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Chapter 7: Problem 75

(a) If we arrange the elements of the second period (Li-Ne) in order of increasing first ionization energy, where would hydrogen fit into this series? (b) If we now arrange the elements of the third period (Na-Ar) in order of increasing first ionization energy, where would lithium fit into this series? (c) Are these series consistent with the assignment of hydrogen as a nonmetal and lithium as a metal?

Short Answer

Expert verified
When arranged in order of increasing first ionization energy, hydrogen fits between carbon and oxygen in the second period, and lithium fits between sodium and aluminum in the third period. This is consistent with the assignment of hydrogen as a nonmetal and lithium as a metal.

Step by step solution

01

Arrange the elements of second and third periods.

The elements of the second period are Li, Be, B, C, N, O, F, Ne. The elements of the third period are Na, K, Al, Si, P, S, Cl, Ar.
02

Find ionization energies

First ionization energies (in eV) of the elements are: First period: H (13.6) Second period: Li (5.4), Be (9.3), B (8.3), C (11.3), N (14.5), O (13.6), F (17.4), Ne (21.6) Third period: Na (5.1), Mg (7.6), Al (5.99), Si (8.2), P (10.5), S (10.4), Cl (12.97), Ar (15.76)
03

Arrange elements by increasing ionization energy

Second period (excluding H): Li (5.4), Be (9.3), B (8.3), C (11.3), N (14.5), O (13.6), F (17.4), Ne (21.6) Third period (excluding Li): Na (5.1), Mg (7.6), Al (5.99), Si (8.2), P (10.5), S (10.4), Cl (12.97), Ar (15.76)
04

(a) Find the position where hydrogen fits into the second period

Compare the first ionization energy of hydrogen (H: 13.6 eV) to the second period elements: Li (5.4) < B (8.3) < Be (9.3) < C (11.3) < H (13.6) < O (13.6) < N (14.5) < F (17.4) < Ne (21.6) The position of hydrogen in the second period is between carbon and oxygen.
05

(b) Find the position where lithium fits into the third period

Compare the first ionization energy of lithium (Li: 5.4 eV) to the third period elements: Li (5.4) < Na (5.1) < Al (5.99) < Mg (7.6) < Si (8.2) < S (10.4) < P (10.5) < Cl (12.97) < Ar (15.76) The position of lithium in the third period is between sodium and aluminum.
06

Determine if the series are consistent with the assignment of hydrogen as a nonmetal and lithium as a metal

In the second period, hydrogen is placed between carbon and oxygen, which are both nonmetals. Therefore, it is consistent with hydrogen being a nonmetal. In the third period, lithium is placed between sodium and aluminum, which are both metals. Therefore, it is consistent with lithium being a metal. Thus, the series are consistent with the assignment of hydrogen as a nonmetal and lithium as a metal.

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Most popular questions from this chapter

For each of the following statements, provide an explanation (a) \(\mathrm{O}^{2-}\) is larger than \(\mathrm{O} ;\) (b) \(\mathrm{S}^{2-}\) is larger than \(\mathrm{O}^{2-}\) : (c) \(S^{2-}\) is larger than \(K^{+}\); (d) \(\mathrm{K}^{+}\) is larger than \(\mathrm{Ca}^{2+}\).

The distance between \(\mathrm{W}\) atoms in tungsten metal is \(2.74 \mathrm{~A}\). What is the atomic radius of a tungsten atom in this environment? (This radius is called the metallic radius)

Detailed calculations show that the value of \(Z_{\text {eff }}\) for \(\mathrm{Si}\) and \(\mathrm{Cl}\) atoms is \(4.29+\) and \(6.12+\), respectively. (a) What value do you estimate for \(Z_{\text {eff }}\) experienced by the outermost electron in both \(\mathrm{Si}\) and \(\mathrm{Cl}\) by assuming core electrons contribute \(1.00\) and valence electrons contribute \(0.00\) to the screening constant? (b) What values do you estimate for \(Z_{\text {eff }}\) using Slater's rules? (c) Which approach gives a more accurate estimate of \(Z_{\text {eff }} ?\) (d) Which method of approximation more accurately accounts for the steady increase in \(Z_{\text {eff }}\) that occurs upon moving left to right across a period?

(a) If the core electrons were totally effective at shielding the valence electrons and the valence electrons provided no shielding for each other, what would be the effective nuclear charge acting on the 3 s and \(3 p\) valence electrons in \(P\) ? (b) Repeat these calculations using Slater's rules. (c) Detailed calculations indicate that the effective nuclear charge is \(5.6+\) for the 3 s electrons and \(4.9+\) for the \(3 p\) electrons. Why are the values for the 3 s and \(3 p\) electrons different? (d) If you remove a single electron from a \(\mathrm{P}\) atom, which orbital will it come from? Explain.

Detailed calculations show that the value of \(Z_{\text {eff }}\) for \(\mathrm{Na}\) and \(K\) atoms is \(2.51+\) and \(3.49+\), respectively. (a) What value do you estimate for \(Z_{\text {eff }}\) experienced by the outermost electron in both Na and \(K\) by assuming core electrons contribute \(1.00\) and valence electrons contribute \(0.00\) to the screening constant? (b) What values do you estimate for \(Z_{\text {eff }}\) using Slater's rules? (c) Which approach gives a more accurate estimate of \(Z_{\text {eff }} ?\) (d) Does either method of approximation account for the gradual increase in \(Z_{\text {eff }}\) that occurs upon moving down a group?
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