Mixing SbCl 3 and GaCl 3 in a one-to-one ratio gives a solid ionic compound of empirical formula GaSbCl 6 . A controversy erupts over whether this compound is [SbCl 2 ] + [GaCl 4 ] ─ or [GaCl 2 ] + [SbCl 4 ] ─ . It is learned that the cation in the compound has a bent structure. Based on this fact, which combination is more likely to be correct? Explain.

Mixing SbCl 3 and GaCl 3 in a one-to-one ratio gives a solid ionic compound of empirical formula GaSbCl 6 . A controversy erupts over whether this compound is [SbCl 2 ] + [GaCl 4 ] ─ or [GaCl 2 ] + [SbCl 4 ] ─ . It is learned that the cation in the compound has a bent structure. Based on this fact, which combination is more likely to be correct? Explain.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter8: The Periodic Table: Structure And Trends

Section: Chapter Questions

Problem 8.97QE

See similar textbooks

Similar questions

Two fourth-period atoms, one of a transition metal, M, and the other of a main-group nonmetal, X, form a compound with the formula M2X3. What is the electron configuration of atom X if M is Fe? What is the configuration of X if M is Co, if X is the same then give the full electron configuration for the Co ion.
Iron(III) sulfate [Fe2(SO4)3] is composed of Fe3+ and SO4 2− ions. Explain why a sample of iron(III) sulfate is uncharged.
1) How does the octet rule explain the formation of a chloride ion? a) What noble gas is isoelectronic with the chloride ion? b) Why are Group 17 (7A) elements found in many compounds but not group 18 (8A) elements?
Using the following thermodynamic data, calculate the lattice enthalpy of lithium oxide: Li(g) → Li*(g) + e* AH₁= 540 kJ /mol Li(s) → Li(g) AHS= +146 kJ/mol O₂(s) → 20(g) AH₂= +488 kJ /mol O(g) + 1e →→ O(g) AHA1= -142 kJ /mol O` (g) + 1e¯ → 0²-(g) AHÃ₂= +844 kJ /mol 2Li(s) + 1/2O₂(g) → Li₂O(s) AH₁= -586 kJ /mol NOTE: Give your answer in kJ mol-¹
a) The element Xenon (Xe) is rarely forming compounds. By knowing its position in the periodic table. Explain why?
Write the electron configurations for: Calcium ion in CaCl₂:
Nitrous oxide, N2O, has the following structure. Which bond in N2O is a coordinate covalent bond? Explain.
Use Born-Mayer equation to calculate the lattice energy for PbS (it crystallizes in theNaCl structure). Then, use the Born–Haber cycle to obtain the value of lattice energy for PbS.You will need the following data following data : ΔH Pb(g) = 196 kJ/mol; ΔHf PbS = –98kJ/mol; electron affinities for S(g)→S- (g) is -201 kJ/mol; ) S- (g) →S2-(g) is 640kJ/mol. Ionizationenergies for Pb are listed in Resource section 2, p.903. Remember that enthalpies of formationare calculated beginning with the elements in their standard states (S8 for sulfur). Diatomicsulfur, S2, is formed from S8 (ΔHf: S2 (g) = 535 kJ/mol. Can you just do the Born-Haber part?
(b) Consider the following energy changes:
Nitrogen ions tend to have a charge of 3-; explain the reason for this pattern/trend.
4. Referring to a periodic table, arrange the following atoms in order of increasing atomic radius, ionization energy and electronegativity: P, Si, N?
Calculate the second ionization energy of the metal M (AHion2 in kJ/mol) using the following data: Lattice enthalpy of MO(s), AH = -2278 kJ/mol Bond dissociation enthalpy of O2(g) = +498 kJ/mol First electron affinity of O = -141 kJ/mol Second electron affinity of O = +744 kJ/mol Enthalpy of sublimation of M = + 125 kJ/mol First ionization energy of M = + 309 kJ/mol Standard enthalpy of formation of MO(s), AH = -341 kJ/mol