3.3.0.0: Bond Types (Problems)
- Page ID
- 210701
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)PROBLEM \(\PageIndex{1}\)
Does a cation gain protons to form a positive charge or does it lose electrons?
- Answer
-
The protons in the nucleus do not change during normal chemical reactions. Only the outer electrons move. Positive charges form when electrons are lost.
PROBLEM \(\PageIndex{2}\)
Iron(III) sulfate [Fe2(SO4)3] is composed of Fe3+ and \(\ce{SO4^2-}\) ions. Explain why a sample of iron(III) sulfate is uncharged.
- Answer
-
Two cations with a +3 charge give a total of +6 charge, while three anions of -2 charge give a total of -6 charge. +6-6=0, so when these ions bond, the charges will cancel, leaving the resulting compound uncharged.
PROBLEM \(\PageIndex{3}\)
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: P, I, Mg, Cl, In, Cs, O, Pb, Co?
- Answer
-
P, I, Cl, and O would form anions because they are nonmetals. Mg, In, Cs, Pb, and Co would form cations because they are metals.
PROBLEM \(\PageIndex{4}\)
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: Br, Ca, Na, N, F, Al, Sn, S, Cd?
- Answer
-
Anions: Br, N, F, S,
Cations: Ca, Na, Al, Sn (because it's a metal), Cd (because it is a metal)
PROBLEM \(\PageIndex{5}\)
Predict the charge on the monatomic ions formed from the following atoms in binary ionic compounds:
- P
- Mg
- Al
- O
- Cl
- Cs
- Answer a
-
P3–
- Answer b
-
Mg2+
- Answer c
-
Al3+
- Answer d
-
O2–
- Answer e
-
Cl–
- Answer f
-
Cs+
PROBLEM \(\PageIndex{6}\)
Predict the charge on the monatomic ions formed from the following atoms in binary ionic compounds:
a. I
b. Sr
c. K
d. N
e. S
f. In
- Answer a
-
I-
- Answer b
-
Sr2+
- Answer c
-
K+
- Answer d
-
N3-
- Answer e
-
S2-
- Answer f
-
In3+
PROBLEM \(\PageIndex{7}\)
Write the noble gas electron configuration for each of the following ions:
a. As3–
b. I–
c. Be2+
d. Cd2+
e. O2–
f. Ga3+
g. Li+
h. N3–
i. Sn2+
j. Co2+
k. Fe2+
l. As3+
- Answer a
-
[Ar]4s23d104p6
- Answer b
-
[Kr]4d105s25p6
- Answer c
-
1s2
- Answer d
-
[Kr]4d10
- Answer e
-
[He]2s22p6
- Answer f
-
[Ar]3d10
- Answer g
-
1s2
- Answer h
-
[He]2s22p6
- Answer i
-
[Kr]4d105s2
- Answer j
-
[Ar]3d7
- Answer k
-
[Ar]3d6
- Answer l
-
[Ar]3d104s2
PROBLEM \(\PageIndex{8}\)
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:
- Al
- Br
- Sr
- Li
- As
- S
- Answer a
-
Al: 1s22s22p63s23p1
Al3+: 1s22s22p6
- Answer b
-
Br: 1s22s22p63s23p63d104s24p5
Br-: 1s22s22p63s23p63d104s24p6
- Answer c
-
Sr: 1s22s22p63s23p63d104s24p65s2
Sr2+: 1s22s22p63s23p63d104s24p6
- Answer d
-
Li: 1s22s1
Li+: 1s2
- Answer e
-
As: 1s22s22p63s23p63d104s24p3
As3-: 1s22s22p63s23p63d104s24p6
- Answer f
-
S: 1s22s22p63s23p4
S2-: 1s22s22p63s23p6
PROBLEM \(\PageIndex{9}\)
What information can you use to predict whether a bond between two atoms is covalent or ionic?
- Answer
-
The position of the two atoms on the periodic table: two nonmetals form a covalent bond, while a metal and a nonmetal form an ionic bond.
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Contributors and Attributions
Paul Flowers (University of North Carolina - Pembroke), Klaus Theopold (University of Delaware) and Richard Langley (Stephen F. Austin State University) with contributing authors. Textbook content produced by OpenStax College is licensed under a Creative Commons Attribution License 4.0 license. Download for free at http://cnx.org/contents/85abf193-2bd...a7ac8df6@9.110).
- Adelaide Clark, Oregon Institute of Technology
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