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Chapter 7: Q9E (page 390)

Write out the full electron configuration for each of the following atoms and for the monatomic ion found in binary ionic compounds containing the element: (a) \({\rm{Al}}\) (b) \({\rm{Br}}\) (c) \({\rm{Sr}}\) (d) \({\rm{Li}}\) (e) \({\rm{As}}\) (f) \({\rm{S}}\) .

Short Answer

Expert verified
  1. The electron configuration of the atom is obtained as: \({\rm{1s^{2}}}{{\rm{2s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{1}}}\) as well as it鈥檚 ion is obtained as: \({\rm{1s^{2}}}{{\rm{2s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}\).
  2. The electron configuration of the atom is obtained as: \({\rm{1s^{2}}}{{\rm{2s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{5}}}\) as well as it鈥檚 ion is obtained as: \({\rm{1s^{2}}}{{\rm{2s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{6}}}\) .
  3. The electron configuration of the atom is obtained as:\({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{6}}}{\rm{5}}{{\rm{s}}^{\rm{2}}}\) as well as it鈥檚 ion is obtained as: \({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{6}}}\).
  4. The electron configuration of the atom is obtained as: \({\rm{1s^{2}}}{{\rm{2s}}^{\rm{1}}}\) as well as it鈥檚 ion is obtained as: \({\rm{1s}^{2}}\) .
  5. The electron configuration of the atom is obtained as: \({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{3}}}\) as well as it鈥檚 ion is obtained as: \({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{6}}}\).
  6. The electron configuration of the atom is obtained as: \({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{4}}}\) as well as it鈥檚 ion is obtained as: \({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}\).

Step by step solution

01

Define Chemical Bonding

A chemical bond is a long-term attraction between atoms, ions, or molecules that allows chemical compounds to form.

02

Writing the electron configuration for atom and monoatomic ion

a.

The electronic configuration for the atom \({\rm{Al}}\) is: \({\rm{1s^{2}}}{{\rm{2s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{1}}}\) .

The ion \({\rm{A}}{{\rm{l}}^{{\rm{3 + }}}}\) having the electronic configuration as: \({\rm{1s^{2}}}{{\rm{2s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}\) .

Therefore, electron configuration of the ion is: \({\rm{1s^{2}}}{{\rm{2s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}\) and the atom is:\({\rm{1s^{2}}}{{\rm{2s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{1}}}\) .

03

Writing the electron configuration for atom and monoatomic ion

b.

The electronic configuration for the atom \({\rm{Br}}\) is: \({\rm{1s^{2}}}{{\rm{2s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{5}}}\) .

The ion \({\rm{B}}{{\rm{r}}^{\rm{ - }}}\) having the electronic configuration as: \({\rm{1s^{2}}}{{\rm{2s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{6}}}\) . .

Therefore, electron configuration of the ion is: \({\rm{1s^{2}}}{{\rm{2s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{6}}}\) . and the atom is: \({\rm{1s^{2}}}{{\rm{2s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{5}}}\) .

04

Writing the electron configuration for atom and monoatomic ion

c.

The electronic configuration for the atom \({\rm{Sr}}\) is: \({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{6}}}{\rm{5}}{{\rm{s}}^{\rm{2}}}\) .

The ion \({\rm{S}}{{\rm{r}}^{{\rm{2 + }}}}\) having the electronic configuration as: \({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{6}}}\). .

Therefore, electron configuration of the ion is: \({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{6}}}\). and the atom is: \({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{6}}}{\rm{5}}{{\rm{s}}^{\rm{2}}}\) .

05

Writing the electron configuration for atom and monoatomic ion

d.

The electronic configuration for the atom \({\rm{Li}}\) is: \({\rm{1s^{2}}}{{\rm{2s}}^{\rm{1}}}\) .

The ion \({\rm{L}}{{\rm{i}}^{\rm{ + }}}\) having the electronic configuration as: \({\rm{1s}^{2}}\) .

Therefore, electron configuration of the ion is: \({\rm{1s}^{2}}\) and the atom is: \({\rm{1s^{2}}}{{\rm{2s}}^{\rm{1}}}\) .

06

Writing the electron configuration for atom and monoatomic ion

e.

The electronic configuration for the atom \({\rm{As}}\) is: \({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{3}}}\) .

The ion \({\rm{A}}{{\rm{s}}^{{\rm{3 - }}}}\) having the electronic configuration as: \({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{6}}}\) .

Therefore, electron configuration of the ion is:\({\rm{1s^{2}2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}\) and the atom is:\({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{3}}}\)

07

Writing the electron configuration for atom and monoatomic ion

f.

The electronic configuration for the atom \({\rm{S}}\) is:\({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{4}}}\) .

The ion \({{\rm{S}}^{{\rm{2 - }}}}\) having the electronic configuration as:\({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}\). .

Therefore, electron configuration of the ion is: \({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{6}}}\). and the atom is:\({\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{6}}}{\rm{3}}{{\rm{s}}^{\rm{2}}}{\rm{3}}{{\rm{p}}^{\rm{4}}}\) .

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Most popular questions from this chapter

What feature of a Lewis structure can be used to tell if a molecule鈥檚 (or ion鈥檚) electron-pair geometry and molecular structure will be identical?

Use the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises for a real molecule. You may need to rotate the molecules in three dimensions to see certain dipoles. (a) Sketch the bond dipoles and molecular dipole (if any) for O3. Explain your observations. (b) Look at the bond dipoles for NH3. Use these dipoles to predict whether N or H is more electronegative. (c) Predict whether there should be a molecular dipole for NH3 and, if so, in which direction it will point. Check the molecular dipole box to test your hypothesis.

Use the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises for a two-atom molecule: (a) Adjust the electronegativity value so the bond dipole is pointing toward B. Then determine what the electronegativity values must be to switch the dipole so that it points toward A. (b) With a partial positive charge on A, turn on the electric field and describe what happens. (c) With a small partial negative charge on A, turn on the electric field and describe what happens. (d) Reset all, and then with a large partial negative charge on A, turn on the electric field and describe what happens.

The reaction of a metal, \({\rm{M}}\), with a halogen, \({{\rm{X}}_{\rm{2}}}\), proceeds by an exothermic reaction as indicated by this equation: \({\rm{M(s) + }}{{\rm{X}}_{\rm{2}}}{\rm{(g)}} \to {\rm{M}}{{\rm{X}}_{\rm{2}}}{\rm{(s)}}\). For each of the following, indicate which option will make the reaction more exothermic. Explain your answers.

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(c) an increasing bond energy for the halogen

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Which of the following atoms would be expected to form negative ions in binary ionic compounds and which would be expected to form positive ions:\({\rm{P, I, Mg, Cl, In, Cs, O, Pb, Co}}\)?
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