Element First Ionization Energy (kJImol) Second Ionization Energy (kiImol) I K 419 3050 Ca 590 1140 75. Use principles of atomic structure to answer each of the following: (a) The radius of the Ca atom is 197 pm; the radius of the Ca 2 + ion is 99 pm. Account for the difference. (b) The lattice energy of CaO ( s ) is −3460 kJ/mol; the lattice energy of K 2 O is −2240 kJ/mol. Account for the difference. (c) Given these ionization values, explain the difference between Ca and K with regard to their first and second ionization energies. Element First Ionization Energy (kJ/mol) Second Ionization Energy (kJ/mol) K 419 3050 Ca 590 1140 (d) The first ionization energy of Mg is 738 kJ/mol and that of Al is 578 kJ/mol. Account for this difference.
Element First Ionization Energy (kJImol) Second Ionization Energy (kiImol) I K 419 3050 Ca 590 1140 75. Use principles of atomic structure to answer each of the following: (a) The radius of the Ca atom is 197 pm; the radius of the Ca 2 + ion is 99 pm. Account for the difference. (b) The lattice energy of CaO ( s ) is −3460 kJ/mol; the lattice energy of K 2 O is −2240 kJ/mol. Account for the difference. (c) Given these ionization values, explain the difference between Ca and K with regard to their first and second ionization energies. Element First Ionization Energy (kJ/mol) Second Ionization Energy (kJ/mol) K 419 3050 Ca 590 1140 (d) The first ionization energy of Mg is 738 kJ/mol and that of Al is 578 kJ/mol. Account for this difference.
Suppose a chemist discovers a new metallic element and names it "Xercisium" (Xr). Xr exhibits chemical behaviour similar to an alkaline earth.
Xr(s) + Cl2(g) → XrCl2(s)
Lattice energy for XrCl2
-2020. kJ/mol
First Ionization energy of Xr
500. kJ/mol
Second Ionization energy of Xr
950. kJ/mol
Electron affinity of Cl
-348.7 kJ/mol
Bond energy of Cl2
239 kJ/mol
Enthalpy of sublimation (atomization) of Xr
200. kJ/mol
Use the above data to calculate ΔH°f for Xercisium chloride.
The ionic radii of element E and a different metallic element, M, are shown in the following table: Both elements form oxides, E2O and MO. If lattice energy is defined as the energy required to separate an ionic solid into individual separate gaseous ions, would the lattice energy of MO be less than, equal to, or greater than the lattice energy of the oxide E2O? Justify your answer in terms of Coulomb's law
Suppose a chemist discovers a new metallic element and names it "Xhaustium" (Xh).Xh exhibits chemical behaviour similar to an alkaline earth.
Xh(s) + F2(g) → XhF2(s)
Lattice energy for XhF2
-2140. kJ/mol
First Ionization energy of Xh
310. kJ/mol
Second Ionization energy of Xh
589 kJ/mol
Electron affinity of F
-327.8 kJ/mol
Bond energy of F2
154 kJ/mol
Enthalpy of sublimation (atomization) of Xh
150. kJ/mol
Use the above data to calculate ΔH°f for Xhaustium fluoride.
Your answer must be accurate and precise to the nearest 1 kJ/mol, as are the given parameters.
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Calorimetry Concept, Examples and Thermochemistry | How to Pass Chemistry; Author: Melissa Maribel;https://www.youtube.com/watch?v=nSh29lUGj00;License: Standard YouTube License, CC-BY