Concept explainers
(a)
Interpretation:
The reason behind the greater lattice energy of LiCl than LiBr has to be determined.
Concept Introduction:
The magnitude of the lattice energy for any given ionic solid is determined by equation written as follows:
Here,
k is a constant.
r is their distance of separation in the compound.
Energy is released if the particles come together and have opposite signs for their charges. It is an exothermic process.
Energy is absorbed if the charges are of the same sign on the particles. It is an endothermic process.
Two main factors that contribute to the magnitude of the lattice energy are the charge and radius of the bonded ions.
The effect of those factors is as follows:
1. If the charge of the ions increases, the lattice energy increases.
2. If the size of the ions increases, the lattice energy decreases.
If charges are constant, the lattice energies for ionic solids that consist of smaller ions are higher than those of larger ions. The smaller the ionic radii, the closer the ions are to each other and hence the larger the attractive force between the ions.
(b)
Interpretation:
The reason behind greater lattice energy of
Concept Introduction:
The magnitude of the lattice energy for any given ionic solid is determined by equation written as follows:
Here,
k is a constant.
r is their distance of separation in the compound.
Energy is released if the particles come together and have opposite signs for their charges. It is an exothermic process.
Energy is absorbed if the charges are of the same sign on the particles. It is an endothermic process.
Two main factors that contribute to the magnitude of the lattice energy are the charge and radius of the bonded ions.
The effect of those factors is as follows:
1. If the charge of the ions increases, the lattice energy increases.
2. If the size of the ions increases, the lattice energy decreases.
If charges are constant, the lattice energies for ionic solids that consist of smaller ions are higher than those of larger ions. The smaller the ionic radii, the closer the ions are to each other and hence the larger the attractive force between the ions.
Want to see the full answer?
Check out a sample textbook solutionChapter 9 Solutions
Chemistry: Principles and Practice
- One of the following pictures(Figure 1) represents NaCl and one represents MgO. Which is which? (a) is NaCl and (b) is MgO (b) is NaCl and (a) is MgO Which has the larger lattice energy? NaCl MgOarrow_forwardAn ionic compound of formula XY2 (X = cation with two positive charges, Y = anion with one negative charge) has the following mass composition: Mg 10.9%, Cl 31.8%, O57.3%. (a) What is the chemical formula and name of the compound? (b) Give the most probable Lewis structure for the ions contained in the compound.arrow_forwardWrite the Lewis structures for the following, and include resonance structures where appropriate. Indicate which has the strongest carbon-oxygen bond.(a) CO2(b) COarrow_forward
- Two substances with empirical formula HNO are hyponi-trous acid ( μ=62.04 g /mol) and nitroxyl (μ=31.02 g/mol).(a) What is the molecular formula of each species?(b) For each species, draw the Lewis structure having the lowestformal charges. (Hint:Hyponitrous acid has an N=N bond.)(c) Predict the shape around the N atoms of each species.(d) When hyponitrous acid loses two protons, it forms the hy-ponitrite ion. Draw cisand transforms of this ion.arrow_forward(c) Draw the orbital diagrams and Lewis symbols to depict the formation of Na* and CI ions from the atoms. Give the formula of the compound formed. (d) The predicted bond length for HF is 109 pm (the sum of the covalent radii of H, 37 pm and F. 72 pm), however the actual bond length for HF is shorter (92 pm). It was observed that the difference between predicted and actual bond lengths becomes smalleor going down the halogen group from HF to HI Describe these observationsarrow_forwardNa+ forms an “ionic bond” (i.e. an electrostatic attraction) with the OCN− ion. (a) Draw the full Lewis structure of the ionic compound. Be sure to show how you have derived this. (b) Which atom in the OCN− anion is the sodium cation most likely to attract? Explain.arrow_forward
- Write electron configurations and Lewis structures for each element. Indicate which of the electrons in the electron configuration are shown in the Lewis structure.(a) Ca(b) Ga(c) As(d) Iarrow_forwardiv. Assign formal charges to the atoms in the following structures and decide which the more important contributor to the resonance hybrid is. (a) (b) H H C=N=N c-N=N H H v. What factor accounts for each of the following differences in bond length? (a) I, has a longer bond than Br,. (b) C-N bonds are shorter than C-C bonds. (c) H-C bonds are shorter than the C-O bond. (d) The C-O bond in formaldehyde, H,C=0, is longer than the bond in carbon monoxide, C=0.arrow_forwardWhich 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_forward
- An elemental analysis of a hydrocarbon, which contains only carbon and hydrogen, shows the mass%: element mass% carbon 92.26 hydrogen 7.743 (A) * Determine the empirical formula of the hydrocarbon. (B) The compound has a molar mass of 26.04 g/mol. Determine its molecular formula. (C, Draw the Lewis structure of the molecular compound. Count the total number of sigma bonds and pi bonds each, present in the molecule. (D, What is the hybridization of carbon in the molecule? Explain.arrow_forwardUse Lewis electron-dot symbols to represent the formationof (a) BrF₃ from bromine and fluorine atoms; (b) AlF₃ from alu-minum and fluorine atoms.arrow_forwardThe cyanate ion, NCO– , has three (3) possible Lewis structures. (a) Draw these three structures and assign formal charges in each. (b) Which Lewis structure is dominant?arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY