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- Why does the lightest halogen, which is also the most chemically reactive, exhibit a decrease in reactivity as you move down the column of halogens in the periodic table? Explain this trend in terms of periodic properties.
Problem 104
- What are the general outer electron configurations (nsx npy) for groups 6A and 7A in the periodic table? The electron affinity of each group 7A element is more negative than that of each corresponding group 6A element. Use the electron configurations to explain why this is so.
Problem 105
- Why is the electron affinity of each group 5A element more positive than that of each corresponding group 4A element? Use the outer electron configurations for these columns to suggest a reason for this observation.
Problem 106
Problem 107
The elements with atomic numbers 35 and 53 have similar chemical properties. Based on their electronic configurations, predict the atomic number of a heavier element that also should share these chemical properties.
- What are the electron configurations of the six cations that sulfur forms, by losing one to six electrons? For cations with unpaired electrons, please provide orbital diagrams.
Problem 108
Problem 109
You have cracked a secret code that uses elemental symbols to spell words. The code uses numbers to designate the elemental symbols. Each number is the sum of the atomic number and the highest principal quantum number of the highest occupied orbital of the element whose symbol is to be used. The message may be written forward or backward. Decode the following messages: a. 10, 12, 58, 11, 7, 44, 63, 66
Problem 111
Use Coulomb's law to calculate the ionization energy in kJ>mol of an atom composed of a proton and an electron separated by 100.00 pm. What wavelength of light has sufficient energy to ionize the atom?
Problem 112
The first ionization energy of sodium is 496 kJ/mol. Use Coulomb's law to estimate the average distance between the sodium nucleus and the 3s electron. How does this distance compare to the atomic radius of sodium? Explain the difference.
Problem 113
Consider the elements: B, C, N, O, F. d. Which element has three unpaired electrons?
Problem 114
Consider the elements: Na, Mg, Al, Si, P. a. Which element has the highest second ionization energy?
Problem 114b
Consider the elements: Na, Mg, Al, Si, P. b. Which element has the smallest atomic radius?
Problem 114c
Consider the elements: Na, Mg, Al, Si, P. c. Which element is least metallic?
Problem 114d
Consider the elements: Na, Mg, Al, Si, P. d. Which element is diamagnetic?