Problem 35
Arrange the following atoms in order of increasing atomic radius: \(\mathrm{Na}, \mathrm{Al}, \mathrm{P}, \mathrm{Cl}, \mathrm{Mg}\).
Problem 36
Which is the largest atom in the third period of the periodic table?
Problem 37
Which is the smallest atom in Group \(7 \mathrm{~A}\) ?
Problem 41
Use the second period of the periodic table as an example to show that the size of atoms decreases as we move from left to right. Explain the trend.
Problem 42
Arrange the following in order of increasing first ionization energy: \(\mathrm{Na}, \mathrm{Cl}, \mathrm{Al}, \mathrm{S},\) and \(\mathrm{Cs}\).
Problem 43
Arrange the following in order of increasing first ionization energy: F, K. P, Ca, and Ne
Problem 44
Use the third period of the periodic table as an example to illustrate the change in first ionization energies of the elements as we move from left to right. Explain the trend.
Problem 45
In general, the first ionization energy increases from left to right across a given period. Aluminum, however, has a lower first ionization energy than magnesium. Explain.
Problem 46
The first and second ionization energies of \(\mathrm{K}\) are 419 and \(3052 \mathrm{~kJ} / \mathrm{mol}\), and those of \(\mathrm{Ca}\) are 590 and \(1145 \mathrm{~kJ} /\) mol, respectively. Compare their values and comment on the differences.
Problem 47
Two atoms have the electron configurations \(1 s^{2} 2 s^{2} 2 p^{6}\) and \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}\). The first ionization energy of one is \(2080 \mathrm{~kJ} / \mathrm{mol}\), and that of the other is \(496 \mathrm{~kJ} / \mathrm{mol}\). Match each ionization energy with one of the given electron configurations. Justify your choice.
