Sci c un5elctrncnfgrtnorbtldgrms

Maximum Number of Electrons In Each SublevelMaximum Number of Electrons In Each Sublevel

Maximum Number Sublevel Number of Orbitals of Electrons

s 1 2

p 3 6

d 5 10

f 7 14

LeMay Jr, Beall, Robblee, Brower, Chemistry Connections to Our Changing World , 1996, page 146

General Rules

Aufbau PrincipleAufbau Principle

– Electrons fill the lowest energy orbitals first.

– “Lazy Tenant Rule”

Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

2s

3s

4s

5s

6s

7s

1s

2p

3p

4p

5p

6p

3d

4d

5d

6d

4f

5f

1s

2s

2p

3s

3p

4s

4p

3d

4d5s

5p6s

7s

6p

6d

4f

5f

5d

En

erg

y

Order in which subshells are filled with electrons

1s

2s

3s

4s

5s

6s

7s

2p

3p

4p

5p

6p

3d

4d

5d

6d

4f

5f

1s 2s 2p 3s 3p 4s 3d 4p 5s 4d … 2 2 6 2 6 2 10 6 2 10

Energy Level Diagram of a Many-Electron Atom

ArbitraryEnergy Scale

18

18

32

8

8

2

1s

2s 2p

3s 3p

4s 4p 3d

5s 5p 4d

6s 6p 5d 4f

NUCLEUS

O’Connor, Davis, MacNab, McClellan, CHEMISTRY Experiments and Principles 1982, page 177

Orbital Diagrams

General Rules

• Pauli Exclusion PrinciplePauli Exclusion Principle

– Each orbital can hold TWO electrons with

opposite spins.


Wolfgang Pauli

RIGHTWRONG

General Rules

• Hund’s RuleHund’s Rule

– Within a sublevel, place one electron per orbital before pairing them.

– “Empty Bus Seat Rule”


Filling Rules for Electron Orbitals

Aufbau Principle: Electrons are added one at a time to the lowest energy orbitals available until all the electrons of the atom have been accounted for.

Pauli Exclusion Principle: An orbital can hold a maximum of two electrons.To occupy the same orbital, two electrons must spin in opposite directions.

Hund’s Rule: Electrons occupy equal-energy orbitals so that a maximum number of unpaired electrons results.

*Aufbau is German for “building up”

