11. Bonding & Molecular Structure

Lattice Energy

11. Bonding & Molecular Structure

Lattice Energy

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Lattice Energy Example 1

Lattice Energy Example 2

Lattice Energy Example 3

Lattice Energy Example 4

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14:07

Lattice Energies for Ionic Compounds

Lattice Enthalpy and Enthalpy Changes | A-level Chemistry | OCR, AQA, Edexcel

Lattice Energies - Chemistry Tutorial

Lattice Energy Summary in 4 Minutes (With Examples & Practice Problems)

Lattice Energy of Ionic Compounds, Basic Introduction, Charge vs Ionic Radius

The Organic Chemistry Tutor

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Multiple Choice

The lattice energy for ionic crystals decreases as the charge of the ions _____ and the size of the ions _____.

a) Increases, increases

b) Increases, decreases

c) Decreases, increases

d) Decreases, decreases

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Multiple Choice

Which of the following compounds would you expect to have the highest boiling point?

a) MgCl₂

b) SrO

c) SrCl₂

d) CsI

e) LiBr

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Multiple Choice

The 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?

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Multiple Choice

Which of the following reactions has ΔH_rxn = ΔH_lattice?

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Multiple Choice

Which of the following should have the largest magnitude for the lattice energy?

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Multiple Choice

Which of the following should have the smallest magnitude for the lattice energy?

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Textbook Question

Illustrated 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?

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Textbook Question

A 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?

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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?

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Textbook Question

(b) Write the chemical equation that represents the process of lattice energy for the case of NaCl.

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Textbook Question

NaCl 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.

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Textbook Question

NaCl 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?

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Textbook Question

The 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.

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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?

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Textbook Question

Which 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.

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Textbook Question

Which of the following alkali metal halides has the largest lat-tice energy? Explain. (a) (b) (c)

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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?

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Textbook Question

Silver 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.

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Textbook Question

Use 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?

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Textbook Question

Potassium 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?

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Textbook Question

Rubidium 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?

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Textbook Question

The lattice energy of CsF is -744 kJ>mol, whereas that of BaO is -3029 kJ>mol. Explain this large difference in lattice energy.

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Textbook Question

Arrange these compounds in order of increasing magnitude of lattice energy: KCl, SrO, RbBr, CaO.

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Textbook Question

Consider 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?

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Textbook Question

Calculate 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.

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Textbook Question

The 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?

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Textbook Question

NaCl 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.

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Textbook Question

The 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 -1g2

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Textbook Question

Sodium 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.)

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Open Question

Consider the lattice energy of any ionic compound. what combination of ions and charges will produce the largest (in magnitude) lattice energies?

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Open Question

Which of the following trends in lattice energy is due to differences in ionic radii?

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Open Question

Rank the following ionic compounds by lattice energy.

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Open Question

MX(s) + crystal lattice energy → M⁺(g) + X^- (g) is the reaction for crystal lattice energy.

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11. Bonding & Molecular Structure

Lattice Energy

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