General Chemistry: Principles and Modern Applications (11th Edition)
11th Edition
ISBN: 9780132931281
Author: Ralph H. Petrucci, F. Geoffrey Herring, Jeffry D. Madura, Carey Bissonnette
Publisher: PEARSON
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Textbook Question
Chapter 23, Problem 58E
For the straight-line graphs in Figure 23-8 explain why (a) breaks occur at the melting points and boiling points of the metals; (b) the slopes of the lines become more positive at these breaks, (c) the break at the boiling point is sharper than at the melting point.
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Determine the second ionization energy of
calcium (in kJ mol-1) from the given data (all in
kJ mol-1):
AH°[CaCl,(s)] = -796
AH¡[Ca(g)] = 178
AH°[CI(g)] = 122
First ionization energy of Ca(g) = 590
Electron affinity of Cl(g) = -349
Lattice enthalpy of CaCl,(s) = -2260
А
1150
В
1235
C
1093
D
1210
24. Which member of the following pairs has the larger radius? Provide your reasoning.
(a) Al or S
(b) Cl or Ca²+
(c) Ba or Sn
(d) Na+ or K
The melting points of the alkali metals decrease from Li to Cs. In contrast, the melting points of the halogens increase from F2 to I2.
(a) Using bonding principles, account for the decrease in the melting points of the alkali metals.
(b) Using bonding principles, account for the decrease in the melting points of the halogens.
(c) What is the expected trend in the melting points of the compounds LiF, NaCl, KBr, and CsI? Explain this trend using bonding principles.
Note: Please briefly explain all the questions listed above. Thank you.
Chapter 23 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
Ch. 23 - By means of orbital diagrams, write electron...Ch. 23 - Arrange the following species according to the...Ch. 23 - Describe how the transition elements compare with...Ch. 23 - With only minor irregularities, the melting points...Ch. 23 - Why do the atomic radii vary so much for two...Ch. 23 - Prob. 6ECh. 23 - Which of me first transition series elements...Ch. 23 - Why is the number of common oxidation states for...Ch. 23 - As a group, the lanthanides are more reactive...Ch. 23 - The maximum difference in standard reduction...
Ch. 23 - Complete and balance the following equations. If...Ch. 23 - By means of e chemical equation, give an example...Ch. 23 - Prob. 13ECh. 23 - Prob. 14ECh. 23 - Prob. 15ECh. 23 - Prob. 16ECh. 23 - Prob. 17ECh. 23 - According to Figure 23-8, G decreases with...Ch. 23 - Prob. 19ECh. 23 - Prob. 20ECh. 23 - Write plausible half-equations to represent each...Ch. 23 - Prob. 22ECh. 23 - Use electrode potential data from this chapter or...Ch. 23 - You are given these three reducing agents: Zn(s);...Ch. 23 - Prob. 25ECh. 23 - Prob. 26ECh. 23 - Prob. 27ECh. 23 - Use data from the text to construct a standard...Ch. 23 - When a soluble lead compound is added to a...Ch. 23 - Prob. 30ECh. 23 - Prob. 31ECh. 23 - If CO2(g) under pressure is passed into...Ch. 23 - Use equation (23.19) to determine [Cr2O72] in a...Ch. 23 - If a solution is prepared by dissolving 1.505 g...Ch. 23 - Prob. 35ECh. 23 - Prob. 36ECh. 23 - Prob. 37ECh. 23 - Prob. 38ECh. 23 - Will reaction (23.25) still be spontaneous in the...Ch. 23 - Prob. 40ECh. 23 - Prob. 41ECh. 23 - Prob. 42ECh. 23 - Prob. 43ECh. 23 - Prob. 44ECh. 23 - Prob. 45ECh. 23 - Prob. 46ECh. 23 - Prob. 47ECh. 23 - At 400C , 2Hg(I)+O2(g)2HgO(s) for the reaction...Ch. 23 - Prob. 49ECh. 23 - Prob. 50ECh. 23 - Prob. 51ECh. 23 - Prob. 52ECh. 23 - Prob. 53ECh. 23 - Prob. 54ECh. 23 - The text notes that in small quantities, zinc is...Ch. 23 - Prob. 56ECh. 23 - What formulas would you expect for the metal...Ch. 23 - For the straight-line graphs in Figure 23-8...Ch. 23 - Prob. 59ECh. 23 - Prob. 60ECh. 23 - Prob. 61ECh. 23 - Prob. 62ECh. 23 - Prob. 63ECh. 23 - Prob. 64ECh. 23 - Prob. 65ECh. 23 - Prob. 66ECh. 23 - Prob. 67ECh. 23 - Prob. 68ECh. 23 - Prob. 69ECh. 23 - Prob. 70ECh. 23 - Prob. 71ECh. 23 - For a coordination number of four, the radius of...Ch. 23 - Prob. 73ECh. 23 - Prob. 74FPCh. 23 - Several transition metal ions are found in cation...Ch. 23 - Prob. 76SAECh. 23 - Briefly describe each of the following ideas. phe...Ch. 23 - Prob. 78SAECh. 23 - Prob. 79SAECh. 23 - Prob. 80SAECh. 23 - Prob. 81SAECh. 23 - Prob. 82SAECh. 23 - Prob. 83SAECh. 23 - Prob. 84SAECh. 23 - Prob. 85SAECh. 23 - Provide the missing name or formula for the...Ch. 23 - Prob. 87SAECh. 23 - Prob. 88SAECh. 23 - Prob. 89SAECh. 23 - Prob. 90SAE
