IB Chemistry on Quantum Numbers and Electronic Configuration

Periodic Table of elements – divided into s, p, d, f blocks

p block • p orbital partially fill

d block • d orbitals partially filled • transition elements

f block • f orbital partially fill

s block • s orbitals partially fill

Aufbau Principle • electron occupy orbitals of lower energy first • building up, construction from bottom up

Electron filled according to 3 Principles

Click here to view simulation

1

1s

2s

2p

4Be - 1s2 2s2 5B - 1s2 2s2 2p1

1s

2s

2p

lower energy

High energy

Hund’s Principle • electron occupy orbitals singly first before pairing up

2

7N - 1s2 2s2 2p3

1s

2s

2p

High energy 8O - 1s2 2s2 2p4

Click here to view simulation

lower energy

Pauli Exclusion Principle • each orbital occupy by 2 electron opposite spin

3

4Be - 1s2 2s2 10Ne - 1s2 2s2 2p6

lower energy

High energy

Click here to view simulation

4s

3p

3p

3p

3d

2s

1s

3d

2s

Energy level and sublevels

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 2s2 2p6 3s2 3p2

15 P 1s2 2s2 2p6 3s2 3p3

16 S 1s2 2s2 2p6 3s2 3p4

17 CI 1s2 2s2 2p6 3s2 3p5

18 Ar 1s2 2s2 2p6 3s2 3p6

19 K 1s2 2s2 2p6 3s2 3p6 4s1

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 1s2 2s2 2p6 3s2 3p6 4s2 3d10

4s energy level lower than 3d

4s then 3d is fill

18Ar – 1s2 2s2 2p6 3s2 3p6

19K – 1s2 2s2 2p6 3s2 3p6 4s1

21Sc – 1s2 2s2 2p6 3s2 3p6 4s2 3d1

4s 3d

1s

2s

2p

3s

1s

2p

3s

3s

2p

4s

Electron configuration

Electrons fill 4s first

Electron occupy 4s first then 3d

Electron Notation

s, p, d, f notation Complete configuration

Noble gas notation Condensed configuration

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 2s2 2p6 3s2 3p2

15 P 1s2 2s2 2p6 3s2 3p3

16 S 1s2 2s2 2p6 3s2 3p4

17 CI 1s2 2s2 2p6 3s2 3p5

18 Ar 1s2 2s2 2p6 3s2 3p6

19 K 1s2 2s2 2p6 3s2 3p6 4s1

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 1s2 2s2 2p6 3s2 3p6 4s2 3d10

10 Ne [Ne]

11 Na [Ne] 3s1

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 [Ar]

19 K [Ar] 4s1

20 Ca [Ar] 4s2

21 Sc [Ar] 4s2 3d1

22 Ti [Ar] 4s2 3d2

23 V [Ar] 4s2 3d3

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

[Ne]

[Ar]

Positive/Negative Ion Atom

10 Ne 1s2 2s2 2p6 /[Ne]

11 Na+ 1s2 2s2 2p6 / [Ne]

12 Mg2+ 1s2 2s2 2p6 / [Ne]

13 Al3+ 1s2 2s2 2p6 / [Ne]

14 Si4+ 1s2 2s2 2p6 / [Ne]

15 P3- 1s2 2s2 2p6 3s2 3p6 /[Ar]

16 S2- 1s2 2s2 2p6 3s2 3p6 /[Ar]

17 CI- 1s2 2s2 2p6 3s2 3p6/ [Ar]

18 Ar [Ar]

19 K+ 1s2 2s2 2p6 3s2 3p6 /[Ar]

20 Ca2+ 1s2 2s2 2p6 3s2 3p6 / [Ar]

Noble gas notation Complete configuration

4s

3p

3p

3p

3d

2s

1s

3d

2s

Exception to d block elements

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 1s2 2s2 2p6 3s2 3p6 4s2 3d10

4s energy level lower than 3d 21Sc – 1s2 2s2 2p6 3s2 3p6 4s2 3d1

4s 3d

1s

2s

2p

3s

1s

2p

3s

4s

3s

2p

Electron configuration d block

24Cr – 1s2 2s2 2p6 3s2 3p6 4s13d5

24Cr – 1s2 2s2 2p6 3s2 3p6 4s2 3d4

✔

✗

29Cu –1s2 2s2 2p6 3s2 3p6 4s1 3d10

29Cu –1s2 2s2 2p6 3s2 3p6 4s2 3d9

✗ Half fill energetically more stable

✔

Half fill energetically more stable

d block

4s energy level lower than 3d

Periodic Table – s, p, d, f blocks elements s block elements • s orbitals partially fill

p block elements • p orbital partially fill

d block elements • d orbitals partially fill • transition elements

1 H 1s1

2 He 1s2

11 Na [Ne] 3s1

12 Mg [Ne] 3s2

5 B [He] 2s2 2p1

6 C [He] 2s2 2p2

7 N [He] 2s2 2p3

8 O [He] 2s2 2p4

9 F [He] 2s2 2p5

10 Ne [He] 2s2 2p6

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 [Ar] 4s1

20 Ca [Ar] 4s2

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

n = 2 period 2

3 Li [He] 2s1

4 Be [He] 2s2

Click here video s,p,d,f blocks, Click here video on s,p,d,f notation Click here electron structure

Video on electron configuration

f block elements • f orbitals partially fill

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

Electron structure Germanium p block, Gp 4 (Period 4)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2

