1. 5.2 Electron Configuration & The Periodic Table
Chapter 5
The Periodic Law
5.2 Electron Configuration & The Periodic Table
In the modern periodic table, elements are arranged in order of increasing atomic number.

2. 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

3. 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.

4. 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

5. Metalloids stair-step pattern 7 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.

6. 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.

7. 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

8. PERIODS

9. GROUPS
(families)

10. MAIN GROUP ELEMENTS s-block and p-block
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
s-block and p-block

11. 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

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

13. Electron Configurations in Groups
In atoms of the Group 14 elements below, there are four electrons in the highest occupied energy level.

14. 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.

15. Ch 5 Notes s-block: Groups 1-2 1. Group 1 – alkali metals -
2. Group 2 – alkaline-earth metals
* H and He do not fit in chemically

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

17. 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?

18. s-Block Elements: Group 1 = Alkali Metals
lithium
- silvery, soft, low melting point
most reactive metals (not free)
react strongly with water (produce H2 and alkalis)
react with halogens to form salts
easily lose 1 valence e-
reactivity increases
sodium
potassium

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

20. Group 2 = Alkaline-earth Metals
s-Block Elements:
Group 2 = Alkaline-earth Metals
harder, denser, stronger than alkali metals
higher melting points
less reactive than alkali, too reactive to be found free
easily lose 2 valence e-

21. Alkaline Earth Metals Beryllium
- used in metal alloys adding strength, durability and temperature stability
Magnesium
- often mixed with aluminum and zinc to manufacture airplane parts.
- photosynthesis (chlorophyll)
Calcium
- bones & teeth
- Chalk, limestone, pearls, plaster
Strontium
- produces brilliant red color when burned, mixed with fireworks and flares
Barium
- barium sulfate used a lubricating mud in drilling and taken to silence stomach aches

22. Ch 5 Notes
C. d-block: Groups D. p-block: Groups 1. nonmetals - 2. metalloids - 3. metals - 4. Group Group 18 - E. f-block: Inner-transition elements (rare-earth) 1. 4f f -

23. d-Block Elements: Groups 3-18
TRANSITION METALS
d1 d2 d3 d4 d5 d6 d7 d8 d9 d10

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

25. d-Block Elements: Groups 3-12
- transition metals
good conductors of electricity
high luster (shiny)
malleable and ductile
some are free in nature
Note: Fe, Co, and Ni produce magnetic field

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

27. p-block elements

28. Ch 5 Notes
C. d-block: Groups D. p-block: Groups 1. nonmetals – 2. metalloids – 3. metals - 4. Group Group 18 - E. f-block: Inner-transition elements (rare-earth) 1. Lanthanides - 4f - 2. Actinides - 5f -
13-18
upper right-hand corner
6 along zig-zag line (semiconductors)
8 metals left of zig-zag line (post-transition metals)

29. Label the Boron Family on your PT

30. Boron Family -3 valence e- Boron Hard/brittle
never found pure in nature
in borax...used to make detergents & cosmetics

31. Boron Family Aluminum most abundant metal in earth’s crust
13 Al Aluminum 26.98
Aluminum
most abundant metal in earth’s crust
important metal for industry
light, strong, slow to corrode

32. Label the Carbon Family on your PT

33. Carbon Family - 4 valence e- Can gain 4 e-, lose 4 e-, or share e-
Most compounds in body contain C
Si is 2nd most abundant element in Earth’s crust
Si used to tip saw blades

34. Label the Nitrogen Family on your PT

35. Nitrogen Family - 5 valence e- Tend to gain 3 e-
N and P used in fertilizers
P on tips of matches

36. Label the Oxygen Family on your PT

37. Oxygen Family - 6 valence e- Tend to gain 2 e- O very abundant element
S used in fertilizers
O needed for digestion

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

39. Group 17 = Halogens (“salt-former”)
- 7 valence e-
- most reactive nonmetals
- react with most metals to form salts
- never found pure in nature

40. F compounds in toothpaste Cl kills bacteria
Halogens Uses
F compounds in toothpaste
Cl kills bacteria
I keeps thyroid gland working properly

41. Halogen Uses in Everyday Life
Fluorine: Refrigerator Fluids
Tooth Paste (Most well known use)  
    > Helps make your teeth whiter and not decay
Chlorine: Swimming Pools
Water Purification (Helped stop Cholera)
Plastics, such as PVC
Bleach
Making Paper (Makes the paper white) 
Bromine: Pesticides 
Flame Resistant Plastics 
Photography
Medicine
Water Purification 
   > Disinfects fresh water
Iodine: 
Eye Health
Astatine: No real uses 

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

43. 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).

44. The Noble Gases (Inert Gases)
- non-reactive
outermost e- shell is full (8 valence e-)
In “neon” lights
- in earth’s atmosphere (less than 1%)

45. 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.

46. 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

47. Ch 5 Notes
C. d-block: Groups D. p-block: Groups 1. nonmetals - 2. metalloids - 3. metals - 4. Group Group 18 - E. f-block: Inner-transition elements (rare-earth) 1. Lanthanides - 4f - 2. Actinides - 5f -

48. f-Block Elements: Lanthanides and Actinides
INNER TRANSITION (Rare Earth) METALS
f1 f f f4 f f6 f7 f8 f9 f10 f f12 f13 f d1

49. The Lanthanides
Early 1900's the elements from cerium (#58) to lutetium (#71) are separated and identified. Also known as the rare earth elements, less than 0.01% naturally occurring.
The Actinides
Discovery (or synthesis) of thorium, # 90 to lawrencium #103
Both groups pulled out of the table for space reasons.

50. 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

51. Rare Earth Elements Lanthanide series (period 6)
Actinide Series (period 7)
Some radioactive
Separated from table to make easy to read/print
silver, silvery-white, or gray metals.
Conduct electricity

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

53. Properties of Lanthanides
Soft, silvery metals
Similar reactivity to alkaline-earth metals
strong magnets
laser lights
flint in lighters

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

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

56. Blocks of Elements
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?

57. 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.

58. 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

59. 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 #

60. End of Section 5.2
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