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Chapter 7: Problem 103

There are certain similarities in properties that exist between the first member of any periodic family and the element located below it and to the right in the periodic table. For example, in some ways Li resembles \(\mathrm{Mg}\), Be resembles \(\mathrm{Al}\), and so forth. This observation is called the diagonal relationship. Using what we have learned in this chapter, offer a possible explanation for this relationship.

Short Answer

Expert verified
In conclusion, the diagonal relationship in the periodic table can be explained by considering factors such as electronic configuration, atomic size, and electronegativity. Elements with a diagonal relationship have similar electronic configurations (with a small difference in p-orbitals), comparable atomic sizes, and electronegativity values due to the periodic trends. These factors contribute to the similarities in properties between the elements in the diagonal relationship, such as Li with Mg and Be with Al.

Step by step solution

01

Identify elements and their positions

First, identify the elements that exhibit the diagonal relationship in the periodic table. These include: 1. Lithium (Li) and Magnesium (Mg) 2. Beryllium (Be) and Aluminum (Al) The relationship occurs between elements from Group 1 (alkali metals) and Group 2 (alkaline earth metals).
02

Electronic configuration

Analyze the electronic configuration of these elements and how they are related. Electronic configurations are as follows: 1. Li: \(1s^2 2s^1\) 2. Mg: \(1s^2 2s^2 2p^6 3s^2\) 3. Be: \(1s^2 2s^2\) 4. Al: \(1s^2 2s^2 2p^6 3s^2 3p^1\) We can see that both Li and Mg have two outermost electrons in the s-orbital, and Be and Al have a similar configuration, with Al having one additional electron in the p-orbital.
03

Atomic size

Examine the trend in atomic size across the periodic table. Typically, atomic size decreases going across a period (left to right) and increases going down a group (top to bottom). Due to this trend, elements having a diagonal relationship have similar atomic sizes. This similarity in atomic size can also partly explain the resemblance of properties between the elements with diagonal relationships.
04

Electronegativity

Investigate the trend in electronegativity across the periodic table. Electronegativity generally increases going across a period (left to right) and decreases going down a group (top to bottom). Looking at the elements with diagonal relationships, we can see that they have similar electronegativity values: 1. Li: 0.98 2. Mg: 1.31 3. Be: 1.57 4. Al: 1.61 The similarity in electronegativity values also contributes to the likeness in properties between the elements with diagonal relationships.
05

Conclusion

In conclusion, the diagonal relationship in the periodic table can be explained by considering factors such as electronic configuration, atomic size, and electronegativity. Elements with a diagonal relationship have similar electronic configurations (with a small difference in p-orbitals), comparable atomic sizes, and electronegativity values due to the periodic trends. These factors contribute to the similarities in properties between the elements in the diagonal relationship, such as Li with Mg and Be with Al.

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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 \(\mathrm{Ca}^{2+}\).

Some ions do not have a corresponding neutral atom that has the same electron configuration. For each of the following ions identify the neutral atom that has the same number of electrons and determine if this atom has the same electron configuration. If such an atom does not exist explain why: (a) \(\mathrm{Cl}^{-}\) (b) \(\mathrm{Sc}^{3+}\) (c) \(\mathrm{Fe}^{2+}\), (d) \(\mathrm{Zn}^{2+}\), (e) \(\mathrm{Sn}^{4+}\).

Write a balanced equation for the reaction that occurs in each of the following cases: (a) Potassium metal burns in an atmosphere of chlorine gas, (b) Strontium oxide is added to water. (c) A fresh surface of lithium metal is exposed to oxygen gas. (d) Sodium metal is reacted with molten sulfur.

(a) Why is cesium more reactive toward water than is lithium? (b) 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? (c) Write a balanced chemical equation for reaction of the white substance with water.

(a) Why does Li have a larger first ionization energy than Na? (b) The difference between the third and fourth ionization energies of scandium is much larger than the difference between the third and fourth ionization energies of titanium. Why? (c) Why does Li have a much larger second ionization energy than Be?
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