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Chapter 7: Q7E (page 390)

Write the electron configuration for each of the following ions: (a) \({\rm{A}}{{\rm{s}}^{{\rm{3 - }}}}\) (b) \({{\rm{I}}^{\rm{ - }}}\) (c) \({\rm{B}}{{\rm{e}}^{{\rm{2 + }}}}\) (d) \({\rm{C}}{{\rm{d}}^{{\rm{2 + }}}}\)(e) \({{\rm{O}}^{{\rm{2 - }}}}\) (f) \({\rm{G}}{{\rm{a}}^{{\rm{3 + }}}}\) (g) \({\rm{L}}{{\rm{i}}^{\rm{ + }}}\) (h) \({{\rm{N}}^{{\rm{3 - }}}}\) (i) \({\rm{S}}{{\rm{n}}^{{\rm{2 + }}}}\) (j) \({\rm{C}}{{\rm{o}}^{{\rm{2 + }}}}\) (k) \({\rm{F}}{{\rm{e}}^{{\rm{2 + }}}}\) (l) \({\rm{A}}{{\rm{s}}^{{\rm{3 + }}}}\) .

Short Answer

Expert verified
  1. The electronic configuration is obtained as: \(\left[ {{\rm{Ar}}} \right]{\rm{4s^{{\rm{2}}}} {3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{p}}^{\rm{6}}}\) .
  2. The electronic configuration is obtained as: \(\left[ {{\rm{Kr}}} \right]{\rm{4}}{{\rm{d}}^{{\rm{10}}}}{\rm{5s^{{\rm{2}}}} {5}}{{\rm{p}}^{\rm{6}}}\) .
  3. The electronic configuration is obtained as: \({\rm{1s}}^{\rm{2}} \).
  4. The electronic configuration is obtained as: \(\left[ {{\rm{Kr}}} \right]{\rm{4}}{{\rm{d}}^{{\rm{10}}}}\).
  5. The electronic configuration is obtained as: \(\left[ {{\rm{He}}} \right]{\rm{4s^{\rm{2}} \ 2}}{{\rm{p}}^{\rm{6}}}\) .
  6. The electronic configuration is obtained as:\(\left[ {{\rm{Ar}}} \right]{\rm{3}}{{\rm{d}}^{{\rm{10}}}}\)
  7. The electronic configuration is obtained as: \({\rm{1s}}^{\rm{2}} \) .
  8. The electronic configuration is obtained as: \(\left[ {{\rm{He}}} \right]{\rm{2s^{\rm{2}} \ 2}}{{\rm{p}}^{\rm{6}}}\) .
  9. The electronic configuration is obtained as: \(\left[ {{\rm{Kr}}} \right]{\rm{4}}{{\rm{d}}^{{\rm{10}}}}{\rm{5}}{{\rm{s}}^{\rm{2}}}\) .
  10. The electronic configuration is obtained as: \(\left[ {{\rm{Ar}}} \right]{\rm{3}}{{\rm{d}}^{\rm{7}}}\) .
  11. The electronic configuration is obtained as: \(\left[ {{\rm{Ar}}} \right]{\rm{3}}{{\rm{d}}^{\rm{6}}}\) .
  12. The electronic configuration is obtained as:\(\left[ {{\rm{Kr}}} \right]{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}\) .

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 electronic configuration for ion

a. The electric configuration for the ion \({\rm{A}}{{\rm{s}}^{{\rm{3 - }}}}\)is: \(\left[ {{\rm{Ar}}} \right]{\rm{4s^{\rm{2}} \ 3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{p}}^{\rm{6}}}\).

Therefore, electric configuration is: \(\left[ {{\rm{Ar}}} \right]{\rm{4s^{\rm{2}} \ 3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{p}}^{\rm{6}}}\). .

