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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

Methanol,\({{\text{H}}_{\text{3}}}{\text{COH}}\), is used as the fuel in some race cars. Ethanol,\({{\text{C}}_{\text{2}}}{{\text{H}}_{\text{5}}}{\text{OH}}\), is used extensively as motor fuel in Brazil. Both methanol and ethanol produce\({\text{C}}{{\text{O}}_{\text{2}}}\)and\({{\text{H}}_{\text{2}}}{\text{O}}\)when they burn. Write the chemical equations for these combustion reactions using Lewis structures instead of chemical formulas.

There are three possible structures for \({\rm{PC}}{{\rm{l}}_{\rm{2}}}{\rm{\;}}{{\rm{F}}_{\rm{3}}}\)with phosphorus as the central atom. Draw them and discuss how measurements of dipole moments could help distinguish among them.

From their positions in the periodic table, arrange the atoms in each of the following series in order of increasing electronegativity: (a)\({\rm{As, H, N, P, Sb}}\)(b)\({\rm{Cl, H, P, S, Si}}\)(c)\({\rm{Br, Cl, Ge, H, Sr}}\)(d)\({\rm{Ca, H, K, N, Si}}\)(e)\({\rm{Cl, Cs, Ge, H, Sr}}\).

Write Lewis structures for the following: (a)\({\rm{Se}}{{\rm{F}}_{\rm{6}}}\)(b)\({\rm{Xe}}{{\rm{F}}_{\rm{4}}}\)(c)\({\rm{SeC}}{{\rm{l}}_{\rm{3}}}^{\rm{ + }}\)(d)\({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{BBC}}{{\rm{l}}_{\rm{2}}}\)(contains a\({\rm{B - B}}\)bond).

Predict the electron pair geometry and the molecular structure of each of the following ions:

  1. \({{\rm{H}}_{\rm{3}}}{{\rm{O}}^{\rm{ + }}}\,\)
  2. \({\rm{PC}}{{\rm{l}}_{\rm{4}}}{\rm{ - }}\)
  3. \({\rm{SnC}}{{\rm{l}}_{\rm{3}}}^{\rm{ - }}\)
  4. \({\rm{BrC}}{{\rm{l}}_{\rm{4}}}^{\rm{ - }}\)
  5. \({\rm{IC}}{{\rm{l}}_{\rm{3}}}\)
  6. \({\rm{Xe}}{{\rm{F}}_{\rm{4}}}\)
  7. \({\rm{S}}{{\rm{F}}_{\rm{2}}}\)
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