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Problem 33a
Consider S, Cl, and K and their most common ions. (a) List the atoms in order of increasing size.
Problem 33b,c
Consider S, Cl, and K and their most common ions. (b) List the ions in order of increasing size. (c) Explain any differences in the orders of the atomic and ionic sizes.
Problem 34
Arrange each of the following sets of atoms and ions in order of increasing size. Se2−,Te2−, Se
Problem 35c
True or false? c. S2− is larger than K+.
Problem 36b
In the ionic compounds LiF, NaCl, KBr, and RbI, the measured cation–anion distances are 2.01 Å (Li–F), 2.82 Å (Na–Cl), 3.30 Å (K–Br), and 3.67 Å (Rb–I), respectively. b. Calculate the difference between the experimentally measured ion–ion distances and the ones predicted from Figure 7.8.
Problem 36c
In the ionic compounds LiF, NaCl, KBr, and RbI, the measured cation–anion distances are 2.01 Å (Li–F), 2.82 Å (Na–Cl), 3.30 Å (K–Br), and 3.67 Å (Rb–I), respectively. c. What estimates of the cation–anion distance would you obtain for these four compounds using neutral atom bonding atomic radii? Are these estimates as accurate as the estimates using ionic radii?
Problem 38
Write the electron configurations for the following ions, and determine which have noble-gas configurations.
a. Ru3+
b. As3−
c. Y3+
d. Pd2+
e. Pb2+
f. Au3+
- Give three examples of +2 ions that have an electron configuration of nd10 (n = 3, 4, 5...).
Problem 39
Problem 40
Which of the ions Ni2+, Fe2+, Co3+, and Pt2+ has an electron configuration of 𝑛𝑑6(𝑛=3,4,5,…)?
a. Ni2+
b. Fe2+
c. Co3+
d. Pt2+
e. More than one of these
Problem 41
a. Write an equation for the second electron affinity of chlorine.
b. Would you predict a positive or a negative quantity for this process?
Problem 42
rue or false: If the electron affinity for an element is a negative number, then the anion of the element is more stable than the neutral atom.
Problem 43
Write equations that show the processes that describe the first, second, and third ionization energies of an aluminum atom. Which process would require the least amount of energy?
Problem 43a,b,c,d,e
Based on their positions in the periodic table, predict which atom of the following pairs will have the smaller first ionization energy: (a) Br, Kr (b) C, Ca (c) Li, Rb (d) S, Ge (e) Al, B.
Problem 44
Write equations that show the process for a. the first two ionization energies of lead and b. the fourth ionization energy of zirconium.
Problem 45
Which element has the highest second ionization energy: Li, K, or Be?
Problem 46
Identify each statement as true or false.
a. Ionization energies are always negative quantities.
b. Oxygen has a larger first ionization energy than fluorine.
c. The second ionization energy of an atom is always greater than its first ionization energy.
d. The third ionization energy is the energy needed to ionize three electrons from a neutral atom.
Problem 47a
Pick the correct word to complete the sentence: The larger the atom, the (smaller/larger) its first ionization energy.
Problem 47b
Which element in the periodic table has the largest first ionization energy?
- For each of the following pairs, indicate which element has the smaller first ionization energy: (a) Cs, Cl (b) Fe, Zn (c) I, Cl (d) Se, Sn.
Problem 50
Problem 51
Would a neutral K atom or a K+ ion have a more negative value of electron affinity?
- What is the relationship between the ionization energy of an anion with a 1- charge, such as F-, and the electron affinity of the neutral atom, F?
Problem 52
- Consider the first ionization energy of neon and the electron affinity of fluorine. (b) These two quantities have opposite signs. Which will be positive, and which will be negative? (c) Would you expect the magnitudes of these two quantities to be equal? If not, which one would you expect to be larger?
Problem 53
Problem 54
Consider the following equation:
Ca+(𝑔)+e−⟶Ca(𝑔)
Which of the following statements are true?
i. The energy change for this process is the electron affinity of the Ca+ ion.
ii. The energy change for this process is the negative of the first ionization energy of the Ca atom.
iii. The energy change for this process is the negative of the electron affinity of the Ca atom.
a. Only statement i is true.
b. Only statement ii is true.
c. Only statement iii is true.
d. Only statements i and ii are true.
e. All three statements are true.
- (a) Does metallic character increase, decrease, or remain unchanged as one goes from left to right across a row of the periodic table? (b) Does metallic character increase, decrease, or remain unchanged as one goes down a column of the periodic table?
Problem 55
- You read the following statement about two elements X and Y: One of the elements is a good conductor of electricity, and the other is a semiconductor. Experiments show that the first ionization energy of X is twice as great as that of Y. Which element has the greater metallic character?
Problem 56
- Discussing this chapter, a classmate says, “An element that commonly forms a cation is a metal.” Do you agree or disagree?
Problem 57
Problem 58
True or false: Because elements that form cations are metals, and elements that form anions are nonmetals, elements that do not form ions are metalloids.
Problem 59
Predict whether each of the following oxides is ionic or molecular: SnO2, Al2O3, CO2, Li2O, Fe2O3, H2O.
Problem 61
Would you expect manganese(II) oxide, MnO, to react more readily with HCl(aq) or NaOH(aq)?
Problem 62
Arrange the following oxides in order of increasing acidity: CO2,CaO,Al2O3,SO3,SiO2,P2O5.