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Chapter 7: Problem 82

As we move across a period of the periodic table, why do the sizes of the transition elements change more gradually than those of the representative elements?

Short Answer

Expert verified
The sizes of transition elements change more gradually across a period compared to the representative elements because the additional d-electrons filling their d orbitals are less effective at shielding the outermost electrons from the increasing nuclear charge. This results in a slower decrease in atomic size compared to the regular trend observed in representative elements, which are primarily filling their s and p orbitals.

Step by step solution

01

Identifying the transition and representative elements

The representative elements are the elements found in groups 1A to 7A in the periodic table, while the transition elements are the ones located in group 3 through group 12, the d-block. Representative elements exhibit regular trends in atomic size, ionization energy, and electron affinity, while transition elements have more complicated trends owing to their electron configurations.
02

Details about atomic size

Atomic size is generally measured by the atomic radius, the distance from the nucleus to the outermost electron shell. It's important to note that as we move across a period, the atomic number (number of protons) increases, leading to a higher effective nuclear charge on the electrons. This increased charge causes the electrons to be more strongly attracted to the nucleus, reducing the atomic size.
03

Comparing atomic size trends in representative elements

Representative elements follow a predictable trend in atomic size across a period. As the atomic number increases, the atomic size decreases. This decrease in atomic size is due to the increase in effective nuclear charge experienced by the outermost electrons. These elements adhere closely to this trend since they are filling their s and p orbitals across the period, and there is limited shielding effect from inner electron shells.
04

Exploring atomic size trends in transition elements

In transition elements, the size changes more gradually as we move across a period. The transition metals fill their d orbitals, which are located between the outermost s and p electrons. The d-orbitals' ability to shield the outer electrons from the nucleus's increasing positive charge is weaker compared to the s and p orbitals. Therefore, the increase in effective nuclear charge is only partially offset by the increased shielding provided by the additional d-electrons. Consequently, the atomic size does not reduce as drastically as it does in the representative elements.
05

Concluding the explanation

In summary, the sizes of transition elements change more gradually across a period compared to the representative elements because the additional d-electrons filling their d orbitals are less effective at shielding the outermost electrons from the increasing nuclear charge. This results in a slower decrease in atomic size compared to the regular trend observed in representative elements, which are primarily filling their s and p orbitals.

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Most popular questions from this chapter

Consider the isoelectronic ions \(\mathrm{F}^{-}\)and \(\mathrm{Na}^{+}\). (a) Which ion is smaller? (b) Using Equation \(7.1\) and assuming that core electrons contribute \(1.00\) and valence electrons contribute \(0.00\) to the screening constant, \(S\), calculate \(Z_{\text {eff }}\) for the \(2 p\) electrons in both ions. (c) Repeat this calculation using Slater's rules to estimate the screening constant, \(S\). (d) For isoelectronic ions, how are effective nuclear charge and ionic radius related?

Discussing this chapter, a classmate says, "Since elements that form cations are metals and elements that form anions are nonmetals, elements that do not form ions are metalloids." Do you agree or disagree? Explain your answer.

The As - As bond length in elemental arsenic is \(2.48 \AA\). The \(\mathrm{Cl}-\mathrm{Cl}\) bond length in \(\mathrm{Cl}_{2}\) is \(1.99 \AA\). (a) Based on these data, what is the predicted As - Cl bond length in arsenic trichloride, \(\mathrm{AsCl}_{3}\), in which each of the three \(\mathrm{Cl}\) atoms is bonded to the As atom? (b) What bond length is predicted for \(\mathrm{AsCl}_{3}\), using the atomic radii in Figure 7.7?

Which of the following is the expected product of the reaction of \(\mathrm{K}(s)\) and \(\mathrm{H}_{2}(g)\) ? (i) \(\mathrm{KH}(s)\), (ii) \(\mathrm{K}_{2} \mathrm{H}(s)\), (iii) \(\mathrm{KH}_{2}(s)\), (iv) \(\mathrm{K}_{2} \mathrm{H}_{2}(s)\), or (v) \(\mathrm{K}(s)\) and \(\mathrm{H}_{2}(g)\) will not react with one another.

(a) One of the alkali metals reacts with oxygen to form a solid white substance. When this substance is dissolved in water, the solution gives a positive test for hydrogen peroxide, \(\mathrm{H}_{2} \mathrm{O}_{2}\). When the solution is tested in a burner flame, a lilac-purple flame is produced. What is the likely identity of the metal? (b) Write a balanced chemical equation for the reaction of the white substance with water.
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