Answered: The atomic radii of Na* and Cl" ions…

The atomic radii of Na* and Cl" ions are 0.190 nm and 0.079 nm, respectively. What is their equilibrium interionic separation distance? 0.111 nm 0.269 nm 0.079 nm 0.190 nm

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter8: Molecules And Materials

Section: Chapter Questions

Problem 8.22PAE

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Calculate the lattice energy of ionic solid MX, given the following thermodynamic data: M(s) + X2(9) → MX(s) AHræn M(s) → M(g) AHrän= 88. kJ Bond energy of X2 = 196. kJ/mol lonization energy for M(s) = 485. kJ /mol Electron affinity of X = -281. kJ/mol AHrxn = -616. Enter your answer in decimal notation, rounded to the appropriate number of significant figures.
7. During a lab, a student filled in the following table regarding three unknown substances that could be jonic, molecular/covalent or metallic. Determine the type of bond based on the data: Appearance at room temperature Fine white solid crystals Conductivity of aqueous solution Melting point (high or low) Solubility in Conductivity of solid Type of Bond in substance Unknown water Non- A Soluble conductive High conductive Non- White solid shiny crystals Dull hard grey solid strip with shiny interior. Malleable. Non- B. Soluble Low conductive conductive Non- High insoluble high conductive conductivity
Equations 7.1a and 7.1b, expressions for Burgers vectors for FCC and BCC crystal structures, are of the form b = uvw) where a is the unit cell edge length. Also, since the magnitudes of these Burgers vectors may be determined from the following equation: 1/2 + v? + w²)" determine values of |b| for aluminum and chromium. You may want to consult Table 3.1. Part 1 Incorrect. Review Section 3.4 and Example Problem 3.1. It may help you to review your homework from Chapter 3. Review the relationships between the unit cell length and the atomic radius.lf you are having difficulty with this problem, you may wish to review: Solving Equations, Equations, Symbols and Units, Review of 2D and 3D Geometry. What is a, the unit cell length, in nm, for aluminum? a = i nm
Calculate the lattice energy of KCI(s) using the following thermodynamic data (all data is in kJ/mol) K(s) AHsublimation = 69 kJ/mol K(g) Ionization energy = 399 kJ/mol CI-CI(g) Bond energy = 223 kJ/mol Cl(g) Electron affinity = -369 kJ/mol KCI(s) AH°r= -457 kJ/mol kJ/mol
The distance between the centers of the Lit and F ions is 143 pm. Determine the energy of interaction between the pair of ions for a mole of Lit and F (Hint: use k = 4TE0 -527 kJ/mol -892 kJ/mol -613 kJ/mol -488 kJ/mol -973 kJ/mol
A student investigates the physical and chemical properties of various carbon-containing compounds. Thr complete Lewis electron-dot diagrams and boiling points for two compounds, Q and Z, are shown in the following table: B) Any C — H bond in compound Q is shorter than the S — H bond in compound Z. Explain the reason for this difference using principles of atomic structure.
Given the data below (taken from standard data tables), calculate the crystal lattice energy for sodium oxide: (remember to ALWAYS enter units as well as numerical values) ΔHf° (Na2O(s) ) = –413 kJ/mol E.A.1(O) = –133 kJ/mol E.A.2(O) = 247 kJ/mol B.D.E. (O2) = 495 kJ/mol I.E.1(Na) = 495.5 kJ/mol I.E.2(Na) = 4562 kJ/mol I.E.3(Na) = 6912 kJ/mol ΔHsub° (Na) = 105 kJ/mol
Use a Born-Haber cycle (Sec. 5-13) to calculate the lattice energy of MgF2 using these thermodynamic data. Compare this lattice energy with that of SrF2, −2496 kJ/mol. Explain the difference in the values in structural terms.
Which of the following molecules or ions contain polar bonds? (a) O3 (b) S8 (c) O22 (d) NO3 (e) CO2 (f) H2S (g) BH4
Data are given in Appendix 1 for white phosphorus, P4(s). P4(g) has the following thermodynamic values: Hf=58.9kJ/mol , S=280.0J/kmol . What is the temperature at which white phosphorus sublimes at 1 atm pressure?
10. Calculate the energy for vacancy formation in copper, given that the equilibrium number of vacancies at 1000° C (1273 K) is 2.2 x 1025 m³. The atomic weight and density (at 1000° C) for copper are, respectively, 63.5 g/mol and 8.4 g/cm³. Where: IIIIII - N₁ = Nexp exp(-X). KT N Q T N = N₁ P/Ncu is the total number of atomic sites. is the energy required for the formation of a vacancy is the absolute temperature in kelvins k is the gas or Boltzmann's constant = 8.62 x 105 eV/atom-K. NA is Avogadro's number 6.022 x 1023 atoms/mol P is the atomic density New is Atomic weight for copper. 2
3

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