General Chemistry
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Refer to the illustration below.
(i) Identify the sphere that depicts a metal atom and the sphere that depicts a nonmetal atom.
(ii) Among the products, identify the spheres that depict a cation and the sphere that depicts an anion.
Identify the ion that has a smaller radius, Co2+ or Co3+. Justify your answer.
What is the difference between the predicted and experimentally measured ion-ion distances for LiI, NaBr, KCl, and RbF if their measured cation-anion distances were 2.94 pm (Li–I), 2.90 pm (Na–Br), 3.20 pm (K–Cl), and 2.88 pm (Rb–F), respectively? (Hint: Use the given image to calculate the predicted ion-ion distances)
Give an explanation as to why Br is smaller than Br–.
Neutral atoms are smaller in size compared to their anion forms. Is this statement true or false?
List the following from largest to smallest size: Sb, Sb3+, Sb3–.
Consider the elements Na, F, O
Order of atomic size: F < O < NaOrder of ionic size: Na+ < F– < O2–
Which of the following statement best explains the difference in the orders of the ionic and atomic sizes?
The relative ionic sizes of Be2+, Na+, F–, and S2– are shown below. In between which ions would you place Mg2+ and O2– ions?
The cation-anion distance in KBr is experimentally determined to be 330 pm. The atomic radius and ionic radius are given below:
Atomic radius (pm)K 203Br 120
Ionic radius (pm)K+ 152Br– 182
Which would be a more accurate estimation of the ionic cation-anion distances, the atomic radius or ionic radius?
Calculate the cation-ion distance for the following compounds: MgS, CaO, SrO. The ionic radii of some elements are given below:
Ion Ionic Radius (pm)Be2+ 59Mg2+ 86Ca2+ 114Sr2+ 132O2– 126S2– 170Se2– 184Te2– 207
Rank the following isoelectronic ions from largest to smallest size: Al3+, O2–, N3–, Na+.
Identify the element/ion that is larger in size in each of the following sets:
a. S or S2–b. N– or N+c. Ba or Ba2+d. Cu– or Cu2+
Which of the following cations has the smallest radius?
Which of the following options below show the isoelectronic ions in order of decreasing radii?
a. Cl – > Br – > F –
b. S2- > Cl – > Ar
c. Ca2+ > Na + > Ar
d. Ca2+ > Sr 2+ > Mg2+
LiCl, NaF, KBr, RbI
The experimentally measured cation-anion distances are: LiCl = 2.50 Å; NaF = 2.31 Å; KBr = 3.30 Å and RbI = 3.67 Å
Use the diagram below to determine the theoretical cation-anion distances for the ionic compounds above.
Provide a brief explanation for each of the following.
Cl- is larger than Ar.
K+ is larger than Na+.
True or false: S is larger than S2–.
Arrange this isoelectronic series in order of increasing atomic radius: Se2-, Sr2+, Rb+, Br-.
Which is the larger species in each pair?
a. Mg or Mg2+
b. Fe- or Fe2+
c. Nb- or Nb5+
d. Se or Se2-