10. Periodic Properties of the Elements

Paramagnetism and Diamagnetism

10. Periodic Properties of the Elements

Paramagnetism and Diamagnetism

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Paramagnetism and Diamagnetism

Paramagnetism and Diamagnetism Example 1

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What are the Types of Magnets? | Don't Memorise

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What are the Types of Magnets? | Don't Memorise

DIAMAGNETIC SUBSTANCES

Diamagnetic || Paramagnetic || Ferromagnetic material || What is magnetic material?

Molecular Orbital Theory VI: Paramagnetism and Diamagnetism

Paramagnetic & Diamagnetic Elements - Paired & Unpaired Electrons

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Paramagnetism and Diamagnetism

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Multiple Choice

Which of the following atoms has the most unpaired electrons?

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Open Question

Write the condensed electron configuration for the nickel (III) ion and state if it is paramagnetic or diamagnetic.

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Multiple Choice

Write the condensed electron configuration for the copper (I) ion and is it magnetic?

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Multiple Choice

Which one of the following atoms or ions is diamagnetic?

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Textbook Question

State where in the periodic table these elements appear: (a) elements with the valence-shell electron configuration ns2np5 (b) elements that have three unpaired p electrons (c) an element whose valence electrons are 4s24p1 (d) the d-block elements [Section 6.9]

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Textbook Question

Write orbital diagrams for each of these ions.Determine if the ion is diamagnetic or paramagnetic. a. V5+ b. Cr3+ c. Ni2+ d. Fe3+

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Textbook Question

Write orbital diagrams for each ion and determine if the ion is diamagnetic or paramagnetic. a. Cd2+ b. Au+ c. Mo3+ d. Zr2+

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Textbook Question

An experiment called the Stern–Gerlach experiment helped establish the existence of electron spin. In this experiment, a beam of silver atoms is passed through a magnetic field, which deflects half of the silver atoms in one direction and half in the opposite direction. The separation between the two beams increases as the strength of the magnetic field increases. (c) Would this experiment work for a beam of fluorine (F) atoms?

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Textbook Question

Write the condensed electron configurations for the following atoms and indicate how many unpaired electrons each has: (f) Lu.

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Textbook Question

Write the condensed electron configurations for the following atoms and indicate how many unpaired electrons each has: (a) Mg.

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Textbook Question

Identify the specific element that corresponds to each of the following electron configurations and indicate the number of unpaired electrons for each: (d) 3Kr45s24d105p4.

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Textbook Question

Identify the specific element that corresponds to each of the following electron configurations and indicate the number of unpaired electrons for each: (c) 3Ar44s13d5

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Textbook Question

Identify the specific element that corresponds to each of the following electron configurations and indicate the number of unpaired electrons for each: (a) 1s22s2

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Textbook Question

(a) What does the term paramagnetism mean? (b) How can one determine experimentally whether a substance is paramagnetic? (c) Which of the following ions would you expect to be paramagnetic: O2+ , N22 -, Li2+ , O22 - ? For those ions that are paramagnetic, determine the number of unpaired electrons.

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Textbook Question

Both vanadium and its 3+ ion are paramagnetic. Refer to their electron configurations to explain this statement.

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Textbook Question

Using the periodic table as a guide, write the condensed electron configuration and determine the number of unpaired electrons for the ground state of (d) As.

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Textbook Question

In the experiment shown schematically below, a beam of neutral atoms is passed through a magnetic field. Atoms that have unpaired electrons are deflected in different directions in the magnetic field depending on the value of the electron spin quantum number. In the experiment illustrated, we envision that a beam of hydrogen atoms splits into two beams. (c) What do you think would happen if the beam of hydrogen atoms were replaced with a beam of helium atoms? Why?

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Textbook Question

In the experiment shown schematically below, a beam of neutral atoms is passed through a magnetic field. Atoms that have unpaired electrons are deflected in different directions in the magnetic field depending on the value of the electron spin quantum number. In the experiment illustrated, we envision that a beam of hydrogen atoms splits into two beams. (a) What is the significance of the observation that the single beam splits into two beams?

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Textbook Question

Carbon monoxide is produced by incomplete combustion of fossil fuels. (b) Do you expect CO to be paramagnetic or diamagnetic?

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Textbook Question

How many unpaired electrons are present in each of the following ground-state atoms? (a) O (b) Si (c) K (d) As

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Textbook Question

Consider the elements: B, C, N, O, F. d. Which element has three unpaired electrons?

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Textbook Question

Consider the elements: Na, Mg, Al, Si, P. d. Which element is diamagnetic?

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Textbook Question

Cyclooctatetraene dianion, C8H8 2-, is an organic ion with the structure shown. Considering only the p bonds and not the s bonds, cyclooctatetraene dianion can be described by the following energy diagrams of its p molecular orbitals:

(d) Based on your MO energy diagram, is the dianion paramagnetic or diamagnetic?

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Open Question

In the ground-state electron configuration of Fe³⁺, how many unpaired electrons are present?

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Open Question

Select the element(s) that will have one unpaired electron in the p orbital.

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Open Question

Identify the general outer electron configuration for each group of elements shown in this periodic table outline.

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Open Question

Sort the following atom or ions as paramagnetic or diamagnetic according to the electron configurations determined in part a.

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Open Question

In the ground-state electron configuration of Fe³⁺, how many unpaired electrons are present?

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Open Question

How many unpaired electrons are present in the ground state of the atoms in group 6A(16)?

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10. Periodic Properties of the Elements

Paramagnetism and Diamagnetism

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