Dr. S. M. Condren

Chapter 8

Electron Configuration and Periodicity

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Orbitals

• region of probability of finding an electron around the nucleus

• 5 types => s p d f g

• maximum of 2 electrons per orbital

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Pure Atomic Orbitals

shape # of orbitals / energy level

s spherical 1

p dumbbell 3

d complex 5

f very complex 7

g extremely complex 9

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Pauli Exclusion Principle

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Electronic Configurations

• The shorthand representation of the occupancy of the energy levels (shells and subshells) of an atom by electrons.

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Electronic Configuration

shells => energy levels

subshells => orbitals

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Dr. S. M. Condren

Regions by Electron Type

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Electron Filling Order Diagram

1s

2s 2p

3s 3p 3d

4s 4p 4d 4f

5s 5p 5d 5f

6s 6p 6d

7s 7p

Start here

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Electronic Configuration

H atom

1 electron

1s1

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Electronic Configuration

He atom

2 electrons

1s2

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Electronic Configuration

Li atom

3 electrons

1s2, 2s1

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Electronic Configuration

Cl atom

17 electrons

1s2, 2s2, 2p6, 3s2, 3p5

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Electronic Configuration

As atom

33 electons

1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p3

or

[Ar] 4s2, 3d10, 4p3

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Mn: [Ar]4s2 3d?

How many d electrons does Mn have?

4, 5, 6

Dr. S. M. Condren

Dr. S. M. Condren

Electronic Configuration

negative ions

add electron(s), 1 electron for each negative charge

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Electronic Configuration

S-2 ion

(16 + 2)electrons

1s2, 2s2, 2p6, 3s2, 3p6

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Electronic Configuration

positive ions

remove electron(s), 1 electron for each positive charge

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Electronic Configuration

Mg+2 ion

(12-2)electrons

1s2, 2s2, 2p6

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How many valence electrons are in Cl, [Ne]3s2 3p5?

2, 5, 7

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For Cl to achieve a noble gas configuration, it is more likely that

electrons would be added

electrons would be removed

Dr. S. M. Condren

Dr. S. M. Condren

Trends in thePeriodic Table

• atomic radius

• ionic radius

• ionization energy

• electron affinity

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Atomic Radius

decrease left to right across a period

as nuclear charge increases, number of electrons increase;

however, the nucleus acts as a unit charge while the electrons act independently, pulling electrons towards the nucleus, decreasing size

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Atomic Radius

increase top to bottom down a group

each additional electron “shell” shields the outer electrons from the nuclear charge

Zeff = Z – Swhere Zeff => effective nuclear charge

Z => nuclear charge, atomic number

S => shielding constant

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Atomic Radius

• increases from upper right corner to the lower left corner

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Atomic Radius vs. Atomic Number

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Atomic Radius

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Ionic Radius

• same trends as for atomic radius

• positive ions smaller than atom

• negative ions larger than atom

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Ionic Radius

Isoelectronic Series

• series of negative ions, noble gas atom, and positive ions with the same electronic confiuration

• size decreases as “positive charge” of the nucleus increases

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Ge is a semiconductor. If half of the Ge atoms of a sample of Ge are replaced with Ga atoms, with what element should the other half of the Ga atoms be replaced in order for this new compound to be isoelectronic with Ge?

Sn, As, Se

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Ionization Energy• energy necessary to remove an electron to

form a positive ion• low value for metals, electrons easily

removed• high value for non-metals, electrons

difficult to remove• increases from lower left corner of periodic

table to the upper right corner

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Ionization Energies

first ionization energy

• energy to remove first electron from an atom

second ionization energy

• energy to remove second electron from a +1 ion

etc.

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Ionization Energy vs. Atomic Number

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Electron Affinity

• energy released when an electron is added to an atom

• same trends as ionization energy, increases from lower left corner to the upper right corner

• metals have low “EA”

• nonmetals have high “EA”

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Magnetism

Result of the spin of electrons

diamagnetism - no unpaired electrons

paramagnetism - one or more unpaired electrons

ferromagentism - case of paramagnetism where the substance retains its magnetism

Dr. S. M. Condren

Magnetism                                                                                                   

Paramagnetism

Ferromagnetism

                   

                                    

Without applied field Without applied field

With applied fieldWith applied field