03

Writing the electronic configuration for ion

b. The electric configuration for the ion \({{\rm{I}}^{\rm{ - }}}\)is: \(\left[ {{\rm{Kr}}} \right]{\rm{4}}{{\rm{d}}^{{\rm{10}}}}{\rm{5s^{\rm{2}} \ 5}}{{\rm{p}}^{\rm{6}}}\).

Therefore, electric configuration is: \(\left[ {{\rm{Kr}}} \right]{\rm{4}}{{\rm{d}}^{{\rm{10}}}}{\rm{5s^{\rm{2}} \ 5}}{{\rm{p}}^{\rm{6}}}\).

04

Writing the electronic configuration for ion

c. The electric configuration for the ion \({\rm{B}}{{\rm{e}}^{{\rm{2 + }}}}\)is: \({\rm{1s}}^{\rm{2}}\).

Therefore, electric configuration is:\({\rm{1s}}^{\rm{2}}\) .

05

Writing the electronic configuration for ion

d. The electric configuration for the ion \({\rm{C}}{{\rm{d}}^{{\rm{2 + }}}}\)is: \(\left( {{\rm{Kr}}} \right){\rm{4}}{{\rm{d}}^{{\rm{10}}}}\).

Therefore, electric configuration is: \(\left( {{\rm{Kr}}} \right){\rm{4}}{{\rm{d}}^{{\rm{10}}}}\).

06

Writing the electronic configuration for ion

e. The electric configuration for the ion \({{\rm{O}}^{{\rm{2 - }}}}\)is: \(\left[ {{\rm{He}}} \right]{\rm{4s^{\rm{2}} \ 2}}{{\rm{p}}^{\rm{6}}}\) .

Therefore, electric configuration is: \(\left[ {{\rm{He}}} \right]{\rm{4s^{\rm{2}} \ 2}}{{\rm{p}}^{\rm{6}}}\) . .

07

Writing the electronic configuration for ion

f. The electric configuration for the ion \({\rm{G}}{{\rm{a}}^{{\rm{3 + }}}}\)is: \(\left( {{\rm{Ar}}} \right){\rm{3}}{{\rm{d}}^{{\rm{10}}}}\).

Therefore, electric configuration is: \(\left( {{\rm{Ar}}} \right){\rm{3}}{{\rm{d}}^{{\rm{10}}}}\).

08

Writing the electronic configuration for ion

g.

The electric configuration for the ion \({\rm{L}}{{\rm{i}}^{\rm{ + }}}\)is: \({\rm{1s}}^{\rm{2}} \) .

Therefore, electric configuration is: \({\rm{1s}}^{\rm{2}} \) .

09

Writing the electronic configuration for ion

h. The electric configuration for the ion \({{\rm{N}}^{{\rm{3 - }}}}\)is: \(\left[ {{\rm{He}}} \right]{\rm{2s^{\rm{2}} \ 2}}{{\rm{p}}^{\rm{6}}}\) .

Therefore, electric configuration is: \(\left[ {{\rm{He}}} \right]{\rm{2s^{\rm{2}} \ 2}}{{\rm{p}}^{\rm{6}}}\) .

10

Writing the electronic configuration for ion

i.

The electric configuration for the ion \({\rm{S}}{{\rm{n}}^{{\rm{2 + }}}}\)is: \(\left( {{\rm{Kr}}} \right){\rm{4}}{{\rm{d}}^{{\rm{10}}}}{\rm{5}}{{\rm{s}}^{\rm{2}}}\).

Therefore, electric configuration is: \(\left( {{\rm{Kr}}} \right){\rm{4}}{{\rm{d}}^{{\rm{10}}}}{\rm{5}}{{\rm{s}}^{\rm{2}}}\).

11

Writing the electronic configuration for ion

j.

The electric configuration for the ion \({\rm{C}}{{\rm{o}}^{{\rm{2 + }}}}\)is: \(\left( {{\rm{Ar}}} \right){\rm{3}}{{\rm{d}}^{\rm{7}}}\).

