Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory
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- What tripositive ion has the electron configuration 3Kr4 4d3?
Problem 45
- There are two elements in the transition-metal series Sc through Zn that have four unpaired electrons in their 2+ ions. Identify them.
Problem 46
- Which element in the transition-metal series Sc through Zn has five unpaired electrons in its +3 ion?
Problem 47
- Which atom or ion in the following pairs would you expect to be larger? (c) O-or O2-
Problem 48
- Which atom or ion in the following pairs would you expect to be larger? (c) Cr3+ or Cr6+
Problem 49
- Order the following ions from smallest to largest: Sr2+, Se2-, Br-, Rb+.
Problem 50
- Order the following ions from smallest to largest: Mg2+, O2-, F-, Na+.
Problem 51
- Which ion has a larger atomic radius, Cu+ or Cu2+? Explain your reasoning.
Problem 52
- Which ion has a larger atomic radius, Fe2+ or Fe3+? Explain your reasoning.
Problem 53
- The following ions all have the same number of electrons: Ti4+, Sc3+, Ca2+, S2-. Order them according to their expected sizes, and explain your answer.
Problem 54
- Which of the ions Se2-, F-, O2-, and Rb+ has the largest radius?
Problem 55
- Which group of elements in the periodic table has the largest first ionization energy (Ei1), and which group has the smallest? Explain.
Problem 56
- Which element in the periodic table has the smallest ionization energy? Which element has the largest ionization energy?
Problem 57
- Which element in each of the following sets has the smallest first ionization energy, and which has the largest? (a) Li, Ba, K (b) B, Be, Cl (c) Ca, C, Cl
Problem 58
- Order the elements in each set from the smallest to largest first ionization energy. (a) Na, I, P (b) P, Sr, Mg (c) Ca, Cs, Se
Problem 59
Problem 61a
(a) Which has the smaller fourth ionization energy, Sn or Sb?
Problem 61b
(b) Which has the larger sixth ionization energy, Se or Br?
- Three atoms have the following electron configurations: (a) 1s2 2s2 2p6 3s2 3p3 (b) 1s2 2s2 2p6 3s2 3p6 (c) 1s2 2s2 2p6 3s2 3p6 4s2 Which of the three has the largest Ei2? Which has the smallest Ei7?
Problem 62
- Three atoms have the following electron configurations: (a) 1s2 2s2 2p6 3s2 3p1 (b) 1s2 2s2 2p6 3s2 3p5 (c) 1s2 2s2 2p6 3s2 3p6 4s1. Which of the three has the largest Ei1? Which has the smallest Ei4?
Problem 63
- The first four ionization energies in kJ/mol of a certain second-row element are 801, 2427, 3660, and 25,025. What is the likely identity of the element?
Problem 64
- What is the likely identity of the second-row element with the first four ionization energies of 900, 1757, 14,849, and 21,007 kJ/mol?
Problem 65
- What is the relationship between the electron affinity of a singly charged cation such as Na+ and the ionization energy of the neutral atom?
Problem 66
- What is the relationship between the ionization energy of a singly charged anion such as Cl- and the electron affinity of the neutral atom?
Problem 67
- Which has the more negative electron affinity, Na or Cl?
Problem 68
- Which has the more negative electron affinity, Br or Br⁻?
Problem 69
- Why is energy usually released when an electron is added to a neutral atom but absorbed when an electron is removed from a neutral atom?
Problem 70
- Why does ionization energy increase regularly across the periodic table from group 1A to group 8A, whereas electron affinity increases irregularly from group 1A to group 7A and then falls dramatically for group 8A?
Problem 71
- Water superheated under pressure to 200 °C and 750 atm has Kw = 1.5 * 10-11. What is 3H3O+ 4 and 3OH-4 at 200 °C? Is the water acidic, basic, or neutral?
Problem 72
- Why does phosphorus have a less negative electron affinity than its neighbors silicon and sulfur?
Problem 73
Problem 74a,c,d
What noble-gas configurations and charge are the following elements likely to attain in reactions in which they form ions? (a) N (c) S (d) Br