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Relate to the following data. An atom with an equal number of spin-up and spindown electrons is said to be diamagnetic because the atom is repelled by a magnetic field. In this case we say that all of the electrons are "paired." If this is not the case - if there are one or more unpaired electrons on an atom - the atom is attracted to a magnetic field, and it is said to be paramagnetic. The strength of the attraction is an experimentally measurable quantity known as the magnetic moment. The magnitude of the \(m a g-\) netic moment (measured in magnetons) is related to (but not proportional to) the number of unpaired electrons present. In other words, the larger the number of unpaired electrons, the larger the magnetic moment. Here are some experimental data collected by an investigator of this phenomenon. $$ \begin{array}{llc} {3}{c} {\text { Magnetic Moments of Several Elements }} \\ \hline & & \\ \text { Element } & \text { Type } & \begin{array}{c} \text { Magnetic Moments } \\ \text { (magnetons) } \end{array} \\ \hline \mathrm{H} & \text { Paramagnetic } & 1.7 \\ \mathrm{He} & \text { Diamagnetic } & 0 \\ \mathrm{~B} & \text { Paramagnetic } & 1.7 \\ \mathrm{C} & \text { Paramagnetic } & 2.8 \\ \mathrm{~N} & \text { Paramagnetic } & 3.9 \\ \mathrm{O} & \text { Paramagnetic } & 2.8 \\ \mathrm{Ne} & \text { Diamagnetic } & 0 \\ \hline \end{array} $$ How many unpaired electrons are in the following atoms? (a) \(C\) (b) \(\mathrm{N}\) (c) \(\mathrm{O}\) (d) \(\mathrm{Ne}\) (e) \(\mathrm{F}\)

Step by step solution

01

Understanding Paired and Unpaired Electrons

Atoms with equal numbers of spin-up and spin-down electrons are diamagnetic and have paired electrons. Atoms with one or more unpaired electrons are paramagnetic and attracted to magnetic fields.

02

Reviewing Magnetic Moments

The magnetic moments provided give insight into the number of unpaired electrons: Higher magnetic moments suggest more unpaired electrons.

03

Identifying Unpaired Electrons for Carbon (C)

Carbon with a magnetic moment of 2.8 is paramagnetic. In its ground state, carbon's electron configuration is 1s虏 2s虏 2p虏, meaning it has 2 unpaired electrons in the 2p orbital.

04

Identifying Unpaired Electrons for Nitrogen (N)

Nitrogen has a magnetic moment of 3.9, reflecting its paramagnetic nature. The electron configuration 1s虏 2s虏 2p鲁 contains three unpaired electrons in the 2p orbitals.

05

Identifying Unpaired Electrons for Oxygen (O)

Oxygen, with a magnetic moment of 2.8, is also paramagnetic. Its electron configuration 1s虏 2s虏 2p鈦� results in 2 unpaired electrons in the 2p orbitals.

06

Identifying Unpaired Electrons for Neon (Ne)

Neon is diamagnetic with a magnetic moment of 0, confirming that all of its electrons are paired. The configuration is 1s虏 2s虏 2p鈦�, with no unpaired electrons.

07

Identifying Unpaired Electrons for Fluorine (F)

Fluorine, not provided in the table but can be deduced, has an electron configuration of 1s虏 2s虏 2p鈦�. This results in one unpaired electron in the 2p orbitals.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Diamagnetism

Diamagnetism refers to the behavior of atoms or molecules that have all their electrons paired. This means each electron's spin, which can be visualized as an arrow pointing up or down, is matched or paired with another electron of opposite spin. Because these pairs cancel out each other's magnetic effects, the atom or molecule is not attracted to a magnetic field and is actually slightly repelled.

Some key points to remember about diamagnetic materials:

• They have zero net magnetic moment.
• All their electrons are paired.
• They exhibit no net magnetic effect under an external magnetic field.

Elements like Helium (He) and Neon (Ne) are common examples of diamagnetic substances, where their electron configurations allow them to have no unpaired electrons.

Understanding Diamagnetism in Daily Life

In practical terms, diamagnetism might be subtle and less noticeable compared to other magnetic behaviors, but it's an interesting fundamental property. If you ever tried to place a strong magnet near many substances like water, wood, or plastic, you've observed diamagnetic properties in action, although they are quite weak compared to ferromagnetism or paramagnetism.

Paramagnetism

Paramagnetism is exhibited by materials that have one or more unpaired electrons. Unlike diamagnetic materials, paramagnetic substances are attracted to magnetic fields. This is due to the fact that unpaired electrons contribute a magnetic moment due to their spin, which, when aligned, enhances the material's interaction with the magnetic field.

The characteristics of paramagnetic materials include:

• Presence of unpaired electrons.
• Positive magnetic susceptibility, meaning they are attracted by magnetic fields.
• This attraction is temporary and disappears when the external magnetic field is removed.

For example, atoms of Hydrogen (H), Carbon (C), Nitrogen (N), and Oxygen (O) display paramagnetic behavior due to their unpaired electrons. The strength of the paramagnetic effect is determined by the number of these unpaired electrons, as seen in their different magnetic moments measured in magnetons.

Effects in Everyday Materials

Though less visible in daily life compared to ferromagnetic materials like iron, paramagnetic properties can be crucial in understanding the behavior of certain metals and compounds in chemistry. When evaluating a material鈥檚 electronic structure, noticing unpaired electrons can help predict magnetic behavior.

Magnetic Moment

The term "magnetic moment" describes the strength and orientation of a magnet's magnetism. In atomic and molecular physics, a magnetic moment results from both the motion of electrons around the nucleus and their spin. It quantitatively describes how strong a magnetic source is and is typically measured in units called Bohr magnetons.

A magnetic moment is pivotal because:

• It indicates the degree of magnetic behavior a material may exhibit under an external magnetic field.
• It is often proportional to the number of unpaired electrons in an atom or molecule, but not directly so.
• The magnetic moment can help predict whether a substance is likely to be diamagnet or paramagnet based on empirical measurements.

For instance, elements like Carbon (C) and Nitrogen (N) show different magnetic moments (2.8 and 3.9 magnetons, respectively), which reflect the number and organization of their unpaired electrons.

Real-World Implications of Magnetic Moment

An understanding of magnetic moments provides critical insights into the electronic configuration of atoms. It plays a significant role in technologies such as MRI in medical imaging and enhances the study of electromagnetic fields and materials used in various electronic devices.