The document discusses the periodic table and electron configuration. It explains that the periodic table is divided into s, p, d and f blocks based on which atomic orbitals are being filled. It describes the patterns of electron filling according to the Aufbau principle, Hund's rule and Pauli exclusion principle. Examples of electron configurations are provided for elements in the s, p, d and f blocks to illustrate partial filling of the respective orbitals.
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Periodic Table Elements - s, p, d, f Blocks
1. Periodic Table of elements – divided into s, p, d, f blocks
s block
• s orbitals partially fill
d block
• d orbitals partially filled
• transition elements
f block
• f orbital partially fill
p block
• p orbital partially fill
2. Electron filled according to 3 Principles
1
Aufbau Principle
• electron occupy orbitals of lower energy first
• building up, construction from bottom up
4Be
High energy
- 1s2 2s2
5B
- 1s2 2s2 2p1
2p
2p
2s
2s
Click here to view simulation
1s
1s
lower energy
2
Hund’s Principle
• electron occupy orbitals singly first before pairing up
7N
High energy
- 1s2 2s2 2p3
8O
- 1s2 2s2 2p4
2p
2s
Click here to view simulation
1s
3
lower energy
Pauli Exclusion Principle
• each orbital occupy by 2 electron opposite spin
4Be
- 1s2 2s2
High energy
10Ne
- 1s2 2s2 2p6
Click here to view simulation
lower energy
3. Electron configuration
5
B
1s2 2s2 2p1
6
C
1s2 2s2 2p2
7
N
1s2 2s2 2p3
8
O
1s2 2s2 2p4
9
F
1s2 2s2 2p5
10
Ne
1s2 2s2 2p6
11
Na
1s2 2s2 2p6 3s1
12
Mg
1s2 2s2 2p6 3s2
13
Al
1s2 2s2 2p6 3s2 3p1
14
Si
1s2
15
P
1s2 2s2 2p6 3s2 3p3
16
S
1s2 2s2 2p6 3s2 3p4
17
CI
1s2
18
Ar
1s2 2s2 2p6 3s2 3p6
19
K
1s2
20
Ca
1s2 2s2 2p6 3s2 3p6 4s2
21
Sc
1s2 2s2 2p6 3s2 3p6 4s2 3d1
22
Ti
1s2 2s2 2p6 3s2 3p6 4s2 3d2
23
V
1s2 2s2 2p6 3s2 3p6 4s2 3d3
24
Cr
1s2 2s2 2p6 3s2 3p6 4s1 3d5
25
Mn
1s2 2s2 2p6 3s2 3p6 4s2 3d5
26
Fe
1s2 2s2 2p6 3s2 3p6 4s2 3d6
27
Co
1s2 2s2 2p6 3s2 3p6 4s2 3d7
28
Ni
1s2 2s2 2p6 3s2 3p6 4s2 3d8
29
Cu
1s2 2s2 2p6 3s2 3p6 4s1 3d10
30
Zn
Electron occupy 4s first then 3d
Energy level and sublevels
1s2 2s2 2p6 3s2 3p6 4s2 3d10
2s2
2s2
2s2
2p6
2p6
2p6
4s energy level lower than 3d
3s2
3s2
3s2
4s
3d
3p
3p2
3s
18Ar
– 1s2 2s2 2p6 3s2 3p6
2p
2s
3p5
3p6 4s1
Electrons fill 4s first
3d
4s
1s
3p
19K
– 1s2 2s2 2p6 3s2 3p6 4s1
3s
4s then 3d is fill
2p
3d
2s
4s
1s
21Sc
3p
3s
– 1s2 2s2 2p6 3s2 3p6 4s2 3d1
2p
2s
1s
4. Electron Notation
Atom
Positive/Negative Ion
s, p, d, f notation
