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Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN: 9781938168390
Author: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher: OpenStax
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Textbook Question
Chapter 8, Problem 3E
Explain why bonds occur at specific average bond distances instead of the atoms approaching each other infinitely close.
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8) In an exothermic reaction, the enthalpy of the reaction can be calculated by
a. Subtracting the sum of all the bond energies of the
products from the sum of all the bond energies of the
reactants.
b. Subtracting the sum of all the bond energies of the reactants
from the sum of all the bond energies of the products
c. Finding the sum of the enthalpies of formation of all the
products and reactants together d. All of the above
Chapter 8 Solutions
Chemistry by OpenStax (2015-05-04)
Ch. 8 - Explain how and bonds are similar and how they...Ch. 8 - Draw a curve that describes the energy of a system...Ch. 8 - Explain why bonds occur at specific average bond...Ch. 8 - Use valence bond theory to explain the bonding in...Ch. 8 - Use valence bond theory to explain the bonding in...Ch. 8 - How many and bonds are present in the molecule...Ch. 8 - A friend tells you N2 has three bonds due to...Ch. 8 - Draw the Lewis structures for CO2 and CO, and...Ch. 8 - Why is the concept of hybridization required in...Ch. 8 - Give the shape that describes each hybrid orbital...
Ch. 8 - Explain why a carbon atom cannot form five bonds...Ch. 8 - What is the hybridization of the central atom in...Ch. 8 - A molecule with the formula AB3 could have one of...Ch. 8 - Methionine, CH3SCH2CH2CH(NH2)CO2H, is an amino...Ch. 8 - Sulfuric acid is manufactured by a series of...Ch. 8 - Two important industrial chemicals, ethene, C2H4,...Ch. 8 - For many years after they were discovered, it was...Ch. 8 - Consider nitrous acid, HNO2 (HONO). (a) Write a...Ch. 8 - Strike-anywhere matches contain a layer of KClO3...Ch. 8 - Identify the hybridization of each carbon atom in...Ch. 8 - Write Lewis structures for NF3 and PP5. On the...Ch. 8 - In addition to NF3, two other fluoro derivatives...Ch. 8 - The bond energy of a C—C single bond averages 347...Ch. 8 - For the carbonate ion, CO32, draw all of the...Ch. 8 - A useful solvent that will dissolve salts as well...Ch. 8 - For the molecule allene, H2C=C=CH2, give the...Ch. 8 - Identify the hybridization of the central atom in...Ch. 8 - Describe the molecular geometry and hybridization...Ch. 8 - For each of the following molecules, indicate the...Ch. 8 - For each of the following structures, determine...Ch. 8 - Draw the orbital diagram for carbon in CO2 showing...Ch. 8 - Sketch the distribution of electron density in the...Ch. 8 - How are the following similar, and how do they...Ch. 8 - If molecular orbitals are created by combining...Ch. 8 - Can a molecule with an odd number of electrons...Ch. 8 - Can a molecule with an even number of electrons...Ch. 8 - Why are bonding molecular orbitals lower in energy...Ch. 8 - Calculate the bond order for an ion with this...Ch. 8 - Explain why an electron in the bonding molecular...Ch. 8 - Predict the valence electron molecular orbital...Ch. 8 - Determine the bond order of each member of the...Ch. 8 - For the first ionization energy for an N2...Ch. 8 - Compare the atomic and molecular orbital diagrams...Ch. 8 - Which of the period 2 homonuclear diatomic...Ch. 8 - A friend tells you that the 2s orbital for...Ch. 8 - True or false: Boron contains 2s22p1 valence...Ch. 8 - What charge would be needed on F2 to generate an...Ch. 8 - Predict whether the MO diagram S2 would show s-p...Ch. 8 - Explain why N22+ is diamagnetic, while O24+, which...Ch. 8 - Using the MO diagrams, predict the bond order for...
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- Bond 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_forwardWhat aspect of the following Lewis structure indicates that the concept of coordinate covalency is needed to explain the bonding in the molecule?arrow_forwardhy do atoms form bonds with one another? What can make a molecule favored compared with the lone atoms?arrow_forward
- hat is the enthalpy change for a process? Is enthalpy a state function? In what experimental apparatus are enthalpy changes measured?arrow_forwardThe element sulphur has atomic number Sulphur forms a molecular compound with chloride with a molecular formula SCl2. The atomic number of chlorine is 17. Write down the electronic configuration of a sulphur atom and a chlorine Draw a Lewis structure of an SCl2 molecule, by showing the electrons in the outer shells of the State how many bond pairs and lone pairs of electrons are arranged around the sulphur atoms in SCl2 molecule. Sketch the shape and state the molecular geometry of SCl2 Explain the hybridisation of the central atom in SCl2 Explain the intermolecular forces exists in SCl2arrow_forward4. The standard enthalpies of formation of SO(g), S(g) and O(g) are -359.7, +2788 and +249.0 kJ mol, respectively. Use these data to calculate the average bond energy (in kJ mol ¹) of the S-O double bond. A) +297.9 B) +325.0 C) -461.8 D) +461.8 E) +317.8arrow_forward
- In an ionic compound, the size of the ions affects the internuclear distance (the distance between the centers of adjacent ions), which affects lattice energy (a measure of the attractive force holding those ions together). Based on ion sizes, arrange these compounds by their expected lattice energy. Note that many sources define lattice energies as negative values. Please arrange by magnitude and ignore the sign. K2S Cs2S Rb2S Na2S Li2Sarrow_forwardExplain the trend that bond formation does to atomic order by selecting all those that apply. Larger molecules have higher entropies than smaller molecules. Larger molecules have larger entropies on a per atom basis. Larger molecules have lower entropies than smaller molecules. Larger molecules have smaller entropies on a per atom basis.arrow_forwardIn an ionic compound, the size of the ions affects the internuclear distance (the distance between the centers of adjacent ions), which affects lattice energy (a measure of the attractive force holding those ions together). Based on ion sizes, arrange these compounds by their expected lattice energy. Note that many sources define lattice energies as negative values. Please arrange by magnitude and ignore the sign. |lattice energy| = absolute value of the lattice energy CSF Greatest lattice energy (strongest bonds) Least lattice energy (weakest bonds) CsBr Answer Bank CsCl CSIarrow_forward
- What feature of a Lewis structure can be used to tell if a molecule’s (or ion’s) electron-pair geometry and molecular structure will be identical?arrow_forwardA certain element X forms two compounds with hydrogen, XH3 and X2H4 (H2X–XH2). The total bond enthalpies of XH3(g) and X2H4(g) are 846 kJ/mol and 1341 kJ/mol, respectively. What is the average bond enthalpy of the X–X bond?arrow_forwardWhen a firecracker explodes, energy is obviously released. The compounds in the firecracker can be viewed as being “energy rich.” What does this mean? Explain the source of the energy in terms of chemical bonds.arrow_forward
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