1 Introduction To Chemistry 2 Atoms And Molecules 3 Molecules, Moles, And Chemical Equations 4 Stoichiometry 5 Gases 6 The Periodic Table And Atomic Structure 7 Chemical Bonding And Molecular Structure 8 Molecules And Materials 9 Energy And Chemistry 10 Entropy And The Second Law Of Thermodynamics 11 Chemical Kinetics 12 Chemical Equilibrium 13 Electrochemistry 14 Nuclear Chemistry Chapter7: Chemical Bonding And Molecular Structure
Chapter Questions Section: Chapter Questions
Problem 1CO: List some factors influencing the biocompatibility of materials and explain how those factors are... Problem 2CO: • use electron configurations to explain why metals tend to form cations whereas nonmetals tend to... Problem 3CO: • describe die energy changes in the formation of an ionic bond. Problem 4CO: • define electronegativity and state how electronegativity varies with position in the periodic... Problem 5CO: • identify or predict polar, nonpolar, and ionic bonds by comparing electronegativities. Problem 6CO: • write Lewis electron structures for molecules or ions. Problem 7CO: • describe chemical bonding using a model based on the overlap of atomic orbitals and recognize... Problem 8CO: • explain how hybridization reconciles observed molecular shapes with the orbital overlap model. Problem 9CO: • predict the geometry of a molecule from its, Lewis structure. Problem 10CO: • use models (real or software) to help visualize common molecular shapes. Problem 11CO: • explain the formation of multiple bonds in terms of the overlap of a combination of hybridized and... Problem 12CO: • identify sigma and pi bonds in a molecule and explain the difference between them. Problem 7.1PAE: Define the term biocompatibility. Problem 7.2PAE: List some properties associated with biomaterials used for joint replacements. Problem 7.3PAE Problem 7.4PAE Problem 7.5PAE Problem 7.6PAE Problem 7.7PAE: Why is the ion not found in nature? Problem 7.8PAE: Why do nonmetals tend to form anions rather than cations? Problem 7.9PAE Problem 7.10PAE: 7.10 Arrange the members of each of the following sets of cations in order of increasing ionic... Problem 7.11PAE: 7.11 Arrange the following sets of anions in order of increasing ionic radii. (a) Cl,P3,S2, (b)... Problem 7.12PAE: 7.12 Which pair will form a compound with the larger lattice energy: Na and F or Mg and F? Why? Problem 7.13PAE: 7.13 Figure 7-2 depicts the interactions of an ion with its first nearest neighbors, second nearest... Problem 7.14PAE: 7.14 Describe the difference between a covalent bond and an ionic bond. Problem 7.15PAE: 7.15 Covalently bonded compounds tend to have much lower melting and boiling points than ionic... Problem 7.16PAE Problem 7.17PAE: 7.17 Coulombic forces are often used to explain ionic bonding. Are coulombic forces involved in... Problem 7.18PAE: 7.18 In terms of the strengths of the covalent bonds involved, why do combustion reactions release... Problem 7.19PAE: 7.19 If the formation of chemical bonds always releases energy, why don't all elements form dozens... Problem 7.20PAE: 7.20 Draw the Lewis dot symbol for each of the following atoms, (a) boron, (b) fluorine, (c)... Problem 7.21PAE: 7.21 Theoretical models for the structure of atomic nuclei predict the existence of superheavy... Problem 7.22PAE: 7.22 Use Lewis dot symbols to explain why chlorine bonds with only one hydrogen atom. Problem 7.23PAE: 7.23 Define the term lone pair. Problem 7.24PAE: 7.24 How many electrons are shared between two atoms in (a) a single covalent bond, (b) a double... Problem 7.25PAE: 7.25 How does the bond energy of a double bond compare to that of two single bonds between the same... Problem 7.26PAE: 7.26 How is electronegativity defined? Problem 7.27PAE: 7.27 Distinguish between electron affinity and electronegativity. Problem 7.28PAE: 7.28 Certain elements in the periodic table shown in Figure 7.7 had no electronegativity value... Problem 7.29PAE: 7.29 When two atoms with different electronegativities form a covalent bond, what does the electron... Problem 7.30PAE: 7.30 The bond in HF is said to be polar, with the hydrogen carrying a partial positive charge. For... Problem 7.31PAE: 7.31 Why is a bond between two atoms with different electronegativities called a polar bond? Problem 7.32PAE Problem 7.33PAE: 7.33 In each group of three bonds, which bond is likely to be the most polar? Which will be the... Problem 7.34PAE Problem 7.35PAE: 7.35 Which one of the following contains botb ionic and covalent bonds? (a) BaCO3 , (b) MgCl2 , (c)... Problem 7.36PAE Problem 7.37PAE: 7.37 Draw the Lewis structure for each of the following molecules. (a) CO , (b) H2S , (c) SF6 , (d)... Problem 7.38PAE: 7.38 Draw a Lewis structure for each of the following molecules or ions. (a) CS2 , (b) BF4 , (c)... Problem 7.39PAE Problem 7.40PAE: 7.40 Why is it impossible for hydrogen to be the central atom in the Lewis structure of a polyatomic... Problem 7.41PAE