The lattice energy of CaO(s) is -3,460 kilojoules per mole; the lattice energy for K2O is -2,240 kilojoules per mole. The lattice energy of CaO(s) is –3460 kJ/mol; the lattice energy of K 2 O is –2240 kJ/mol. The lattice energy of an ionic solid is a measure of the strength of bonds in that compound. Lattice energy, U, is defined as the enthalpy required to dissociate one mole of crystalline solid in its standard state into the gaseous ions of which … Lattice Energy is proportional to the product of charges of anion and cation. My guess : LE for CaO larger because Ca has 20 protons while K has 19 protons, so Ca's nucleus is stronger and pulls electrons in tighter, making them harder to "grab" (Therefore needing more energy to pull Ca and O apart?) Thus, CaO has a greater lattice energy than KI or LiBr. Thus, we expect the lattice energy of CaO, which has 2+ and 2– ions, to be the greatest of the three. The potential energy between two ions is given (here as a proportion) roughly by. Ca2+ is bonded to six equivalent O2- atoms to form a mixture of corner and edge-sharing CaO6 octahedra. Lattice Energies of the Alkali Metal Halides : Compound: Lattice Energy, kJ/mole : LiF-1045: LiCl-864: LiBr-819: LiI-765: NaF-924 F = (q_1q_2)/r^2 The distance between the charges r is the sum of the ionic radii. By doing physics-style calculations, it is possible to calculate a theoretical value for what you would expect the lattice energy to be. asked by re on March 3, 2011 Chemistry – solubility enthalpy change/ kJ mol –1. [math]L.E ∝ |q1.q2|[/math] Here, for CaO, Charge on Calcium is +2 and charge on Oxygen is -2. The force of attraction F is directly proportional to the charges (q_1 and q_2) on the two ions and on the distance r between them. Consequently, we expect RbCl, with a (−1)(+1) term in the numerator, to have the lowest lattice energy, and GaP, with a (+3)(−3) term, the highest. Theoretical values for lattice energy. The greater the lattice enthalpy the more stabler the ionic bond formed. Please help. Why? If the signs on the charges are oppositive, we have a negative energy corresponding to attraction.If the charges have the same sign, we have a positive energy of repulsion. The lattice energies for the alkali metal halides is therefore largest for LiF and smallest for CsI, as shown in the table below. L.E ∝ |2. Expert Answer . Account for the difference. Lattice Energy is directly proportional to charge on cation/anion and inversely proportional to center-to-center distance of cation and anion atoms… (P.S. Use an enthalpy diagram to calculate the lattice energy of CaCl2 from the following information. The table below shows the enthalpy changes needed to calculate the lattice enthalpy of calcium oxide, CaO. ions, and CaO of Ca. The lattice enthalpy is greater for ions of higher charge and smaller radii. Sro • CaO < MgO CaO → MgO < SHO MgOSro • CaO MgO • CaO • STO SHO< MgO • CaO. (1) MgO has the highest lattice energy. Let us use the Born - Haber cycle for determining the lattice enthalpy of NaCl as follows : The lattice energy of CaO(s) is -3,460 kilojoules per mole; the lattice energy for K2O(s) is -2,240 kilojoules per mole. therefore, the lattice energy of CaO is four times the lattice energy of NaCl, i.e., 4U. Lattice energy is an estimate of the bond strength in ionic compounds. Use the Born–Haber cycle and data from Appendix IIB and Table 9.3 to calculate the lattice energy of CaO. The structure is three-dimensional. CaO is Halite, Rock Salt structured and crystallizes in the cubic Fm-3m space group. So -lattice energy = -3414 => Lattice Energy = 3414 kJ/mol. The incorrect order of lattice energy is : View solution The lattic energy of N a 2 C O 3 ( s ) is 2 0 5 k J / m o l and the hydration energies of N a + and C O 3 2 − ions are − 8 0 and − 4 0 k J / m o l , respectively. The energy of the lattice will be higher for B, which is the second, said Kassim Oxide has more of the electrostatic forces, so which means that there's more of those that need to be broken and therefore the latest energy of calcium oxide will be the higher. Alternately, it can be defined as the energy that must be supplied to one mole of an ionic crystal in order to separate it into gaseous ions in a vacuum via an endothermic process. Account for this difference. Q. 2. ions. Which compound has the highest lattice energy? 1 is a little confusing with the use of the word largest. Given these ionization values, explain the difference between Ca and K with regard to their first and second ionization energies. Q. Question: Arrange MgO, CaO, And Sro In Order Of Increasing Absolute Value Of The Lattice Energy. The bond between ions of opposite charge is strongest when the ions are small. Of KCl and NaCl, which has a higher lattice energy? Let's assume that a compound is fully ionic. 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