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Chapter 9: Problem 37

Must all atoms with an odd atomic number be paramagnetic? Must all atoms with an even atomic number be diamagnetic? Explain.

Short Answer

Expert verified
No, not all atoms with an odd atomic number must be paramagnetic nor must all atoms with an even atomic number be diamagnetic. Whether an atom is paramagnetic or diamagnetic is not primarily determined by whether its atomic number is odd or even, but by whether it has unpaired electrons (paramagnetic) or all electrons are paired (diamagnetic).

Step by step solution

01

Understanding Atomic Number and Electron Configuration

Atomic number specifies the number of protons in an atom, and in an atom that is electrically neutral, this equals the number of electrons as well. Since the atomic number determines the electron configuration of an atom, we now need to assess if an odd or even atomic number directly relate to paramagnetic or diamagnetic properties.
02

Analyzing Paramagnetic Atoms

Paramagnetism occurs when an atom possesses one or more unpaired electrons. This does not necessarily relate to the atomic number being odd. For instance, helium (He) with an atomic number 2, and Neon (Ne) with atomic number 10 both have all their atomic orbitals fully filled and shows no unpaired electron, hence they are not paramagnetic.
03

Analyzing Diamagnetic Atoms

Diamagnetism is displayed by atoms that have all their electrons paired up in their atomic orbitals, and hence, are repelled by a magnetic field. This doesn't directly relate to the atomic number being even. Take for example, lithium (Li) with an atomic number of 3 and oxygen (O) with an atomic number of 8 both have paired electrons and are diamagnetic.

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Most popular questions from this chapter

Which is (a) the smallest atom in group \(13 ;\) (b) the smallest of the following atoms: Te, In, Sr, Po, Sb? Why?

Describe how the ionization energies of the ions \(\mathrm{He}^{-}, \mathrm{Li}^{-}, \mathrm{Be}^{-}, \mathrm{B}^{-}, \mathrm{C}^{-}, \mathrm{N}^{-}, \mathrm{O}^{-},\) and \(\mathrm{F}^{-}\) vary with atomic number.

The largest of the following is (a) an Ar atom; (b) a \(\mathrm{K}^{+}\) ion; \((c) a C a^{2+}\) ion; \((d) a C l^{-}\) ion.

Assuming that the seventh period is 32 members long, what should be the atomic number of the noble gas following radon (Rn)? Of the alkali metal following francium (Fr)? What would you expect their approximate atomic masses to be?

Arrange the following elements in order of decreasing metallic character: $\mathrm{Sc}, \mathrm{Fe}, \mathrm{Rb}, \mathrm{Br}, \mathrm{O}, \mathrm{Ca}, \mathrm{F}, \mathrm{Te}.$
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