Chemistry by OpenStax (2015-05-04) 1st Edition
ISBN: 9781938168390
Author: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
1 Essential Ideas 2 Atoms, Molecules, And Ions 3 Composition Of Substances And Solutions 4 Stoichiometry Of Chemical Reactions 5 Thermochemistry 6 Electronic Structure And Periodic Properties Of Elements 7 Chemical Bonding And Molecular Geometry 8 Advanced Theories Of Covalent Bonding 9 Gases 10 Liquids And Solids 11 Solutions And Colloids 12 Kinetics 13 Fundamental Equilibrium Concepts 14 Acid-base Equilibria 15 Equilibria Of Other Reaction Classes 16 Thermodynamics 17 Electrochemistry 18 Representative Metals, Metalloids, And Nonmetals 19 Transition Metals And Coordination Chemistry 20 Organic Chemistry 21 Nuclear Chemistry Chapter7: Chemical Bonding And Molecular Geometry
Chapter Questions Section: Chapter Questions
Problem 1E: Does a cation gain protons to form a positive charge or does it lose electrons? Problem 2E: Iron(III) sulfate [Fe2( SO 4)3] is composed of Fe3+ and SO42 ions. Explain why a sample of iron(III)... Problem 3E: Which of the following atoms would be expected to form negative ions in binary ionic compounds and... Problem 4E: Which of the following atoms would be expected to form negative ions in binary ionic compounds and... Problem 5E: Predict the charge on the monatomic ions formed from the following atoms in binary ionic compounds:... Problem 6E: Predict the charge on the monatomic ions formed from the following atoms in binary ionic compounds:... Problem 7E: Write the electron configuration for each of the following ions: (a) As3 (b) I (c) Be2+ (d) Cd2+ (e)... Problem 8E: Write the electron configuration for the monatomic ions formed from the following elements (which... Problem 9E: Write out the full electron configuration for each of the following atoms and for the monatomic ion... Problem 10E: From the labels of several commercial products, prepare a list of six ionic compounds in the... Problem 11E: Why is it incorrect to speak of a molecule of solid NaCl? Problem 12E: What information can you use to predict whether a bond between two atoms is covalent or ionic? Problem 13E: Predict which of the following compounds are ionic and which are covalent, based on the location of... Problem 14E: Explain the difference between a nonpolar covalent bond, a polar covalent bond, and an ionic bond. Problem 15E: From its position in the periodic table, determine which atom in each pair is more electronegative:... Problem 16E: From its position in the periodic table, determine which atom in each pair is more electronegative:... Problem 17E: From their positions in the periodic able, arrange the atoms in each of the following series in... Problem 18E: From their positions in the periodic table, arrange the atoms in each of the following series in... Problem 19E: Which atoms can bond to sulfur so as to produce a positive partial charge on the sulfur atom? Problem 20E: Which is the most polar bond? (a) CC (b) CH (c) NH (d) OH (e) Se-H Problem 21E: Identify the more polar bond in each of the following pairs of bonds: (a) HF or HCl (b) NO or CO... Problem 22E: Which of the following molecules or ions contain polar bonds? (a) O3 (b) S8 (c) O22 (d) NO3 (e) CO2... Problem 23E: Write the Lewis symbols for each of the following ions: (a) As3 (b) I (c) Be2+ (d) O2 (e) Ga3+ (f)... Problem 24E: Many monatomic ions are found in seawater, including the ions formed from the following list of... Problem 25E: Write the Lewis symbols of the ions in each of the following ionic compounds and the Lewis symbols... Problem 26E: Iii (he Lewis structures listed here, M and X represent various elements iii the third period of the... Problem 27E: Write the Lewis structure for the diatomic molecule P2, an unstable form of phosphorus found in high... Problem 28E: Write Lewis structures for the following: (a) H2 (b) HBr (c) PCl3 (d) SF2 (e) H2CCH2 (f) HNNH (g)... Problem 29E: Write Lewis structures for the following: (a) O2 (b) H2CO (c) AsF3 (d) ClNO (e) SiCl4 (f) H3O+ (g)... Problem 30E: Write Lewis structures for the following: (a) ClF3 (b) PCl5 (c) BF3 (d) PF6 Problem 31E: Write Lewis structures for the following: (a) SeF6 (b) XeF4 (c) SeCl3+ Problem 32E: Write Lewis structures for: (a) PO43 (b) ICl4 (c) SO32 (d) HONO Problem 33E: Correct the following statement: The bonds in solid PbCl2 are ionic; the bond in a HCl molecule is... Problem 34E: Write Lewis structures for the following molecules or ions: (a) SbH3 (b) XeF2 (c) Se8 (a cyclic... Problem 35E: Methanol, H3COH, is used as the fuel in some race cars. Ethanol, C2H5OH, is used extensively as... Problem 36E: Many planets in our solar system contain organic chemicals including methane (CH4) and traces of... Problem 37E: Carbon tetrachloride was formerly used in fire extinguishers for electrical fires. It is no longer... Problem 38E: Identify the atoms that correspond to each of the following electron configurations. Then, write the... Problem 39E: The arrangement of atoms in several biologically important molecules is given here. Complete the... Problem 40E: A compound with a molar mass of about 28 g/mol contains 85.7% carbon and 14.3% hydrogen by mass.... Problem 41E: A compound with a molar mass of about 42 g/mol contains 85.7% carbon and 14.3% hydrogen by mass.... Problem 42E: Two arrangements of atoms are possible for a compound with a molar mass of about 45 g/mol that... Problem 43E: How are single, double, and triple bonds similar? How do they differ? Problem 44E: Write resonance forms that describe the distribution of electrons in each of these molecules or... Problem 45E: Write resonance forms that describe the distribution of electrons in each of these molecules or... Problem 46E: Write the resonance forms of ozone, Q3, the component of the upper atmosphere that protects the... Problem 47E: Sodium nitrite, which has been used to preserve bacon and other meats, is an ionic compound. Write... Problem 48E: In terms of the bonds present, explain why acetic acid, CH3CO2H, contains two distinct types of... Problem 49E: Write the Lewis structures for the following, and include resonance structures where appropriate.... Problem 50E: Toothpastes containing sodium hydrogen carbonate (sodium bicarbonate) and hydrogen peroxide are... Problem 51E: Determine the formal charge of each element in the following: (a) HCl (b) CF4 (c) PCl3 (d) PF5 Problem 52E: Determine the formal charge of each element in the following: (a) H3O+ (b) SO42 (c) NH3 (d) O22 (e)... Problem 53E: Calculate the formal charge of chlorine in the molecules Cl2, BeCl2, and ClF5. Problem 54E: 54. Calculate the formal charge of each element in the following compounds and ions: (a) F2CO (b) NO... Problem 55E: Draw all possible resonance structures for each of these compounds. Determine the formal charge on... Problem 56E: Based on formal charge considerations, which of the following would likely be the correct... Problem 57E: Based on formal charge considerations, which of the following would likely be the correct... Problem 58E: Based on formal charge considerations, which of the following would likely be the correct... Problem 59E: Draw the structure of hydroxylamine, H3NO, and assign formal charges; look up the structure. Is the... Problem 60E: Iodine forms a series of fluorides (listed here). Write Lewis structures for each of the four... Problem 61E: Write the Lewis structure and chemical formula of the compound with a molar mass of about 70 g/mol... Problem 62E: Which of the following structures would we expect for nitrous acid? Determine the formal charges: Problem 63E: Sulfuric acid is the industrial chemical produced in greatest quantity worldwide. About 90 billion... Problem 64E: Which bond in each of the following pairs of bonds is the strongest? (a) CCorC=C (b) CNorCN (c)... Problem 65E: Using the bond energies in Table 7.2, determine the approximate enthalpy change for each of the... Problem 66E: Using the bond energies in Table 7.2, determine the approximate enthalpy change for each of the... Problem 67E: When a molecule can form two different structures, the structure with the stronger bonds is usually... Problem 68E: How does the bond energy of HCl(g) differ from the standard enthalpy of formation of HCl(g)? Problem 69E: Using the standard enthalpy of formation data in Appendix G, show how the standard enthalpy of... Problem 70E: Using the standard enthalpy of formation data in Appendix G, calculate the bond energy of the... Problem 71E: Using the standard enthalpy of formation data in Appendix G, determine which bond is stronger: the... Problem 72E: Using the standard enthalpy of formation data in Appendix G. determine which bond is stronger: the... Problem 73E: Complete the following Lewis structure by adding bonds (not atoms), and then indicate the longest... Problem 74E: Use the bond energy to calculate an approximate value of H for the following reaction. Which is the... Problem 75E: Element First Ionization Energy (kJImol) Second Ionization Energy (kiImol) I K 419 3050 Ca 590 1140... Problem 76E: The lattice energy of LiF is 1023 kJ/mol, and the Li—F distance is 200.8 pm. NaF crystallizes in the... Problem 77E: For which of the following substances is the least energy required to convert one mole of the solid... Problem 78E: The reaction of a metal, M, with a halogen, X2, proceeds by an exothermic reaction as indicated by... Problem 79E: The lattice