[Ar] 4s2 3d10 4p2

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

Electron structure Iodine p block, Gp 7 (Period 5)

1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p5

[Kr] 5s2 4d10 5p5

Electron structure Cadmium d block (Period 5)

1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10

[Kr] 5s2 4d10

Electron structure Mercury d block (Period 6)

1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p6 6s2 4f14 5d10

[Xe] 6s2 4f14 5d10

Gp 4 -4 valence electron Gp 7 - 7 valence electron

Gp 4 -4 valence electron d block – d partially filled d block – d partially filled

d block – d partially filled

Periodic Table – s, p, d, f blocks elements s block elements • s orbitals partially fill

p block elements • p orbital partially fill

1 H 1s1

2 He 1s2

11 Na [Ne] 3s1

12 Mg [Ne] 3s2

5 B [He] 2s2 2p1

6 C [He] 2s2 2p2

7 N [He] 2s2 2p3

8 O [He] 2s2 2p4

9 F [He] 2s2 2p5

10 Ne [He] 2s2 2p6

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 [Ar] 4s1

20 Ca [Ar] 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

n = 2 period 2

3 Li [He] 2s1

4 Be [He] 2s2

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

Element Group Period

X 2 3

Y 15 2

Z 18 3

X – 1s2 2s2 2p6 3s2

Y – 1s2 2s2 2p3

Z – 1s2 2s2 2p6 3s2 3p6

Answer Answer

1 2 Write electron configuration for X, Y and Z

1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p6 6s2 4f14 5d106p2

[Xe] 6s2 4f14 5d10 6p2

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+ -

3

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

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', 'ml' and ’ms’ - (n, l, ml, ms)

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)

Angular Momentum Quantum Number (l): l = 0 to n-1. • Orbital Shape • Divides shells into subshells/sublevels. • Letters (s, d, p, f)

1

2

No TWO electron have same 4 quantum number

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

3

4

p orbital s orbital

d orbital

electron spin up/down

writing electron spin

Principal and Angular Momentum Quantum numbers

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)

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

Angular Momentum Quantum Number (l)

Principal Quantum Number (n)

1

2

Principal Quantum #, n (Size , energy)

Angular momentum quantum number, l (Shape of orbital)

n= 1

n= 2

l=0 1s sublevel

l=0

l=1

2s sublevel

2p sublevel

Quantum number, n and l

1 2

1 2

1st energy level Has ONE sublevel

2nd energy level Has TWO sublevels

2s sublevel – contain 2s orbital

2p sublevel – contain 2p orbital

1s sublevel – contain 1s orbital

• 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', 'ml' and ’ms’ - (n, l, ml, ms)

Electronic Orbitals

Principal Quantum #, n (Size , energy)

Angular momentum quantum number, l (Shape of orbital)

Allowed values n = 1, 2, 3,….

n= 1

n= 2

l=0 1s sublevel

Allowed values l = 0 to n-1

l=0

l=1

2s sublevel

2p sublevel

1 2

n= 3 l=1

l=2

l=0 3s sublevel

3p sublevel

3d sublevel

Magnetic Quantum Number (ml) (Orientation orbital)

3

ml =0

ml =0

ml = 0

ml =-1

ml =+1

ml = 0

ml = 0

ml =-1

ml =+1

ml = -l, 0, +l- (2l+ 1 ) for each ℓ value

ml =+1

ml =-1

ml =+2

ml =-2

ml = 0

1s orbital

2s orbital

2px orbital

2py orbital

2pz orbital

3s orbital

3px orbital

3py orbital

3pz orbital

3dxy orbital

3dxz orbital

3dyz orbital

3dz2 orbital

3dx2 – y

2 orbital

Click here to view simulation

Click here to view simulation

Click here to view simulation

Simulation Electronic Orbitals

Energy Level

Quantum Numbers and Electronic Orbitals

n= 1

n= 2

l=0 1s sublevel

l=0

l=1

2s sublevel

2p sublevel

n= 3

l=1

l=2

l=0 3s sublevel

3p sublevel

3d sublevel

ml =0

ml =0

ml = 0

ml =-1

ml =+1

ml = 0

ml = 0

ml =-1

ml =+1

ml =+1

ml =-1

ml =+2

ml =-2

ml = 0

1s orbital

2s orbital

2px orbital

2py orbital

2pz orbital

3s orbital

3px orbital

3py orbital

3pz orbital

3dxy orbital

3dxz orbital

3dyz orbital

3dz2 orbital

3dx2 – y

2orbital

Click here to view simulation

Click here to view simulation

Click here to view simulation

Simulation Electronic Orbitals

Energy Level

Shape

Click here video on quantum number Click here video on quantum number

Concept Map Quantum number

l

4 numbers

No TWO electron have same 4 quantum number

n ms

Electron has special number codes ml

Size/distance Orientation Electron spin

(n,l,ml,,ms) – (1, 0, 0, +1/2) 1s orbital

(n,l,ml,,ms) – (3, 1, 1, +1/2) 3py orbital

Quantum number = genetic code for electron

Electron with quantum number given below

Number + letter

Video on Quantum numbers

1

2 What values of l, ml, allow for n = 3? How many orbitals exists for n=3?

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

What are these 4 numbers? (1, 0, 0, +1/2) 0r (3, 1, 1, +1/2)