Based on the radius ratio rules what is the predicted (i) coordination number and (ii) geometry of the cation in the following compounds (a) KBr (b) MgTe The radii of the ions are in (pm): K+ = 138 Br= 196 Mg2+ %3D %3D = 72 Te2= 221 %3D %3D (a) KBr: CN=. ....and geometry is.... (b) Mg Te: CN=. .and geometry is....

Based on the radius ratio rules what is the predicted (i) coordination number and (ii) geometry of the cation in the following compounds (a) KBr (b) MgTe The radii of the ions are in (pm): K+ = 138 Br= 196 Mg2+ %3D %3D = 72 Te2= 221 %3D %3D (a) KBr: CN=. ....and geometry is.... (b) Mg Te: CN=. .and geometry is....

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter3: Atomic Shells And Classical Models Of Chemical Bonding

Section: Chapter Questions

Problem 25P

See similar textbooks

Similar questions

3. On the basis of ionic charge and ionic radii given in Table 1, predict crystal structures for the following materials: ( a. CaO (b) MnS (c) KBr (d) CsBr b. Justify your selections. Table 1: Ionic Radii for Several Cations and Anions Ionic Radius (am) Ionic Cation Radius (nm) Anion 0.053 Br 0.196 Ba?+ Ca?+ 0.136 0.181 0.100 F 0.133 Cs* 0.170 0.220 Fe2+ 0.077 0.140 Fe 0.069 0.184 K* 0.138 Mg Mn2* 0.072 0.067 Na* 0.102 Ni+ 0.069 Sit+ 0.040 0.061
Mixing SbCl3 and GaCl3 in a 1;1 molar ratio (usingliquid sulfur dioxide as a solvent) gives a solid ioniccompound of empirical formula GaSbCl6. A controversyarises over whether this compound is ( ) SbCl2 + ( ) GaCl 4 - or( ) GaCl+ 2 ( ) SbCl 4 -(a) Predict the molecular structures of the two anions.(b) It is learned that the cation in the compound has abent structure. Based on this fact, which formulationis more likely to be correct?
The main reason alkali metal dihalides (MX₂) do notformis the high IE₂ of the metal. (a) Why is IE₂ so high for alkalimetals? (b) The IE2for Cs is 2255 kJ/mol, low enough for CsF₂to form exothermically (ΔHf=-125 kJ/mol). This compoundcannot be synthesized, however, because CsF forms with a muchgreater release of heat (ΔHf=-530 kJ/mol). Thus, the break-down of CsF₂ to CsF happens readily. Write the equation for thisbreakdown, and calculate the heat of reaction per mole of CsF.
In XCI, which crystallizes in CSCI structure, the sum of the anionic and cationic radii is found to be 318 pm. The density of the compound is 7.799 g cm. Calculate the mass of the cation as g mol. Do not write units, only enter numerical values. Use two digits at most for decimal numbers, use dot (.) as decimal separator (i.e. two-point-fifty-one should be entered as 2.51). Do not use comma (,) as decimal separator.
Determine the second ionization energy of calcium (in kJ mol-1) from the given data (all in kJ mol-1): AH°[CaCl,(s)] = -796 AH¡[Ca(g)] = 178 AH°[CI(g)] = 122 First ionization energy of Ca(g) = 590 Electron affinity of Cl(g) = -349 Lattice enthalpy of CaCl,(s) = -2260 А 1150 В 1235 C 1093 D 1210
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
Energy is required to remove two electrons from Ca to formCa2+, and energy is required to add two electrons to O toform O2 - . Yet CaO is stable relative to the free elements.Which statement is the best explanation? (a) The latticeenergy of CaO is large enough to overcome these processes.(b) CaO is a covalent compound, and these processes areirrelevant. (c) CaO has a higher molar mass than either Ca orO. (d) The enthalpy of formation of CaO is small. (e) CaO isstable to atmospheric conditions.
The illustrations below depict differences in orbital hy-bridization of some tellurium (Te) fluorides. (a) Which depictsthe difference, if any, between TeF₆(left) and TeF₅(right)? (b) Which depicts the difference, if any, between TeF₄(left) and TeF₆(right)?
On heating a crystal of KC1 in potassium vapour, the crystal starts exhibitinga violet colour. What is this due to?
d) Explain the following trend in the lattice energy of oxides (in kJ.mol1) assuming all have the same structure: MnO (3810), FeO (3921), CoO (3988), NiO (4071).
3. Consider [Fe(H2O)]Cl;. The bonding between iron(III) and water is best described as: (a) metallic (b) ionic (c) covalent (d) coordinate covalent
The compound gallium arsenide is a commonly used semiconductor,having an energy gap Eg of 1.43 eV. Its crystal structureis like that of silicon, except that half the silicon atoms are replacedby gallium atoms and half by arsenic atoms. Draw a flattened-outsketch of the gallium arsenide lattice, following the pattern.What is the net charge of the (a) gallium and (b) arsenic ioncore? (c) How many electrons per bond are there? (Hint: Consultthe periodic table in Appendix G.)