Learning Goal: To use electron configuration to explain magnetic behavior. An im

Question

Learning Goal:To use electron configuration to explain magnetic behavior. An important property that results from the electron configuration of an atom or an ion is behavior in the presence of an external magnetic field. Due to the random orientations of electron spins most materials have no permanent magnetic effect without an external magnetic field.

Electron configuration The magnetic behavior of an atom or ion depends on its electron configuration Part A Select the correct electron configurations from the list below. You can refer to the periodic table for atomic numbers Check all that apply Hints The electron configuration of Fe is Arl4s23d6 The electron configuration of Si is [Ne] 3s23p2 The electron configuration of S2- is |Ne 3s23p6 The electron configuration of Rb is Kr]5s 4d The electron configuration of Ag is [Kr]5s14d. Submit My Answers Give Up Correct The electron configuration of an atom is a designation of how electrons are distributed among various orbitals. The electron configurations for the atoms and the ions are as shown in the following table Atom or ion Electron configuration Fe[Ar]4s23d6 Ag Rb Si Ne]3s23p2 Kr)4d10 Krj5s1 Nej3s23p Many of the physical and chemical properties (such as magnetic properties) of atoms or ions can be correlated with electron configurations

Explanation / Answer

If atoms or ions contains unpaired electrons, Those substances are paramagnetic nature.

If atoms or ions, electron are paired in orbital, Those substances are Diamagnetic nature.

Fe contains 4 unpaired electrons in d orbital, So it is an paramagnetic.

Ag+ all electrons are paired in d orbital. So it is an diamagnetic

Rb has one unpaired electron. So it is an para magnetic.

Si also has 2 unpaired electrons in p orbital, it is an para magnetic.

S-2 all electrons filled in their respective orbitals. It is an diamagnetic.

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