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Problem 73b
Choose the element with the higher first ionization energy from each pair. b. Na or Rb
Problem 73c
Choose the element with the higher first ionization energy from each pair. c. As or At
Problem 73d
Choose the element with the higher first ionization energy from each pair. d. P or Sn
Problem 74
Choose the element with the higher first ionization energy from each pair. a. P or I b. Si or Cl c. P or Sb d. Ga or Ge
Problem 75
Arrange these elements in order of increasing first ionization energy: Si, F, In, N.
- Arrange these elements in order of decreasing first ionization energy: Cl, S, Sn, Pb.
Problem 76
Problem 77
For each element, predict where the 'jump' occurs for successive ionization energies. (For example, does the jump occur between the first and second ionization energies, the second and third, or the third and fourth?) a. Be b. N c. O d. Li
Problem 78
Consider this set of ionization energies. IE1 = 578 kJ/mol IE2 = 1820 kJ/mol IE3 = 2750 kJ/mol IE4 = 11,600 kJ/mol To which third-period element do these ionization values belong?
Problem 79a
Choose the element with the more negative (more exothermic) electron affinity from each pair. a. Na or Rb
Problem 79b
Choose the element with the more negative (more exothermic) electron affinity from each pair. b. B or S
Problem 79c,d
Choose the element with the more negative (more exothermic) electron affinity from each pair. c. C or N d. Li or F
Problem 80
Choose the element with the more negative (more exothermic) electron affinity in each pair. a. Mg or S b. K or Cs c. Si or P d. Ga or Br
Problem 81
Choose the more metallic element from each pair. c. Cl or O
Problem 82
Choose the more metallic element from each pair. a. Sb or Pb b. K or Ge c. Ge or Sb d. As or Sn
Problem 83
Arrange these elements in order of increasing metallic character: Fr, Sb, In, S, Ba, Se.
Problem 84
Arrange these elements in order of decreasing metallic character: Sr, N, Si, P, Ga, Al.
Problem 85
Write the balanced chemical equation for the reaction of solid strontium with iodine gas.
- Which alkali metal, based on ionization energies, would you expect to undergo the most exothermic reaction with chlorine gas?
Problem 86
Problem 87
Write the balanced chemical equation for the reaction of solid lithium with liquid water.
Problem 88
Write the balanced chemical equation for the reaction of solid potassium with liquid water.
Problem 89
Write the balanced equation for the reaction of hydrogen gas with bromine gas.
- Bromine is a highly reactive liquid while krypton is an inert gas. Explain this difference based on their electron configurations.
Problem 91
- Potassium is a highly reactive metal while argon is an inert gas. Explain this difference based on their electron configurations.
Problem 92
Problem 93
Both vanadium and its 3+ ion are paramagnetic. Refer to their electron configurations to explain this statement.
- Refer to their electron configurations to explain why copper is paramagnetic, whereas its 1+ ion is not.
Problem 94
Problem 97
Life on Earth evolved based on the element carbon. Based on periodic properties, what two or three elements would you expect to be most like carbon?
- Consider these elements: N, Mg, O, F, Al. a. Write the electron configuration for each element. b. Arrange the elements in order of decreasing atomic radius. c. Arrange the elements in order of increasing ionization energy. d. Use the electron configurations in part a to explain the differences between your answers to parts b and c.
Problem 99
- Explain why atomic radius decreases as you move to the right across a period for main-group elements but not for transition elements.
Problem 101
- Explain why vanadium (radius = 134 pm) and copper (radius = 128 pm) have nearly identical atomic radii, even though the atomic number of copper is about 25% higher than that of vanadium. Predict the relative densities of these two metals. Look up the densities in a reference book, periodic table, or on the Internet to check if your predictions are correct.
Problem 102
- The lightest noble gases, such as helium and neon, are completely inert—they do not form any chemical compounds whatsoever. In contrast, the heavier noble gases do form a limited number of compounds. Explain this difference in terms of trends in fundamental periodic properties.
Problem 103