O

8e-

• Orbital Diagram

• Electron Configuration

1s1s22 2s2s22 2p2p44

Notation

1s 2s 2p


O15.9994

8

Orbital Filling

Element 1s 2s 2px 2py 2pz 3s Configuration

Orbital Filling


Electron ConfigurationsElectron

H

He

Li

C

N

O

F

Ne

Na

1s1

1s22s22p63s1

1s22s22p6

1s22s22p5

1s22s22p4

1s22s22p3

1s22s22p2

1s22s1

1s2

NOT CORRECTViolates Hund’s

Rule


H

He

Li

C

N

O

F

Ne

Na

1s1

1s22s22p63s1

1s22s22p6

1s22s22p5

1s22s22p4

1s22s22p3

1s22s22p2

1s22s1

1s2

Orbital Filling



H

He

Li

C

N

O

F

Ne

Na

1s1

1s22s22p63s1

1s22s22p6

1s22s22p5

1s22s22p4

1s22s22p3

1s22s22p2

1s22s1

1s2

Energy Level Diagram

Arb

itrar

y E

nerg

y S

cale

1s

2s 2p

3s 3p

4s 4p 3d

5s 5p 4d

6s 6p 5d 4f

NUCLEUS

Bohr Model

Electron Configuration

CLICK ON ELEMENT TO FILL IN CHARTS

N

H He Li C N Al Ar F Fe La


Arb

itrar

y E

nerg

y S

cale

1s

2s 2p

3s 3p

4s 4p 3d

5s 5p 4d

6s 6p 5d 4f

NUCLEUS

Bohr Model



N

H = 1s1

Hydrogen



Arb

itrar

y E

nerg

y S

cale

1s

2s 2p

3s 3p

4s 4p 3d

5s 5p 4d

6s 6p 5d 4f

NUCLEUS

Bohr Model



N

He = 1s2

Helium



Arb

itrar

y E

nerg

y S

cale

1s

2s 2p

3s 3p

4s 4p 3d

5s 5p 4d

6s 6p 5d 4f

NUCLEUS

Bohr Model



N

Li = 1s22s1

Lithium



Arb

itrar

y E

nerg

y S

cale

1s

2s 2p

3s 3p

4s 4p 3d

5s 5p 4d

6s 6p 5d 4f

NUCLEUS

Bohr Model



N

C = 1s22s22p2

Carbon



Arb

itrar

y E

nerg

y S

cale

1s

2s 2p

3s 3p

4s 4p 3d

5s 5p 4d

6s 6p 5d 4f

NUCLEUS



N

N = 1s22s22p3

Bohr Model

Nitrogen

Hund’s Rule “maximum number of unpaired

orbitals”.



Arb

itrar

y E

nerg

y S

cale

1s

2s 2p

3s 3p

4s 4p 3d

5s 5p 4d

6s 6p 5d 4f

NUCLEUS

Bohr Model



N

F = 1s22s22p5

Fluorine



Arb

itrar

y E

nerg

y S

cale

1s

2s 2p

3s 3p

4s 4p 3d

5s 5p 4d

6s 6p 5d 4f

NUCLEUS

Bohr Model



N

Al = 1s22s22p63s23p1

Aluminum



Arb

itrar

y E

nerg

y S

cale

1s

2s 2p

3s 3p

4s 4p 3d

5s 5p 4d

6s 6p 5d 4f

NUCLEUS



N

Ar = 1s22s22p63s23p6

Bohr Model

Argon



Arb

itrar

y E

nerg

y S

cale

1s

2s 2p

3s 3p

4s 4p 3d

5s 5p 4d

6s 6p 5d 4f

NUCLEUS


Fe = 1s22s22p63s23p64s23d6

N


Bohr Model

Iron



Arb

itrar

y E

nerg

y S

cale

1s

2s 2p

3s 3p

4s 4p 3d

5s 5p 4d

6s 6p 5d 4f

NUCLEUS


La = 1s22s22p63s23p64s23d10

4s23d104p65s24d105p66s25d1

N


Bohr Model

Lanthanum


sp

d (n-1)

f (n-2) 67

Periodic Patterns

11ss

22ss

33ss

44ss

55ss

66ss

77ss

33dd

44dd

55dd

66dd

11ss

22pp

33pp

44pp

55pp

66pp

77pp

44ff

55ff

1234567

Periodic Patterns

• Period #– energy level (subtract for d & f)

• A/B Group # – total # of valence e-

• Column within sublevel block– # of e- in sublevel


s-block1st Period

1s11st column of s-block

Periodic Patterns

• Example - Hydrogen


• Full energy level

1

2

3

4

5

6

7

• Full sublevel (s, p, d, f)• Half-full sublevel

Stability


Write out the complete electron configuration for the following:1) An atom of nitrogen

2) An atom of silver

3) An atom of uranium (shorthand)

Fill in the orbital boxes for an atom of nickel (Ni)

2s 2p 3s 3p 4s 3d1s

Which rule states no two electrons can spin the same direction in a single orbital?

Extra credit: Draw a Bohr model of a Ti4+ cation.

Ti4+ is isoelectronic to Argon.

POP QUIZ

Write out the complete electron configuration for the following:1) An atom of nitrogen

2) An atom of silver

3) An atom of uranium (shorthand)

Fill in the orbital boxes for an atom of nickel (Ni)

2s 2p 3s 3p 4s 3d1s

Which rule states no two electrons can spin the same direction in a single orbital?

1s22s22p3

1s22s22p63s23p64s23d104p65s24d9

[Rn]7s26d15f3

Extra credit: Draw a Bohr model of a Ti4+ cation. 22+n = n

Pauli exclusion principle

Ti4+ is isoelectronic to Argon.

Answer Key

Sci c un5elctrncnfgrtnorbtldgrms

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