Concept explainers
Interpretation:
Out of anions
Concept Introduction:
Three-dimensional array of ions constitute the ionic compound lattice. They are stabilized because of attractive forces between oppositely charged ions that lower the potential energy.
Stability of ionic compound depends upon two factors and that is size and charge. Higher the charge and less will be the stability of ionic compound and vice-versa. Smaller the size of anion more will be the stability
Lower is the potential energy of interaction and more stable is the ionic solid. Hence the compounds that have high charge density on small space are most stable ionic solids. For example, calcium phosphate is made up of
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CHEM PRINCIPLES LL W/ACHIEVE ONE-SEM
- 19. :O: || :0-N- O: Which of the following statements, if true, would support the claim that the NO3 ion, represented above, has three resonance structures? (A) The NO3 ion is not a polar species. (B) The oxygen-to-nitrogen-to-oxygen bond angles are 90°. (C) One of the bonds in NO3 is longer than the other two. (D) One of the bonds in NO3¯ is shorter than the other two.arrow_forwardWhich of these statements about resonance is true?(a) When you draw resonance structures, it is permissibleto alter the way atoms are connected.(b) The nitrate ion has one long N¬O bond and two shortN¬O bonds.(c) “Resonance” refers to the idea that molecules areresonating rapidly between different bonding patterns.(d) The cyanide ion has only one dominant resonancestructure.(e) All of the above are true.arrow_forwardCalculate the lattice energy,U (in kJ), of the fictitious compound, MCl2, given the following information: ΔHppt for MCl2 = 17.1 kJ/mol, ΔHhyd for M2+ = -450 kJ/mol, ΔHhyd for Cl- = -370 kJ/mol Your answer should have 4 sig figs.arrow_forward
- Which compound in each of the following pairs has the larger lattice energy? Note: Mg2+ and Li+ have similar radii; O2– and F– have similar radii. Explain your choices.(a) MgO or MgSe(b) LiF or MgO(c) Li2O or LiCl(d) Li2Se or MgOarrow_forwardThe attractive force between a pair of Sr2+ and O2- ions is 1.52 x 108 N and the ionic radius of O2- ions is 0.134 nm. Calculate the ionic radius of the Sr2+ ion. (Given: Electron charge, e = 1.6 x 101ºC, the permittivity of free space, Eo = 8.85 x 101ºC²N'm²)arrow_forwardArrange the following in the order of the property indicated for each set–(a) F2, Cl2, Br2, I2(Increasing bond dissociation energy).(b) HF, HCl, HBr, HI (decreasing acid strength).(c) NH3, PH3, ASH3, SbH3, BiH3(decreasing base strength).arrow_forward
- Three main group elements, X, Y and Z, from three different groups inthe Periodic Table, each form a neutral trifluoride, i.e. XF3, YF3 andZF3. (a) To which three groups of the Periodic Table could the elementsX, Y and Z belong? Are any of these atoms X, Y or Zhypervalent in the trifluorides formed? (b) Use VSEPR theory to deduce the shapes of the molecules XF3,YF3 and ZF3, showing full working, and sketch these shapes (c) Only two of the three trifluorides have a non-zero dipole moment.For these molecules to which groups of the Periodic Table do thecentral atoms belong?arrow_forwardSulfur tetrafluoride (SF4) reacts slowly with O2 to form sulfurtetrafluoride monoxide (OSF4) according to the followingunbalanced reaction: SF4(g) + O2(g)---->OSF4(g)The O atom and the four F atoms in OSF4 are bonded to acentral S atom. (a) Balance the equation. (b) Write a Lewisstructure of OSF4 in which the formal charges of all atomsare zero. (c) Use average bond enthalpies (Table 8.3) to estimatethe enthalpy of the reaction. Is it endothermic or exothermic?(d) Determine the electron-domain geometry ofOSF4, and write two possible molecular geometries for themolecule based on this electron-domain geometry. (e) Foreach of the molecules you drew in part (d), state how manyfluorines are equatorial and how many are axial.arrow_forwardWhich compound in each of the following pairs has the larger lattice energy? Note: Ba2+ and K+ have similar radii; S2– and Cl– have similar radii. Explain your choices.(a) K2O or Na2O(b) K2S or BaS(c) KCl or BaS(d) BaS or BaCl2arrow_forward
- . Calculate the lattice energy of Li₂O(S). (AH(sublimation) K(s) = 77 kJ/mole, and AHƒ (Li₂O(s)) = −361 kJ/mole)arrow_forwardCommon exceptions to the octet rule are compounds and polyatomic ions with central atoms having more than 8 electrons around them. Phosphorus pentafluoride, PF5; sulfur tetrafluoride, SF4; xenon tetrafluoride, XeF4; and tri-iodide ion, I3, are all examples of exceptions to the octet rule. (a) Draw the Lewis structures of these substances.(b) For which elements in these substances can theatoms have more than 8 electrons around them?(c) How can the atoms of the elements youidentified in Part (b) be surrounded by morethan 8 electrons?arrow_forwardCalculate the lattice enthalpy for RbC1. You will need the following information: Species AfH°, kJ/mol Rb(g) RbCl(s) Cl(g) 80.9 - 435.4 121.3 Enthalpy of ionization for Rb(g) is 403.0 kJ/mol; electron attachment enthalpy for Cl(g) is −349.0 kJ/mol. Lattice enthalpy = kJ/molarrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning