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Chapter 8: Problem 65

Use the alkali metals and alkaline earth metals as examples to show how we can predict the chemical properties of elements simply from their electron configurations.

Short Answer

Expert verified
Chemical properties of elements can be predicted by their electron configurations. Alkali metals, having 1 valence electron, are highly reactive and tend to form +1 cations. Alkaline earth metals, with 2 valence electrons, are less reactive but form +2 cations. The same concept could be used to predict the chemical properties of other elements.

Step by step solution

01

Understand Electron Configuration

Electron configuration refers to the arrangement of electrons in the atomic orbitals. Alkali metals, found in Group 1 of the periodic table, have an electron configuration of [noble gas]ns1, where 'noble gas' represents the electron configuration of the closest preceding noble gas and 'ns1' shows that alkali metals have 1 electron in their outermost (valence) shell. On the other hand, Alkaline earth metals, in Group 2, possess the electron configuration [noble gas]ns2, meaning they have 2 electrons in their valence shell.
02

Relate Electron Configuration to Chemical Properties

The chemical properties of an element are predominantly determined by the electrons in the valence shell. Elements with similar electron configurations exhibit similar chemical properties. Alkali metals are highly reactive due to the single electron in their outer shell, which is readily given up to form a positive ion (cation). Similarly, alkaline earth metals tend to lose both electrons in their valence shell, forming a +2 cation. They are less reactive than alkali metals though, as the removal of two electrons requires more energy.
03

Predict Chemical Properties

Using alkaline metals, we can predict that elements with a single valence electron (ns1 configuration) will be highly reactive and form +1 cations upon losing that electron. From the alkaline earth metals, we infer that elements with two valence electrons (ns2 configuration) will be less reactive than those in the first group and form +2 cations upon ionization. This principle can be applied to predict the chemical properties of other elements based on their electron configurations.

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Most popular questions from this chapter

State whether each of the elements listed here is a gas, a liquid, or a solid under atmospheric conditions. Also state whether it exists in the elemental form as atoms, as molecules, or as a three-dimensional network: \(\mathrm{Mg}, \mathrm{Cl}, \mathrm{Si}, \mathrm{Kr}, \mathrm{O}, \mathrm{I}\) \(\mathrm{Hg}, \mathrm{Br}\).

An ion \(\mathrm{M}^{2+}\) derived from a metal in the first transition metal series has four and only four electrons in the \(3 d\) subshell. What element might \(\mathrm{M}\) be?

Give the physical states (gas, liquid, or solid) of the representative elements in the fourth period at 1 atm and \(25^{\circ} \mathrm{C}: \mathrm{K}, \mathrm{Ca}, \mathrm{Ga}, \mathrm{Ge}, \mathrm{As}, \mathrm{Se}, \mathrm{Br}\).

Acidic oxides are those that react with water to produce acid solutions, whereas the reactions of basic oxides with water produce basic solutions. Nonmetallic oxides are usually acidic, whereas those of metals are basic. Predict the products of the reactions of these oxides with water: \(\mathrm{Na}_{2} \mathrm{O}, \mathrm{BaO}, \mathrm{CO}_{2}\), \(\mathrm{N}_{2} \mathrm{O}_{5}, \mathrm{P}_{4} \mathrm{O}_{10}, \mathrm{SO}_{3} .\) Write an equation for each of the reactions.

What is Moseley's contribution to the modern periodic table?
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