science

1. Welcome to Science Class!

2. !
Opening Prayer
Our Lord God in heaven. Thank you for the new day you've bestowed
upon us. Until this moment, we still have our borrowed life and strength
from you. We worship and praise Your Holy Name.
This moment, we will continue to study and acquire new knowledge.
May you bless your students with witty brain to think fast and an
inquiring mind to be curious on whatever knowledge they will learn
today. Most importantly bless them with Your wisdom and a heart that
will follow your commandments in order for them to become worthy in
their studies.
We hope that you heard our prayer.
We ask all of these. In the name of Jesus Christ, our Saviour.
Amen.

3. Good Morning
Grade 8

4. Objective for the Week
•Determine the number of protons,
neutrons, and electrons in a particular
atom.
•Use the periodic table to predict the
chemical behavior of an element.

5. Review

8. Integers 1,2 and 3.. Used to indicate
principal quantum numbers
Symbols s, p, d and f indicate
sublevels.
The number of superscript indicates
the number of electrons occupying
sublevels
s2
p 6
d10
f14

9. s: Sharp
p: Principal
d: Diffuse
f: Fundamental
•These refer to the sublevels within the principal
quantum level (n).
•So, for
•n = 1, there is only one sublevel, s.
•n = 2, there are 2 sublevels: s & p
•n = 3, there are 3 sublevels: s, p, & d
•n = 4, there are 3 sublevels: s, p, d & f
s2 = 2 e
s2p6 = 8 e
s2p6d10 = 18 e
s2p6d10 f14 = 32 e

10. Orbital Diagrams

11. Orbitals
•Each sublevel (s, p, d, f) contains orbitals.
•Remember, orbitals are electron-clouds that
hold the electrons 90% of the time.
•Each orbital can hold TWO electrons, so
• s - 2 electrons, 1 orbital
• p – 6 electrons, 3 orbitals
• d – 10 electrons, 5 orbitals
• f – 14 electrons, 7 orbitals

12. Energy Levels, Sublevels, and Orbitals
1. Principal energy levels – n, assigned values 1-7
(Like floors in a hotel)
2. Energy sublevels- s, p, d, f (Type of suite in a
hotel)
 s sublevel – 1 orbital
 p sublevel – 3 orbitals
 d sublevel – 5 orbitals
 f sublevel – 7 orbitals
3. Orbitals – Two electrons per orbital (Two people
per room)

13. Three Rules in Writing the
Electronic Configuration

14. The Aufbau Principle
•Each electron
occupies the
lowest energy
orbital available
Filling Diagram
for Sublevels

15. Example Nitrogen
number of electrons
= 7
principal quantum
number
= 2
ℓ= s and p

16. Example Nitrogen
number of electrons
= 7
principal quantum number
= 2 s and p
Filling Diagram
for Sublevels
Maximum number of
electrons
s=2
p=6
d=10
f=14
1s2 2s2

17. Example Nitrogen
number of electrons
= 7
principal quantum number
= 2 s and p
Filling Diagram
for Sublevels
Maximum number of
electrons
s=2
p=6
d=10
f=14
1s2 2s2
2p?
1s2 2s2
2p3
= 7

18. Example Na (Sodium)
number of electrons
= 11
principal quantum
number
= 3
ℓ= s and p

19. Example Sodium
number of electrons
= 11
principal quantum number
= 3 s and p
Filling Diagram
for Sublevels
Maximum number of
electrons
s=2
p=6
d=10
f=14
1s2 2s2 2p6

20. Example Sodium
number of electrons
= 11
principal quantum number
= 3 s and p
Filling Diagram
for Sublevels
Maximum number of
electrons
s=2
p=6
d=10
f=14
1s2 2s2 2p6
3s?
1s2 2s2 2p6
3s1
= 11

21. s
p
d
f

22. 1
2
3
4
5
6
7

25. 1s2 2s2 2p6 3s2 3p3

26. 1s2 2s2 2p6 3s2

27. 1s2 2s2 2p6

28. 1s2 2s2 2p6 3s2 3p1

29. 1s2 2s2 2p6 3s2 3p5

30. Pauli Exclusion Principle
•A maximum of two electrons
may occupy a single orbital, but
only if the electrons have
opposite spins.
•Spin -- Electrons has an
associated “spin,” either one
way or the other, like a top.
•These spins are called “spin
up” (+) and “spin down.” (-)
Box = orbital
Arrow = electron

31. Hund’s Rule
•Single electrons with the
same spin must occupy
each equal-energy orbital
before additional
electrons with opposite
spins can occupy the
same orbitals.
1s2 2s2 2p4
1s2 2s2 2p4
NOT
Ex. Oxygen:
•1s2 2s2 2p4

32. Three rules:
•electrons fill orbitals starting with lowest n and
moving upwards;
•no two electrons can fill one orbital with the
same spin (Pauli);
•for degenerate orbitals, electrons fill each orbital
singly before any orbital gets a second electron
(Hund’s rule).
Electron Configurations

