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Chapter 7: Problem 67

(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 has a lower second ionization energy, attributed to its larger atomic size and higher electron shielding effect, making it easier for calcium to lose electrons. (b) Calcium is generally less reactive than potassium because potassium has a lower first ionization energy, which results from its lower nuclear charge and larger atomic size, allowing potassium to lose an electron more easily and be more reactive than calcium.

Step by step solution

01

Part (a): Electron configurations

First, let's look at the electron configurations and the periodic table positions of calcium (Ca) and magnesium (Mg). Calcium (Ca): Atomic number 20, Electron configuration: [Ar] 4s虏 Magnesium (Mg): Atomic number 12, Electron configuration: [Ne] 3s虏 Both calcium and magnesium belong to the same group (Group 2) in the periodic table, making them alkaline earth metals.
02

Part (a): Ionization energy

In order to compare reactivity, we can look at the ionization energy, which represents the energy needed to remove an electron from an atom. The lower the ionization energy, the more easily an element loses an electron, and the more reactive it is. Group 2 elements typically lose 2 electrons to form a 虏鈦� ion, so we will compare the second ionization energies of calcium and magnesium.
03

Part (a): Trends in the periodic table

As we move down a group in the periodic table, ionization energies generally decrease due to: 1. An increase in atomic size 2. Electron shielding effect Calcium has a lower second ionization energy than magnesium because it has a larger atomic size and higher electron shielding effect, which makes it easier for calcium to lose electrons and be more reactive than magnesium.
04

Part (b): Electron configurations

Now, let's compare the reactivity of calcium (Ca) and potassium (K). Potassium (K): Atomic number 19, Electron configuration: [Ar] 4s鹿 Note that potassium is in the same period as calcium but belongs to a different group (Group 1) in the periodic table, making it an alkali metal.
05

Part (b): Ionization energy

Alkali metals typically lose 1 electron to form a 鹿鈦� ion, so we will compare the first ionization energies of calcium and potassium.
06

Part (b): Trends in the periodic table

As we move from left to right in a period in the periodic table, ionization energies generally increase due to: 1. An increase in nuclear charge 2. A decrease in atomic size Potassium has a lower first ionization energy than calcium because it has a lower nuclear charge and larger atomic size, making it easier for potassium to lose an electron and be more reactive than calcium.

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Most popular questions from this chapter

Consider the following equation: $$ \mathrm{Ca}^{+}(g)+\mathrm{e}^{-} \longrightarrow \mathrm{Ca}(g) $$ Which of the following statements are true? (i) The energy change for this process is the electron affinity of the \(\mathrm{Ca}^{+}\)ion. (ii) The energy change for this process is the negative of the first ionization energy of the Ca atom. (iii) The energy change for this process is the negative of the electron affinity of the \(\mathrm{Ca}\) atom.

Write equations that show the process for (a) the first two ionization energies of lead and (b) the fourth ionization energy of zirconium.

Which will experience the greater effective nuclear charge, the electrons in the \(n=3\) shell in Ar or the \(n=3\) shell in \(\mathrm{Kr}\) ? Which will be closer to the nucleus?

Arrange each of the following sets of atoms and ions, in order of increasing size: (a) \(\mathrm{Se}^{2-}, \mathrm{Te}^{2-}, \mathrm{Se} ;\) (b) \(\mathrm{Co}^{3+}, \mathrm{Fe}^{2+}, \mathrm{Fe}^{3+}\); (c) \(\mathrm{Ca}^{2 \mathrm{Ti}^{4+}}, \mathrm{Sc}^{3+}\); (d) \(\mathrm{Be}^{2+}, \mathrm{Na}^{+}, \mathrm{Ne}\).

Using only the periodic table, arrange each set of atoms in order from largest to smallest: (a) K, Li, Cs; (b) Pb, Sn, Si; (c) F, O, N.
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