Complete configuration
Noble gas notation
Condensed configuration
Noble gas notation
Complete configuration
10
Ne
1s2 2s2 2p6
10
Ne
[Ne]
10
Ne
1s2 2s2 2p6 /[Ne]
11
Na
1s2 2s2 2p6 3s1
11
Na
[Ne] 3s1
11
Na+
1s2 2s2 2p6 / [Ne]
12
Mg
1s2 2s2 2p6 3s2
12
Mg
[Ne] 3s2
12
Mg2+
1s2 2s2 2p6 / [Ne]
13
Al
1s2 2s2 2p6 3s2 3p1
13
Al
[Ne] 3s2 3p1
13
Al3+
1s2 2s2 2p6 / [Ne]
14
Si
1s2 2s2 2p6 3s2 3p2
14
Si
[Ne] 3s2 3p2
14
Si4+
1s2 2s2 2p6 / [Ne]
15
P
1s2 2s2 2p6 3s2 3p3
15
P
[Ne] 3s2 3p3
15
P3-
1s2 2s2 2p6 3s2 3p6 /[Ar]
16
S
1s2 2s2 2p6 3s2 3p4
16
S
[Ne] 3s2 3p4
16
S2-
1s2 2s2 2p6 3s2 3p6 /[Ar]
17
CI
1s2 2s2 2p6 3s2 3p5
17
CI
[Ne] 3s2 3p5
17
CI-
1s2 2s2 2p6 3s2 3p6/ [Ar]
18
Ar
1s2 2s2 2p6 3s2 3p6
18
Ar
[Ar]
19
[Ne]
18
Ar
[Ar]
K
[Ar]
4s1
19
K+
1s2 2s2 2p6 3s2 3p6 /[Ar]
20
Ca
[Ar] 4s2
20
Ca2+
1s2 2s2 2p6 3s2 3p6 / [Ar]
21
Sc
[Ar] 4s2 3d1
22
Ti
[Ar] 4s2 3d2
1s2 2s2 2p6 3s2 3p6 4s2 3d3
23
V
[Ar] 4s2 3d3
Cr
1s2 2s2 2p6 3s2 3p6 4s1 3d5
24
Cr
[Ar] 4s1 3d5
25
Mn
1s2 2s2 2p6 3s2 3p6 4s2 3d5
25
Mn
[Ar] 4s2 3d5
26
Fe
1s2 2s2 2p6 3s2 3p6 4s2 3d6
26
Fe
[Ar] 4s2 3d6
27
Co
1s2 2s2 2p6 3s2 3p6 4s2 3d7
27
Co
[Ar] 4s2 3d7
28
Ni
1s2 2s2 2p6 3s2 3p6 4s2 3d8
28
Ni
[Ar] 4s2 3d8
29
Cu
1s2 2s2 2p6 3s2 3p6 4s1 3d10
29
Cu
[Ar] 4s1 3d10
30
Zn
1s2 2s2 2p6 3s2 3p6 4s2 3d10
30
Zn
[Ar] 4s2 3d10
K
1s2
2s2
2p6
3s2
3p6 4s1
19
20
Ca
1s2 2s2 2p6 3s2 3p6 4s2
21
Sc
1s2 2s2 2p6 3s2 3p6 4s2 3d1
22
Ti
1s2 2s2 2p6 3s2 3p6 4s2 3d2
23
V
24
[Ar]
5. d block
Exception to d block elements
4s energy level lower than 3d
3d
4s
3p
Electron configuration d block
21
Sc
1s2 2s2 2p6 3s2 3p6 4s2 3d1
22
Ti
V
24
Cr
25
Mn
1s2 2s2 2p6 3s2 3p6 4s2 3d5
26
Fe
1s2 2s2 2p6 3s2 3p6 4s2 3d6
27
Co
Ni
1s2 2s2 2p6 3s2 3p6 4s2 3d8
29
Cu
1s2 2s2 2p6 3s2 3p6 4s1 3d10
30
Zn
1s2 2s2 2p6 3s2 3p6 4s2 3d10
2s2
2p6
3s2
3p6 4s1
3d5
4s energy level lower than 3d
2p
1s2 2s2 2p6 3s2 3p6 4s2 3d7
28
– 1s2 2s2 2p6 3s2 3p6 4s2 3d1
1s2 2s2 2p6 3s2 3p6 4s2 3d3
1s2
21Sc
1s2 2s2 2p6 3s2 3p6 4s2 3d2
23
3s
2s
1s
24Cr
– 1s2 2s2 2p6 3s2 3p6 4s13d5
24Cr
– 1s2 2s2 2p6 3s2 3p6 4s2 3d4
3d
✔
4s
3p
3s
✗
Half fill energetically more stable
2p
2s
1s
29Cu
29Cu
–1s2 2s2 2p6 3s2 3p6 4s1 3d10
–1s2 2s2 2p6 3s2 3p6 4s2 3d9
✔
✗
4s
3p
3s
Half fill energetically more stable
2p
2s
1s
3d
6. s block elements
• s orbitals partially fill
1
H
He
p block elements
• p orbital partially fill
5
1s2
n = 2 period 2
B
[He] 2s2 2p1
6
1s1
2
Periodic Table – s, p, d, f blocks elements
C
[He] 2s2 2p2
7
N
[He] 2s2 2p3
3
Li
[He] 2s1
8
O
[He] 2s2 2p4
4
Be
[He] 2s2
9
F
[He] 2s2 2p5
