1.16: Additional Exercises
- Page ID
- 122434
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)Bond Formation: The Octet Rule
1-1 Identify the number of valence electrons for each of the following elements. Then, identify the maximum number of covalent bonds it can form with other atoms while keeping a neutral net charge.
a) Oxygen
b) Carbon
c) Chlorine
d) Sulfur
e) Hydrogen
f) Boron
1-2 Which of the following atoms can bond with Br - to satisfy the octet rule?
a) Mg+2
b) O-2
c) Cl-
d) K+
1-3 Draw the Lewis dot structure of the correct answer from the previous problem 1-2 (a) - (d).
1-4 Identify which of the following compounds could not form due to an unfilled octet.
a) NCl3
b) NaOH
c) PCl
d) CF4
Lewis Structures
1-5 Draw the Lewis structures for the following compounds.
a) H2O
b) O3
c) BH3
d) SOCl2
1-6 Name the element that corresponds to each electronic configuration and identify how many valence electrons it has.
a) 1s22s22p6
b) 1s22s22p63s2
c) 1s22s22p4
d) 1s22s22p63s23p64s23d104p5
1-7 Draw the Lewis structures for PF3 and PF5.
1-8 Draw the Lewis structure for furan.
1-9 Identify the correct Lewis structure for hydroperoxyl, HO2.
Electronegativity and Bond Polarity
1-10 For the indicated bond in each of the following compounds, identify which atom is more electronegative, if applicable.
1-11 For each of the compounds in the previous problem, add a dipole moment arrow.
Formal Charges
1-12 For the following compounds, draw the structural formula. Then calculate the formal charge on each atom other than hydrogen.
a) N(CH3)4+
b) HSO4-
c) CH3CC-
1-13 Identify the formal charge for the following compounds.
1-14 Identify the formal charges for the central carbon in each of the following compounds.
Ionic Structures
1-15 Identify the substituent ions that make up the following salts.
a) NaCl
b) MgBr2
c) KNO3
d) NaH2PO4
1-16 Identify the products of the following reactions.
1-17 Give the correct nomenclature or write the correct chemical formula for the following ionic compounds.
a) NaCN
b) calcium oxalate
c) Al(OH)3
d) tin (II) phosphate
e) potassium hypochlorite
Resonance
1-18 For the following structure, draw its resonance structure(s).
1-19 Which resonance form from the previous problem has the most stable carbocation? Explain your answer.
1-20 Draw the important resonance forms to show the delocalization of charges in the following compounds.
1-21 Explain how resonance contributes to the lower pKa of acetic acid CH3CO2H (pKa= 4.75) compared to the pKa of ethanol CH3CH2OH (pKa=15.9).
1-22 Draw the resonance structure(s) for fulminic acid (HCNO).
Structural, Molecular and Empirical Formulas
1-23 Identify the molecular and empirical formula for the following structures.
1-24 Draw all possible structural formulas for the following compounds.
a) C4H10
b) CHN
c) C4H9Cl
1-25 True or False: You can always calculate the exact molecular weight of a molecule from its empirical formula.
1-26 For the following molecular formulas, provide the empirical formula.
a) C4H4O2
b) C8H6N2
c) C9H21N3O3
Acids and Bases - Arrhenius, Bronsted-Lowry, and Lewis
1-27 Briefly explain the three different definitions of acids and bases.
1-28 Calculate the Ka of nitric acid (HNO3). pKa of nitric acid is -1.4.
1-29 Rank the following in order of decreasing acidity: NH4+ HF H3O+ H2O
1-30 Rank the following in order of decreasing basicity: HSO4- H2O CH3COO- NH2-
1-31 Identify which compound is the stronger base. Identify which compound is the stronger acid.
1.32 Identify which group is more likely to grab a H+.