33. Let us Apply !

34. Example Nitrogen
number of electrons = 7
principal quantum number
= 2 s and p
Filling Diagram
for Sublevels
Maximum number of
electrons
s=2
p=6
d=10
f=14
1s2 2s2 2p3
( Aufbau principle)
ELECTRON CONFIGURATION
No.of orbitals
(ORBITAL DIAGRAM)
 s sublevel – 1 orbital
 p sublevel – 3 orbitals
 d sublevel – 5 orbitals
 f sublevel – 7 orbitals
Hund’s Rule and Pauli Exclusion Principle

35. Example Sodium
number of electrons = 11
principal quantum number= 3 s and p
Filling Diagram
for Sublevels
Maximum number of
electrons
s=2
p=6
d=10
f=14
1s2 2s2 2p6
 s sublevel – 1 orbital
 p sublevel – 3 orbitals
 d sublevel – 5 orbitals
 f sublevel – 7 orbitals
Hund’s Rule and Pauli Exclusion Principle
3s1
( Aufbau principle)
ELECTRON CONFIGURATION
No.of orbitals
(ORBITAL DIAGRAM)

36. Example Oxygen
number of electrons = 8
principal quantum number= 2 s and p
Filling Diagram
for Sublevels
Maximum number of
electrons
s=2
p=6
d=10
f=14
1s2 2s2 2p4
 s sublevel – 1 orbital
 p sublevel – 3 orbitals
 d sublevel – 5 orbitals
 f sublevel – 7 orbitals
Hund’s Rule and Pauli Exclusion Principle
( Aufbau principle)
ELECTRON CONFIGURATION
No.of orbitals
(ORBITAL DIAGRAM)

37. Application

38. Assign quantum numbers to
the valence electrons of a
lithium atom
See your periodic table
1s22s1
Number of electrons= 3

39. 1st: Principal Quantum Number (n)
1s22s1
Answer: n= 2

40. 2nd: The angular momentum quantum
Number (ℓ) or subshell
Answer: ℓ= 0
1s22s1
s= 0
P = 1
d =2
f= 3

41. 3rd: Magnetic Quantum
Number (ml)
-l to +l
ml = 0 ,
because the value of l is 0
1s22s1
Sublevel ℓ mℓ
s 0 0
p 1 -1, 0, +1
d 2 -2, -1, 0, +1, +2
f 3 -3, -2, -1, 0, +1, +2,
+3

42. 4th: Spin Quantum Number (ms )
Answer: 1
2
1s22s1 1
2
+
+
1
2
+
1
2
-

43. The quantum
numbers are:
Principal=2
Azimuthal=0
Magnetic= 0
Spin= + 1/2
Lithium
1s22s1
Sublevel ℓ mℓ
s 0 0
p 1 -1, 0, +1
d 2 -2, -1, 0, +1, +2
f 3 -3, -2, -1, 0, +1, +2, +3

44. Assign quantum numbers to
the valence electrons of a
Bromine atom
See your periodic table
1s2 2s2 2p6 3s2 3p6
4s2 3d10 4p5
Number of electrons= 35

45. 1st: Principal Quantum Number (n)
Answer: n= 4
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

46. 2nd: The angular momentum quantum Number
(ℓ) or subshell
Answer: ℓ= 1
s= 0
P = 1
d =2
f= 3
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

47. 3rd: Magnetic Quantum Number
(ml) -l to +l
ml = -1, 0, +1
because the value of l is 1
Sublevel ℓ mℓ
s 0 0
p 1 -1, 0, +1
d 2 -2, -1, 0, +1, +2
f 3 -3, -2, -1, 0, +1,
+2, +3
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

48. 4th: Spin Quantum Number (ms )
Answer: 1
2
1s2 2s2 2p6 3s2 3p6
4s2 3d10 4p5

49. The quantum numbers
are:
Principal=4
Azimuthal=1
•Magnetic= -1, 0, +1
Spin= + 1/2
Bromine
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5
Sublevel ℓ mℓ
s 0 0
p 1 -1, 0, +1
d 2 -2, -1, 0, +1, +2
f 3 -3, -2, -1, 0, +1, +2, +3

50. Let Us Test Your Understanding
s sublevel – 1 orbital
p sublevel – 3 orbitals
d sublevel – 5 orbitals
 f sublevel – 7 orbitals

51. 1s2 2s2 2p6
3s2
3p3

52. 1s2
2s2 2p6
3s2

53. 1s2
2s2 2p6

54. 1s2
2s2
2p6 3s2
3p1

55. 1s2 2s2
2p6
3s2 3p5

56. Assignment: Write the orbital diagram of the
following elements.
1. Boron
2. Chlorine
3. Silicon
4. Krypton
5. Argon

57. !
Closing Prayer
We thank you Lord, for allowing us to end this class successfully.
We may not be together physically but through your blessing, we were able to
learn and advance our knowledge and skills.
Grant that we continue to pursue our education despite the problems that come our
way.
May you allow us to gain more information that we could use to serve other
people.
May you send the Holy Spirit to guide us in sharing this information to the world.
We pray for the safety of the teachers, students, families, and all people in the
world.
We ask all these, in your powerful name.
Amen

58. Thank You!