11
Na
[Ne] 3s1
10
Ne
[He] 2s2 2p6
12
Mg
[Ne] 3s2
13
Al
[Ne] 3s2 3p1
14
20
K
Ca
[Ne] 3s2 3p2
[Ar]
15
P
[Ne] 3s2 3p3
[Ar]
4s2
16
S
[Ne] 3s2 3p4
17
19
Si
4s1
CI
[Ne] 3s2 3p5
18
Ar
[Ne] 3s2 3p6
d block elements
• d orbitals partially fill
• transition elements
21
Sc
[Ar] 4s2 3d1
22
Ti
[Ar] 4s2 3d2
23
V
[Ar] 4s2 3d13
24
Cr
[Ar] 4s1 3d5
25
Mn
[Ar] 4s2 3d5
26
Fe
[Ar] 4s2 3d6
27
Co
[Ar] 4s2 3d7
28
Ni
[Ar] 4s2 3d8
29
Cu
[Ar] 4s1 3d10
30
Zn
[Ar] 4s2 3d10
f block elements
• f orbitals partially fill
Video on electron configuration
Click here electron structure
Click here video on s,p,d,f notation
Click here video s,p,d,f blocks,
7. Periodic Table – s, p, d, f blocks elements
Electron structure
Chromium d block (Period 4)
1s2 2s2 2p6 3s2 3p6 4s1 3d5
[Ar] 4s1 3d5
d block – d partially filled
Electron structure
Cadmium d block (Period 5)
1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10
[Kr] 5s2 4d10
d block – d partially filled
Electron structure
Germanium p block, Gp 4 (Period 4)
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2
[Ar] 4s2 3d10 4p2
Gp 4 -4 valence electron
Electron structure
Mercury d block (Period 6)
1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p6 6s2 4f14 5d10
[Xe] 6s2 4f14 5d10
d block – d partially filled
Electron structure
Iodine p block, Gp 7 (Period 5)
1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p5
[Kr] 5s2 4d10 5p5
Gp 7 - 7 valence electron
Electron structure
Lead p block, Gp 4 (Period 6)
1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p6 6s2 4f14 5d106p2
[Xe] 6s2 4f14 5d10 6p2
Gp 4 -4 valence electron
8. Periodic Table – s, p, d, f blocks elements
s block elements
• s orbitals partially fill
1
H
He
5
1s2
n = 2 period 2
B
[He] 2s2 2p1
6
1s1
2
p block elements
• p orbital partially fill
C
[He] 2s2 2p2
7
N
[He] 2s2 2p3
3
Li
[He] 2s1
8
O
[He] 2s2 2p4
4
Be
[He] 2s2
9
F
[He] 2s2 2p5
11
Na
[Ne] 3s1
10
Ne
[He] 2s2 2p6
12
Mg
[Ne] 3s2
13
Al
[Ne] 3s2 3p1
14
Si
[Ne] 3s2 3p2
15
P
[Ne] 3s2 3p3
16
S
[Ne] 3s2 3p4
17
CI
[Ne] 3s2 3p5
18
Ar
[Ne] 3s2 3p6
19
K
20
1
Ca
[Ar]
[Ar]
1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p6 6s2 4f14 5d106p2
[Xe] 6s2 4f14 5d10 6p2
4s1
4s2
Identify position elements P, Q, R, S and T
Electron configuration :
P – 3s2 3p6
Q – 4s2 4p5
R – 3s2 3p6 4s2
S – 1s2 2s2 2p6 3s2 3p6 3d3 4s2
T – 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6
Answer
2
Write electron configuration for X, Y and Z
Element
Group
Period
X
2
3
Y
15
2
Z
18
3
Answer
Element
Group
Period
