Periodic Block Presentation

periodic block notes

2. Periodic Blocks
Chapter 6

3. Quick review (Stuff u should know
already!!!!)
What is a valence electron?
–Electrons in the highest principle energy level
–What’s the principle energy level?
1, 2, 3, 4, 5…. (n)
Remember Aufbau diagram…

5. Sublevels
How many electrons in s?
–2
How many electrons in p?
–6
How many electrons in d?
–10
How many electrons in f?
–14

6. Observations???

7. Observations
What was the connection between period
number and the elements that you were
assigned?
–Valence electrons?
–Principle quantum number?
–Sublevel?
–Orbital?
–Partially filled or completely filled?

8. Period # & Valence electrons
The energy level of the valence electrons of
an element tell you the period that it will be in
(the row!!!)
Remember, energy level is your principle
quantum number (n)

9. S-Block
Groups 1a and 2a
Valence electrons occupy only s-orbitals
Group 1a partially filled s
Group 2a completely filled s
How many max electrons can an s-orbital
hold?
Soooo how many groups are going to
makeup the s-block?
–2

10. So what sublevel do we go to after we
fill an s-sublevel?
P-sublevel….

11. P-block
How many orbitals does the p sublevel have?
–3…remember, three lines _ _ _
Do you think we will have more or less electrons here than
the s-block?
–MORE!!!
Groups 3a thru 8a
Why is there no p-block elements in period 1?
–Because at energy level (principal quantum #) 1, we do
not have any p sublevels
How many max electrons can a p-sublevel hold?
SO how many groups is the p-block going to have?
–6

12. Noble gases in P-block
What do we notice about their s and p
orbital???
–They are completely full
–So they are stable…no chemical reaction
–Important later when we talk about ions….

13. Welcome to the D-Block!
Contains transition metals
How many elements are going to reside on the D-block?
–Lots!
There are many exceptions but….
–Filled outermost s-orbital of energy level n
–Filled or partially filled d-orbitals of energy level n-1
What happens to the d orbitals as we move across a period?
How many groups do you think are going to make up the d-
block?
–Hint: How many electrons can a d-sublevel hold?
–10!!!!

14. F-Block elements…uh-oh….
What do we have left on the periodic table?
–Lanthanide and actinide series (inner transition metals)
–They fall into periods 6 and 7
Characterized by:
–Filled or partially filled outer most s-orbital
–Filled or partially filled 4f and 5f orbitals
Sorry guys…these electrons in the f-block do not fill in
a predictable manner
How many columns are going to make up the f-block?
–Hint: How many electrons can an f-sublevel hold?
–14!!!!

15. So….
Now we see why the periodic table has that
funny shape!
We can now also do electron notations in
less tedious manner!

18. Tell me what happens….
To the principle energy levels as we move
down a period?
–Princ. E level increases
To the number of sublevels containing
electrons as we move down a period?
–Increases too!!!

22. Practice problems!!!
Periodic tables away!!!
Tell me the group, period, and block of an
atom with the following electron
configurations:
–[Ne]3s
2
–[He]2s
2
–[Kr]5s
2
4d
10
5p
5

23. Answers
–[Ne]3s
2
Group 2a
Period 3
S-block
–[He]2s
2
Group 2a
Period 2
S-block
–[Kr]5s
2
4d
10
5p
5
Group 7a
Period 5
p-block

24. More problems…
Write the electron configuration for the
following elements:
–The group 4b element in the fifth period?
–The group 1a element in the seventh period?

25. Answers
–The group 4b element in the fifth period?
Zirconium
[Kr]5s
2
4d
2
–The group 1a element in the seventh period?
Francium
[Rn]7s
1

26. REPRESENTATIVE BLOCK PARTY!!!
Make cube…how many sides is this?
–6
Side 1…Artistically symbol of element with vitals
Side 2…Label the elements group
Side 3…Write the element’s electron configuration
Side 4…Illustrate/describe Properties of the element
Side 5…Illustrate/describe Uses of element
Side 6…Important compounds this element is found
in

28. Periodic Trends
What’s a trend