04:03Lattice Energy Summary in 4 Minutes (With Examples & Practice Problems)Conquer Chemistry1422views
13:30Lattice Energy of Ionic Compounds, Basic Introduction, Charge vs Ionic RadiusThe Organic Chemistry Tutor738views
Multiple ChoiceThe lattice energy for ionic crystals decreases as the charge of the ions _____ and the size of the ions _____.882views
Multiple ChoiceWhich of the following compounds would you expect to have the highest boiling point?629views
Multiple ChoiceThe solubilities of CaCrO4 and PbCrO4 in water at 25°C are approximately 0.111 g/L and 0.0905 g/L in H2O respectively. Based on this information, which compound do you think has the smaller lattice energy?459views1rank
Multiple ChoiceWhich of the following should have the largest magnitude for the lattice energy?209views
Multiple ChoiceWhich of the following should have the smallest magnitude for the lattice energy?258views
Textbook QuestionIllustrated are four ions — A, B, X, and Y— showing their relative ionic radii. The ions shown in red carry positive charges: a 2+ charge for A and a 1+ charge for B. Ions shown in blue carry negative charges: a 1- charge for X and a 2- charge for Y. (b) Among the combinations in part (a), which leads to the ionic compound having the largest lattice energy? 592views
Textbook QuestionA portion of a two-dimensional 'slab' of NaCl(s) is shown here (see Figure 8.2) in which the ions are numbered. (d) Consider ion 5. How many repulsive interactions are shown for it? 510views
Textbook Question(c) Would you expect salts like NaCl, which have singly charged ions, to have larger or smaller lattice energies compared to salts like CaO which are composed of doubly-charged ions?469views
Textbook Question(b) Write the chemical equation that represents the process of lattice energy for the case of NaCl.1764views
Textbook QuestionNaCl and KF have the same crystal structure. The only difference between the two is the distance that separates cations and anions. (b) Use the ionic radii given in Figure 7.8 to estimate the Na¬Cl and K¬F distances.542views
Textbook QuestionNaCl and KF have the same crystal structure. The only difference between the two is the distance that separates cations and anions. (a) The lattice energies of NaCl and KF are given in Table 8.1. Based on the lattice energies, would you expect the Na¬Cl or the K¬F distance to be longer?1500views
Textbook QuestionThe substances NaF and CaO are isoelectronic (have the same number of valence electrons). (d) Using the lattice energies in Table 8.1, predict the lattice energy of ScN.896views
Textbook Question(a) Does the lattice energy of an ionic solid increase or decrease (i) as the charges of the ions increase, (ii) as the sizes of the ions increase?806views
Textbook QuestionWhich of the following trends in lattice energy is due to differences in ionic radii? (a) LiF 7 NaF 7 CsF, (b) CaO 7 KCl, (c) PbS 7 Li2O.761views
Textbook QuestionWhich of the following alkali metal halides has the largest lat-tice energy? Explain. (a) (b) (c)340views
Textbook Question(a) Based on the lattice energies of MgCl2 and SrCl2 given in Table 8.1, what is the range of values that you would expect for the lattice energy of CaCl2?1339views
Textbook QuestionSilver nitrate has a lattice energy of -820 kJ>mol and a heat of solution of 22.6 kJ>mol. Calculate the heat of hydration for silver nitrate.1268views2rank
Textbook QuestionUse the data to calculate the heats of hydration of lithium chloride and sodium chloride. Which of the two cations, lithium or sodium, has stronger ion–dipole interactions with water? Why? 1170viewsTextbook QuestionPotassium nitrate has a lattice energy of -163.8 kcal>mol and a heat of hydration of -155.5 kcal>mol. How much potassium nitrate has to dissolve in water to absorb 1.00 * 102 kJ of heat?2378viewsTextbook QuestionRubidium iodide has a lattice energy of -617 kJ>mol, while potassium bromide has a lattice energy of -671 kJ>mol. Why is the lattice energy of potassium bromide more exothermic than the lattice energy of rubidium iodide?1485viewsTextbook QuestionThe lattice energy of CsF is -744 kJ>mol, whereas that of BaO is -3029 kJ>mol. Explain this large difference in lattice energy.2187viewsTextbook QuestionArrange these compounds in order of increasing magnitude of lattice energy: KCl, SrO, RbBr, CaO.2566viewsTextbook QuestionConsider the lattice energies of the following Group 2A compounds: BeH2, 3205 kJ/mol; MgH2, 2791 kJ/mol; CaH2, 2410 kJ/mol; SrH2, 2250 kJ/mol; BaH2, 2121 kJ/mol. (a) What is the oxidation number of H in these compounds?880viewsTextbook QuestionCalculate the energy change in kilojoules per mole when lithium atoms lose an electron to bromine