Classification
P
8/18
3
Noble gas
Q
7/17
4
p block
R
2
4
s block
S
5
4
d block
T
8/18
4
Noble gas
X – 1s2 2s2 2p6 3s2
Y – 1s2 2s2 2p3
Z – 1s2 2s2 2p6 3s2 3p6
3
Write electron structure for ions:
•
•
•
•
•
•
O - 1s2 2s2 2p4
O2- V - 1s2 2s2 2p6 3s2 3p6 4s2 3d3
V3+ Cu - 1s2 2s2 2p6 3s2 3p6 4s2 3d9
Cu2+ -
Answer
Write electron structure for ions:
•
•
•
•
•
•
O - 1s2 2s2 2p4
O2- -1s2 2s2 2p6
V - 1s2 2s2 2p6 3s2 3p6 4s2 3d3
V 3+ - 1s2 2s2 2p6 3s2 3p6 4s0 3d2
Cu - 1s2 2s2 2p6 3s2 3p6 4s2 3d9
Cu 2+ - 1s2 2s2 2p6 3s23p6 4s0 3d9
9. Four Quantum Numbers
•
•
•
Electrons arrange in specific energy level and sublevels
Orbitals of electrons in atom differ in size, shape and orientation.
Allow states call orbitals, given by four quantum number 'n', 'l', 'm l' and ’ms’ - (n, l, ml, ms)
1
Principal Quantum Number (n): n = 1, 2, 3,.. ∞
• Energy of electron and size of orbital/shell
• Distance from nucleus, (higher n – higher energy)
• Larger n - farther e from nucleus – larger size orbital
• n=1, 1stprincipal shell ( innermost/ground shell state)
2
Angular Momentum Quantum Number (l): l = 0 to n-1.
• Orbital Shape
• Divides shells into subshells/sublevels.
• Letters (s, d, p, f)
s orbital
p orbital
No TWO electron have same
4 quantum number
3
4
Magnetic Quantum Number (ml): ml = -l, 0, +l.
• Orientation orbital in space/direction
• mℓ range from −ℓ to ℓ,
• ℓ = 0 -> mℓ = 0
–> s sublevel -> 1 orbital
• ℓ = 1 -> mℓ = -1, 0, +1
-> p sublevel -> 3 diff p orbitals
• ℓ = 2 -> mℓ = -2, -1, 0, +1, +2 -> d sublevel -> 5 diff d orbitals
• (2l+ 1 ) quantum number for each ℓ value
Spin Quantum Number (ms): ms = +1/2 or -1/2
• Each orbital – 2 electrons, spin up/down
• Pair electron spin opposite direction
• One spin up, ms = +1/2
• One spin down, ms = -1/2
• No net spin/cancel out each other– diamagnetic electron
writing electron spin
electron spin up/down
d orbital
10. Principal and Angular Momentum Quantum numbers
•
•
•
Electrons arrange in specific energy level and sublevels
Orbitals of electrons in atom differ in size, shape and orientation.
Allow states call orbitals, given by four quantum number 'n', 'l', 'm l' and ’ms’ - (n, l, ml, ms)
1
Principal Quantum Number (n): n = 1, 2, 3, …, ∞
• Energy of electron and size of orbital /shell
• Distance from nucleus, (higher n – higher energy)
• Larger n - farther e from nucleus – larger size orbital
• n=1, 1stprincipal shell ( innermost/ground shell state)
2
Angular Momentum Quantum Number (l): l = 0, ..., n-1.
