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Chapter 8: Q7 CYL (page 443)

How many unpaired electrons would be present on a Be22- ion? Would it be paramagnetic or diamagnetic?

Short Answer

Expert verified

It is paramagnetic and has two unpaired electrons.

Step by step solution

01

Define electron

An electron is a negatively charged component of an atom that is stable. Electrons exist outside and around the nucleus of the atom.

02

Explanation

There are two unpaired electrons that are paramagnetic.

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Most popular questions from this chapter

For many years after they were discovered, it was believed that the noble gases could not form compounds. Now we know that belief to be incorrect. A mixture of xenon and fluorine gases, confined in a quartz bulb and placed on a windowsill, is found to slowly produce a white solid. Analysis of the compound indicates that it contains \({\rm{77}}{\rm{.55\% }}\)Xe and \({\rm{22}}{\rm{.45\% \;F}}\)by mass.

(a) What is the formula of the compound?

(b) Write a Lewis structure for the compound.

(c) Predict the shape of the molecules of the compound.

(d) What hybridization is consistent with the shape you predicted?

Strike-anywhere matches contain a layer of \({\rm{KCl}}{{\rm{O}}_{\rm{3}}}\) and a layer of \({{\rm{P}}_{\rm{4}}}{{\rm{S}}_{\rm{3}}}\). The heat produced by the friction of striking the match causes these two compounds to react vigorously, which sets fire to the wooden stem of the match. \({\rm{KCl}}{{\rm{O}}_{\rm{3}}}\) contains the \({\rm{Cl}}{{\rm{O}}_{\rm{3}}}^{\rm{ - }}\) ion. \({{\rm{P}}_{\rm{4}}}{{\rm{S}}_{\rm{3}}}\) is an unusual molecule with the skeletal structure.

  1. Write Lewis structures for \({{\rm{P}}_{\rm{4}}}{{\rm{S}}_{\rm{3}}}\) and the \({\rm{Cl}}{{\rm{O}}_{\rm{3}}}^{\rm{ - }}\) ion.
  2. Describe the geometry about the \({\rm{P}}\) atoms, the \({\rm{S}}\) atom, and the \({\rm{Cl}}\) atom in these species.
  3. Assign a hybridization to the \({\rm{P}}\) atoms, the \({\rm{S}}\)atom, and the \({\rm{Cl}}\) atom in these species.
  4. Determine the oxidation states and formal charge of the atoms in \({{\rm{P}}_{\rm{4}}}{{\rm{S}}_{\rm{3}}}\) and the \({\rm{Cl}}{{\rm{O}}_{\rm{3}}}^{\rm{ - }}\) ion.

How many \({\rm{\sigma }}\)and \({\rm{\pi }}\)bonds are present in the molecule HCN?

Predict whether the MO diagram for S2 would show s-p mixing or not.

Explain why N22+ is diamagnetic, while O24+, which has the same number of valence electrons, is paramagnetic.
See all solutions

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