Therefore, electric configuration is: \(\left( {{\rm{Ar}}} \right){\rm{3}}{{\rm{d}}^{\rm{7}}}\).

12

Writing the electronic configuration for ion

k.

The electric configuration for the ion \({\rm{F}}{{\rm{e}}^{{\rm{2 + }}}}\)is: \(\left( {{\rm{Ar}}} \right){\rm{3}}{{\rm{d}}^{\rm{6}}}\).

Therefore, electric configuration is: \(\left( {{\rm{Ar}}} \right){\rm{3}}{{\rm{d}}^{\rm{6}}}\).

13

Writing the electronic configuration for ion

l

The electric configuration for the ion \({\rm{A}}{{\rm{s}}^{{\rm{3 + }}}}\)is: \(\left( {{\rm{Kr}}} \right){\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}\).

Therefore, electric configuration is: \(\left( {{\rm{Kr}}} \right){\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}\).

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Most popular questions from this chapter

The lattice energy of \({\rm{KF}}\) is \({\rm{794kJ/mol}}\), and the interionic distance is \({\rm{269 pm}}\). The \({\rm{Na - F}}\) distance in \({\rm{NaF}}\), which has the same structure as \({\rm{KF}}\), is \({\rm{231 pm}}\). Which of the following values is the closest approximation of the lattice energy of \({\rm{NaF}}\): \({\rm{682 kJ/mol, 794 kJ/mol, 924 kJ/mol, 1588 kJ/mol,}}\) or \({\rm{3175 kJ/mol}}\)? Explain your answer.

Which of the following molecules and ions contain polar bonds? Which of these molecules and ions have dipole moments?

  1. \({\rm{Cl}}{{\rm{F}}_{\rm{5}}}\)
  2. \({\rm{Cl}}{{\rm{O}}_{\rm{2}}}{\rm{ - }}\)
  3. \({\rm{TeC}}{{\rm{l}}_{\rm{4}}}^{{\rm{2 - }}}\)
  4. \({\rm{PC}}{{\rm{l}}_{\rm{3}}}\)
  5. \({\rm{Se}}{{\rm{F}}_{\rm{4}}}\)
  6. \({\rm{P}}{{\rm{H}}_{\rm{2}}}^{\rm{ - }}\)
  7. \({\rm{Xe}}{{\rm{F}}_{\rm{2}}}\)

Predict the charge on the monatomic ions formed from the following atoms in binary ionic compounds: (a) \({\rm{I}}\) (b) \({\rm{Sr}}\) (c) \({\rm{K}}\) (d) \({\rm{N}}\) (e) \({\rm{S}}\) (f) \({\rm{In}}\).

Write the electron configuration for the monatomic ions formed from the following elements (which form the greatest concentration of monatomic ions in seawater): (a) \({\rm{Cl}}\) (b) \({\rm{Na}}\) (c) \({\rm{Mg}}\)(d) \({\rm{Ca}}\) (e) \({\rm{K}}\) (f) \({\rm{Br}}\) (g) \({\rm{Sr}}\) (h) \({\rm{F}}\).

Which compound in each of the following pairs has the larger lattice energy? Note: \({\rm{B}}{{\rm{a}}^{{\rm{2 + }}}}\) and \({{\rm{K}}^{\rm{ + }}}\) have similar radii; \({{\rm{S}}^{{\rm{2 - }}}}\) and \({\rm{C}}{{\rm{l}}^{\rm{ - }}}\) have similar radii. Explain your choices.

(a) \({{\rm{K}}_{\rm{2}}}{\rm{O}}\) or \({\rm{N}}{{\rm{a}}_{\rm{2}}}{\rm{O}}\)

(b) \({{\rm{K}}_{\rm{2}}}{\rm{S}}\) or \({\rm{BaS}}\)

(c) \({\rm{KCl}}\) or \({\rm{BaS}}\)

(d) \({\rm{BaS}}\) or \({\rm{BaC}}{{\rm{l}}_{\rm{2}}}\)
See all solutions

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