(a)
Interpretation:
The increasing order of radius of given pairs have to be arranged and the same has to be explained.
Concept introduction:
The distance from centre of nucleus to the valence shell electron of an atom or ion is called atomic or ionic radius.
Radius of parent atom is always higher than the size of cation.
Radius of parent atom is always smaller than the size of anion due to the effective nuclear charge.
(b)
Interpretation:
The increasing order of radius of given pairs have to be arranged and the same has to be explained.
Concept introduction:
The distance from centre of nucleus to the valence shell electron of an atom or ion is called atomic or ionic radius.
Radius of parent atom is always higher than the size of cation.
Radius of parent atom is always smaller than the size of anion due to the effective nuclear charge.
Want to see the full answer?
Check out a sample textbook solutionChapter 9 Solutions
OWLv2 for Ebbing/Gammon's General Chemistry, 11th Edition, [Instant Access], 1 term (6 months)
- Arrange the following species in the order of decreasing ionic radii. Explain your answer. Ar, P3, K, Ca, S2-arrow_forwardConsider an ionic compound, MXMX, composed of generic metal MM and generic, gaseous halogen XX. The enthalpy of formation of MXMX is Δ?∘f=−411ΔHf∘=−411 kJ/mol. The enthalpy of sublimation of MM is Δ?sub=101ΔHsub=101 kJ/mol. The ionization energy of MM is IE=461IE=461 kJ/mol. The electron affinity of XX is Δ?EA=−325ΔHEA=−325 kJ/mol. (Refer to the hint). The bond energy of X2X2 is BE=189BE=189 kJ/mol. Determine the lattice energy of MXMX.arrow_forwardConsider an ionic compound, MXMX, composed of generic metal MM and generic, gaseous halogen XX. The enthalpy of formation of MXMX is Δ?∘f=−553ΔHf∘=−553 kJ/mol. The enthalpy of sublimation of MM is Δ?sub=129ΔHsub=129 kJ/mol. The ionization energy of MM is IE=491IE=491 kJ/mol. The electron affinity of XX is Δ?EA=−325ΔHEA=−325 kJ/mol. (Refer to the hint). The bond energy of X2X2 is BE=219BE=219 kJ/mol. Determine the lattice energy of MXMX. Δ?lattice=ΔHlattice= kJ/molarrow_forward
- Which of the following species has the smallest ionic radius? S2- CI- A13+ D Na+ Mg2+arrow_forwardFill in the orbital energy diagram for the nitride ion. E 2s 1s 2parrow_forwardConsider an ionic compound, MXMX, composed of generic metal MM and generic, gaseous halogen XX. The enthalpy of formation of MXMX is Δ?∘f=−553ΔHf∘=−553 kJ/mol. The enthalpy of sublimation of MM is Δ?sub=105ΔHsub=105 kJ/mol. The ionization energy of MM is IE=483IE=483 kJ/mol. The electron affinity of XX is Δ?EA=−307ΔHEA=−307 kJ/mol. (Refer to the hint). The bond energy of X2X2 is BE=213BE=213 kJ/mol. Determine the lattice energy of MXMX. Δ?lattice=ΔHlattice= kJ/molarrow_forward
- Arrange the members in order of increasing size. Sc3+, Ca2+, Ti4+arrow_forwardRank the following five ions in order of decreasing radius. Use the periodic table as necessary. Rank from largest to smallest radius. To rank items as equivalent, overlap them. F− Cl− Br− I− At−arrow_forwardArrange these ions according to ionic radius. Ca2+, K+, Cl-, S^2-, P^3-arrow_forward
- Arrange the members in order of increasing size. K+, Li+, Rb+arrow_forwardConsider an ionic compound, MX3, composed of generic metal M and generic gaseous halogen X. The enthalpy of formation of MX3 is ΔHf∘=−965 kJ/mol. The enthalpy of sublimation of M is ΔHsub=123 kJ/mol. The first, second, and third ionization energies of M are IE1=557 kJ?mol, IE2=1751 kJ/mol, and IE3=2731 kJ/mol. The electron affinity of X is ΔHEA=−339 kJ/mol The bond energy of X2 is BE=235 kJ/mol. Determine the lattice energy of MX3.arrow_forwardSome of the batteries currently used in your smartphone contain lithium ions (Li +) as their electricity conductors. Currently, researchers are also developing batteries that use sodium ions (Na +) as a substitute for lithium ions due to their abundance in nature. Of course, lithium (Li) and sodium (Na) atoms have different properties due to their different electronic structures. Compare the radius sizes of the following atoms and ions: -Li and Na -ion Li + and Li -ion Li + and Na + ions. 2. How does the first ionization energy change from lithium to sodium? Is it getting bigger or smaller? Explain why.arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning