Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Textbook Question
Chapter 8, Problem 38PS
Draw the resonance structures for the formate ion, HCO2−, and find the formal charge on each atom. If an H+ ion is attached to HCO2− (to form formic acid), does it attach to C or O?
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Consider the Lewis structure for CO. Which statement best explains which
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Chapter 8 Solutions
Chemistry & Chemical Reactivity
Ch. 8.2 - Draw Lewis electron dot structures for CH3Cl...Ch. 8.2 - Prob. 2CYUCh. 8.2 - Prob. 3CYUCh. 8.2 - Prob. 4CYUCh. 8.2 - Prob. 1RCCh. 8.2 - 2. Which one of the species in the list below is...Ch. 8.2 - Prob. 3RCCh. 8.2 - Prob. 4RCCh. 8.3 - Prob. 1CYUCh. 8.3 - 1. What is the formal charge of the P atom in the...
Ch. 8.4 - Draw resonance structures for the bicarbonate ion,...Ch. 8.4 - 1. For which of the following species, SO32−, NO+,...Ch. 8.4 - Prob. 2RCCh. 8.5 - Sketch the Lewis structures for CIF2+ and CIF2....Ch. 8.5 - Prob. 1QCh. 8.5 - Prob. 2QCh. 8.5 - Prob. 1RCCh. 8.5 - Prob. 2RCCh. 8.6 - What is the shape of the dichloromethane (CH2C12)...Ch. 8.6 - Give the electron-pair geometry and molecular...Ch. 8.6 - Draw the Lewis structure for lCl2, and then decide...Ch. 8.6 - Prob. 4CYUCh. 8.6 - Which of the following species has...Ch. 8.6 - Prob. 2RCCh. 8.6 - What is the approximate ClCCl bond angle in...Ch. 8.6 - 4. What is the molecular geometry of N2O (where...Ch. 8.7 - Draw the resonance structures for SCN. What are...Ch. 8.7 - For each of the following molecules, decide...Ch. 8.7 - Prob. 1RCCh. 8.7 - 2. Which of the following best describes the...Ch. 8.7 - Three resonance forms can be drawn for the...Ch. 8.8 - The electrostatic potential surface for SOCl2 is...Ch. 8.8 - Using the bond dissociation enthalpies in Table...Ch. 8.8 - Prob. 1RCCh. 8.8 - Prob. 2RCCh. 8.9 - 1. Which of the following species has the longest...Ch. 8.9 - 2. Which of the following species has the largest...Ch. 8.9 - 3. Use bond dissociation enthalpies to estimate...Ch. 8 - Give the periodic group number and number of...Ch. 8 - Give the periodic group number and number of...Ch. 8 - For elements in Groups 4A-7A of the periodic...Ch. 8 - Prob. 4PSCh. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Show all possible resonance structures for each of...Ch. 8 - Show all possible resonance structures for each of...Ch. 8 - Prob. 11PSCh. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Determine the formal charge on each atom in the...Ch. 8 - Determine the formal charge on each atom in the...Ch. 8 - Determine the formal charge on each atom in the...Ch. 8 - Determine the formal charge on each atom in the...Ch. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Prob. 18PSCh. 8 - Prob. 19PSCh. 8 - The following molecules or ions all have three...Ch. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Give approximate values for the indicated bond...Ch. 8 - Give approximate values for the indicated bond...Ch. 8 - Phenylalanine is one of the natural amino acids...Ch. 8 - Acetylacetone has the structure shown here....Ch. 8 - For each pair of bonds, indicate the more polar...Ch. 8 - For each of the bonds listed below, tell which...Ch. 8 - Urea, (NH2)2CO, is used in plastics and...Ch. 8 - Considering both formal charges and bond...Ch. 8 - Considering both formal charge and bond...Ch. 8 - Three resonance structures are possible for...Ch. 8 - Three resonance structures are possible for the...Ch. 8 - Compare the electron dot structures of the...Ch. 8 - Compare the electron dot structures of the...Ch. 8 - The chemistry of the nitrite ion and HNO2: (a) Two...Ch. 8 - Draw the resonance structures for the formate ion,...Ch. 8 - Prob. 39PSCh. 8 - Consider the following molecules: (a) CH4 (b)...Ch. 8 - Which of the following molecules is(are) polar?...Ch. 8 - Prob. 42PSCh. 8 - Give the bond order for each bond in the following...Ch. 8 - Prob. 44PSCh. 8 - In each pair of bonds, predict which is shorter....Ch. 8 - In each pair of bonds, predict which is shorter....Ch. 8 - Prob. 47PSCh. 8 - Compare the carbon-oxygen bond lengths in the...Ch. 8 - Consider the carbon-oxygen bond in formaldehyde...Ch. 8 - Compare the nitrogen-nitrogen bond in hydrazine,...Ch. 8 - Ethanol can be made by the reaction of ethylene...Ch. 8 - Methanol can be made by partial oxidation of...Ch. 8 - Hydrogenation reactions, which involve the...Ch. 8 - Phosgene, Cl2CO, is a highly toxic gas that was...Ch. 8 - The compound oxygen difluoride is quite reactive,...Ch. 8 - Oxygen atoms can combine with ozone to form...Ch. 8 - Prob. 57GQCh. 8 - Prob. 58GQCh. 8 - Which of the following compounds or ions do not...Ch. 8 - Prob. 60GQCh. 8 - Draw resonance structures for the formate ion,...Ch. 8 - Prob. 62GQCh. 8 - Prob. 63GQCh. 8 - What is the principle of electroneutrality? Use...Ch. 8 - Prob. 65GQCh. 8 - Draw resonance structures for the SO2 