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Chapter 7: Problem 71

(a) Why is calcium generally more reactive than magnesium? (b) Why is calcium generally less reactive than potassium?

Short Answer

Expert verified
(a) Calcium is generally more reactive than magnesium because it is located below magnesium in Group 2 of the periodic table. This means that calcium's outer electron shell is further from the nucleus, making it easier for calcium to lose its valence electrons compared to magnesium. (b) Calcium is generally less reactive than potassium because potassium is in Group 1, with only one valence electron, making it inherently more reactive than calcium which has two valence electrons. Additionally, the tendency of potassium to lose its valence electron is stronger due to its position in Group 1, despite the shorter distance between its nucleus and the outer electron shell.

Step by step solution

01

(Understand the periodic table)

(First of all, let's locate calcium (Ca), magnesium (Mg), and potassium (K) in the periodic table. Calcium and magnesium are both in Group 2, known as the alkaline earth metals, and potassium is in Group 1, known as the alkali metals. Calcium is located below magnesium in the same group, and potassium is located to the left of calcium in a different group. In general, elements in Group 1 are more reactive than those in Group 2, and reactivity increases as you move down a group. This is because elements in Group 1 have one valence electron, whereas elements in Group 2 have two. Additionally, as you move down a group, the outer electron shell is further from the nucleus, making it easier to lose the valence electrons in chemical reactions.)
02

(Analyze the electron configurations)

(Let's examine the electron configurations of calcium, magnesium, and potassium to better understand their reactivity: Calcium (Ca): \([Ar] 4s^2\) Magnesium (Mg): \([Ne] 3s^2\) Potassium (K): \([Ar] 4s^1\) The reactivity of these elements is determined by the ease with which they can lose their valence electrons to form positive ions.)
03

(a) Explain reactivity difference between calcium and magnesium)

(As mentioned earlier, both calcium and magnesium are in Group 2 and have two valence electrons. Since calcium is located below magnesium in the periodic table, its outer electron shell is further from the nucleus, and the attraction between these valence electrons and the nucleus is weaker. As a result, calcium can lose its valence electrons more easily than magnesium, making it more reactive.)
04

(b) Explain reactivity difference between calcium and potassium)

(On the other hand, potassium is in Group 1 and has only one valence electron. This makes it inherently more reactive than calcium with its two valence electrons. Furthermore, potassium is also located above calcium in the periodic table, and its outer electron shell is closer to the nucleus. However, due to being in Group 1, the tendency of potassium to lose its valence electron is stronger than that of calcium, even with the shorter distance between the nucleus and the outer electron shell. So, potassium is generally more reactive than calcium.)

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Most popular questions from this chapter

(a) What is the general relationship between the size of an atom and its first ionization energy? (b) Which element in the periodic table has the largest ionization energy? Which has the smallest?

(a) Write the electron configuration for \(\mathrm{Li}\), and estimate the effective nuclear charge experienced by the valence electron. (b) The energy of an electron in a one-electron atom or ion equals \(\left(-2.18 \times 10^{-18} \mathrm{~J}\right)\left(\frac{Z^{2}}{n^{2}}\right)\) where \(Z\) is the nuclear charge and \(n\) is the principal quantum number of the electron. Estimate the first ionization energy of Li. (c) Compare the result of your calculation with the value reported in Table 7.4 and explain the difference. (d) What value of the effective nuclear charge gives the proper value for the ionization energy? Does this agree with your explanation in \((\mathrm{c}) ?\)

(a) What is the trend in first ionization energies as one proceeds down the group 7 A elements? Explain how this trend relates to the variation in atomic radii. (b) What is the trend in first ionization energies as one moves across the fourth period from \(\mathrm{K}\) to \(\mathrm{Kr}\) ? How does this trend compare with the trend in atomic radii?

Arrange the following oxides in order of increasing acidity: \(\mathrm{CO}_{2}, \mathrm{CaO}, \mathrm{Al}_{2} \mathrm{O}_{3}, \mathrm{SO}_{3}, \mathrm{SiO}_{2},\) and \(\mathrm{P}_{2} \mathrm{O}_{5}\)

Chlorine reacts with oxygen to form \(\mathrm{Cl}_{2} \mathrm{O}_{7} .\) (a) What is the name of this product (see Table 2.6 )? (b) Write a balanced equation for the formation of \(\mathrm{Cl}_{2} \mathrm{O}_{7}(l)\) from the elements. (c) Under usual conditions, \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) is a colorless liquid with a boiling point of \(81^{\circ} \mathrm{C}\). Is this boiling point expected or surprising? (d) Would you expect \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) to be more reactive toward \(\mathrm{H}^{+}(a q)\) or \(\mathrm{OH}^{-}(a q) ?\) Explain. (e) If the oxygen in \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) is considered to have the -2 oxidation state, what is the oxidation state of the Cl? What is the electron configuration of \(\mathrm{Cl}\) in this oxidation state?
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