 1s22s22p63s23p64s23d104p65s1 1s22s22p63s23p64s23d104p65s24d10 5p66s1 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s1 H 1 Li 3 Na 11 K 19 Rb 37 Cs 55 Fr 87
Do you notice any similarity in these configurations of the alkali metals?

16. s-Block Elements: Group 2 s2 - ALKALINE-EARTH METALS

17. d-Block Elements: Groups 3-18
TRANSITION METALS
(Level – 1)
d1 d2 d3 d4 d5 d6 d7 d8 d9 d10

18. p-Block Elements: Group 17
HALOGENS – p5

19. p-Block Elements: Group 18
NOBLE GASES – p6

20. 1s2 1s22s22p6 1s22s22p63s23p6 1s22s22p63s23p64s23d104p6 1s22s22p63s23p64s23d104p65s24d105p6 1s22s22p63s23p64s23d104p65s24d10 5p66s24f145d106p6 He
Do you notice any similarity in the configurations of the noble gases? 2 Ne 10 Ar 18 Kr 36 Xe 54 Rn 86

21. f-Block Elements: Lanthanides and Actinides
INNER TRANSITION (Rare Earth) METALS
f1 f2 f3 f4 f5 f6 f7 f8 f9 f10 f11 f12 f13 f14

22. f-Block Elements: Lanthanides and Actinides
4f1 - 4f14

23. f-Block Elements: Lanthanides and Actinides
5f1 - 5f14

24. Elements in the s - blocks
Alkali metals end in s1
Alkaline earth metals end in s2
should include He, but…
He has properties of noble gases
has a full outer level of e-’s
group 8A.

25. Transition Metals - d block
Note the change in configuration.
s1 d5
s1 d10 d1 d2 d3 d5 d6 d7 d8
d10

26. The P-block p1 p2 p3 p4 p6 p5

27. F - block f1 f5 f2 f3 f4 f6 f7 f8 f9 f10 f11 f12 f14 f13
Called “inner transition elements” f1 f5 f2 f3 f4 f6 f7 f8 f9
f10
f11
f12
f14
f13

28. Each period # = energy level for s & p orbitals.1 2 3 4 5 6 7
Period Number
Each period # = energy level for s & p orbitals.

29. 3d 4d 5d “d” orbitals fill up in levels 1 less than period #
first d is 3d found in period 4. 1 2 3 4 5 6 7 3d 4d 5d

30. f orbitals start filling at 4f….2 less than period #1 2 3 4 5 6 7 4f 5f
f orbitals start filling at 4f….2 less than period #

31. Electron Configurations in Groups
6.2
Electron Configurations in Groups
The Noble Gases
The noble gases are the elements in Group 8A of the periodic table. The electron configurations for the first four noble gases in Group 8A are listed below.

32. Electron Configurations in Groups
6.2
Electron Configurations in Groups
In atoms of the Group 1A elements below, there is only one electron in the highest occupied energy level.

33. Electron Configurations in Groups
6.2
Electron Configurations in Groups
In atoms of the Group 4A elements below, there are four electrons in the highest occupied energy level.

34. Transition Elements Blocks of Elements 6.2
This diagram classifies elements into blocks according to sublevels that are filled or filling with electrons. Interpreting Diagrams In the highest occupied energy level of a halogen atom, how many electrons are in the p sublevel?

35. Properties of Alkali Metals
Extremely reactive
Readily react with water and air
Silvery in appearance
Soft enough to cut with a knife
Lower densities than other metals
Lower melting points than other metals

36. Properties of Alkaline-Earth Metals
Harder & stronger than alkali metals
Higher densities & melting points than alkali metals
Less reactive than alkali metals

37. Properties of Halogens
Most reactive nonmetals
React readily with most metals to form salts
Most electronegative elements

38. Properties of Noble Gases
Least reactive elements
highest occupied energy levels completely filled with octet of electrons (except He, which only requires 2 electrons to be filled).

39. Properties of Transition Metals
High densities
High melting points
Good conductors of heat & electricity
High luster
Less reactive than alkali and alkaline-earth metals

40. Properties of p Block Metals
Harder and more dense than the s block metals
Softer and less dense than the d block metals.

41. Properties of Lanthanides
Soft, silvery metals
Similar reactivity to alkaline-earth metals

42. Properties of Actinides
All radioactive
The first 4 have been found naturally on Earth

43. The Properties of Group 1: the Alkali Metals
Easily lose 1 valence electron
(Reducing agents)
React violently with water
React with halogens to form salts

44. The Properties of Group 1: the Alkali Earth Metals
Easily loses 2 valence electron
(Reducing agents)
Harder, denser, stronger than Group 1 metals
Higher melting points
Less reactive than Group 1, but too reactive to be found free in nature