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Trends in Electron Affinity (EA), Exercises of Chemistry

Chemistry

Electronic Configurations of Main Group Ions ... Noble Gas Electron Configurations ... Write the condensed electron configuration of.

Typology: Exercises

2022/2023

Uploaded on 02/28/2023

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Trends in Electron Affinity (EA)
•Electron Affinity (EA) is the energy change
that occurs when 1 mol of electrons is added to
1 mol of gaseous atoms or ions.
•Atoms with a low EA tend to form cations,
while atoms with a high EA tend to form
anions
•Trend are not as regular as those for atomic size
and IE
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Trends in Electron Affinity (EA)

  • Electron Affinity (EA) is the energy change that occurs when 1 mol of electrons is added to 1 mol of gaseous atoms or ions.
  • Atoms with a low EA tend to form cations , while a toms with a high EA tend to form anions
  • Trend are not as regular as those for atomic size and IE

Electron affinities of the main-group

elements (in kJ/mol)

Summary: Trends in 3 atomic

properties

Trends in Metallic Behavior

Metals tend to lose electrons.

  • Lower IE Nonmetals tend to gain electrons.
  • More negative EA.

SODIUM MAGNESIUM ALUMINUM SILICON SULFUR

Properties of Monoatomic Ions

  1. Electronic Configurations of Main Group Ions
  2. Electronic Configurations of Transition Metal Ions
  3. Magnetic Properties of Transition Metal Ions
  4. Atomic Size vs Ionic Size

Noble Gas Electron Configurations

Transition Metal Ions

  • When a cation is formed from a transition metal, electrons are removed first from the ns orbital, then from the (n-1)d orbital.

Fe ([Ar]4s^2 3d^6 ) → Fe2+^ ([Ar]3d^6 ) + 2e-

Fe ([Ar]4s^2 3d^6 ) → Fe3+^ ([Ar]3d^5 ) + 3e-

Magnetic Properties

Magnetic properties as evidence for

proposed electron configuration

Ti ([Ar]4s^2 3d^2 ) → Ti2+^ + 2e-    4s 3d If the electrons were taken from the 3d orbital:  4s 3d If the electrons were taken from the 4s orbital:   4s 3d

Ti2+

Ti2+^ paramagnetic

diamagnetic

Learning Check

  • Write the condensed electron configuration of each transition metal ion, and predict whether it is paramagnetic or not: a) V3+^ (Z=23)

b) Cd2+^ (Z=48)

[Ar] 3 d^2 ; paramagnetic

[Kr] 4 d^10 ;

not paramagnetic

Ionic Size vs Atomic Size

  • Ionic radius increases down a group as n increases.
  • Within an isoelectronic series, ion size decreases with increasing nuclear charge. 3- > 2- > 1- > 1+ > 2+ > 3+