Interpretation:
Whether a cesium atom transfers an electron to a chlorine atom to form isolated
Concept introduction:
Ionization energy is amount of energy needed to eliminate electron from isolated, neutral gaseous atom. It is denoted by
Change in energy when electron is added to neutral isolated atom of gas is called
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CHEMISTRY-TEXT
- What is the electron configuration of the Ba3+ ion? Suggest a reason why this ion is not normally found in nature.arrow_forwardCompare the electron affinity of fluorine to the ionization energy of sodium. Does the process of an electron being pulled from the sodium atom to the fluorine atom have a negative or a positive E? Why is NaF a stable compound? Does the overall formation of NaF have a negative or a positive E? How can this be?arrow_forwardOf the five elements Sn, Si, Sb, O, Te, which has the most endothermic reaction? (E represents an atom.) What name is given to the energy for the reaction? E(g)E+(g)+earrow_forward
- The lattice energy of an ionic solid such as NaCl is the enthalpy change H for the process in which the solid changes to ions. For example, NaCl(s)Na+(g)+Cl(g)H=786kJ/mol Assume that the ionization energy and electron a affinity are H values for the processes defined by those terms. The ionization energy of Na is 496 kJ/mol. Use this, the electron affinity from Table 8.4, and the lattice energy of NaCl to calculate H for the following process: Na(g)+Cl(g)NaCl(s)arrow_forwardThe lattice energy of potassium iodide is the energy required for the following reaction. KI(s) → K+(g) + I−(g) ΔHrxn = ΔHlattice Use the Born-Haber cycle to calculate ΔHlattice for KI(s) from the information given below. Equation 1: 2 K(s) + I2(g) → 2 KI(s) ΔH1 = −655 kJ/mol Equation 2: K(s) → K(g) ΔH2 = 89 kJ/mol Equation 3: I2(g) → 2 I(g) ΔH3 = 214 kJ/mol Equation 4: K(g) → K+(g) + e− ΔH4 = 419 kJ/mol Equation 5: I(g) + e− → I−(g) ΔH5 = −294 kJ/molarrow_forwardCalculate the lattice energy of NaBr(s), given the following thermochemical equations, where A/E and AEA are ionization energy and electron affinity, respectively. Na(s)Na(g) AH = +107 kJ Na(g) Nat(g) + e A/E = +496 kJ -> 1/2 Br₂(g) → Br(g) AHf = +112 kJ - Br(g) + e¯ → Br¯(g) AEA = -325 kJ Na(s) + 1/2 Br₂(g) → NaBr(s) AH = -361 kJ ->> - -1401 kJ -751 kJ +29 kJ -29 kJ +751 kJarrow_forward
- 3. Of the elements Nd, Al, and Ar, which will readily form(s) +3 ions? Why? 4. The atomic radii of Na and Cl are 190 and 79 pm, respectively, but the distance between sodium and chlorine in NaCl is 282 pm. Explain this discrepancy.arrow_forwardWrite electron configurations for the following ions of main group elements: (a) N3−, (b) Ba2+, and (c) Be2+.arrow_forward8. Given the following information: Li(s) HI(g) → H(g) + I(g) enthalpy of sublimation of Li(s) = 166 kJ/mol bond energy of HI = 295 kJ/mol Li(g) Li(g) → Li"(g) + e ionization energy of Li(g)= 520. kJ/mol I(g) + e — Г(g) electron affinity of I(g) = -295 kJ/mol Li"(g) + I(g) → LiI(s) lattice energy of LiI(s) = -737 kJ/mol H2(g) → 2H(g) Calculate the change in enthalpy for: bond energy of H2 = 432 kJ/mol 2Li(s) + 2HI(g) –→ H2(g) + 2LİI(s) a. 330 kJ b. –534 kJ c. -483 kJ d. -984 kJ e. none of thesearrow_forward
- Consider an ionic compound, MXMX, composed of generic metal MM and generic, gaseous halogen XX. The enthalpy of formation of MXMX is Δ?∘f=−411ΔHf∘=−411 kJ/mol. The enthalpy of sublimation of MM is Δ?sub=101ΔHsub=101 kJ/mol. The ionization energy of MM is IE=461IE=461 kJ/mol. The electron affinity of XX is Δ?EA=−325ΔHEA=−325 kJ/mol. (Refer to the hint). The bond energy of X2X2 is BE=189BE=189 kJ/mol. Determine the lattice energy of MXMX.arrow_forwardConsider a hypothetical ionic compound AB (comprised of A* and B ions). Given the following enthalpy data and using a Born-Haber cycle calculation, predict AHiattice in kJ mol. AG) + Bs) - AB 4H = -384 kJ mol As) → Ag) ArH = 105 kJ mol B(s) - Bg) A,H = 101 kJ mol1 First ionization energy of Ag) = 501 kJ mol" Answes=? Electron affinity enthalpy of Bro (exothermic) = -348 kJ molarrow_forwardwhat is be2+ valence electron configuration?arrow_forward
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