Use your knowledge of thermochemistry to calculate the
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Chemistry
- What is the electron configuration of the Ba3+ ion? Suggest a reason why this ion is not normally found in nature.arrow_forwardBoron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively. (a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Draw the orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons in boron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation for the reaction of solid boron with fluorine gas. (e) ΔHf° for BF3(g) is -1135.6 kj/mol. Calculate the standard enthalpy change in the reaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?arrow_forwardUsing the following data, draw the Born Haber cycle for the formation of hypothetical compound of MX(s) from its elements. Using the Born Haber cycle, calculate the electron affinity of X. M (s) → M (g) ∆Hº = 77 kJ mol-1M (g) → M+ (g) + e- ∆Hº = 433 kJ mol-1X2 (g) → 2X (g) ∆Hº = 129 kJ mol-1M (s) + ½ X2(g) → MX(s) ∆Hº = -530 kJ mol-1M+ (g) + X-(g) → MX (s) ∆Hº = -760 kJ mol-1arrow_forward
- Boron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively.(a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Drawthe orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons inboron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation forthe reaction of solid boron with fluorine gas. (e) ΔHf° for BF31g2 is -1135.6 kJ>mol. Calculate the standard enthalpy change in thereaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?arrow_forward1. Arrange the atoms according to both decreasing atomic radius and increasing first ionization energy (IE): Ca, Cl, Ga, P, and S 2. Select the statement(s) that explain(s) the relationship between the arrangement of elements by size and first ionization energy. (a). The two arrangements are the same because IE of elements increases from left to right and the radii of elements decreases from left to right. b). The first set of paired electrons in a p subshell experience a large amount of electron-electron repulsion, making the fourth electron in a p subshell easy to remove. c). A full s subshell is able to shield a newly filled p subshell from the nucleus, making the first electron in a p subshell easy to remove. d). A p subshell with only one unpaired electron is extremely stable, making the fifth electron in a p subshell easy to remove. e). The third unpaired electron in a p subshell causes a lot of electron-electron repulsion among the orbitals, making the third electron…arrow_forwardla) For each of the following pairs indicate which element you would expect to have the larger First Ionization Energy and which one would have the larger radius: (a) Ca and Cl; (b) Sn and Tl; (c) Ba and Bi (d) Fr and Cs b) For each pair indicate which Ion you would expect to have the largest Radius: (a) 0²- and O; (b) N³ and Mg²+ (c) Al3* and Al ne Elearrow_forward
- Arrange the following chemical species in order of increasing atomic radius. Explain your arrangement in each case. (a) K, Mg, Ca, Al (b) F–, S2–, Cl–.arrow_forward(ii) Draw the Born-Haber cycle and use the data below for the formation of calcium chloride, to calculate the electron affinity of chlorine: Ca(s) → Ca(g) AHat = +190 kJ/mol Ca(g) > Caz*(g) + 2e¨ AH¡ɛ = +1730 kJ/mol Cl2{g) 2C1(g) AHat = +121 kJ/mol Caz (g) + 2Cl(g) > CaCl2(s) AHLE = -2184 kJ/mol Ca(s) + Cl2(g) –> CaCl2(s) AH; = -795 kJ/molarrow_forward7. The first ionisation energy of the chlorine atom is 1251 kJ/mol. Without looking at your text book, say which of the following values would be the more likely ionisation energy for the iodine atom. Explain your choice. (a) 1000 kJ/mol (b) 1400 kJ/molarrow_forward
- Use the following data and the Born-Haber cycle to calculate the first ionization energy (ΔH IE1) of K(g) K(s) → K(g) 89 kJ mol-1 Cl(g) + e– → Cl–(g) -349 kJ mol-1 K(s) + ½ Cl2(g) → KCl(s) -437 kJ mol-1 K(g) → K+(g) + e– ΔH IE1 Cl2(g) → 2Cl(g) 244 kJ mol-1 K+(g) + Cl–(g) → KCl(s) -717 kJ mol-1arrow_forwardUse the following data and the Born-Haber cycle to calculate the first ionization energy (ΔH IE1) of K(g) K(s) → K(g) 89 kJ mol-1 Cl(g) + e– → Cl–(g) -349 kJ mol-1 K(s) + ½ Cl2(g) → KCl(s) -437 kJ mol-1 K(g) → K+(g) + e– ΔH IE1 Cl2(g) → 2Cl(g) 244 kJ mol-1 K+(g) + Cl–(g) → KCl(s) -717 kJ mol-1 Use the bond energies listed in the table below to estimate the standard enthalpy of the reaction: CCl3CHCl2(g) + 2HF(g) → CCl3CHF2(g) + 2HCl(g) C – H 412 kJ mol-1 C – C 348 kJ mol-1 C – Cl 338 kJ mol-1 H – Cl 431 kJ mol-1 C – F 484 kJ mol-1 H – F 565 kJ mol-1arrow_forwardA hydrogen-like ion is an ion containing only one electron. The energies of the electron in a hydrogen-like ion are given by (2.180 × 10-¹5 1) 2² (1) J) E = kJ where n is the principal quantum number, and Z is the atomic number of the element. Calculate the ionization energy, in your answer to 4 significant digits. mol Note: Reference the Fundamental constants table for additional information. ·2+ of the Li²+ ion. Round Iarrow_forward
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