energy of LiF is 1023 kJ/mol, and the LiF distance is 201 pm. MgO crystallizes in the... Problem 80E: Which compound in each of the following pairs has the larger lattice energy? Note: Mg2+ and Li+ have... Problem 81E: Which compound in each of the following pairs has the larger lattice energy? Note: Ba2+ and K+ have... Problem 82E: Which of the following compounds requires the most energy to convert one mole of the solid into... Problem 83E: Which of the following compounds requires the most energy to convert one mole of the solid into... Problem 84E: The lattice energy of KF is 794 kJ/mol, and the interionic distance is 269 pm. The Na—F distance in... Problem 85E: Explain why the HOH molecule is bent, whereas the HBeH molecule is linear. Problem 86E: What feature of a Lewis structure can be used to tell if a molecule’s (or ion’s) electron-pair... Problem 87E: Explain the difference between electron-pair geometry and molecular structure. Problem 88E: Why is the HNH angle in NH3 smaller than the HCH bond angle in CH4? Why is the HNH angle in NH4+... Problem 89E: Explain how a molecule that contains polar bonds can be nonpolar. Problem 90E: As a general rule, MX molecules (where M represents a central atom and X represents terminal atoms;... Problem 91E: Predict the electron pair geometry and the molecular structure of each of the following molecules or... Problem 92E: Identify the electron pair geometry and the molecular structure of each of the following molecules... Problem 93E: What are the electron-pair geometry and the molecular structure of each of the following molecules... Problem 94E: Predict the electron pair geometry and the molecular structure of each of the following ions: (a)... Problem 95E: Identify the electron pair geometry and the molecular structure of each of the following molecules:... Problem 96E: Predict the electron pair geometry and the molecular structure of each of the following: (a) IOF5 (I... Problem 97E: Which of the following molecules and ions contain polar bonds? Which of these molecules and ions... Problem 98E: Which of these molecules and ions contain polar bonds? Which of these molecules and ions have dipole... Problem 99E: Which of the following molecules have dipole moments? (a) CS2 (b) SeS2 (c) CCl2F2 (d) PCl3 (P is the... Problem 100E: Identify the molecules with a dipole moment: (a) SF4 (b) CF4 (c) Cl2CCBr2 (d) CH3Cl (e) H2CO Problem 101E: The molecule XF3 has a dipole moment. Is X boron or phosphorus? Problem 102E: The molecule XCl2 has a dipole moment. Is X beryllium or sulfur? Problem 103E: Is the Cl2BBCl2 molecule polar or nonpolar? Problem 104E: There are three possible structures for PCl2F3 with phosphorus as the central atom. Draw them and... Problem 105E: Describe the molecular structure around the indicated atom or atoms: (a) the sulfur atom in sulfuric... Problem 106E: Draw the Lewis structures and predict the shape of each compound or ion: (a) CO2 (b) NO2 (c) SO3... Problem 107E: A molecule with the formula AB2, in which A and B represent different atoms, could have one of three... Problem 108E: A molecule with the formula AB3, in which A and B represent different atoms, could have one of three... Problem 109E: Draw the Lewis electron dot structures for these molecules, including resonance structures where... Problem 110E: What is the molecular structure of the stable form of FNO2? (N is the central atom.) Problem 111E: A compound with a molar mass of about 42 g/mol contains 85.7% carbon and 14.3% hydrogen. What is its... Problem 112E: Use the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises... Problem 113E: Use the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises... Problem 114E: Use the Molecule Shape simulator (http://openstaxcollege.org/I/6MolecShape) to build a molecule.... Problem 115E: Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to explore real... Problem 116E: Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to explore real... Problem 115E: Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to explore real...
Related questions
Draw the structural formula of the ketone or carboxylic acid product when each of the following is oxidized
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Definition Definition Organic compounds that have a carbonyl group, C = O, as their functional group. The carbonyl group in ketones is placed somewhere in the middle of the molecular structure, which means, the C=O is attached to two alkyl groups or benzene rings. Just like all other homologous series, the naming of ketones is done using a common suffix “-one”. The general molecular formula is C n H 2n O. Functional group of a ketone
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