Transcript
Page 1: To learn about the shapes of the  s, p  and  d  orbitals

Section 11.3

Atomic Orbitals

1. To learn about the shapes of the s, p and d orbitals

2. To review the energy levels and orbitals of the wave mechanical model of the atom

3. To learn about electron spin

Objectives

Page 2: To learn about the shapes of the  s, p  and  d  orbitals

Section 11.3

Atomic Orbitals

A. The Hydrogen Orbitals

• Orbitals do not have sharp boundaries.

90% boundary

Page 3: To learn about the shapes of the  s, p  and  d  orbitals

Section 11.3

Atomic Orbitals

A. The Hydrogen Orbitals

• Hydrogen has discrete energy levels.• Called principal energy

levels (electron shells)• Labeled with whole numbers• Energy is related to 1/n2

• En = E1/n2

• Energy levels are closer together the further they are from the nucleus

Hydrogen Energy Levels

Page 4: To learn about the shapes of the  s, p  and  d  orbitals

Section 11.3

Atomic Orbitals

A. The Hydrogen Orbitals

• Each principal energy level is divided into sublevels.

Hydrogen Energy Levels

– Labeled with numbers and letters – Indicate the shape of the orbital

Page 5: To learn about the shapes of the  s, p  and  d  orbitals

Section 11.3

Atomic Orbitals

Orbital Designations

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Section 11.3

Atomic Orbitals

Orbitals Define the Periodic Table

Page 7: To learn about the shapes of the  s, p  and  d  orbitals

Section 11.3

Atomic Orbitals

A. The Hydrogen Orbitals

• The s and p types of sublevel

Hydrogen Energy Levels

Page 8: To learn about the shapes of the  s, p  and  d  orbitals

Section 11.3

Atomic Orbitals

Representation of s, p, d atomic orbitals

Page 9: To learn about the shapes of the  s, p  and  d  orbitals

Section 11.3

Atomic Orbitals

A. The Hydrogen Orbitals

• Why does an H atom have so many orbitals and only 1 electron? – An orbital is a potential space for an electron. – Atoms can have many potential orbitals.

• s, p, d, f orbitals named for sharp, principal, diffuse and fundamental lines on spectra. Further orbitals designated alphabetically

Hydrogen Orbitals

Page 10: To learn about the shapes of the  s, p  and  d  orbitals

Section 11.3

Atomic Orbitals

g g gg

f ff

s p d d

Page 11: To learn about the shapes of the  s, p  and  d  orbitals

Section 11.3

Atomic Orbitals

• Close examination of spectra revealed doublets• Need one more property to determine how electrons

are arranged• Spin – electron modeled as a spinning like a top• Spin is the basis of magnetism

B. The Wave Mechanical Model: Further Development

Electron Spin

Page 12: To learn about the shapes of the  s, p  and  d  orbitals

Section 11.3

Atomic Orbitals

• Pauli Exclusion Principle (Wolfgang Pauli 1925) - an atomic orbital can hold a maximum of 2 electrons and those 2 electrons must have opposite spins

• When an orbital contains two electrons (of opposite spin) it is said to be full

B. The Wave Mechanical Model: Further Development

Pauli Exclusion Principle

What are the four descriptors that define an energy level / electron’s position in an atom?


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