• Orbital Shape
• Divides shells into subshells (sublevels)
• Letters (s,p,d,f)
• < less than n-1
Sublevels, l
Quantum number, n and l
l=1
2p sublevel
l=0
2s sublevel
n= 2
n= 1
1
Principal
Quantum #, n
(Size , energy)
l=0
2
1s sublevel
Angular momentum
quantum number, l
(Shape of orbital)
2p sublevel – contain 2p orbital
2nd energy level
Has TWO sublevels
2s sublevel – contain 2s orbital
1st energy level
Has ONE sublevel
1s sublevel – contain 1s orbital
1
Principal Quantum
Number (n)
2
Angular Momentum
Quantum Number (l)
11. Electronic Orbitals
Simulation Electronic Orbitals
n = 1, 2, 3,….
Allowed values
l = 0 to n-1
Allowed values
ml = -l, 0, +l- (2l+ 1 ) for each ℓ value
ml =+2
ml =+1
ml = 0
l=1
3px orbital
ml = 0
3s sublevel
3py orbital
3s orbital
ml =+1
l=0
3pz orbital
ml = 0
3p sublevel
3dxy orbital
ml =-1
l=1
3dxz orbital
ml =+1
n= 3
3dz2 orbital
ml =-2
3d sublevel
3dyz orbital
ml =-1
l=2
Energy Level
3dx2 – y2 orbital
2py orbital
ml = 0
2p sublevel
2pz orbital
ml =-1
n= 2
2px orbital
l=0
1
Principal
Quantum #, n
(Size , energy)
2
2s sublevel
ml =0
1s sublevel
ml =0
Click here to view simulation
2s orbital
l=0
n= 1
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1s orbital
Angular momentum
quantum number, l
(Shape of orbital)
3
Magnetic Quantum
Number (ml)
(Orientation orbital)
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12. Quantum Numbers and Electronic Orbitals
ml =+2
3dx2 – y2orbital
Simulation Electronic Orbitals
Energy Level
ml =+1
3d sublevel
ml = 0
3dz2 orbital
ml =-1
l=2
3dyz orbital
3dxz orbital
Click here to view simulation
n= 3
ml =-2
3dxy orbital
ml =+1
3p sublevel
ml = 0
3pz orbital
ml =-1
l=1
3py orbital
3px orbital
Click here to view simulation
l=0
2p sublevel
n= 2
ml = 0
3s orbital
ml =+1
l=1
3s sublevel
2py orbital
ml = 0
2pz orbital
ml =-1
2px orbital
l=0
n= 1
2s sublevel
ml =0
2s orbital
l=0
1s sublevel
ml =0
1s orbital
Click here to view simulation
13. Concept Map
No TWO electron have same
4 quantum number
Quantum number
Quantum number = genetic code for electron
What are these 4 numbers?
(1, 0, 0, +1/2) 0r (3, 1, 1, +1/2)
4 numbers
n
l
ml
ms
Size/distance
Shape
Orientation
Electron has special number codes
Electron spin
Number + letter
1
Electron with quantum number given below
(n,l,ml,,ms) – (1, 0, 0, +1/2)
(n,l,ml,,ms) – (3, 1, 1, +1/2)
2
1s orbital
3py orbital
What values of l, ml, allow for n = 3? How many orbitals exists for n=3?
Video on Quantum numbers
For n=3 -> l = n -1 =2 -> ml = -l, 0, +l -> -2, -1, 0, +1, +2
• mℓ range from −ℓ to ℓ,
• ℓ = 0 -> mℓ = 0
–> s sublevel -> 1 orbital
• ℓ = 1 -> mℓ = -1, 0, +1
-> p sublevel -> 3 diff p orbitals
• ℓ = 2 -> mℓ = -2, -1, 0, +1, +2 -> d sublevel -> 5 diff d orbitals
• (2l+ 1 ) quantum number for each ℓ value
Answer = nine ml values – 9 orbitals/total # orbitals = n 2
Click here video on quantum number
Click here video on quantum number