atoms to form isolated Li+ and Br-ions. [The Ei for Li1g2 is 520 kJ/mol; the Eea for Br1g2 is -325 kJ/mol.] Will a lithium atom transfer an elec-tron to a bromine atom to form isolated Li+ 1g2 and Br-1g2 ions? Explain.475viewsTextbook QuestionThe reaction of Fe2O3(s) with Al(s) to form Al2O3(s) and Fe(s) is called the thermite reaction and is highly exothermic. What role does lattice energy play in the exothermicity of the reaction?1194viewsTextbook QuestionNaCl has a lattice energy of -787 kJ>mol. Consider a hypothetical salt XY. X3 + has the same radius of Na+ and Y3 - has the same radius as Cl - . Estimate the lattice energy of XY.1188viewsTextbook QuestionThe electron affinity of oxygen is -141 kJ>mol, corresponding to the reaction O1g2 + e-¡O-1g2 The lattice energy of K2O1s2 is 2238 kJ>mol. Use these data along with data in Appendix C and Figure 7.10 to calculate the 'second electron affinity' of oxygen, corresponding to the reaction O-1g2 + e-¡O2 -1g22411viewsTextbook QuestionSodium hydroxide (NaOH) has a lattice energy of -887 kJ>mol and a heat of hydration of -932 kJ>mol. How much solution could be heated to boiling by the heat evolved by the dissolution of 25.0 g of NaOH? (For the solution, assume a heat capacity of 4.0 J>g # °C, an initial temperature of 25.0 °C, a boiling point of 100.0 °C, and a density of 1.05 g>mL.)1768viewsOpen QuestionConsider the lattice energy of any ionic compound. what combination of ions and charges will produce the largest (in magnitude) lattice energies?163viewsOpen QuestionWhich of the following trends in lattice energy is due to differences in ionic radii?249viewsOpen QuestionRank the following ionic compounds by lattice energy.344viewsOpen QuestionMX(s) + crystal lattice energy → M+(g) + X- (g) is the reaction for crystal lattice energy.168viewsShowing 33 of 33 practiceMore practice (0)
Textbook QuestionPotassium nitrate has a lattice energy of -163.8 kcal>mol and a heat of hydration of -155.5 kcal>mol. How much potassium nitrate has to dissolve in water to absorb 1.00 * 102 kJ of heat?2378views
Textbook QuestionRubidium iodide has a lattice energy of -617 kJ>mol, while potassium bromide has a lattice energy of -671 kJ>mol. Why is the lattice energy of potassium bromide more exothermic than the lattice energy of rubidium iodide?1485views
Textbook QuestionThe lattice energy of CsF is -744 kJ>mol, whereas that of BaO is -3029 kJ>mol. Explain this large difference in lattice energy.2187views
Textbook QuestionArrange these compounds in order of increasing magnitude of lattice energy: KCl, SrO, RbBr, CaO.2566views
Textbook QuestionConsider the lattice energies of the following Group 2A compounds: BeH2, 3205 kJ/mol; MgH2, 2791 kJ/mol; CaH2, 2410 kJ/mol; SrH2, 2250 kJ/mol; BaH2, 2121 kJ/mol. (a) What is the oxidation number of H in these compounds?880views
Textbook QuestionCalculate the energy change in kilojoules per mole when lithium atoms lose an electron to bromine atoms to form isolated Li+ and Br-ions. [The Ei for Li1g2 is 520 kJ/mol; the Eea for Br1g2 is -325 kJ/mol.] Will a lithium atom transfer an elec-tron to a bromine atom to form isolated Li+ 1g2 and Br-1g2 ions? Explain.475views
Textbook QuestionThe reaction of Fe2O3(s) with Al(s) to form Al2O3(s) and Fe(s) is called the thermite reaction and is highly exothermic. What role does lattice energy play in the exothermicity of the reaction?1194views
Textbook QuestionNaCl has a lattice energy of -787 kJ>mol. Consider a hypothetical salt XY. X3 + has the same radius of Na+ and Y3 - has the same radius as Cl - . Estimate the lattice energy of XY.1188views
Textbook QuestionThe electron affinity of oxygen is -141 kJ>mol, corresponding to the reaction O1g2 + e-¡O-1g2 The lattice energy of K2O1s2 is 2238 kJ>mol. Use these data along with data in Appendix C and Figure 7.10 to calculate the 'second electron affinity' of oxygen, corresponding to the reaction O-1g2 + e-¡O2 -1g22411views
Textbook QuestionSodium hydroxide (NaOH) has a lattice energy of -887 kJ>mol and a heat of hydration of -932 kJ>mol. How much solution could be heated to boiling by the heat evolved by the dissolution of 25.0 g of NaOH? (For the solution, assume a heat capacity of 4.0 J>g # °C, an initial temperature of 25.0 °C, a boiling point of 100.0 °C, and a density of 1.05 g>mL.)1768views
Open QuestionConsider the lattice energy of any ionic compound. what combination of ions and charges will produce the largest (in magnitude) lattice energies?163views
Open QuestionWhich of the following trends in lattice energy is due to differences in ionic radii?249views
Open QuestionMX(s) + crystal lattice energy → M+(g) + X- (g) is the reaction for crystal lattice energy.168views