7.3: Electron Configuration of Atoms
- Page ID
- 169580
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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
Exercise \(\PageIndex{1}\)
Which of the following elements is found in the d-block of the periodic table?
- Ir
- Tb
- Li
- Cl
- None of these
- Answer
-
a Ir
Exercise \(\PageIndex{2}\)
An element that has the same ground state valence-shell electron configuration as thallium is
a. gallium b. carbon c. krypton d. cesium e. magnesium
- Answer
-
a. gallium
Exercise \(\PageIndex{3}\)
How many valence electrons does an arsenic atom have?
a. 5 b. 8 c. 7 d. 2 e. 33
- Answer
-
a. 5
Exercise \(\PageIndex{4}\)
How many unpaired electrons are found in the ground state electron configuration of Barium (Ba)?
a. 0 b. 1 c. 2 d. 3 e. 5
- Answer
-
a. 0
Exercise \(\PageIndex{5}\)
Which of the following orbital diagrams represents a paramagnetic atom?
1s 2s 2p
a. 1 only b. 2 only c. 3 only d. 1 and 2 e. 2 and 3
- Answer
-
e. 2 and 3
Exercise \(\PageIndex{6}\)
Which of the following atoms is diamagnetic in its ground state?
- Mercury (Hg)
- Tin (Sn)
- Rhenium (Re)
- Berkelium (Bk)
- Phosphorus (P)
- Answer
-
a. Mercury (Hg)
Exercise \(\PageIndex{7}\)
Which of the following orbital diagrams represents a diamagnetic atom?
1s 2s 2p
- Answer
-
a.
Exercise \(\PageIndex{8}\)
Which atom has the ground state electronic configuration 1s22s22p63s23p64s23d3?
a. Ga b. V c. As d. Nb e. none
- Answer
-
b. V
Exercise \(\PageIndex{9}\)
Which of the following elements has the ground state electron configuration [Ar]3d104s1?
a. Cu b. Zn c. Ge d. Ag e. Cd
- Answer
-
a. Cu
Exercise \(\PageIndex{10}\)
What is the ground-state electron configuration of sulfur (S)?
a. [Ne]3s33sp3 b. [Ar]3s23p4 c. [Ar]3p6 d. [Ne]3s23p4 e. [Ar]3p6
- Answer
-
d. [Ne]3s23p4
Exercise \(\PageIndex{11}\)
Which of the following electron configurations corresponds to the ground state of an atom of a transition element?
- 1s22s22p1
- 1s22s22p63s23p63d104s24p3
- 1s22s22p63s23p63d14s2
- 1s22s22p63s23p64s1
- 1s22s22p63s23p4
- Answer
-
c. 1s22s22p63s23p63d14s2
Exercise \(\PageIndex{12}\)
The complete electron configuration of tin is _____.
- 1s22s22p63s23p64s23d104p65s24d105p2
- 1s22s22p63s23p64s23d104p65s24d105p2
- 1s22s22p63s23p64s23d104d104p2
- 1s22s22p63s23p64s23d104p65s24d105d105p2
- None of these
- Answer
-
a. 1s22s22p63s23p64s23d104p65s24d105p2
Exercise \(\PageIndex{13}\)
Hund's rule states that the most stable arrangement of electrons (for a ground state electron configuration)
- has a filled valence shell of electrons.
- has three electrons per orbital, each with identical spins.
-
has values greater than or equal to +1.
-
has the maximum number of unpaired electrons, all with the same spin.
-
has two electrons per orbital, each with opposing spins.
- Answer
-
d. has the maximum number of unpaired electrons, all with the same spin.
Exercise \(\PageIndex{14}\)
All of the following ground-state electron configurations are correct except
- V: [Ar]4s24d3
- K: [Ar]4s1
- Sb: [Kr]4d105s25p3
- Cr: [Ar]3d54s1
- Te: [Kr]4d105s25p4
- Answer
-
a. V: [Ar]4s24d3
Exercise \(\PageIndex{15}\)
What noble gas core precedes the valence shell ground state electron configuration for potassium (K)?
a. [Ar] b. [Rn] c. [Kr] d. [Ne] e. [Xe]
- Answer
-
a. [Ar]
Exercise \(\PageIndex{16}\)
Which ground-state electron configuration is incorrect?
- Br: [Ar]3d104s24p5
- K: [Ar]4s1
- Ni: [Ar]3d5
- Mg: 1s22s22p63s2
- Co: [Ar]3d74s2
- Answer
-
c. Ni: [Ar]3d5
Exercise \(\PageIndex{17}\)
Which element has the following ground state electron configuration?
a. Be b. O c. Li d. Si e. N
- Answer
-
e. N
Exercise \(\PageIndex{18}\)
Which element has the following ground state electron configuration?
3d 4s
[Ar]
a. Sc b. Ni c. Co d. Fe e. V
- Answer
-
a. Sc
Exercise \(\PageIndex{19}\)
Which element has the following ground state electron configuration?
a. In b. Y c. Nb d. Tl e. Ga
- Answer
-
a. In
Exercise \(\PageIndex{20}\)
Which is the correct valence shell orbital box notation for the ground state electron configuration of Fe?
3d 4s
- Answer
-
a.
Exercise \(\PageIndex{21}\)
What is a possible set of quantum numbers for an unpaired electron in the orbital box diagram below?
- n = 1, l = 1, = –1, ms = \(+\frac{1}{2}\)
- n = 4, l = 2, = –1, ms = \(-1\frac{1}{2}\)
- n = 5, l = 2, = –2, ms = \(+\frac{1}{2}\)
- n = 5, l = 0, = 0, ms = \(-1\frac{1}{2}\)
- n = 5, l = 1, = –1, ms = \(+\frac{1}{2}\)
- Answer
-
e. n = 5, l = 1, = –1, ms = \(+\frac{1}{2}\)