Problem 7.42PAE: 7.42 Draw resonance structure for (a) (b) and (c) Problem 7.43PAE Problem 7.44PAE Problem 7.45PAE Problem 7.46PAE: 7.46 Consider the nitrogen-oxygen bond lengths in NO2+ , NO2 , and NO3 . In which ion is the bond... Problem 7.47PAE: 7.47 Which of the species listed has a Lewis structure with only one lone pair of electrons? F2 ,... Problem 7.48PAE: 7.48 Identify what is incorrect in the Lewis structures shown for BBr3 and SO2 Problem 7.49PAE: 7.49 Identify what is incorrect in the Lewis structures shown for O3 and XeF4 . Problem 7.50PAE: 7.50 Chemical species are said to be isoelectronic if they have the same Lewis structure (regardless... Problem 7.51PAE: 7.51 Explain the concept of wave interference in your own words. Distinguish between constructive... Problem 7.52PAE: 7.52 How does orbital overlap explain the buildup of electron density between nuclei in a chemical... Problem 7.53PAE: 7.53 How do sigma and pi bonds differ? How are they similar? Problem 7.54PAE: 7.54 CO , CO2 , CH3OH , and CO32 , all contain carbon-oxygen bonds. Draw Lewis structures for these... Problem 7.55PAE: 7.55 Draw the Lewis dot structure of the following species and identify the number of pi bonds in... Problem 7.56PAE: 7.56 Draw the Lewis dot structures of the following compounds and identify the number of pi bonds in... Problem 7.57PAE: 7.57 What observation about molecules compels us to consider the hybridization of atomic orbitals? Problem 7.58PAE Problem 7.59PAE: 7.59 What type of hybrid orbital is generated by combining the valence s orbital and all three... Problem 7.60PAE: 7.60 What type of hybridization would be expected for the central atom X in each of the following... Problem 7.61PAE: 7.61 What hybrid orbitals would be expected for the central atom in each of the following molecules?... Problem 7.62PAE: 7.62 What type of hybridization would you expect for the carbon atom in each of the following... Problem 7.63PAE: 7.63 What physical concept forms the premise of VSEPR theory? Problem 7.64PAE: 7.64 Predict the geometry of the following species, (a) (b) (c) (d) Problem 7.65PAE Problem 7.66PAE Problem 7.67PAE Problem 7.68PAE: 7.68 Give approximate values for the indicated bond angles. (a) Cl—S—Cl in SCl2, (b) N—N—O in N2O,... Problem 7.69PAE: 7.69 Propene has the chemical formula Describe the overall shape of the molecule by considering the... Problem 7.70PAE Problem 7.71PAE Problem 7.72PAE: 7.72 How does an MSN differ from amorphous silica so that is has improved biocompatibility? Problem 7.73PAE Problem 7.74PAE: 7.74 In a lattice, a positive ion is often surrounded by eight negative ions. We might reason,... Problem 7.75PAE: 7.75 Use the concept of lattice energy to rationalize why sodium fluoride dissolves in water,... Problem 7.76PAE Problem 7.77PAE Problem 7.78PAE Problem 7.79PAE Problem 7.80PAE Problem 7.81PAE Problem 7.82PAE Problem 7.83PAE Problem 7.84PAE: 7.84 Which of the following molecules is least likely to actually exist OF4,SF4,SeF4 , or TeF4 ?... Problem 7.85PAE: 7.85 Consider the molecule whose structure is shown below. (a) How many carbon atoms are sp3... Problem 7.86PAE: 7.86 Nitrogen triiodide, NI3(s) , is unstable and will spontaneously detonate to form a bright... Problem 7.87PAE: 7.87 Nitrogen is capable of forming single, double, or triple bonds, and the figure that follows... Problem 7.88PAE: 7.88 The N5+ cation has been synthesized and studied. Consider the possible Lewis structure below.... Problem 7.89PAE Problem 7.90PAE Problem 7.91PAE: 7.91 A Lewis structure for the oxalate ion is shown below. (One or more other resonance forms are... Problem 7.92PAE Problem 7.93PAE: 7.93 An unknown metal M forms a chloride with the formula This chloride compound was examined and... Problem 7.94PAE Problem 7.95PAE Problem 7.96PAE: 7.96 Consider the hydrocarbons whose structures are shown below. Which of these molecules would be... Problem 7.97PAE: 7.97 Consider the structure shown below for as well as any other important resonance structures. (a)... Problem 7.98PAE Problem 7.99PAE Problem 7.100PAE Problem 7.101PAE: 7.101 Lead selenide nanocrystals may provide a breakthrough in the engineering of solar panels to be... Problem 7.102PAE Problem 7.103PAE Problem 7.104PAE: 7.104 Hydrogen azide, HN3 , is a liquid that explodes violently when subjected to shock. In the HN3... Problem 7.105PAE Problem 7.106PAE Problem 7.107PAE: 7.107 How do the Lewis symbols for C, Si, and Ge reflect the similarity in their electron... Problem 7.108PAE Problem 7.109PAE Problem 7.102PAE
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Choose two atoms. List what their electron affinity values are including units. Which of these two would be more likely to form a bond with sodium metal? Why?
Definition Definition Change in energy of a neutral gaseous atom when an electron is added to the atom to form a negative ion.
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