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- Given the following thermodynamic data, calculate the lattice energy of LiCl:ΔH°f[LiCl(s)] = -409 kJ/molΔH°sublimation [Li] = 161 kJ/molBond energy [Cl-Cl] = 243 kJ/molIE1 (Li) = 520 kJ/molEA1 (Cl) = -349 kJ/mol -1682 kJ/mol -984 kJ/mol -1560 kJ/mol -862 kJ/mol -1213 kJ/molarrow_forward(f) Potassium permanganate (g) Sodium hypochlorite (h) Beryllium bicarbonate (1) Ammonium dichromate (G) Iron (II) chloridearrow_forwardLook in Appendix D and compare the electron configurations shown there with the fusion enthalpies for the metals shown in Table 9.7. Is there any correlation between these configurations and this property? Does strength of attraction among metal atoms correlate with number of valence electrons? Explain your answers.arrow_forward
- 4. The common oxidation number for an alkaline earth metal is +2. (a) Using the Born-Mayer equation (for determining the lattice enthalpy) and a Born-Haber cycle (draw it), show that CaCl is an exothermic compound (negative AHf). Make a reasonable prediction to estimate the ionic radius of Ca (explain your reasoning). The sublimation (atomization) enthalpy for Ca(s) is 178 kJ/mol. (b) Show that an explanation for the non-existence of CaCl can be found in the enthalpy change for the reaction below. The AHf for CaCl2(s) is -190.2 kcal/mol. 2 CaCl(s) → Ca(s) + CaCl2(s)arrow_forwardMixing SbCl3 and GaCl3 in a 1;1 molar ratio (usingliquid sulfur dioxide as a solvent) gives a solid ioniccompound of empirical formula GaSbCl6. A controversyarises over whether this compound is ( ) SbCl2 + ( ) GaCl 4 - or( ) GaCl+ 2 ( ) SbCl 4 -(a) Predict the molecular structures of the two anions.(b) It is learned that the cation in the compound has abent structure. Based on this fact, which formulationis more likely to be correct?arrow_forwardKsp for Co(OH)2 is 5.92x10^-15arrow_forward
- Calculate the lattice energy of AgBr(s) using the following thermodynamic data (all data is in kJ/mol). Ag(s) ΔHsublimation = 265 kJ/mol Ag(g) Ionization energy = 711 kJ/mol Br-Br(g) Bond energy = 173 kJ/mol Br(g) Electron affinity = -345 kJ/mol AgBr(s) ΔH°f = -120 kJ/mol ______________ kJ/molarrow_forwardDoes metallic character increase, decrease, or remainunchanged as one goes from left to right across a row of theperiodic table?arrow_forwardPlot the melting temperatures of elements in the 4A to 8–10 columns of the periodic table versus atomic number (i.e., plot melting temperatures of Ti through Ni, Zr through Pd, and Hf through Pt). Discuss these relationships, based on atomic bonding and binding energies: (a) as the atomic number increases in each row of the periodic table and (b) as the atomic number increases in each column of the periodic table.arrow_forward
- Complete the following reactions below. If no reaction occurred, write NR. Mg(s) + MgSO4(aq) -> Mg(s) + CusO4(aq) –> Cu(s) + MgSO4(aq) ->arrow_forwarda Spinels are solids with the general formula M²+ (M¹³+)₂ 04 (where M²+ and M¹³ are 3+ 3+ metal cations of the same or different metals). The best-known example is common magnetite, Fe3O4 [which you can formulate as (Fe³+)₂04]. (Fe²+) A crystal of a spinel Given its name, it is evident that magnetite is ferromagnetic. How many unpaired electrons are there in iron (II) and in iron(III) ions? Iron(II) ion: unpaired electron(s) Iron(III) ion: unpaired electron(s)arrow_forwardEnergy is required to remove two electrons from Ca to formCa2+, and energy is required to add two electrons to O toform O2 - . Yet CaO is stable relative to the free elements.Which statement is the best explanation? (a) The latticeenergy of CaO is large enough to overcome these processes.(b) CaO is a covalent compound, and these processes areirrelevant. (c) CaO has a higher molar mass than either Ca orO. (d) The enthalpy of formation of CaO is small. (e) CaO isstable to atmospheric conditions.arrow_forward
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