PeriodicProperties

of the Elements

© 2009, Prentice-Hall, Inc.

Ch. 7 Periodic Propertiesof the Elements

BLB 12th

PeriodicProperties

of the Elements

© 2009, Prentice-Hall, Inc.

Development of Periodic Table

• Elements in the same group generally have similar chemical properties.

• Physical properties are not necessarily similar, however.

PeriodicProperties

of the Elements

© 2009, Prentice-Hall, Inc.

Development of Periodic Table

Dmitri Mendeleev and Lothar Meyer independently came to the same conclusion about how elements should be grouped.

PeriodicProperties

of the Elements

© 2009, Prentice-Hall, Inc.

Development of Periodic Table

Mendeleev, for instance, predicted the discovery of germanium (which he called eka-silicon) as an element with an atomic weight between that of zinc and arsenic, but with chemical properties similar to those of silicon.

PeriodicProperties

of the Elements

© 2009, Prentice-Hall, Inc.

Periodic Trends

• In this chapter, we will rationalize observed trends in– Effective Nuclear Charge– Sizes of atoms and ions.– Ionization energy.– Electron affinity.

PeriodicProperties

of the Elements

7.2 Nuclear Charge• Nuclear charge – the attraction felt for an electron

by the nucleus• Electrons are both attracted to the nucleus and

repelled by other electrons.• The nuclear charge that an electron experiences

depends on both factors.

PeriodicProperties

of the Elements

© 2009, Prentice-Hall, Inc.

Effective Nuclear ChargeThe effective nuclear charge, Zeff, is found this way:

Zeff = Z − S, Z = atomic number

S = screening constant

PeriodicProperties

of the Elements

PeriodicProperties

of the Elements

© 2009, Prentice-Hall, Inc.

What Is the Size of an Atom?The bonding atomic radius is defined as one-half of the distance between covalently bonded nuclei.

PeriodicProperties

of the Elements

© 2009, Prentice-Hall, Inc.

7.3 Sizes of Atoms and Ions

…decrease from left to right across a row(due to increasing Zeff).

…increase from top to bottom of a column(due to increasing value of n).

PeriodicProperties

of the Elements

© 2009, Prentice-Hall, Inc.

Sizes of Ions• Ionic size depends upon:

– The nuclear charge.– The number of electrons.– The orbitals in which electrons reside.

• Cations are smaller than their parent atoms.– The outermost electron is removed and repulsions

between electrons are reduced.

• Anions are larger than their parent atoms.– Electrons are added and repulsions between electrons

are increased.

• Ions increase in size down a group.– This is due to increasing value of n.

PeriodicProperties

of the Elements

PeriodicProperties

of the Elements

© 2009, Prentice-Hall, Inc.

Sizes of Ions

• In an isoelectronic series (same number of electrons), ions have the same number of electrons.

• Ionic size decreases with an increasing nuclear charge.

PeriodicProperties

of the Elements

© 2009, Prentice-Hall, Inc.

7.4 Ionization Energy (IE)

• ionization energy - the amount of energy required to remove an electron from the ground state of a gaseous atom or ion.– first ionization energy - energy required to

remove first electron.– second ionization energy - energy required to

remove second electron, etc.

Na(g) Na+(g) + e− 1st IE 496Na+ (g) Na2+(g) + e− 2nd IE 4562

PeriodicProperties

of the Elements

© 2009, Prentice-Hall, Inc.

Ionization Energy• It requires more energy to remove each

successive electron.• When all valence electrons have been removed,

the ionization energy takes a quantum leap.

PeriodicProperties

of the Elements

PeriodicProperties

of the Elements

© 2009, Prentice-Hall, Inc.

Trends in First Ionization Energies• Down a group, less energy is required to remove

the first electron.– For atoms in the same group, Zeff is essentially the

same, but the valence electrons are farther from the nucleus.

• Across a period, it gets harder to remove an electron.– From left to right, Zeff increases.

PeriodicProperties

of the Elements

© 2009, Prentice-Hall, Inc.

Trends in First Ionization Energies

PeriodicProperties

of the Elements

© 2009, Prentice-Hall, Inc.

7.5 Electron Affinity (EA)

Electron affinity is the energy change that occurs when an electron is added to a gaseous atom:

Cl(g) + e− Cl−(g) EA = -349 kJ/mol