molecule,...Ch. 8 - What are the orders of the NO bonds in NO2 and...Ch. 8 - Which has the greater ONO bond angle, NO2 or NO2+?...Ch. 8 - Compare the FClF angles in CIF2+ and ClF2. Using...Ch. 8 - Draw an electron dot structure for the cyanide...Ch. 8 - Draw the electron dot structure for the sulfite...Ch. 8 - Dinitrogen monoxide, N2O, can decompose to...Ch. 8 - The equation for the combustion of gaseous...Ch. 8 - The cyanate ion, OCN, has the least...Ch. 8 - Vanillin is the flavoring agent in vanilla extract...Ch. 8 - Explain why (a) XeF2 has a linear molecular...Ch. 8 - The formula for nitryl chloride is ClNO2 (in which...Ch. 8 - Hydroxyproline is a less-common amino acid. (a)...Ch. 8 - Amides are an important class of organic...Ch. 8 - Prob. 81GQCh. 8 - The molecule shown here. 2-furylmelhanethiol, is...Ch. 8 - Dihydroxyacetone is a component of quick-tanning...Ch. 8 - It is possible to draw three resonance structures...Ch. 8 - Acrolein is used to make plastics. Suppose this...Ch. 8 - Molecules in space: (a) In addition to molecules...Ch. 8 - 1,2-Dichloroethylene can be synthesized by adding...Ch. 8 - The molecule pictured below is epinephrine, a...Ch. 8 - You are doing an experiment in the laboratory and...Ch. 8 - Prob. 90ILCh. 8 - A paper published in the research Journal Science...Ch. 8 - Uracil is one of the bases in RNA, a close...Ch. 8 - Prob. 93SCQCh. 8 - Prob. 94SCQCh. 8 - Bromine-containing species play a role in...Ch. 8 - Acrylamide, H2C=CHCONH2, is a known neurotoxin and...
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- Consider 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_forwardThe n-propyl cation can be formed from a molecule such as When the C–Cl bond is broken so that both electrons leave with Cl, the fragments formed are The carbon atom that had been attached to Cl is now sharing ____ electron pairs. In each shared pair the carbon atom owns ____ electron. The number of electrons that belong to carbon is ____. The formal charge on the carbon atom is ____. The correct Lewis structure for the n-propyl cation isarrow_forwardConsider the formate ion, HCO2-, which is the anion formed when formic acid lose an H+ ion. The H and the two O atoms are bonded to the central C atom. a) Draw the best Lewis structure for this ion. b) Are resonance structures needed to describe this structure? c) Would you predict that the C-O bond lengths in the formate ion would be longer or shorter relative to those in CO2?arrow_forward
- Draw two different Lewis structures for ClO3-, one which all atoms follow the octet rule and one where the chlorine has an expanded octet. Determine the formal charge on all atoms for each structure. Which do you think is the better Lewis structure? Explain your reasoning.arrow_forward1 ) Draw the Lewis dot structure for RbIO2RbIO2. Include all hydrogen atoms and nonbonding electrons. Show the formal charges of all atoms. To change the symbol of an atom, double-click on the atom and enter the letter of the new atom. b ) Draw the Lewis dot structure for NH4ClNH4Cl. Include all hydrogen atoms and nonbonding electrons. Show the formal charges of all atoms. To change the symbol of an atom, double-click on the atom and enter the letter of the new atom. c) Draw the Lewis dot structure for KOHKOH. Include all hydrogen atoms and nonbonding electrons. Show the formal charges of all atoms. To change the symbol of an atom, double-click on the atom and enter the letter of the new atom. d) Draw the Lewis dot structure for Sr(CN)2Sr(CN)2. Include all hydrogen atoms and nonbonding electrons. Show the formal charges of all atoms. To change the symbol of an atom, double-click on the atom and enter the letter of the new atom. e)arrow_forward-draw the possible resonance structures of IO3^2- ion. -the experimental bond length of P and O bond in PO4^3- ion is in between the bond lengths of P=O and P-O.what is the reason behind this?. -draw the possible resonance structures of C3h3^- ion and on each sructure assign formal charge on each atom.arrow_forward
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- What are the formal charges present in in the ion CH3NH3*? Assume all atoms other an hydrogen hau an octet and that there are two central atoms. O N is 0 and C is +1 O N is +1 and C is -1 O N is +1 and C is 0 O N is 0 and C is 0 O N is +2 and C is -1arrow_forward10.) The structural formula of a certain aldehyde (related to formaldehyde) is H3C-CH2-CHO. Draw a Lewis structure for this aldehyde and determine the number of bonds present. Note that a single or a double or a triple bond counts as one bond. Write the number, not the word.arrow_forwardHow many resonance structures can be drawn for the hydrogen tellurate ion (HTeO4–) in which the central tellurium atom bears a –1 formal charge and the oxygens bear formal charges of either zero or –1? Enter your answer as a whole number.arrow_forward
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