7.4: Electron Configuration of Ions
- Page ID
- 169581
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)Electron Configuration of Ions
Exercise \(\PageIndex{1}\)
For which of the following atoms is the 2+ ion diamagnetic in the ground state?
a. Ni b. Fe c. Zn d. Mn e. Cu
- Answer
-
c. Zn
Exercise \(\PageIndex{2}\)
Which of the following elements in its 1+ ionic state has the ground state electron configuration [Kr]4d10?
a. Ru b. Au c. Ag d. In e. Cd
- Answer
-
c. Ag
Exercise \(\PageIndex{3}\)
If the ground state electron configuration of an element is [Ar]3d104s24p5, what is the typical charge on the monatomic anion of the element?
a. 4+ b. 2+ c. 1- d. 2- e. 3-
- Answer
-
c. 1-
Exercise \(\PageIndex{4}\)
What is the ground state electron configuration for Cr3+?
- [Ar]
- [Ar]3d74s2
- [Ar]3d14s2
- [Ar]3d24s1
- [Ar]3d3
- Answer
-
e. [Ar]3d3
Exercise \(\PageIndex{5}\)
What is the ground state electron configuration for Sn2+?
- [Kr]4d105s2
- [Kr]4d105p2
- [Kr]5s2
- [Kr]4d105s25p2
- [Kr]4d105s25p4
- Answer
-
a. [Kr]4d105s2
Exercise \(\PageIndex{6}\)
Which of the given ions have the same ground state electron configuration: S2–, N3–, Mg2+, and Br–?
- N3– and Mg2+
- S2–, N3–, and Br–
- S2– and Br–
- Mg2+ and Br–
- S2–, N3–, Mg2+, and Br–
- Answer
-
a. N3– and Mg2+
Exercise \(\PageIndex{7}\)
Which of the following has the same (total) number of electrons as Ar?
a. Na+ b. Ca2+ c. Ga3+ d. O2- e. none
- Answer
-
b. Ca2+
Exercise \(\PageIndex{8}\)
What is the ground-state electron configuration of the chloride ion?
- 1s22s22p6
- 1s22s22p63s23p2
- 1s22s22p63s23p6
- 1s22s22p63s2
- 1s22s22p63s23p4
- Answer
-
Add texts here. Do not delete this text first.
Exercise \(\PageIndex{9}\)
What 2– ion has the following ground state electron configuration?
- Oxide ion
- Nitride ion
- Fluoride ion
- Sulfide Ion
- Magnesium Ion
- Answer
-
d. Sulfide Ion
Exercise \(\PageIndex{10}\)
What 2+ ion has the following ground state electron configuration?
a. Mn2+ b. Co2+ c. Ni2+ d. Cu2+ e. Ge2+
- Answer
-
b. Co2+
Exercise \(\PageIndex{11}\)
Which of the following ions has the given ground state electron configuration?
a. Cd2+ b. Sr2+ c. Zn2+ d.Sn2+ None of these
- Answer
-
d. Sn2+
Exercise \(\PageIndex{12}\)
The ground-state electron configuration of a Ni2+ ion is 1s22s22p63s23p63d8 . Therefore, Ni2+ is
- paramagnetic with two unpaired electrons.
- diamagnetic.
- paramagnetic with one unpaired electron.
- paramagnetic with four unpaired electrons.
- paramagnetic with five unpaired electrons.
- Answer
-
a. paramagnetic with two unpaired electrons.
Exercise \(\PageIndex{13}\)
Which of the following cations has the same number of unpaired electrons as Fe2+?
a. Ni2+ b. Fe3+ c. Cr2+ d. Mn2+ e. Co2+
- Answer
-
c. Cr2+