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Concept explainers
(a)
Interpretation:
The shape of
Concept introduction:
Molecular geometry is the 3-D representation of the molecule in a space. The Lewis model is not able to explain the shape of the molecules. In terms of electron density, the bonding electrons as well as lone pair of electrons holds the shape of the molecule.
(b)
Interpretation:
The shape of acetylene,
Concept introduction:
Molecular geometry is the 3-D representation of the molecule in a space. The Lewis model is not able to explain the shape of the molecules. In terms of electron density, the bonding electrons as well as lone pair of electrons holds the shape of the molecule.
(c)
Interpretation:
The shape of
Concept introduction:
Molecular geometry is the 3-D representation of the molecule in a space. The Lewis model is not able to explain the shape of the molecules. In terms of electron density, the bonding electrons as well as lone pair of electrons holds the shape of the molecule.
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Chapter 13 Solutions
Introductory Chemistry: An Active Learning Approach
- Formamide, HC(O)NH2, is prepared at high pressures from carbon monoxide and ammonia, and serves as an industrial solvent (the parentheses around the O indicate that it is bonded only to the carbon atom and that the carbon atom is also bonded to the H and the N atoms). Two resonance forms (one with formal charges) can be written for formamide. Write both resonance structures, and predict the bond angles about the carbon and nitrogen atoms for each resonance form. Are they the same? Describe how the experimental determination of the HNH bond angle could be used to indicate which resonance form is more important.arrow_forward2(a) Provide the Lewis structures for both CH3OH and C2H3Cl. 2(b) What is the largest bond angle among all the bond angles in CH3OH and C2H3Cl? Listthe three atoms making this largest bond angle, and estimate the value of the angle.2(c) What intermolecular forces are present(i) between CH3OH molecules?(ii) between C2H3Cl molecules?arrow_forwardDraw the Lewis structure with lowest formal charges, and determine the charge of each atom in (a) OCS; (b) NO. (C)CN−; (d) ClO−.arrow_forward
- Like several other bonds, carbon-oxygen bonds havelengths and strengths that depend on the bond order. Draw Lewis structures for the following species, and arrange them in order of increasing carbon-oxygen bond length and then by increasing carbon-oxygen bond strength: (a) CO; (b) CO₃²⁻; (c) H₂CO;(d) CH₄O; (e) HCO₃(H attached to O).arrow_forwardThe structural formulas for ethanol, CH3CH2OH, and propene, CH;CH=CH,2, are нн H Н—С—С—0—н H-C-C=C-H нн H H H Ethanol Propene (a) Complete the Lewis structure for each molecule showing all valence electrons. (b) Using the VSEPR model, predict all bond angles in each molecule.arrow_forwardPropylene, C3H6, is a gas that is used to form the importantpolymer called polypropylene. Its Lewis structure is given. (a) What is the total number of valence electrons in the propylenemolecule? (b) How many valence electrons are usedto make σ bonds in the molecule? (c) How many valenceelectrons are used to make π bonds in the molecule? (d) Howmany valence electrons remain in nonbonding pairs in themolecule? (e) What is the hybridization at each carbon atomin the molecule?arrow_forward
- We have just arrived at a bonding description for the formaldehydemolecule. Which of the following statements about themolecule is or are true?(i) Two of the electrons in the molecule are used to make the pbond in the molecule.(ii) Six of the electrons in the molecule are used to make the sbonds in the molecule.(iii) The C¬O bond length in formaldehyde should be shorterthan that in methanol, H3COH.(a) Only one of the statements is true.(b) Statements (i) and (ii) are true.(c) Statements (i) and (iii) are true.(d) Statements (ii) and (iii) are true.(e) All three statements are true.arrow_forwardEthylene, C₂H₄, and tetrafluoroethylene, C₂F₄, are used tomake the polymers polyethylene and polytetrafluoroethylene(Teflon), respectively.(a) Draw the Lewis structures for C₂H₄ and C₂F₄, and give theideal H-C-H and F-C-F bond angles.(b) The actual H-C-H and F-C-F bond angles are 117.4and 112.4, respectively. Explain these deviations.arrow_forwardFrom their Lewis structures, determine the number of sand π bonds in each of the following molecules or ions:(a) CO2; (b) cyanogen,(CN2); (c) formaldehyde, H2CO;(d) formic acid, HCOOH, which has one H and two O atomsattached to C.arrow_forward
- 2.arrow_forwardIn the following compounds, the C atoms form a single ring.Draw a Lewis structure for each compound, identify cases for which resonance exists, and determine the carbon-carbon bondorder(s): (a) C₃H₄; (b) C₃H₆; (c) C₄H₆; (d) C₄H₄; (e) C₆H₆.arrow_forwardOxalic acid, H2C2O4, a poisonous colorless solid, is found in some vegetables such as spinach and rhubarb. It is present in concentrations well below the toxic limit, so you can't use this as a reason to refuse a helping of spinach. The order of atoms in a molecule of oxalic acid is HO2CCO2H. (a) How many unshared pairs of electrons are on each of the carbon atoms? (b) How many unshared pairs of electrons are on each of the oxygen atoms?arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
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