Inorganic Chemistry
5th Edition
ISBN: 9781292134147
Author: Housecroft, Catherine E.
Publisher: Pearson,
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Textbook Question
Chapter 2, Problem 12P
Draw charge-separated resonance structures to give a representation of the bonding in
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Students have asked these similar questions
Draw regular Lewis structures (no need to use dashed lines and wedges) for each of the following molecules
and indicate which exception, if any, to the octet rule is found in each of them: SCI6, CH3, XeF4, BBR3.
Complete the following Lewis structures for the HONS molecule by adding dots for unshared
valence electrons and indicating formal charges. Evaluate the importance of each structure as a
contributor to a resonance hybrid.
H – 0 – N = S, H–0 = N – S
Write resonance forms that describe the distribution of electrons in each of these molecules or ions.
a) nitric acid, HNO3 (N is bonded to an OH group and two O atoms)
b) benzene, C6H6:
c)the formate ion:
Chapter 2 Solutions
Inorganic Chemistry
Ch. 2 - Draw Lewis structures to describe the bonding in...Ch. 2 - Use the Lewis structure model to deduce the type...Ch. 2 - Draw the resonance structures for the O3 molecule....Ch. 2 - 2.4 Draw Lewis structures for (a) , (b) ,(c) and...Ch. 2 - 2.5 Each of the following is a radical. For which...Ch. 2 - (a) Use VB theory to describe the bonding in the...Ch. 2 - 2.7 Use VB theory and Lewis structure model,...Ch. 2 - 2.8 Does VB theory indicate that the diatomic...Ch. 2 - 2.9 (a) Use MO theory to determine the bond order...Ch. 2 - Prob. 10P
Ch. 2 - Prob. 11PCh. 2 - Draw charge-separated resonance structures to give...Ch. 2 - Prob. 13PCh. 2 - In the following table, match a species in list 1...Ch. 2 - Using the data in table 2.2, determine which of...Ch. 2 - Prob. 16PCh. 2 - 2.17 Use the VSEPR model to predict the structures...Ch. 2 - 2.18 Use the VSEPR model to rationalize the...Ch. 2 - Determine the shapes of each of the following...Ch. 2 - 2.20 State whether you expect the following...Ch. 2 - 2.21 (a) Draw resonance structure for the CO,...Ch. 2 - Prob. 22PCh. 2 - Prob. 23PCh. 2 - Suggest reasons for the following observations....Ch. 2 - Prob. 25PCh. 2 - Prob. 26PCh. 2 - 2.27 (a) Write down the ions that are present in...Ch. 2 - 2.28 Assuming that VSEPR model can be applied...Ch. 2 - Critically compare the VB and MO treatments of the...Ch. 2 - The table below gives the average composition of...Ch. 2 - Carbon monoxide is a toxic pollutant which arises...Ch. 2 - 2.32 Volcanoes and deep sea hydrothermal vents are...
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- Write all resonance structures of chlorobenzene, C6H5Cl, a molecule with the same cyclic structure as benzene. In all structures, keep the CCl bond as a single bond. Which resonance structures are the most important?arrow_forwardConsider the pyrosulfate ion, S2O72-. It has no sulfur–sulfur nor oxygen–oxygen bonds. (a) Write a Lewis structure for the pyrosulfate ion using only single bonds. (b) What is the formal charge on the sulfur atoms for the Lewis structure you drew in part (a)? (c) Write another Lewis structure using six bonds and two O—S bonds. (d) What is the formal charge on each atom for the structure you drew in part (c)?arrow_forwardUsing the bond dissociation enthalpies in Table 8.8, estimate the enthalpy of combustion of gaseous methane, CH4, to give water vapor and carbon dioxide gas.arrow_forward
- The study of carbon-containing compounds and their properties is called organic chemistry. Besides carbon atoms, organic compounds also can contain hydrogen, oxygen, and nitrogen atoms (as well as other types of atoms). A common trait of simple organic compounds is to have Lewis structures where all atoms have a formal charge of zero. Consider the following incomplete Lewis structure for an organic compound called histidine (an amino acid), which is one of the building blocks of proteins found in our bodies: Draw a complete Lewis structure for histidine in which all atoms have a formal charge of zero.arrow_forwardWrite reasonable Lewis structures for the following species, none of which follow the octet rule. (a) BF3 (b) NO (c) CO+ (d) ClO3arrow_forwardBond Enthalpy When atoms of the hypothetical element X are placed together, they rapidly undergo reaction to form the X2 molecule: X(g)+X(g)X2(g) a Would you predict that this reaction is exothermic or endothermic? Explain. b Is the bond enthalpy of X2 a positive or a negative quantity? Why? c Suppose H for the reaction is 500 kJ/mol. Estimate the bond enthalpy of the X2 molecule. d Another hypothetical molecular compound, Y2(g), has a bond enthalpy of 750 kJ/mol, and the molecular compound XY(g) has a bond enthalpy of 1500 kJ/mol. Using bond enthalpy information, calculate H for the following reaction. X2(g)+Y2(g)2XY(g) e Given the following information, as well as the information previously presented, predict whether or not the hypothetical ionic compound AX is likely to form. In this compound, A forms the A+ cation, and X forms the X anion. Be sure to justify your answer. Reaction: A(g)+12X2(g)AX(s)The first ionization energy of A(g) is 400 kJ/mol. The electron affinity of X(g) is 525 kJ/mol. The lattice energy of AX(s) is 100 kJ/mol. f If you predicted that no ionic compound would form from the reaction in Part e, what minimum amount of AX(s) lattice energy might lead to compound formation?arrow_forward
- A 0.167-g sample of an unknown acid requires 27.8 mL of 0.100 M NaOH to titrate to the equivalence point. Elemental analysis of the acid gives the following percentages by mass: 40.00% C, 6.71% H, 53.29% O. Determine the molecular formula, molar mass, and Lewis structure of the unknown acid.arrow_forwardDraw two electron-dot resonance structures that obey the octet rule for trichloronitromethane, CCl3NO2, and show the formal charges on N and O in both structures. (Carbon is connected to the chlorines and to nitrogen; nitrogen is also connected to both oxygens.)arrow_forward
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